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Which of the following is true of a reversible reaction? a. Equilibrium can only be reached by mixing the starting material b. Equilibrium can only be reached by mixing the products c. Equilibrium can only be reached by mixing specific amounts of starting materials and products d. Provided one is prepared to wait long enough, equilibrium will always be reached if any combination of starting material and products are mixed

Provided one is prepared to wait long enough, equilibrium will always be reached if any combination of starting material and products are mixed

Which of the following is a mathematical statement of the combined gas law? a. P₁V₂/T₁ = P₂V₁/T₂ b. P₁V₂/T₂ = P₂V₁/T₁ c. P₁V₁/T₂ = P₂V₂/T₁ d. P₁V₁/T₁ = P₂V₂/T₂

P₁V₁/T₁ = P₂V₂/T₂

Name binary ionic compound Ag2S

Silver Sulfide

octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons, it is particularly common among Group 1A-7A.

Sr2+

Strontium ion

SO4 2-

Sulfate

S2 - anion name

Sulfide

SO2 2-

Sulfite

Increasing which of the following will decrease the pH of a buffer made using acetic acid and sodium acetate? a. The amount of water present b. The [C₂H₃O₂-] (sodium acetate) c. The ratio of [C₂H₃O₂-]/[HC₂H₃O₂] d. The [HC₂H₃O₂] (acetic acid)

The [HC₂H₃O₂] (acetic acid)

Lewis Structure Rules

-least electronegative is central atom -hydrogen and halogens (F,Cl,Br, and I) occupy ends -Complete octets of all outer atoms -place extras on central atoms

Which of the following an example of an equilibrium situation?

. a saturated solution

Ammonium ion has the formula NH4+. How many nonbonding electrons must be shown in the Lewis structure?

Which of the following can be characterized as a strong electrolyte? a. 0.001 M KOH b. 3.0 M NH₂ c. both a and b d. neither a nor b

0.001 M KOH

In the reaction 2HgO(s) → 2Hg(l) + O2(g) we measure the evolution of gas to determine the rate of reaction. At the beginning of the reaction (at 0 minutes), 0.020 L of O2 is present. After 15 minutes the volume of O2 is 0.35 L. What is the rate of reaction?

0.022 L/min

In the reaction 2HgO(s) 2Hg(l) + O2(g) we measure the evolution of gas to determine the rate of reaction. At the beginning of the reaction (at 0 minutes), 0.020 L of O2 is present. After 15 minutes the volume of O2 is 0.35 L. What is the rate of reaction?

0.022L/min

Which of the following aqueous solutions of Na₂SO₄ is hypotonic with respect to a 0.15 M NaCl solution? a. 0.05 M b. 0.10 M c. 0.15 M d. none of these

0.05 M

For the reaction given below, at 25°C equilibrium is established when [NOCl] = 2.6 M, [NO] = 1.4 M and [Cl2] = 0.34 M.What is the equilibrium constant for this reaction?

0.099

Which of the following will have the lowest freezing point? [DT = -1.86°C/mole x moles of particles]

0.1 M AlCl3

Which of the following will have the lowest freezing point? a. 0.1 M NaCl b. 0.1 M BaCl₂ c. 0.1 M AlCl₃ d. all have the same freezing point

0.1 M AlCl₃

Which of the following aqueous solutions of Na₂SO₄ is isotonic with a 0.15 M NaCl solution? a. 0.05 M b. 0.10 M c. 0.15 M d. none of these

0.10 M

A vessel under 2.015 atm pressure contains nitrogen, N₂, and water vapor, H₂O. The partial pressure of N₂ is 1.908 atm. What is the partial pressure of the water vapor? a. 0.107 atm b. 1.908 atm c. 2.015 atm d. 3.923 atm

0.107 atm

How many moles of solute are contained in 500. mL of 0.50 M KCl? [Molarity (M) = moles/V(Liters)]

0.25 moles

A solution is prepared by dissolving 3.50 grams of NH4Cl in enough water to make 250. mL of solution. What is the concentration of this solution? [1 mole = MW(grams); Molarity (M) = moles/V(Liters)]

0.262 M

A certain quantity of neon gas is under 1.05 atm pressure at 303 K in a 10.0 L vessel. How many moles of neon are present? [PV = nRT; R = 0.0821L.atm.mol-1.K-1]

0.422 mol

A particular chemical reaction carried out at 20°C takes 2 hours. Approximately how long will it take to carry out the reaction at 40°C?

0.5 hour

A gas is expanded from an initial volume of 20.5 L at 0.92 atm at 23 °C to a final volume of 34.6 L. During the expansion the gas cools to 12 °C. What is the final pressure? [K = 0C + 273; P1V1/T1 = P2V2/T2]

0.52 atm

What is the osmolarity of a 3.3%(w/v) Na₃PO₄ solution? a. 0.20 osmolar b. 0.40 osmolar c. 0.80 osmolar d. 1.6 osmolar

0.80 osmolar

What is the osmolarity of a 3.3%(w/v) Na₃PO₄ solution? a. 0.20 osmolar b. 1.6 osmolar c. 0.40 osmolar d. 0.80 osmolar

0.80 osmolar

Which of the following is called standard temperature and pressure? a. 0°C and 1 atm b. 0°F and 1 atm c. 0 K and 1 atm d. none of these

0°C and 1 atm

Which of the following could be the equilibrium constant for a reaction which does not yield a significant concentration of products? a. 1 x 10⁻¹⁵ c. 1 x 10 ² b. 1 x 10⁻² d. 1 x 10¹⁵

1 x 10⁻¹⁵

resonance structure must

1. Have the same number of valence electrons. 2. Obey the rules of covalent bonding. 3. Differ only in distribution of valence electrons; the position of all nuclei must be the same. 4. Have the same number of paired and unpaired electrons.

Which of the following is the numerical value of Kw at room temperature? a. 1.0 x 10⁻¹⁴ b. 1.0 x 10⁻⁷ c. 1.0 x 10⁷ d. 1.0 x 10¹⁴

1.0 x 10⁻¹⁴

In an aqueous solution the [H⁺] is 1.0 x 10⁻⁶ M. What is the [OH⁻]? a. 1.0 x10⁻⁹ M b. 1.0 x 10⁻⁸ M c. 1.0 x 10⁻⁶ M d. 1.0 x 10⁸ M

1.0 x 10⁻⁸ M

In an aqueous solution the [H⁺] is 1.0x10⁻⁶M. What is the [OH-]? a. 1.0x10⁻⁸M b. 1.0x10⁻⁹M c. 1.0x10⁸M d. 1.0x10⁻⁶M

1.0x10⁻⁸M

What is the mass of one molecule of cholesterol?

1.18 x 10^-21 g

An HCl solution has a pH of 3.10, what is the [OH⁻] in this solution? a. 7.9 x 10⁻¹⁸ M b. 1.3 x 10⁻¹¹ M c. 7.9 x 10⁴ M d. 1.3 x 10³ M

1.3 x 10⁻¹¹ M

An acetic acid solution has a pH of 5.80, what is the [H⁺] in this solution? a. 1.6 x 10⁻²⁰ M b. 6.3 x 10⁻⁹ M c. 1.6 x 10⁻⁶ M d. 6.3 x 10⁵ M

1.6 x 10⁻⁶ M

The pKa of formic acid is 3.75. What is the Ka of formic acid? a. 1.8x10⁻¹⁸ b. 5.6x10⁻¹¹ c. 1.8x10⁻⁴ d. 5.6x10³

1.8x10⁻⁴

If a solution is prepared by dissolving 7.7 g of lithium iodide, LiI, in enough water to make 400. mL of solution, what is the %(w/v) of LiI?

1.9%

A solution is prepared by dissolving 104.10 grams of barium chloride, BaCl2 in 1000. grams of water? What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000g of water]

100.78 C

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000 grams of water. What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000g of water] a. 93.0°C b. 96.5°C c. 103.5°C d. 107.0°C

103.5°C

Which of the following pH's corresponds to a highly basic solution? a. 2.8 b. 6.8 c. 7.2 d. 11.2

11.2

Which of the following pHs corresponds to a highly basic solution? a. 6.8 b. 2.8 c. 2.7 d. 11.2

11.2

Isotonic saline is 0.89% NaCl (w/v). Suppose you wanted to make a liter of isotonic solution of KCl. What weight of KCl would you need? a. 8.9 g b. 11.4 g c. 22.8 g d. 74.6 g

11.4

Formaldehyde has a chemical formula CH2O. How many electrons must be shown in the Lewis structure of formaldehyde.

At constant temperature the pressure on a 6.0 L sample of a gas is reduced from 2.0 atm to 1.0 atm. What is the new volume of the gas sample? [P1V1 = P2V2]

12 L

At constant temperature the pressure on a 6.0 liter sample of a gas is reduced from 2.0 atm to 1.0 atm. What is the new volume of the gas sample? a. 3.0 liters b. 0.083 liters c. 0.33 liters d. 12 liters

12 liters

a trigonal pair has an angle of

120 degrees

If an 8.00 gram sample of molecular oxygen at 1.00 atm pressure occupies 3.00 L, what is the temperature of the sample? a. 73°C b. 73 K c. 146°C d. 146 K

146 K

What volume of 12.0 M HCl must be used to make 300. mL of 0.600 M HCl? [M1V1 = M2V2]

15.0 mL

Dry air is 78.08% nitrogen, 20.95% oxygen and 0.93% argon with the 0.04% being other gases. If the atmospheric pressure is 760.0 torr, what is the partial pressure of oxygen in dry air?

159.2 torr

a linear distribution has a bond angle of

180 degrees

How many electrons are associated with a single bond

How many main types of chemical bonds exist?

The toxic gas hydrogen cyanide has the formula HCN. How many nonbonding electrons must be shown in the Lewis structure of hydrogen cyanide?

the stable oxidation state of oxygen is

2- (negative)

A closed flask contains a 0.25 moles of O₂ which exerts a pressure of 0.50 atm. If 0.75 moles of CO₂ is added to the container what is the total pressure in the flask? a. 0.50 atm b. 1.0 atm c.1.5 atm d. 2.0 atm

2.0 atm

Suppose that the equilibrium constant for the chemical reaction 2A(g)⇌B(g) has an equilibrium constant of 2.3 x 10⁷. What is the equilibrium constant for the reaction 4A(g)⇌2B(g)? a. 1.99 x 10 ⁻¹⁵ c. 2.3 x 10⁷ b. 4.3 x 10 ⁻⁸ d. 5.3 x 10¹⁴

2.3 x 10⁷

Suppose a balloon is filled so that its volume is 2.00 L when the pressure is 1.10 atm and the temperature is 300 K. What volume will it occupy if it rises to an elevation where the pressure is 418 torr (0.55 atm) and the temperature is 200 K? a. 0.303 liters b. 0.375 liters c. 3.30 liters d. 2.67 liters

2.67 liters

At constant temperature the pressure on a 6.0 liter sample of gas is increased from 1.0 atm to 2.0 atm. What is the new volume of the gas sample? a. 0.33 liters b. 0.67 liters c. 1.5 liters d. 3.0 liters

3.0 liters

The Ka for lactic acid is 8.4 x 10 ⁻⁴. What is the pKa of lactic acid? a. -10.92 b. -3.08 c. 3.08 d. 10.92

3.08

For the reaction 472°C equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37 × 10-8M. What is the equilibrium constant for this reaction?

3.60x10^-8

For the reaction 3H₂2(g)+N₂(g)⇌2NH₃(g) at 472°C equilibrium is established when [H₂]=0.0200M and [NH₃]=5.37x10⁻⁸M. What is the equilibrium constant for this reaction? a. 7.21x10⁻¹¹ b. 7.21x10⁻¹⁰ c. 2.69x10⁻⁴ d. 3.60x10⁻⁸

3.60x10⁻⁸

At constant pressure the temperature of a 4.0 liter sample of gas is decreased from 50°C to 25°C. What is the new volume of the gas sample? a. 4.34 liters b. 2.00 liters c. 8.00 liters d. 3.69 liters

3.69 liters

The pKa of acetic acid, HC₂H₃O₂, is 4.75. What is the pH of a buffer in which [HC₂H₃O₂] = 2.0 M and [NaC₂H₃O₂] = 0.20 M? a. 3.75 b. 4.75 c. 5.75 d. 7.00

3.75

The pKa of acetic acid, HC₂H₃O₂, is 4.75. What is the pH of a buffer in which [HC₂H₃O₂]=2.0M and [NaC₂H₃O₂]=0.20M? a. 7.00 b. 3.75 c. 4.75 d. 5.75

3.75

Suppose a balloon is filled so that its volume is 2.00 L when the pressure is 750 torr and the temperature is 24°C. What volume will it occupy if it rises to an elevation where the pressure is 375 torr and the temperature is 12°C? [K = 0C + 273; P1V1/T1 = P2V2/T2]

3.84 L

3.84 liters

The molecular weight of sucrose is

342.3

Carbon atoms typically form

4 bonds

For the reaction 25°C equilibrium is established when [NOCl] = 2.6 M, [NO] = 0.34 M and [Cl2] = 1.4 M. What is the equilibrium constant for this reaction?

4.22 × 10^1

Saline solutions (NaCl in water) which are used to deliver intravenous drugs are 0.89%(w/v). What mass of NaCl is found in 500. mL of such a solution? [hint: a 0.89% solution contains 0.89 grams in 100 mL solution]

4.5 g

For the reaction N2 + 3H22NH3 the equilibrium concentrations, in moles/L, were found to be: [N2] = 0.70, [H2] = 1.4, [NH3] = 3.0. The equilibrium constant for this reaction is

4.7

Carbonic acid has

5 polar bonds

An ammonia solution has a pH of 8.30, what is the [H⁺] in this solution? a. 5.0x10⁻²³M b. 20.x10⁻⁶M c. 2.0x10⁸ d. 5.0x10⁻⁹

5.0x10⁻⁹

Which of the following solutions of glucose is isotonic with a 0.15 M NaCl solution? a. 0.15% b. 0.55% c. 1.5% d. 5.5%

5.5%

What is the volume occupied by an 8.00 gram sample of molecular oxygen at STP? [mole = MW (granms]; STP = 273 K, 1.0 atm; PV = nRT; R = 0.0821L.atm.mol-1.K-1]

5.60 L

The pKa of acetic acid, HC₂H₃O₂, is 4.75. What is the pH of a buffer in which [HC₂H₃O₂] = 0.20 M and [NaC₂H₃O₂] = 2.0 M? a. 3.75 b. 4.75 c. 5.75 d. 7.00

5.75

What is the mass of NaCl is in a 0.500 L bottle of 2.00 M NaCl? [1 mole = MW(grams); Molarity (M) = moles/V(Liters)]

58.5 g

How many electrons are associated with a triple bond?

Avagadro's number

6.02 x 10^23

How many molecules are present in one mole of water

6.02 x 10^23

At constant temperature the pressure on a 10.0 L sample of gas is changed from 1.00 atm to 1140 torr. What is the new volume of the gas sample? [1 atm = 760 torr; P1V1 = P2V2]

6.67 L

At constant temperature the pressure on a 10.0 liter sample of gas is changed from 1.00 atm to 1140 torr. What is the new volume of the gas sample? a. 0.00877 liters b. 6.67 liters c. 15.0 liters d. 11.4 liters

6.67 liters

Which of the following pH's corresponds to a slightly basic solution? a. 2.8 b. 6.8 c. 7.2 d. 11.2

7.2

How many moles of ethanol can be produced from 203 g of ethylene?

7.25

The ammonium ion has the formula NH4+. How many electrons must be show in the Lewis structure of the ammonium ion?

None of the atoms N, C, O can have more than

8 electrons associated

a particular chemical reaction carried out at 40 degrees C takes 2 hours. how long will it take to carry out the reaction at 20 degrees C

8 hours

A solution has a pOH of 5.4. What is its pH? a. -8.6 b. -5.4 c. 5.4 d. 8.6

8.6

If 2.00 moles of NO gas occupies 10.0 L at 295 K, what is the pressure of the gas in atmospheres? a. 0.206 atm b. 2.42 atm c. 4.84 atm d. 9.33 atm

9.33 atm

A compound used in the treatment of manic depression has the formula Li2CO3. Which of the following is the correct name for this compound? a. lithium carbonate b. dilithium carbonate c. lithium carbon trioxide d. lithium carboxide

A solution has a pOH of 5.4. What is its pH? a. 8.6 b. 5.4 c. -5.4 d. -8.6

For the reaction A + B ® 2 C, which of the following statements is true? a. B is consumed at the same rate that A is consumed. b. C is produced at the same rate A is consumed. c. both a and b d. neither a nor b

How many main types of chemical bonds exist? a. 2 b. 4 c. 1 d. 3

How many molecules are present in one mole of water, H2O? a. 6.02 ´ 10^23 b. 1.66 ´ 10^-24 c. 3.24 ´ 10^23 d. 3.00 ´ 10^-23

In a particular titration experiment a 25.0 mL sample of an unknown diprotic acid required 30.0 mL of 0.200 M NaOH for the end point to be reached. What is the concentration of the acid? a. 0.120 M b. 0.333 M c. 0.240 M d. 0.167 M

In the reaction Pb(s) + 2 Ag+(aq) ® Pb2+(aq) + 2 Ag(s) which species is reduced? a. Ag+(aq) b. Ag(s) c. Pb(s) d. Pb2+(aq)

The following represents carbonic acid, an important part of the buffer system in blood. How many total valence electrons were used in constructing this structure? a. 24 b. 12 c. 17 d. 22 e. none of these

What is the correct name for K2HPO4? a. potassium hydrogen phosphate b. potassium hydrogen phosphoxide c. potassium dihydrogen phosphate d. dipotassium hydrogen phosphate

What is the formula of the compound formed by an iron(III) ion and oxygen? a. Fe2O3 b. FeO2 c. FeO d. Fe3O2

What is the maximum diameter of solute particles in a true solution? a. 1 nm b. 1 ìm c. 1 pm d. 1 mm

What is the name of NO2? a. nitrogen dioxide b. nitrous oxide c. nitrogen oxide d. nitrogen oxygen

When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) ® AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO3 and 3.10 g of NaCl react? a. 2.62 b. 4.17 g c. 6.20 g d. 1.55 g

When solutions of H2SO4 and NaOH react, the balanced molecular equation is: H2SO4(aq) + 2 NaOH(aq) ® Na2SO4(aq) + 2 H2O(l) How much Na2SO4 is obtained when 4.00 g of H2SO4 reacts with 2.00 g of NaOH? a. 3.55 g b. 4.20 g c. 0.650 g d. 2.98 g

When we name a molecular binary compound which of the following is true? a. We name the less electronegative element first. b. The element which has more atoms in the molecule is named first. c. We name the more electronegative element first. d. We name the elements in alphabetical order.

Which of the following aqueous solutions of Na2SO4 is hypotonic with respect to a 0.15 M NaCl solution? a. 0.05 M b. 0.10 M c. 0.15 M d. none of these

Which of the following bonds is the most polar? a. C—F b. C—H c. C—N d. C—O

Which of the following combinations will always result in a solution? a. gas + gas b. liquid + liquid c. solid + solid d. none of these

Which of the following concentration units will not change if the solution is heated? a. %(w/w) b. %(w/v) c. both . and b d. neither a nor b

Which of the following elements is most electronegative? a. O b. N c. B d. C

Which of the following increases as temperature increases? a. kinetic energy b. nuclear forces c. potential energy d. none of these

Which of the following is a cause of alkalosis? a. hyperventilation b. intense exercise c. a poor diet d. hypoventilation

Which of the following is an example of a molecular solid? a. P1V1/T1 = P2V2/T2 b. P1V1/T2 = P2V2/T1 c. P1V2/T1 = P2V1/T2 d. P1V2/T2 = P2V1/T1

Which of the following is not true of pH indicators? a. They all change color at pH = 7. b. They all have different colors in acid solutions than in basic solutions. c. They can be papers which have been soaked in specific compounds. d. None of the above, all the statements are true.

Which of the following is reduction? a. gain of electrons b. loss of hydrogen c. gain of oxygen d. none of these

Which of the following is the [H3O+] in pure water at room temperature? a. 1.0 ´ 10-7 M b. 1.0 ´ 107 M c. 1.0 ´ 10-14 M d. 1.0 ´ 1014 M

Which of the following is the conjugate acid of PO43-? a. HPO42- b. H3O+ c. H3PO4 d. H2PO4

Which of the following is the conjugate base of H2PO4-? a. HPO42- b. H3PO4 c. OH- d. PO43-

Which of the following is the conjugate base of H3PO4? a. H2PO4- b. PO43- c. HPO42- d. OH-

Which of the following is the correct way to write the formula of the compound formed between the barium ion and the sulfate ion? a. BaSO4 b. Ba(SO4)2 c. Ba2(SO4)2 d. Ba2SO4

Which of the following is true of London dispersion forces? a. They increase as the number of electrons in a molecule increases. b. They are only present in some molecules. c. Both a and b are correct. d. Neither a nor b is correct.

Which of the following must we know in order to write the equilibrium constant for a chemical reaction? a. the balanced chemical equation for the reaction b. the rate at which the reaction occurs c. both a and b d. neither a nor b

Which of the following solutions will have the highest electrical conductivity? a. 0.1 M Na3PO4 b. 0.1 M Na2HPO4 c. 0.1 M NaH2PO4 d. All have the same conductivity.

Which of the following species is not amphiprotic? a. C2H3O2- b. HC3H2O4- c. HC4H4O4- d. None, all of them are amphiprotic.

Which of the following sulfides is soluble in water? a. K2S b. PbS c. FeS d. Ag2S

Which regions of a heating curve correspond to regions where two phases of a material are present? a. horizontal regions b. regions with negative slope c. regions with positive slope d. It depends on the material.

Which of the following is the best definition of a catalyst?

A catalyst is a material which speeds up the rate of a chemical reaction without being consumed during the reaction

Which of the following is the best definition of a catalyst?

A catalyst is a material which speeds up the rate of a chemical reaction without being consumed during the reaction.

covalent bond

A chemical bond that involves sharing a pair of electrons between atoms in a molecule

Molecular Compounds

A compound in which all bonds are covalent.

polar covalent bond

A covalent bond in which electrons are not shared equally

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

Which of the following is the Bronsted-Lowry definition of a base? a. A hydroxide ion acceptor b. A proton acceptor c. A proton donor d. none of these

A proton acceptor

17. A solution is prepared by dissolving 117 grams of sodium chloride, KCl in 1000 grams of water. What is the freezing point of this solution? *1 mole NaCl = 58.5 g NaCl 1 mole NaCl = 2 moles of particles (Na+, Cl-)* A) - 7.44 °C B.) - 5.58 °C C.) - 3.72 °C C. - 1.86 °C

A) - 7.44 C *Tb = -1.86/1 mole Celsius x 4 moles particles = - 7.44 Celsius*

30. Calculate the rate for the reaction 2H2O(l) + O2(g) ® 2H2O2(l) , when the rate constant, k, is 0.02/min and the initial concentration of H2O2 is 0.5 mol/L. Rate = (0.02/min)x (0.5 mol/L) = 0.010 mol/min .L A). 0.010 mole/min.L B). - 0.010 mole/min.L C). 0.005 mol/min.L D). - 0.005 mole/min.L

A). 0.010 mole/min.L

23. In a particular titration experiment a 25 mL sample of H2SO4 solution required 30 mL of 0.2 M NaOH for the end point to be reached. What is the concentration of the acid? 2NaOH + H2SO4 ® Na2SO4 + 2 H2O A). 0.12 M B). 0.167 M C). 0.24 M D). 0.333 M

A). 0.12 M

34. Which of the following could be the equilibrium constant for a reaction which yields the most significant concentration of reactants? A). 1 x 10^-15 B). 1 x 10^-2 C). 1 x 10^2 D). 1 x 10^15

A). 1 x 10^-15

21. Which of the following correctly represents the electronic configuration of chlorine (Cl)? A). 1s22s22p63s23p5 B). 1s22s22p63s23p3 C). [Ne]3s23p4 D). [Ar]3s23p5

A). 1s22s22p63s23p5

19. Calcium (Ca) has _____ valence electrons A). 2 B). 4 C). 6 D). 8

A). 2

1. Select the correct scientific notation for 0.00000423 A). 4.23 x 10-6 B). 4.23 x 10-7 C). 42.3 x 10-8 D). 42.3 x 10-6

A). 4.23 x 10-6

7. A student dissolves 30 g of NaCl with enough water to make a 600 mL of NaCl solution. What is % (m/v) of this solution? *(30 g /600ml) x 100% = 5 % (m/v)* A). 5 % (m/v) B). 0.05 % (m/v) C). 20 % (m/v) D). 25 % (m/v)

A). 5 % (m/v)

30. A constant volume of nitrogen gas, N2, is heated from 0o C to 273o C. The initial pressure is 2.5 atm. What was the final pressure? A). 5.0 atm B). 3.0 atm C). 2.5 atm D). 1.0 atm

A). 5.0 atm

20. Compared to body fluids, both 0.9% (m/v) NaCl solution and 5% (m/v) glucose solution are isotonic. A red blood cell will undergo crenation in a ____ solution. *7% NaCl is hypertonic* A). 7% NaCl B). 5% glucose C). 3 % glucose D). 0.5% NaCl

A). 7% NaCl

25. The pKa of TRIS is 8.3. If you have the following TRIS buffers with various pH values. They will be active (useful) buffers EXCEPT A). A TRIS buffer at pH 6.55 B). A TRIS buffer at pH 7.55 C). A TRIS buffer at pH 8.30 D). A TRIS buffer at pH 9.00

A). A TRIS buffer at pH 6.55

7. What is the common name for the Group 1A elements (Li, Na, K....)? A). Alkali metals B). Alkaline earth metals C). Halogens D). Noble gases

A). Alkali metals

23. Which of the following element has the smallest atomic radius (atomic size)? A). Ar B). S C). Al D). Na

A). Ar

21. For the reaction A + B = 2 C, which of the following statements is true? A). B is consumed at the same rate that A is consumed. B). C is produced at the same rate that A is consumed. C).Both A and B D).Neither A nor B

A). B is consumed at the same rate that A is consumed.

8. Which of the following can be characterized as a week acid? A). CH3 COOH (acetic acid) B). HCl (hydrochloric acid) C). Both A and B D). Neither A nor B

A). CH3 COOH (acetic acid)

12. When strong acids react with carbonates (CO3 2- ) or bicarbonates (HCO3 - ), __ and ___ will be produced. A). CO2(g); H2O(l) B). H2(g); H2O(l) C). H2O(l) D). CO2(g); H2(g); H2O(l)

A). CO2(g); H2O(l)

13. Select the correct formula for the ionic compound calcium oxide. A). CaO B). CaO2 C). 2CaO D). Ca2O

A). CaO

11. Select the correct statement for ions. A). Cations have positive charges when metals lose their valence electrons. B). Cations have negative charges when metals lose their valence electrons. C). Anions have positive charges when nonmetals gain electrons. D). Anions have negative charges when nonmetals lose electrons.

A). Cations have positive charges when metals lose their valence electrons.

38. Which of the following factors cause colloidal particles to remain in solution without settling? A). Colloidal particles have large solvation layers. B). Colloidal particles acquire different kinds of charges on their large surface areas. C). Colloidal particles have small solvation layers. D). Colloidal particles acquire different kinds of charges on their small surface areas.

A). Colloidal particles have large solvation layers.

36. When Pb-208 is bombarded with Ni-64, a new element with 6 neutrons are produced. what isotope of the new element is produced by this reaction? 208Pb + 64Ni ® 266 ? + 6 1 n 82 28 110 0 A). Ds-266 B). Ds-272 C). Rf-266 D). Rf-272

A). Ds-266

35. Which of the following bonds is the MOST polar? *Electronegativity H: 2.1, F: 4.0, Cl: 3.0, I: 2.5* A). H—F B). H—Cl C). H—Br D). H—I

A). H—F

49. Select the correct equilibrium expression for the following reactions: C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l) A). K = [CO2 ] 6 [ O2] 6 B). K = [O2 ] 6 [CO2] 6 C). K = [CO2] 6 [HO2] 6 [C6H12O6][O2 ] 6 D). K = [C6H12O6][O2 ] 6 [CO2] 6 [HO2] 6

A). K = [CO2 ] 6 [ O2] 6

31. Which of the following is the WEAKEST intermolecular interaction? A). London dispersion forces B). hydrogen bonding C). dipole-dipole interactions D). covalent bonding

A). London dispersion forces

26. Select the correct electron-dot symbol for sodium (Na) and the correct ionic charge of a sodium ion. A). Na · ; Na+ B). · Na · ; Na2+ C). Na · ; Na- D). · Na · ; Na2-

A). Na · ; Na+

9. Which of the following can be characterized as a strong base? A). NaOH (sodium hydroxide) B). NH3 (ammonia) C). Both A and B D). Neither A nor B

A). NaOH (sodium hydroxide)

30. What is the product from the alpha decay of Po-220 ? A). Pb-216 B). Bi-216 C). Po-216 D). At-216

A). Pb-216

56. Which of the following acids has the STRONGEST strength? A). Phosphoric acid, H3PO4, Ka = 7.5 x 10-3 B). Acetic acid, CH3COOH, Ka = 1.8 x 10-5 C). Carbonic acid, H2CO3, Ka = 4.3 x 10-7 D). Boric acid, H3BO3, Ka = 7.3 x 10-10

A). Phosphoric acid, H3PO4, Ka = 7.5 x 10-3

57. Which of the following acids has the STRONGEST strength? A). Phosphoric acid, H3PO4, Ka = 7.5 x 10-3 B). Acetic acid, CH3COOH, Ka = 1.8 x 10-5 C). Carbonic acid, H2CO3, Ka = 4.3 x 10-7 D). Boric acid, H3BO3, Ka = 7.3 x 10-10

A). Phosphoric acid, H3PO4, Ka = 7.5 x 10-3

23. Which of the following is true? A). Reactions with low activation energies are rapid. B). The activation energy of reactions will not affect the rate. C). Reactions with low activation energies are slow. D). The activation energy for an exothermic reaction is negative.

A). Reactions with low activation energies are rapid.

4. Select the correct statement(s) of the solubility of gases in liquids. A). Solubility of gases always decreases as temperature increases. B). Solubility of gases always increases as temperature increases. C). Solubility of gases is unaffected by changes in temperature.

A). Solubility of gases always decreases as temperature increases.

52. What is the effect of adding H2O (l) to a container in which the reaction has reached equilibrium? CH3COOH(g) + C2H5OH(g) ⇔ CH3COOC2H5(g) + H2O(g) A). The reaction will shift to left ( <= ). B). The reaction will shift to right ( =>). C). There will be no effect. D). What happens depends on the temperature

A). The reaction will shift to left ( <= ).

35. What is the effect of removing C2H5OH(l) to a container in which the reaction has reached equilibrium? CH3COOH(g) + C2H5OH(l) Û CH3COOC2H5(g) + H2O(g) A). The reaction will shift to left (¬). B). The reaction will shift to right (®). C). There will be no effect. D). What happens depends on the temperature

A). The reaction will shift to left.

37. What happens to the following equilibrium reaction when the pressure is increased? 2A(g) + 3B(g) Û 5C(g) A). There will not be shifted B). The reaction will shift to left. C). The reaction will shift to right. D). What happens depends on the temperature.

A). There will not be shifted

22. In this reaction Zn + 2 H+ → Zn2+ + H2 , which reactant is oxidized? A). Zn B). 2H+ C). Zn2+ D). H2

A). Zn

17. Which of the following is the correct expression for Kw of water? H2O(l) + H2O(l) H3O+ (aq) + OH- (aq) A). [H3O+ ][OH- ] B). [H2O]/[ H3O+][OH- ] C). [H3O+][OH- ]/[H2O] D). [H3O+][OH- ]/[H2O]2

A). [H3O+ ][OH- ]

14. Which of the following is a description of a hydrated salt? A). a salt with water incorporated in its crystal structure B). a salt with no water incorporated in its crystal structure C). a salt which is insoluble in water D). a salt which is soluble in water

A). a salt with water incorporated in its crystal structure

2. A beaker of salt water contains some solid salt at the bottom. What type of solution is in the beaker? A). a saturated solution B). a supersaturated solution C). an unsaturated solution D). We cannot tell.

A). a saturated solution

6. A hydrogen bond is ______ A). an attraction between molecules where a partially positive hydrogen is attracted to a N, O, or F atom. B). a covalent bond between H and O. C). an ionic bond between H and another atom. D). a bond that is stronger than an ionic bond.

A). an attraction between molecules where a partially positive hydrogen is attracted to a N, O, or F atom.

28. The reaction, A + B + 150 kcal → C + D, is ______. A). an endothermic reaction B). an exothermic reaction C). a single replacement reaction D). a combination reaction

A). an endothermic reaction

36. The boiling point of covalent compounds depends primarily on the followings EXCEPT A). color B). intermolecular forces C). number of sites (surface area) for intermolecular interaction. D). molecular shape

A). color

7. Which of the following is an example of a physical change? A). grinding coffee beans B). baking a cake C). converting water to hydrogen and oxygen D). digesting a cheeseburger

A). grinding coffee beans

16. The Tyndall effect is associated with which of the following? A). light scattering by colloidal particles B). keeping colloidal particles from settling C). freezing point depression D). boiling point elevation

A). light scattering by colloidal particles

22. When an acid reacts with a base the reaction is called which of the following? A). neutralization B). precipitation C). redox D). single displacement

A). neutralization

11. Which of the following elements is a nonmetal? A). nitrogen B). sodium C). iron D). silver

A). nitrogen

37. The following equation is an example of _______. 1 n + 235 U ® 91 Kr + 142 Ba + 3 1 n + Energy A). nuclear fission B). nuclear fusion C). Bothe A and B D). Neither A nor B

A). nuclear fission

64. The following nuclear reactions as an example of ______. 1 n + 235 U → 91Kr + 142 Ba + 3 1 n + Energy 0 92 36 56 0 A). nuclear fission B). nuclear fusion C). both A and B D). neither A nor B

A). nuclear fission

16. The following elements are nonmetals EXCEPT ______. A). sodium B). phosphorus C). nitrogen D). carbon

A). sodium

8. The following form of energy can be classified as kinetic energy EXCEPT ____. A). water held by a dam B). a speeding train C). swimming D). electrical energy

A). water held by a dam

21. A gas has an initial pressure of 0.5 atm at 0o C. What is the new pressure after the temperature of the gas is increased to 273o C, if the amount and the volume of gas are constant? A. 1 atm B. 2 atm C. 3.3 atm D. 5.5 atm

A. 1 atm

23. What is the volume occupied by a 14 gram sample of nitrogen gas (N2) at STP? A. 11.2 L B. 22.4 L C. 33.6 L D. 44.8 L

A. 11.2 L

17. The decomposition of mercury(II) oxide is an exothermic reaction. 2 Hg(l) + O2(g) → 2 HgO(s) + 43.4 kcal How many kcal of heat are liberated when 401.2 g of Hg reacts? *1mole Hg =200.6 g Hg; 2 moles Hg = 43.4 kcal* A. 43.4 kcal B. 21.7 kcal C. 86.8 kcal D. 173.6 kcal

A. 43.4 kcal

9. What is the molar mass of sodium chloride (NaCl)? *1 mole NaCl = 23 g + 35.5 g = 58.5 g* A. 58.5 grams B. 58.5 amu C. 28 grams D. 28 amu

A. 58.5 grams

2. When a solution of barium chloride, BaCl2, is added to a solution of sodium sulfate, Na2SO4, a white precipitate of barium sulfate, BaSO4, forms. BaCl2(aq) + Na2SO4(aq) --> BaSO4(s) + 2NaCl(aq) Select the correct NET ionic equation for this reaction. A. Ba2+ (aq) + SO4 2- (aq) --> BaSO4(s) B. Na+ (aq) + Cl- (aq) --> NaCl(aq) C. Ba2+ (aq) + 2 Cl- (aq) + 2Na+ (aq) + SO4 2- (aq) --> BaSO4(s) +2 Na+ (aq) + 2 Cl- (aq) D. BaCl2(aq) + Na2SO4(aq) --> BaSO4(s) + 2 NaCl (aq)

A. Ba2+ (aq) + SO4 2- (aq) --> BaSO4(s)

29. Which of the following WILL NOT affect the boiling point of a liquid? A. The color of the liquid molecule B. The formula weight of the liquid molecules C. The intermolecular forces between the liquid molecules D. The shape of the liquid molecules

A. The color of the liquid molecule

CH3COO-

Acetate

After 2 minutes 0.08 moles of B were produced.

Al3+ and S2- form

Al2S3 (aluminum sulfide)

Which of the following will change the numerical value of the equilibrium constant of a particular reaction? a. Increasing the concentration reactants b. Increasing the concentration products c. Increasing the temperature d. All of the above

All of the above

Al3+

Aluminum ion

NH4+

Ammonium

reaction order

An increase in a reactant concentration and the reaction rate increase (or decrease) is expressed as an exponential term

Chloroform has a normal boiling point of 61.7°C. Which of the following is true? a. At any temperature the vapor pressure of chloroform is greater than that of water. b. Chloroform is less volatile than water. c. both a. and b. d. Neither a. nor b.

At any temperature the vapor pressure of chloroform is greater than that of water.

The temperature effect on reaction rate is the result of which of the follwoing?

At higher temperatures there are more collisions and at higher temperatures a larger fraction of the collisions are effective collisions.

Anion

Atom that gains an electron becomes an ion with a negative charge.

Cation

Atom that loses electrons become an ion with a positive charge.

Use the periodic table to determine the number of Protons, Neutrons, and Electrons in Iron (Fe)

Atomic number is 26, with an atomic mass of 56: Protons = 56, Electrons = 56 56-26 = 30 neutrons

A covalent bond is associated with which of the following? a. interactions between nuclei b. the sharing of electrons c. the transfer of electrons d. all of these

A particular reaction has an equilibrium constant of 1 x 10-15. Which of the following best describes the relationship between the equilibrium constant and the reaction rate? a. Because the equilibrium constant is small the reaction proceeds slowly. b. There is no relationship between the size of the equilibrium constant and the rate of the reaction. c. Both a and b are true. d. Neither a nor b is true.

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 15.0%(w/v) KOH to make a solution which is 10.0%(w/v)? a. 23.3 mL b. 17.5 mL c. 15.0 mL d. 52.5 mL

Consider the following hypothetical acid-base reaction. A(aq) + B(aq) = C(aq) + D(aq) weaker acid weaker base stronger acid stronger base a. The position of the equilibrium favors the forward reaction. b. The position of the equilibrium favors the reverse reaction. c. Neither the forward nor the reverse reaction are favored at equilibrium. d. The position of equilibrium cannot be predicted from the given data.

How many molecules are present in one mole of glucose, C6H12O6? a. 3.34 ´ 10^21 b. 6.02 ´ 10^23 c. 6.92 ´10^-26 d. 1.44 ´ 10^25

Hydrocyanic acid, HCN, is a weak acid. Which of the following is the correct expression for the Ka of hydrocyanic acid? a. [HCN]/[ H3O+][CN-] b. [H3O+][CN-]/[HCN] c. [HCN][CN-]/[ H3O+] d. [H3O+][HCN]/[CN-]

If you need a sample of 2.84 mol of Na2S, how many grams do you need? a. 78.1 g b. 222 g c. 2.84 g d. 0.00451 g

In a particular chemical reaction 2 bonds are broken and no bonds are formed. Based only on this information, which of the following is true? a. The reaction has a high activation energy. b. The reaction is endothermic. c. The reaction is exothermic. d. We cannot determine which of the above is true.

In an acid-base equilibrium the equilibrium lies in the direction which favors which species? a. the stronger acid b. the weaker base c. both a and b d. neither a nor b

In the reaction CH2O(g) + O2(g) ® HCOOH(g) + H2O(g) which species is reduced? a. CH2O(g) b. O2(g) c. HCOOH(g) d. H2O(g)

In the reaction Pb(s) + 2 Ag+(aq) ® Pb2+(aq) + 2 Ag(s) which species is reducing agent? a. Ag+(aq) b. Pb(s) c. Pb2+(aq) d. Ag(s)

In which of the following molecules does the carbon atom have a nearly trigonal planar distribution of electron density? a. C2H2 b. C2H4 c. C2H6 d. none of these

Sodium sulfite, Na2SO3(aq), is added to wine as an antioxidant since it reacts with the oxygen of the air to form sodium sulfate, Na2SO4(aq). Which of the following is the balanced equation for this reaction? a. Na2SO3(aq) + 2 O(g) ® Na2SO4(aq) b. 2 Na2SO3(aq) + O2(g) ® 2 Na2SO4(aq) c. Na2SO3(aq) + O(g) ® Na2SO4(aq) d. Na2SO3(aq) + O2(g) ® Na2SO4(aq)

The chemical formula of rust is Fe2O3. Which of the following is the correct common name for this compound? a. iron oxide b. ferric oxide c. ferrous oxide d. diiron trioxide

The rate of reaction for the decomposition of hydrogen peroxide to yield water and oxygen is given by the equation: Rate = k[H2O2]. Which of the following is indicated by this equation? a. The rate of the reaction is unaffected by the concentration of H2O2. b. The rate of the reaction will increase with increasing concentration of H2O2. c. The rate of the reaction will decrease with increasing concentration of H2O2. d. none of these

The specific heat of water is 1.0 cal/g·°C. The heat of vaporization of water is 540 cal/g. Which of the following is true? a. It takes less energy to evaporate one gram of water than it does to heat one gram of water from 0°C to 100°C. b. It takes more energy to evaporate one gram of water than it does to heat one gram of water from 0°C to 100°C. c. It takes the same amount of energy to evaporate one gram of water as it does to heat one gram of water from 0°C to 100°C. d. There is insufficient information to answer the question.

The synthesis of a certain drug requires 4 steps. First three steps were relatively easy with percent yields of 97.1%, 94.3% and 92.8% respectively. However, the last step was very difficult with a percent yield of 72.7%. What was the overall percent yield? a. 85.0% b. 61.8% c. 72.7% d. 27. 9%

The term molecular weight is strictly correct for which of the following? a. ionic compounds b. covalent compounds c. both a and b d. neither a nor b

What is the formula of the compound formed by calcium and fluorine? a. CaF3 b. CaF2 c. CaF d. Ca2F

What is the volume occupied by a 8.00 gram sample of molecular oxygen at STP? a. 44.8 L b. 5.60 L c. 11.2 L d. 22.4 L

When wine turns sour it is the result of the conversion of ethanol, C2H5OH, to acetic acid, HC2H3O2. Which of the following happens to ethanol in this reaction? a. It is reduced. b. It is oxidized. c. It is both oxidized and reduced. d. It is neither oxidized nor reduced.

Which of the following buffers will have the lowest pH? a. a solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 b. a solution containing 0.25 M HC2H3O2 and 0.15 M NaC2H3O2 c. a solution containing 0.15 M HC2H3O2 and 0.25 M NaC2H3O2 d. They all have the same pH.

Which of the following compounds has the largest formula weight? a. sodium acetate b. aluminum acetate c. potassium acetate d. calcium acetate

Which of the following elements is the least electronegative? N,C,B,O

Which of the following is found in baking powder but not in baking soda? a. NaHCO3(s) b. KH2PO4(s) c. both a and b d. neither a nor b

Which of the following is the conjugate acid of water? a. HCl b. H3O+ c. OH- d. NH4+

Which of the following is true of effective collisions? a. The number of effective collisions decreases as the temperature is increased. b. the number of effective collisions determines the reaction rate. c. both a and b d. neither a nor b

Which of the following is true of pure water? a. [H3O+] < [OH-] b. [H3O+] = [OH-] c. [H3O+] > [OH-] d. pure water is an electrolyte

Which of the following molecules is(are) polar? a. BCl3 b. NH3 c. both of them d. neither of them

Which of the following solutions will have the higher electrical conductivity? a. 0.1 M NaCl b. 0.2 M NaCl c. Both a and b have the same conductivity. d. Neither conducts electricity.

Which of the following symbols is used to denote that two or more representations of a species are resonance structures? a. ¬ b. « c. ®

Which of the following will have the lowest freezing point? a. 0.1 M acetic acid, HC2H3O2 b. 0.1 M hydrochloric acid, HCl c. 0.1 M hydrofluoric acid, HF d. All have the same freezing point.

For the reaction A + B → 2 C, which of the following statements is true?

B is consumed at the same rate that A is consumed.

26 In the reaction 2HgO(s) ® 2Hg(l) + O2(g), we measure the evolution of O2 gas to determine the rate of reaction. At the beginning of the reaction (at 0 minutes), 0.00 L of O2 is present. After 20 minutes the volume of O2 is 0.80 L, what is the rate of reaction? Rate = (0.80 L/20 min) - 0.00 L = 0.04 L O2/min ************************************************** A).- 0.040 L O2/min B). 0.040 L O2/min C). - 0.015 L O2/min D). 0.015 L O2/min

B). 0.040 L O2/min

18. Which of the following solutions has the highest osmolarity? *NaCl Osmol = 0.2 M x 2 = 0.4 Osmol* *BaCl2 Osmol = 0.15 M x 3 =0.45 Osmol* *AlCl3 Osmol = 0.10 M x 4 =0.40 Osmol* A). 0.20 M NaCl B). 0.15 M BaCl2 C). 0.10 M AlCl3 D). All have the same osmolarity.

B). 0.15 M BaCl2

59. If 40 mL of 0.1 M NaOH is needed to neutralize 20 mL of HCl solution with a few drops of phenolphthalein (pH indicator), what is the concentration (M) of the HCl solution? NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) A). 0.1 M B). 0.2 M C). 0.3 M D). 0.4 M

B). 0.2 M

43. What is the bond angle in water (H2O)? A). 90.0o B). 104.5o C). 120.0o D). 180.0o

B). 104.5o

2. Given the calculation: 1.987 × 6.020 = ___. what is the answer reported to the correct number of significant figures? A). 11.96174 B). 11.96 C). 12.0 D). 12

B). 11.96

41. What bond angle is most closely associated with a trigonal planer distribution of electron density? A). 109.5 °C B). 120 °C C). 90 °C D). 180 °C

B). 120 °C

6. The density of titanium is 4.54 g/mL. What is the volume (mL) of 113.5 g of titanium? Density = 4.54 g/mL *113.5 g x 1 mL = 25 mL 4.54 g* A). 0.04 mL B). 25 mL C). 35.9 mL D). 515.3 mL

B). 25 mL

2. How many calories are required to heat 20 g of copper from 10o C to 210 o C? (SH for Cu = 0.092 cal/g o C) A). 184 cal B). 368 cal C). 440 cal D). 880 cal

B). 368 cal

34. Iron-59 has a half-life of 46 days. If the lab received a sample of 32 g iron-59. How many grams are still active after 138 days? A). 8 g B). 4 g C). 2 g D). 1 g

B). 4 g

27. What is the pH of a buffer prepared by mixing 200. mL of 0.50 M HEPES in its acid form with 100. mL of 0.50 M HEPES in it basic form? pKa of HEPES = 7.55 pH = 7.55 + (log 100/200) = 7.25 A). 6.55 B). 7.25 C). 7.85 D). 8.55

B). 7.25

11. How many mL of 2 M NaCl solution will provide 1.5 moles of NaCl? *2 M NaCl => 2 moles NaCl = 1L 1 L = 1000 mL 1.5 moles NaCl x 1 L x 1000 mL = 750 mL 2 moles NaCl 1 L* A). 800 mL B). 750 mL C). 350 mL D). 300 mL

B). 750 mL

60. What is the pH of a solution that is 0.4 M in TRIS in the acid form and 0.2 M in TRIS in the basic form? ( pKa of TRIS acid form = 8.3) A). 7.9 B). 8.0 C). 8.6 D). 9.0

B). 8.0

8. Which of the following element has 2 valence electrons? A). Li (Lithium) B). Ba (Barium) C). F (Fluorine) D). O (Oxygen)

B). Ba (Barium)

29. What is the correct formula for calcium nitride? A). CaN3 B). Ca3N2 C). Ca(NO3)2 D). Ca(NO2)2

B). Ca3N2

12. Which of the following ion has a charge of + 2? A). Aluminum ion B). Calcium ion C). Chloride ion D). Phosphide ion

B). Calcium ion

10. The ionization energy is the energy needed to remove the least tightly bound electron from an atom in the gaseous (g) state. Which one of the following elements has the HIGHEST ionization energy? A). Na B). Cl C). Al D). Si

B). Cl

32. What is the correct IUPAC name for Cu2CO3? A). Copper carbonate B). Copper(I) carbonate C). Copper (II) carbonate D).Copper (II) bicarbonate

B). Copper(I) carbonate

11. Which of the following gases is produced when an acid reacts with an active metal? A). CO2 B). H2 C). O2 D). H2O

B). H2

4. Which of the following species can be characterized as amphiprotic? A). H3O+ B). H2PO4 - C). H3PO4 D). PO4 3-

B). H2PO4 -

56. The following species can be characterized as amphiprotic EXCEPT A). HPO4 2- B). H2SO4 C). HCO3 - D). H2O

B). H2SO4

33. What is the equilibrium constant for the following reaction? Equilibrium concentrations are given under the formula of each component. A + B = 2C 2 M 2 M 2 M A). K = 0 B). K = 1 C). K = 2 D). K = 8

B). K = 1

40. A student is attempting to draw several resonance structures for a species. Which of the following is allowed? A). Change the connectivities of the nuclei. B). Move electrons from one location to another. C). both A and B D). neither A nor B

B). Move electrons from one location to another.

12. Sodium bicarbonate has sodium, hydrogen, carbon and oxygen atoms in the ratio 1:1:1:3. What is the correct formula for sodium bicarbonate? A). NaBiCO3 B). NaHCO3 C). NHCO3 D). SoHCO3

B). NaHCO3

14. Identify the element located in Group 5A, period 2. A). Bromine (Br) B). Nitrogen (N) C). Phosphorus(P) D). Silicon (Si)

B). Nitrogen (N)

1. According to Arrhenius which species is associated with all bases? A). H3O+ B). OH- C). H2O D). None of the above

B). OH-

16. Select the correct IUPAC name for SO2. mono: 1 Di: 2 Tri: 3 Tetra: 4 A). Monosulfur dioxide B). Sulfur dioxide C). Sulfur trioxide D). Dioxygen sulfide

B). Sulfur dioxide

37. What is the correct chemical name for a compound with the formula SO3? A). sulfur oxide B). Sulfur trioxide C). Trisulfur oxide D). Trioxygen sulfide

B). Sulfur trioxide

22. Which of the following is true of effective collisions? A). The number of effective collisions decreases as the temperature is increased. B). The number of effective collisions determines the reaction rate. C). Both A and B D). Neither A nor B

B). The number of effective collisions determines the reaction rate.

25. Which of the following occurs when an oxygen atom is converted to an oxide ion? A). The oxygen atom gains one electron and becomes an anion with a charge of -1. B). The oxygen atom gains two electrons and becomes an anion with a charge of -2. C). The oxygen atom loses one electron and becomes a cation with a charge of +1. D). The oxygen atom loses two electrons and becomes a cation with a charge of +2.

B). The oxygen atom gains two electrons and becomes an anion with a charge of -2.

51. The following reaction is endothermic: 3O2(g) + Heat <=> 2O3(g). If the reaction is at equilibrium. Use Le Chatelier's Principle to predict the direction of reaction, when the pressure decreases. A). The position of equilibrium shifts to the right ( =>). B). The position of equilibrium shifts to the left ( <= ). C). There is no change in the position of equilibrium.

B). The position of equilibrium shifts to the left ( <= ).

13. Consider the following hypothetical acid-base reaction. A(aq) + B(aq) C(aq) + D(aq) stronger acid stronger base weaker acid weaker base A). The position of the equilibrium favors the reverse reaction (shift to left). B). The position of the equilibrium favors the forward reaction (shift to right). C). Neither the forward nor the reverse reaction are favored at equilibrium. D). The position of equilibrium cannot be predicted from the given data.

B). The position of the equilibrium favors the forward reaction (shift to right).

14. The position of the equilibrium favors CH3COOH + NH3 CH3COO- + NH4 + A). The position of the equilibrium favors the reverse reaction (shift to left). B). The position of the equilibrium favors the forward reaction (shift to right). C). Neither the forward nor the reverse reaction are favored at equilibrium

B). The position of the equilibrium favors the forward reaction (shift to right).

27. The rate of reaction for the decomposition of hydrogen peroxide to yield water and oxygen is given by the equation: Rate = k[H2O2]. Which of the following is indicated by this equation? ********************************************************* A). The rate of the reaction is unaffected by the concentration of H2O2. B). The rate of the reaction will increase with increasing concentration of H2O2. C). The rate of the reaction will decrease with increasing concentration of H2O2. D). None of the above

B). The rate of the reaction will increase with increasing concentration of H2O2.

36. The following reaction is exothermic: 2NO2(g) Û N2O4(g) + 13,700 cal. If the reaction is at equilibrium, what will happen if you decrease the temperature? A). The reaction will shift to left (¬) B). The reaction will shift to right (®). C). There will be no effect. D). Not sufficient information to predict the direction of the reaction.

B). The reaction will shift to right (®).

34. A covalent bond is associated with which of the following? A). Interactions between nuclei B). The sharing of electrons between two nonmetals C). The transfer of electrons between a metal and a nonmetal D). The sharing of electrons between metals and nonmetals

B). The sharing of electrons between two nonmetals

20. The balanced equation 3 H2 (g) + N2 (g) → 2 NH3 (g) means which of the following? A). Three grams of hydrogen react with one gram of nitrogen to form two grams of ammonia. B). Three moles of hydrogen react with one mole of nitrogen to form two moles of ammonia. C). Three grams of hydrogen react with one gram of nitrogen to form two moles of ammonia. D). Three moles of hydrogen react with one mole of nitrogen to form two grams of ammonia.

B). Three moles of hydrogen react with one mole of nitrogen to form two moles of ammonia.

53. Which of the following is the Brønsted-Lowry definition of an acid? A). a proton acceptor B). a proton donor C). a hydroxide ion acceptor D). a hydroxide ion donor

B). a proton donor

61. When an alpha particle bombard with Cm-248Assuming, one proton, two neutrons and ___ will be produced. A). americium-249 B). berkelium-249 C). californium-249 D). curium - 249

B). berkelium-249

17. The following elements are transition metals EXCEPT A). cobalt B). lead C). silver D). strontium

B). lead & D). strontium

19. In an aqueous solution the [OH- ] is 10- 6 M. What is the pH for this solution? *pOH = - log 10-6 = 6* A). pH = 6 B). pH = 8 C). pH = 14 D). pH = 12

B). pH = 8

3. For which of the following types of compounds is water generally a good solvent? A). nonpolar compounds B). polar compounds C). both nonpolar and polar compounds D). neither nonpolar or polar compounds

B). polar compounds

47. When a reaction has reached equilibrium, _____. A). the reactants have been completely converted to products B). the rate of the forward reaction is equal to the rate of the reverse reaction C). the rate of the forward reaction is slower than the rate of the reverse reaction D). the rate of the forward reaction is faster than the rate of the reverse reaction

B). the rate of the forward reaction is equal to the rate of the reverse reaction

28. A nuclear equation is balanced when A). the same elements are found on both sides of the equation. B). the sum of the mass numbers and the sum of the atomic numbers of the particles and atoms are the same on both sides of the equation. C). the same particles and atoms are on both sides of the equation. D). different particles and atoms are on both sides of the equation

B). the sum of the mass numbers and the sum of the atomic numbers of the particles and atoms are the same on both sides of the equation.

12. Iron (Fe) reacts with sulfur (S) to form Iron(III) sulfide (Fe2S3). How many moles of Fe are needed to react with 6 moles of S? 2Fe(s) + 3S(s) → Fe2S3(s) A. 2 moles B. 4 moles C. 6 moles D. 8 moles

B. 4 moles 6 moles S x (2 moles Fe/3 moles) = 4 moles Fe 3 moles S

16. If 900 cal of heat is added to a 90.0 gram sample of water initially at 40.0°C, what will be the final temperature of the water? (Specific heat of water is 1 cal/go C) A. 30 °C B. 50 °C C. 70 °C D. 90 °C

B. 50 °C

30. Which of the following molecules can have only London dispersion forces? A. H2O B. CH4 C. NH3 D. HF

B. CH4

5. Select the correct statement for the following reaction: Pb(s) + 2Ag+ (aq) → Pb2+ (aq) + 2Ag(s) A. Pb is reduced and is an oxidizing agent; 2Ag+ is oxidized and is a reducing agent. B. Pb is oxidized and is a reducing agent; 2Ag+ is reduced and is an oxidizing agent. C. Pb is oxidized and is an oxidizing agent; 2Ag+ is reduced and is a reducing agent. D. Pb is reduced and is a reducing agent; 2Ag+ is oxidized and is an oxidizing agent.

B. Pb is oxidized and is a reducing agent; 2Ag+ is reduced and is an oxidizing agent.

What is the formula of the compound formed between barium and oxygen?

BaO

Ba2+ and I- form

Bal2 (barium iodide)

Ba2+

Barium ion

At high altitudes atmospheric pressure is lower than at sea level. Which of the following is true? a. Boiling water is cooler in Denver than in New York. b. Boiling water is hotter in Denver than in New York. c. Water boils at the same temperature in Denver and New York. d. We cannot predict the relationship between the boiling points in the two cities.

Boiling water is cooler in Denver than in New York.

Which law relates the volume and pressure of a gas under conditions of constant temperature?

Boyle's Law

Br - anion name

Bromide

A catalyst speeds up a chemical reaction as a result of which of the following? a. It makes the reaction more endothermic. b. It increases the number of collisions between reacting molecules. c. It provides an alternate pathway with a lower activation energy. d. It makes the reaction more exothermic.

A sample of carbon dioxide occupies 22.4 L at STP. Which of the following statements apply to the sample? a. The sample contains 6.02 ´ 1023 carbon atoms. b. The sample contains 6.02 ´ 1023 molecules. c. Both a. and b are correct. d. Neither a nor b is correct.

According to the kinetic molecular theory, which of the following is not true? a. Gas molecules are assumed to have no volume. b. Gas pressure is caused by collisions between gas molecules and the container walls. c. When gas molecules collide they stick together. d. None, all of the above are true.

An acetic acid solution has a pH of 5.80, what is the [OH-] in this solution? a. 1.6 ´ 10-20 M b. 6.3 ´ 105 M c. 6.3 ´ 10-9 M d. 1.6 ´ 10- 6 M

At constant temperature the pressure on a 6.0 L sample of a gas is reduced from 2.0 atm to 1.0 atm. What is the new volume of the gas sample? a. 0.083 L b. 0.33 L c. 12 L d. 3.0 L

Formaldehyde has the chemical formula CH2O. How many electrons must be shown in the Lewis structure of formaldehyde? a. 4 b. 8 c. 12 d. 16

Given the following information determine which of these acids is the strongest? Ka for boric acid is 7.3 ´ 10-10 pKa of acetic acid is 4.75 Ka for lactic acid is 8.4 ´ 10-4 pKa of phenol is 9.89 a. formic acid b. phenol c. lactic acid d. acetic acid

In the reaction CH2O(g) + O2(g) ® HCOOH(g) + H2O(g) which species is oxidizing agent? a. CH2O(g) b. H2O(g) c. O2(g) d. HCOOH(g)

In the reaction Pb(s) + 2 Ag+(aq) ® Pb2+(aq) + 2 Ag(s) which species is oxidized? a. Pb2+(aq) b. Ag+(aq) Correctc. Pb(s) d. Ag(s)

In the reaction Pb(s) + 2 Ag+(aq) ® Pb2+(aq) + 2 Ag(s) which species is the oxidizing agent? a. Ag(s) b. Pb(s) c. Ag+(aq) d. Pb2+(aq)

Le Châtelier's Principle applies to which of the following systems? a. a system in which the reaction is moving left to right b. a system in which the reaction is moving right to left c. a system which has reached equilibrium d. all of the above

Lime, CaO, is produced by the reaction CaCO3(s) ® CaO(s) + CO2(g). What weight of CO2 is obtained by the decomposition of 38.7 g of CaCO3? a. 23.2 g b. 15.5 g c. 17.0 g d. 21.7 g

The ammonium ion has the formula NH4+. How many nonbonding electrons must be shown in the Lewis structure of the ammonium ion? a. 4 b. 9 c. 0 d. 8

The atomic weight of platinum is less than that of gold. If you have a 10 g sample of each of these metals, which of the following is true? a. You have fewer of atoms of platinum than of gold. b. You have equal numbers of atoms of platinum and gold. c. You have more atoms of platinum than of gold. d. There is insufficient information to determine which of the above is true.

The species H+ can be called which of the following? a. hydrogen ion b. proton c. either a or b d. neither a nor b

What bond angle is most closely associated with a trigonal planar distribution of electron density? a. 109.5° b. 90° c. 120° d. 180°

What is the formula weight ammonium carbonate, (NH4)2CO3? a. 138.2 amu b. 108.4 amu c. 96.1 amu d. 78.1 amu

What is the molecular weight of sucrose, C12H22O11? a. 360.4 amu b. 319.6 amu c. 342.3 amu d. 180.2 amu

What temperature scale should be used if we wish to express Charles's Law as a simple direct proportionality? a. Fahrenheit b. Celsius c. Kelvin d. It makes no difference.

When acetic acid is dissolved in water which of the following is true of the equilibrium which is established as represented below? CH3COOH (aq) + H2O = CH3COO- (aq) + H3O+ (aq) a. It lies very far to the right. b. It lies slightly to the left. c. It lies very far to the left. d. It lies slightly to the right.

When comparing the strength of two weak acids which factor do we use to determine which is the stronger of the two? a. the formula weights of the acids b. the number of protons the acids can lose c. the size of the acid dissociation constants d. none of the above

When dealing with solutions which of the following laws is not applicable? a. law of conservation of energy b. law of conservation of mass c. law of constant composition d. None, all of the above laws are applicable.

Which law applies only to mixtures of gases? a. Charles's law b. Avogadro's law c. Dalton's law d. Boyle's law

Which must we do when preparing a solution of specific molarity? a. Carefully weigh the solute, carefully weigh the solvent. b. Carefully weigh the solute, carefully measure the volume of solvent. c. Carefully weigh the solute, fill the volumetric flask to the mark. d. None of the above is the correct procedure.

Which of the following can be characterized as a strong electrolyte? a. 0.001 M KOH b. 3.0 M KOH c. both a and b d. neither a nor b

Which of the following compounds is soluble in water? a. AgBr b. AgI c. AgC2H3O2 d. AgBr

Which of the following describes the effect of raising the temperature of an endothermic reaction which has not yet reached equilibrium? a. The rate of reaction slows and less product is produced. b. The rate of reaction slows, but more product is produced. c. The rate of reaction speeds up and more product is produced. d. The rate of reaction speeds up, but less product is produced.

Which of the following is generally not included when writing an equilibrium constant expression? a. liquids b. solids c. both a and b d. neither a nor b

Which of the following is relates the name of an electrode to its sign? a. The anode is the positive electrode. b. The cathode is the negative electrode. c. both a and b d. neither a nor b

Which of the following is the conjugate acid of HPO42- a. H3O+ b. H3PO4 c. H2PO4- d. PO43-

Which of the following is the correct formula for dinitrogen trioxide? a. N3O2 b. O3N2 c. N2O3 d. O2N3

Which of the following is the correct set of integer coefficients for the balanced equation respectively: ___ C5H12(g) + ___O2(g) ® ___CO2(g) + ___H2O(g) a. 5, 12, 2, 4 b. 5, 1, 8, 6 c. 1, 8, 5, 6 d. 1, 5, 5, 6

Which of the following is the net ionic equation for the reaction of the strong acid HCl with the strong base NaOH? a. H3O+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) ® Na+(aq) + Cl-(aq) + 2H2O(l) b. HCl(aq) + NaOH(aq) ® NaCl(aq) + H2O(l) c. H3O+(aq) + OH-(aq) ® H2O(l) d. none of these

Which of the following is true of a solid which is hygroscopic? a. It will gain weight when exposed to a damp environment. b. It may change its color upon being exposed to a damp environment. c. both a and b d. neither a nor b

Which of the following is true of methanol, CH3OH, when it dissolves in water? a. It dissociates into ions. b. It forms covalent bonds with water. c. It forms hydrogen bonds with water. d. None of the above, methanol does not dissolve in water.

Which of the following is true of the formula weights of a material which exists in both anhydrous and hydrated forms? a. They have the same formula weight. b. The hydrated form always has a lower formula weight. c. The hydrated form always has a higher formula weight. d. We cannot make any general statement about the formula weights of the two forms.

Which of the following is true of the types attractive forces present in the three states of matter? a. They are the same in liquids and solids, but different in gases. b. They are different in each of the three states. c. They are the same in each of the three states. d. They are the same in gases and liquids, but different in solids.

Which of the following pH's corresponds to a slightly basic solution? a. 6.8 b. 2.8 c. 7.2 d. 11.2

Which of the following will determine the pH of a buffer made using acetic acid and sodium acetate? a. the amount of water present b. the [HC2H3O2] c. the ratio [C2H3O2-]/[HC2H3O2] d. the [C2H3O2-]

Which of the following will occur if the temperature of a gas is increased from 20 K to 40 K at constant pressure? a. The volume will increase slightly. b. The volume will decrease slightly. c. The volume will double. d. The volume will be halved.

Why will increasing the temperature of a reaction speed up the reaction? a. The activation energy for the reaction is lowered. b. The heat of reaction is increased. c. There are more effective collisions between molecules. d. none of these

You have a sample of 3.01 ´ 1023 atoms of silver. How much does this sample weigh? a. 2.00 g b. 0.0500 g c. 53.9 g d. 107.9 g

48. In the reaction 2HgO(s) → 2Hg (l) + O2(g), we measure the evolution of O2 gas to determine the rate of reaction. At the beginning of the reaction (at 0 minutes), 0.025 L of O2 is present. After 20 minutes the volume of O2 is 0.425 L. What is the rate of reaction? A). 0.005 L O2/min B). 0.01 L O2/min C). 0.02 L O2/min D). 0.04 L O2/min

C). 0.02 L O2/min

39. Which of the following solutions has the HIGEST osmolarity? *Osmolarity = M x i* A). 0.1 M NaCl B). 0.1 M CaCl2 C). 0.1 M AlCl3 D). All have the same osmolarity

C). 0.1 M AlCl3

9. The density of methanol at 20oC is 0.791 g/mL. What is its specific gravity? A). 1 B). 1 g/mL C). 0.791 D). 0.791 g/mL

C). 0.791

5. Which of the following solutions will have the highest electrical conductivity? A). 1 M NaCl B). 1 M BaCl2 C). 1 M AlCl3 D). 1 MC6H2O6 ------------------- 1 M NaCl (Na+ , Cl-) 1 M BaCl2 (Ba2+ , 2 Cl-) 1 M AlCl3 (Al3+ , 3 Cl-) C6H12O6 dissolves in water but doesn't conduct electricity.

C). 1 M AlCl3

19. What is the Osmolarity of a 0.6 M of NaCl solution? A). 0.3 Osmol B). 0.6 Osmol C). 1.2 Osmol D). 1.8 Osmol

C). 1.2 Osmol

23. 2 moles of water (H2O) contains ____water molecules. (Avogadro's number = 6.02 x 1023) A). 6.02 x 10^23 B). 9.03 x 10^23 C). 1.204 x 10^24 D). 1.806 x 10^24

C). 1.204 x 10^24

41. 175.5 g of NaCl is dissolved in enough water to make 2 L of solution, what is the molarity of the NaCl solution? A). 0.5 M B). 1.0 M C). 1.5 M D). 3.0 M

C). 1.5 M

18. In an aqueous solution the [OH- ] is 10- 3 M. What is the concentration of [H3O+] in this solution? Kw = [H3O+][H3O+] = 10^-14 A). 10-14 M B). 10-12 M C). 10- 11 M D). 10- 3 M

C). 10- 11 M

46. Calculate the boiling point of a solution prepared by dissolving 87.8 g of sodium chloride (NaCl) in 1000 mL of water? A). 100 o C B). 100.512 o C C). 101.536 o C D). 102.048 o C

C). 101.536 o C

18. What bond angle is most closely associated with a tetrahedral distribution of electron density? A). 90o B). 120o C). 109.5o D). 180o

C). 109.5o

36. The total number of valence electrons in methanol, CH3OH, is _____. *4 + 4 x (1) + 6 = 14* A). 10 B). 12 C). 14 D). 24

C). 14

20. Select the correct e- energy level arrangement for phosphorus (P). A). 2, 8, 1 B). 2, 8, 3 C). 2, 8, 5 D). 2, 8, 7

C). 2, 8, 5

34. A vessel under 5 atm pressure contains nitrogen, N2, and water vapor, H2O. The partial pressure of N2 is 3 atm. What is the partial pressure of the water vapor? A). 0.5 atm B). 1.0 atm C). 2.0 atm D). 9.0 atm

C). 2.0 atm

25. ____moles of water (H2O) are present in 54 g H2 O. A). 2.0 B). 2.5 C). 3.0 D). 3.5

C). 3.0

How many mL of 25 % (m/v) NaCl solution is needed to prepare 200 mL of a 0.5 % (m/v) NaCl solution? A). 25 mL B). 12.5 mL C). 4 mL D). 2 mL

C). 4 mL

42. How many mL of 30% w/v NaCl solution is needed to prepare 600 mL of a 0.2% w/v NaCl solution? A). 1.5 mL B). 3.3 mL C). 4.0 mL D). 10 mL

C). 4.0 mL

29. At constant temperature, the pressure of a 3.0 L gas sample is reduced from 3.0 atm to 2.0 atm. What is the new volume of the gas sample? A). 1.5 L B). 3.0 L C). 4.5 L D). 6.0 L

C). 4.5 L

21. Balance the following equation and select the coefficient that is placed in front of O2 . _C3 H8 + ? O2 → _CO2 + _H2 O A). 1 B). 3 C). 5 D). 7

C). 5

26. The pKa of acetic acid, HC2H3O2, is 4.75. What is the pH of a buffer in which [HC2H3O2] = 0.20 M and [NaC2H3O2] = 2.0 M? pH = 4.75 + (log 2.0/2.0) = 5.75 A). 3.75 B). 4.75 C). 5.75 D). 7.00

C). 5.75

32. How many grams of nitrogen gas (N2) are in 44.8 L of N2 at STP? A). 16 g B). 32 g C). 56 g D). 64 g

C). 56 g

44. What is the mass of NaCl in a 1 L of 1 M NaCl? A). 29.3 g B). 39.3 g C). 58.5 g D). 87.8 g

C). 58.5 g

8. What is the mass of NaCl in a 400 g of 1.5 % (m/m) NaCl solution? *1.5% (m/m) => 1.5 g NaCl = 100 g solution* A). 1.5 g B). 5.5 g C). 6 g D). 2.7 g

C). 6 g

33. Cobalt-60 is a gamma emitter. What isotope is formed when 60Co emits gamma radiation? A). 60Mn B). 60Fe C). 60Co D). 60Ni

C). 60Co

33. If a sample of 16 grams oxygen (O2) gases at 1.00 atm pressure occupies 3 L, what is the temperature of the sample? PV=nRT, R= 0.0821 atm.L/mole.K A). 18.3 K B). 36.5 K C). 73.1 K D). 146 K

C). 73.1 K

18. How many neutrons are in Iodine-131? neutron = 131-53 = 78* A). 53 B). 72 C). 78 D). 197

C). 78

9. Which of the following element has an e - energy level arrangement of 2, 8, 3? A). Sodium (Na) B). Magnesium (Mg) C). Aluminum (Al) D). Chlorine (Cl)

C). Aluminum (Al)

6. The following elements are metals EXCEPT A). Aluminum (Al) B). Potassium (K) C). Boron (B) D). Sodium (Na)

C). Boron (B)

15. Which of the following factors cause colloidal particles to remain in solution without settling? (50% credit for A or B) A). Colloidal particles acquire same kind of charges on their large surface areas. B). Colloidal particles have large solvation layers. C). Both A and B D). Neither A nor B

C). Both A and B

25. In an energy diagram for an exothermic chemical reaction which of the following is true? (see Fig. 7.4, in the reference sheet) (50% for A or B). ---------------------------------------------------- A). The energy of the products is lower than that of the reactants. B). The energy of the transition state is higher than that of the reactants. C). Both A and B D). Neither A nor B

C). Both A and B

27. 16 g of CH4 is mixed with 96 g of O2 according the following reaction: CH4(g) + 2 O2(g) → CO2(g) + 2H2O(g) Which reagent is the limiting reagent? A). O2 B). CO2 C). CH4 D). H2O

C). CH4

42. The following are polar covalent compounds EXCEPT A). HCl B). NH3 C). CH4 D). H2O

C). CH4

6. Which of the following is the conjugate base of an acid, HCO3 - ? A). H2CO3 B). HCO3 - C). CO3 2- D). CO2

C). CO3 2-

33. Select the correct formula for calcium sulfite. A). CaS B). CaSO4 C). CaSO3 D). CSO4

C). CaSO3

31. Select the correct IUPAC name for CuCl2. A). Copper(I) monochloride B). Copper(I) chloride C). Copper(II) chloride D). Copper(II) monochloride

C). Copper(II) chloride

30. What is the correct formula for iron (III) oxide? A). PbO B). PbO2 C). Fe2O3 D). Fe3O2

C). Fe2O3

3. Which of the following is a diprotic acid? A). HCl B). HNO3 C). H2SO4 D). H3PO4

C). H2SO4

29. A catalyst speeds up a chemical reaction as a result of which of the following? A). It makes the reaction more endothermic. B). It makes the reaction more exothermic. C). It provides an alternative reaction pathway to reduce the activation energy. D). It decreases the number of collisions between reacting molecules.

C). It provides an alternative reaction pathway to reduce the activation energy.

7. What is the name of HNO3? ( NO3 - , nitrate ion) A). Hydronitric acid B). Hydronitrous acid C). Nitric acid D). Nitrous acid

C). Nitric acid

55. Which of the following is the conjugate base of an acid, HPO4 2- ? A). H3PO4 B). H2PO4 - C). PO4 3- D). H3O+

C). PO4 3-

19. Predict the shape of ammonia molecules (NH3) and their polarity. A). Bent shape; polar B). Tetrahedral shape; nonpolar C). Pyramidal shape, polar D). Linear, nonpolar

C). Pyramidal shape, polar

15. Carbonate ion (CO3 2- ) is a polyatomic ion. Select the IUPAC name for the ionic compound Na2CO3. A). Disodium carbonate B). Sodium (I) carbonate C). Sodium carbonate D). Sodium carbon oxide

C). Sodium carbonate

24. If a reaction occurs very rapidly, even at a relatively low temperature, which of the following is probably true? A). The reaction is endothermic. B). The reaction is exothermic. C). The reaction has a low activation energy. D). The reaction occurs as a single step.

C). The reaction has a low activation energy.

27. An ionic bond is associated with which of the following? A). Interactions between nuclei B). The sharing of electrons between two nonmetals C). The transfer of electrons from a metal to a nonmetal D). Both metals and nonmetals gain electrons

C). The transfer of electrons from a metal to a nonmetal

32. The product from the positron emission of Cs-127 is ________. A). Cs-127 B). I-127 C). Xe-127 D). Ba-127

C). Xe-127

44. Predict the shape of the water molecule, H2O and its polarity. A). tetrahedral shape; nonpolar B). pyramidal shape; polar C). bent shape; polar D). linear; polar

C). bent shape; polar

5. A sample of material is found to weigh 42.96 grams, and have a volume of 4.8 cm3. The sample could be ____. Density of metals: Aluminum = 2.70 g/cm3 copper = 8.95 g/cm3 silver = 12.59 g/cm3 gold = 19.32 g/cm3 A). silver B). gold C). copper D). aluminum

C). copper

29. Which of the following has the STRONGEST penetrating power of radiation? A). alpha B). beta C). gamma D). All of them have similar strength of penetration.

C). gamma

15. Group 7A elements: F, Cl, Br and I are ____. A). alkali metals B). alkaline earth metals C). halogens D). noble gases

C). halogens

20. In an aqueous solution the [H3O+] is 10- 4 M. What is the pH for this solution? pH = - log 10-4 = - (-4) = 4 A). pH = 14 B). pH = 12 C). pH = 4 D). pH = 10

C). pH = 4

38. Under which of the following conditions is the A—B bond considered to be polar covalent? A). when A and B have the same electronegativity B). when the difference between the electronegativities of the atoms is 0.3 C). when the difference between the electronegativities of the atoms is 0.9 D). when the difference between the electronegativities of the atoms is 2.0

C). when the difference between the electronegativities of the atoms is 0.9

6. What is the molecular weight of carbon monoxide, CO? *CO = 12 amu + 16 amu = 28 amu* A. 14 amu B. 22 amu C. 28 amu D. 44 amu

C. 28 amu

10. How many moles of sodium chloride (NaCl), are present in 234 g of NaCl? A. 1 B. 2 C. 4 D. 8

C. 4

20. At constant pressure the temperature of a 1 L sample of gas is increased from 100 K to 400 K. What is the new volume of the gas sample? A. 1 L B. 2 L C. 4 L D. 6 L

C. 4 L

26. If 2 moles of NO gas occupies 10.0 L at 295 K, what is the pressure of the gas in atmospheres (atm)? A. 0.206 atm B. 2.42 atm C. 4.84 atm D. 9.33 atm

C. 4.84 atm

24. What is the mass of 33.6 L of nitrogen gas (N2) at STP? A. 14 g B. 28 g C. 42 g D. 56 g

C. 42 g

13. Consider the following equation: 4 Na + O2 → 2 Na2O ____grams of O2 are needed to produce 3 moles of Na2O. *1 mole O2 = 2 moles Na2O, 1 mole O2 = 32 g O2* A. 16 B. 32 C. 48 D. 64

C. 48

11. What is the mass (grams) of 3 moles of water (H2O)? A. 36 grams B. 48 grams C. 54 grams D. 90 grams

C. 54 grams

8. 0.5 mole of glucose, C6H12O6, contains ________ moles of H. A. 2 B. 3 C. 6 D. 12

C. 6

15. In an experiment forming ethanol, the theoretical yield is 60 g. The actual yield is 57 g. What is the percent yield? A. 58.5% B. 90.0 % C. 95.0 % D. 97.5 %

C. 95.0 %

3. Which of the following compounds is INSOLUBLE in water? A. CuC2H3O2 B. CuNO3 C. CuOH D. Cu2SO4

C. CuOH

28. For small molecules, which of the following usually is the WEAKEST intermolecular interaction? A. dipole-dipole interactions B. hydrogen bonding C. London dispersion forces D. covalent bonding

C. London dispersion forces

Which of the following is true when comparing a dialysis membrane with an osmotic semipermeable membrane? A. Both membranes allow solute particles to pass through. B.The osmotic membrane has larger openings. C. Neither A or B

C. Neither A nor B

18. The following statements for the kinetic molecular theory of gases are correct EXCEPT A. A gas consists of small particles (atoms or molecules) that move randomly, constantly, rapidly in straight paths. B. The actual volume occupied by gas particles is extremely small so the gas is compressible. C. The averaged kinetic energy of gas molecules is proportional to the Celsius (o C) temperature D. Gas pressure is caused by collisions between gas molecules and the container walls.

C. The averaged kinetic energy of gas molecules is proportional to the Celsius (o C) temperature

37. Diamond and graphite are both ___ of carbon that occur in the solid state. This specific term refers to one or more forms of a chemical element that occur in the same physical state. A. isotopes B. amorphous forms C. allotropes D. isomers

C. allotropes

4. Which of the following is reduction? A. loss of electrons B. gain of oxygen C. gain of electrons D. loss of hydrogen

C. gain of electrons

Which of the following molecules cannot engage in hydrogen bonding? a. CH₄ b. NH₃ c. H₂O d. all of them

CH4

Which of the following molecules can have only London dispersion forces? a. CH₄ b. CO c. both a. and b. d. Neither a. nor b.

CH₄

what is the formula of the compound formed by calcium and fluorine?

CaF2

The term "limelight" is derived from the old name for calcium oxide. What is the formula of calcium oxide?

CaO

Ca2+

Calcium ion

Which of the following best describes the rates of chemical reaction?

Chemical reactions have a wide range of rates, from extremely fast to extremely slow

Which of the following best describes the rates of chemical reaction?

Chemical reactions have a wide range of rates, from extremely fast to extremely slow.

Cl- anion name

Chloride

CrO4 2-

Chromate

Cu+

Copper (I) ion

Cu2+

Copper (II) ion

CN-

Cyanide

A solution is prepared by dissolving 53.5 grams of ammonium chloride, NH4Cl in 4000. grams of water? What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000g of water] a. 100.39°C b. 100.13°C c. 100.52°C d. 100.26°C

In a Lewis structure, which of the following atoms can have more than eight electrons associated with it? a. C b. N c. O d. none of these

In a particular chemical reaction 3 bonds are broken and 4 bonds are formed. Based only on this information, which of the following is true? a. The reaction has a high activation energy. b. The reaction is endothermic. c. the reaction is exothermic. d. We cannot determine which of the above is true.

In an aqueous solution thee [OH-] is 1.0 x 10- 6 M. What is the [H+]? a. 1.0 ´ 108 M b. 1.0 ´ 10-9 M c. 1.0 ´ 10- 6 M d. 1.0 ´ 10-8 M

In the reaction CH2O(g) + O2(g) ® HCOOH(g) + H2O(g) which species is oxidized? a. O2(g) b. HCOOH(g) c. H2O(g) d. CH2O(g)

In which of the following cases is a polar covalent bond formed? a. when an electron is transferred from one atom to another b. when a metallic element forms a bond with a non-metallic element c. when the electrons of a bond are shared equally by the two atoms d. when the electrons of a bond are shared unequally by the two atoms whose difference in electronegativity is less than 1.9

Laughing gas, sometimes called nitrous oxide, has the formula N2O. What is the proper chemical name for nitrous oxide? a. nitrogen oxide b. nitrogen dioxide c. dinitrogen oxygen d. dinitrogen oxide

Of the following ions, which always forms soluble compounds? a. Na+ b. NH4+ c. C2H3O2- d. all of these

Saline solutions (NaCl in water) used to deliver intravenous drugs are 0.89%(w/v). What mass of NaCl is found in 500. mL of such a solution? a. 0.45 g b. 0.89 g c. 8.9 g d. 4.5 g

The combined gas law combines which gas laws? a. Boyle's and Charles's b. Boyle's and Gay-Lussac's c. Charles's and Gay-Lussac's d. Boyle's, Charles's and Gay-Lussac's

The synthesis of a certain drug requires 3 steps. The percent yield for the steps are 95.2%, 91.4% and 93.8% respectively. What is the overall percent yield? a. 87.0% b. 91.4% c. 89.3% d. 81.6%

The tin compound used to strengthen teeth has the formula SnF2. Which of the following is the common name for this compound? a. stannic fluoride b. tin fluoride c. tin(II) fluorine d. stannous fluoride

The toxic gas hydrogen cyanide has the formula HCN. How many electrons must be shown in the Lewis structure of hydrogen cyanide? a. 6 b. 2 c. 12 d. 10

What is the correct systematic name for the compound with the formula CuCl2? a. cupric chloride b. copper(II) chlorine c. cuprous chloride d. copper(II) chloride

What is the effect of increasing the temperature at which a reaction is carried out? a. In virtually all cases the rate of reaction decreases. b. In all cases the rate of reaction decreases. c. In all cases the rate of reaction increases. d. In virtually all cases the rate of reaction increases.

What is the molar mass of CuSO4·5H2O? a. 159.6 g/mol b. 177.6 g/mol c. 90.0 g/mol d. 249.6 g/mol

When a solution of ammonium chloride, NH4Cl, is added to a solution of lead(II) nitrate, Pb(NO3)2, a white precipitate of lead chloride, PbCl2, forms. Which of the following is the total ionic equation for this reaction? a. Pb2+(aq) + 2 Cl-(aq) ® PbCl2(s) b. Pb2+(aq) + Cl22-(aq) ® PbCl2(s) c. 2 NH4Cl(aq) + Pb(NO3)2(aq) ® PbCl2(s) + 2 NH4NO3(aq) d. 2 NH4+(aq) + 2 Cl-(aq) + Pb2+(aq) + 2 NO3-(aq) ® PbCl2(s) + 2 NH4+(aq) + 2 NO3-(aq)

Which of the following best describes the rates of chemical reaction? a. Most chemical reactions occur at moderate rates. b. Most chemical reactions occur very slowly. c. Most chemical reactions occur very rapidly. d. Chemical reactions have a wide range of rates, from extremely fast to extremely slow.

Which of the following does not affect the boiling point of a liquid? a. the formula weight of the liquid molecules b. the shape of the liquid molecules c. the intermolecular forces between the liquid molecules d. None, all of the above affect the boiling point.

Which of the following is a unit of pressure? a. mm of Hg b. pascals c. torr d. They are all units of pressure.

Which of the following is associated with gout? a. calcium sulfate dihydrate b. anhydrous calcium sulfate c. anhydrous sodium urate d. sodium urate monohydrate

Which of the following is the correct unit for formula weight? a. grams b. ounces c. pounds d. atomic mass units

Which of the following is true about a molecule which contains three polar bonds which have the same degree of polarity? a. The molecule will always be polar. b. The molecule will never be polar. c. The molecule will be polar if the electron distribution is trigonal planar. d. None of the above is true.

Which of the following laws describes the relationship between pressure and the solubility of gases? a. Avogadro's b. Dalton's c. Boyle's d. Henry's

Which of the following molecules cannot engage in hydrogen bonding? a. SiH4 b. PH3 c. H2S d. all of these

Which of the following solutions will require the most NaOH in a titration experiment? a. 25 mL of 0.5 M HCl b. 25 mL of 0.5 M HCOOH c. 25 mL of 0.5 M HC2H3O2 d. They all require the same amount.

Which of the following statements best describes the acid/base relationship? a. As acid strengths increase conjugate base strengths increase. b. As base strengths increase conjugate acid strengths increase. c. both a and b d. neither a nor b

Which of the following will change the numerical value of the equilibrium constant of a particular reaction? a. increasing the concentration of the reactants b. increasing the concentration of the products c. both a and b d. neither a nor b

Which of the following will have the highest electrical conductivity? a. 0.3 M CH3COOH b. 0.1 M NaCl c. 0.4 M CH3COOH d. 0.2 M NaCl

16. The Ka for an acid is 7.3 x 10-10. What is the pKa of this acid? pKa = - log[Ka] (- log 7.3 x 10-10 = 9.14) A). - 9.14 B). - 4.86 C). 4.86 D). 9.14

D) 9.14

45. If you add 117 g of sodium chloride (NaCl) to 1000 g of water, what will be the freezing point of the solution? A). - 1.86 o C B). - 3.72 o C C). - 5.58 o C D). - 7.44 o C

D). - 7.44 o C

9. How many moles of NaCl are contained in 1.2 L of 0.6 M NaCl? A). 0.25 moles B). 0.2 moles C). 1.8 moles D). 0.72 moles

D). 0.72 moles

63 Iodine-131 (I-131) has a half-life of 8 days. If the lab received a sample of 160 g of I-131, how many grams are still active after 32 days? A). 5 g B). 40 g C). 20 g D). 10 g

D). 10 g

24. 2 moles of sodium chloride (NaCl) weigh _____ grams. A). 29.3 g B). 58.5 g C). 87.8 g D). 117 g

D). 117 g

3. The temperature of an experiment is designed at 60 ºC. What is it in ºF? A). 108 F B). 15.6 F C). 33.3 F D). 140 F

D). 140 F

13. A solution contains 15 ppm of sodium (Na+) ions. Which of the following is another way to describe the concentration of Na+ in this solution? *ppm = 1 mg/kg* A). 15 mcg Na+ ions/ 1mg solution B). 15 mg Na+ ions/ 1 g solution C). 15 mcg Na+ ions/ 1 kg solution D). 15 mg Na+ ions/ 1 kg solution

D). 15 mg Na+ ions/ 1 kg solution

35. If the intensity of radiation 3 cm from a source is 20 mCi, what is the intensity 1 cm from the source? A). 2.2 mCi B). 33 mCi C). 270 mCi D). 180 mCi

D). 180 mCi

What is the mass of NaCl in a 2 L bottle of 2 M NaCl? A). 29.3 g B). 58.5 g C). 117 g D). 234 g

D). 234 g

4. The boiling point of methanol is 64.7 oC. What is this temperature on the Kelvin scale? K = oC +273 K = 64.7 + 273 = 337.7 K A). 18.17K B). 148.46 K C). 208.3 K D). 337.7 K

D). 337.7 K

26. How many grams of NH3 are required to produce 112 g of N2 in the following reaction? 4NH3 + 6NO → 5N2 + 6H2 O A). 18 g B). 72 g C). 80 g D). 54.4 g

D). 54.4 g

43. How many moles of solute, KCl, are contained in 2 L of 3 M KCl solution? A). 0.4 mole B). 2 moles C). 4 moles D). 6 moles

D). 6 moles

21. A solution has a pH of 7.4 What is its pOH? pH + pOH =14 pOH = 14 - 7.4 = 6.6 A). - 6.6 B). - 7.4 C). 7.4 D). 6.6

D). 6.6

28. A particular chemical reaction carried out at 40°C takes 2 hours. Approximately how long will it take to carry out the reaction at 20°C? 40oC = 30oC = 20oC 2 hour 4 hours 8 hours ************************* A). 0.5 hour B). 1 hour C). 4 hours D). 8 hours

D). 8 hours

3. Sucrose is a disaccharide and consists of carbon(C), hydrogen (H) and oxygen (O) atoms in the ratio 12:22:11. What is the correct formula for sucrose? A). 12C22H11O B). C6H11O5 C). C6H12O6 D). C12H22O11

D). C12H22O11

14. Copper (Cu) is a transition metal element. What is the correct name for CuO? A). Dicopper oxide B). Copper oxide C). Copper (I) oxide D). Copper (II) oxide

D). Copper (II) oxide

5. Which of the following is the conjugate acid of a base, HPO4 2- ? A). H3PO4 B). HPO4 2- C). PO4 3- D). H2PO4 -

D). H2PO4 -

54. What is an Arrhenius acid? A). It is a proton acceptor B). It is a proton donor C). It produces hydroxide ions (OH- ) in an aqueous solution D). It produces hydronium (H3O+ ) ions in an aqueous solution

D). It produces hydronium (H3O+ ) ions in an aqueous solution

50. A catalyst speeds up a chemical reaction as a result of which of the following? A). It makes the reaction more endothermic. B). It makes the reaction more exothermic. C). It increases the number of collisions between reacting molecules. D). It provides an alternate pathway with a lower activation energy.

D). It provides an alternate pathway with a lower activation energy.

32. For the reaction N2(g) + 3H2(g) Û 2NH3(g), which of the following is the correct equilibrium constant expression? A). K = [N2] [H2]3 [NH3] B). K = [N2] [H2] [NH3] C). K = [NH3] [N2] [H2] D). K = [NH3]2 [N2] [H2]3

D). K = [NH3]2 [N2] [H2]3

65. Select the proper shielding for the radioactive gamma (γ) rays. A). Don't need any shielding at all B). Heavy clothing, lab coat, gloves C). Paper, clothing D). Lead, thick concrete

D). Lead, thick concrete

10. What are the two acids in the following reaction? NH4 + + HPO4 =2- NH3 + H2PO4 - A). NH4 + and HPO4 2- B). NH4 + and NH3 C). HPO4 2- and H2PO4 - D). NH4 + and H2PO4 -

D). NH4 + and H2PO4 -

24. The ionization energy is the energy required to remove an electron from an atom. Which of the following atoms has the LOWEST ionization energy? A). Ar B). S C). Al D). Na

D). Na

17. Which of the following bond is an ionic bond? *Electronegativity H: 2.1 Cl: 3.0 N: 3.0 Na: 0.9 F: 4.0* A). H - H B). H - Cl C). N - N D). Na - F

D). Na - F

62. What is the product from the beta decay of fluorine-19 (F -19)? A). N - 14 B). O - 19 C). N - 19 D). Ne - 19

D). Ne - 19

4. Which subatomic particle(s) are found in the nucleus? A). Electrons B). Neutrons and electrons C). Protons and electrons D). Protons and neutrons

D). Protons and neutrons

35. Which of the following have no effect on the strength of London dispersion forces? A). The shape of the interacting molecules B). The number of electrons of the interacting molecules C). The mass of the interacting molecules D). The pH of the interacting molecules

D). The pH of the interacting molecules

31. Which of the following is true of a reaction which has reached equilibrium? A). The rate of the forward reaction is slower than the rate of the reverse reaction. B). The rate of the forward reaction is faster than the rate of the reverse reaction. C). The reactants have been completely converted to products. D). The rate of the forward reaction is equal to the rate of the reverse reaction.

D). The rate of the forward reaction is equal to the rate of the reverse reaction.

1. Which of the following is true of a solution? A). The components of a solution can be separated by filtration. B). The components of a solution separate on standing. C). The separation of a solution into its components is a chemical change. D). The separation of a solution into its components is a physical change.

D). The separation of a solution into its components is a physical change.

31. What is the product from the beta decay of iodine-131 ? A). Sb - 131 B). Te - 131 C). I - 131 D). Xe - 131

D). Xe - 131

22. Which of the following correctly represents the electronic configuration of radium (Ra)? A). [Xe]7s1 B). [Xe]6s1 C). [Xe]7s2 D). [Rn]7s2

D). [Rn]7s2

2. Which of the following is the Brønsted-Lowry definition of an acid? A). a hydroxide (OH- ) ion acceptor B). a hydroxide ion donor C). a proton (H+) acceptor D). a proton (H+) donor

D). a proton (H+) donor

1. A metal sample has a mass of 10.8 grams and a volume of 4 cm3. The sample could be *Density of metals: Aluminum = 2.70 g/cm3 Copper = 8.95 g/cm3 Silver = 12.60 g/cm3 Gold = 19.32 g/cm3* A). silver B). gold C). copper D). aluminum

D). aluminum

10. Air is a(n) A). compound B). heterogeneous mixture C). element D). a homogeneous mixture

D). homogeneous mixture

58. The [OH- ] of a solution is 1 x 10-4 M. What is the pH of the solution? A). pH= 4.0 B). pH= 6.0 C). pH= 8.0 D). pH=10.0

D). pH=10.0

15. Given the following information determine which of these acids is the WEAKEST? Ka for boric acid is 7.3 x 10-10 pKa of acetic acid is 4.75 Ka for lactic acid is 8.4 x 10-4 pKa of phenol is 9.89 A). acetic acid B). boric acid C). lactic acid D). phenol

D). phenol

39. The VSEPR theory allows us to determine the ___. A). bond type for a molecule. B). charge on an ion. C). color of a compound. D). shape of a molecule.

D). shape of a molecule.

5. The ___ atom has 54 protons. A). bromine (Br) B). chlorine (Cl) C). tellurium (Te) D). xenon (Xe)

D). xenon (Xe)

22. A gas is expanded from an initial volume of 1 L at 1 atm at 7 °C to a final volume of 5 L. During the expansion the gas increases to 287 °C. What is the final pressure? A. 1.49 atm B. 0.57 atm C. 0.52 atm D. 0.40 atm

D. 0.40 atm

1. Select the correct balanced equation for the chemical reaction below: __ Ba(NO3)2 + __H2S → __ BaS + __ HNO3 A. 2, 2, 2, 4 B. 2, 1, 1, 4 C. 1, 2, 1, 4 D. 1, 1, 1, 2

D. 1, 1, 1, 2

7. 2 moles of fluorine (F) contain ____ fluorine atoms. A. 3.01 × 10^23 B. 6.02 × 10^23 C. 9.03 × 10^23 D. 1.20 x 10^24

D. 1.20 x 10^24

27. A vessel contains a mixture of nitrogen (N2), oxygen (O2) and water vapor, H2O. The partial pressure of N2 is 4 atm, the partial pressure of O2 is 4 atm, and the partial pressure of water vapor is 2 atm. What is the total pressure of the vessel? A. 2 atm B. 6 atm C. 8 atm D. 10 atm

D. 10 atm

19. A gas has a volume of 4 L at 1 atm. If the volume of the gas changes to 2 L, what is the final pressure of the gas, assuming constant temperature? *P1 = 1 atm P2 = ? V1 = 4 L V2 = 2 L* A. 0.4 atm B. 0.8 atm C. 1.25 atm D. 2 atm

D. 2 atm

14. 24 g of C is mixed with 5 g of H2 according the following reaction: C(s) + 2H2(g) → CH4(g) How many grams of CH4 will be produced in the reaction? A. 4 g B. 8 g C. 16 g D. 24 g

D. 24 g

25. If a 44 gram sample of carbon dioxide gas (CO2) at 1.00 atm pressure occupies 2 L, what is the temperature of the sample? A. 146 K B. 73 K C. 48.7 K D. 24.4 K

D. 24.4 K

28. Which of the following ions has the same electronic configuration as argon (Ar)? A. Na+ B. F- C. Li+ D. S^2-

D. S^2-

13. The followings do occur naturally as diatomic molecules EXCEPT A. oxygen B. hydrogen C. nitrogen D. helium

D. helium

Which of the following is true? a. Decreasing the activation energy decreases the reaction rate. b. Decreasing the activation energy increases the reaction rate. c. The activation energy of an exothermic reaction is negative. d. There is no relationship between activation energy and reaction rate.

Decreasing the activation energy increases the reaction rate.

Which of the following is true?

Decreasing the activation energy increases the reaction rate?

CrO7 2-

Dichromate

Consider the following Lewis structure. What is the correct name for this compound? a. phophorus pentachlorine b. monphosphorus pentachloride c. phosphorus chloride d. pentaphosphorus chloride e. phosphorus pentachloride

For the reaction A + B → 2 C, which of the following best describes how we can measure the reaction rate?

Either of the above procedures can be used.

What is the formula compound formed by iron III ion and oxygen?

Fe2O3

iron III is written

Fe^3+

F- anion name

Fluoride

ionic bond

Formed when one or more electrons are transferred from one atom to another

Which of the following bonds is the most polar?

H----F

CO3 2- + 2H^+ = [H2 CO3] which goes to

H2O + CO2

OH -

Hydroxide

Which of the following occurs when hydrogen chloride gas is dissolved in water to form hydrochloric acid? a. a complex between HCl and water is formed b. H⁺ is transferred from HCl to water c. H⁺ is transferred from water to HCl d. there is no reaction, HCl molecules remain present

H⁺ is transferred from HCl to water

The order of strenght of the following acids is H₂SO₄>H₃PO₄>HC₂H₃O₂ (acetic acid)>C₆H₅OH(phenol). Which of these acids has the weakest conjugate base? a.C₆H₅OH b. H₂SO₄ c. H₃PO₄ d. HC₂H₃O₂

H₂SO₄

Which of the following is a diprotic acid? a. HNO₃ b. H₂SO₄ c. H₃SO₄ d. HCl

H₂SO₄

Which of the following is the conjugate acid of H₂PO₄⁻? a. H₃PO₄ b. HPO₄²⁻ c. PO₄²⁻ d. H₃O⁺

H₃PO₄

Which of the following is most important in determining if a material will be a solid, a liquid or a gas? a.covalent bonds c.intramolecular forces b.intermolecular forces d.nuclear forces

INTERmolecular forces

I - anion name

Iodide

Fe3+

Iron (III) ion

Which of the following is true of a catalyst for a reaction?

It has no effect on the equilibrium constant for the reaction.

Which of the following is true of a catalyst for a reaction?

It increases the equilibrium constant for the reaction.

When HCl is dissolved in water which of the following is true of the equilibrium which is established? a. it lies virtually completely to the left b. it lies slightly to the right c. it lies virtually completely to the right d. it lies slightly to the left

It lies virtually completely to the right

A catalyst speeds up a chemical reaction as a result of which of the following?

It provides an alternate pathway with a lower activation energy.

For the reaction 2NH₃(g)⇌3H₂(g)+N₂(g) which of the following is the equilibrium constant expression? a. K = [H₂][N₂]/[NH₃] b. K = [NH₃]/[H₂][N₂] c. K = [H₂]³[N₂]/[NH₃]² d. K = [NH₃]²/[H₂]³[N₂]

K = [H₂]³[N₂]/[NH₃]²

K+ and PO4 3- forms

K3PO4. (potassium phosphate)

What temperature scale should be used if we wish to express Charles's Law as a simple direct proportionality? a. Fahrenheit b. Celsius c. Kelvin d. it makes no difference

Kelvin

Li+ and Br- form

LiBr (Lithium Bromide)

In what form is lithium administered when it is used as a drug in the treatment of manic depression?

Li^+

Li+

Lithium ion

Mg2+

Magnesium ion

Hg+

Mercury (I) Ion

Which of the following is the conjugate acid of ammonia, NH3? a. H⁺ b. H₃O⁺ c. NH₂⁻ d. NH₄⁺

NH₄⁺

Na+ and HCO3 - form

NaHCO3 (sodium bicarbonate)

When solid sodium hydroxide is dissolved in water which of the following species is not present in the solution? a. NaOH(aq) b. H2O(l) c. OH⁻(aq) d. none, they are all present

NaOH(aq)

NO3 -

Nitrate

NO2 -

Nitrite

Which of the following accounts for the fact that reactions between ions in solution are usually very fast?

No covalent bonds need to be broken for reaction to occur.

Which of the following elements is most electronegative? O, B, N, C

O2 - anion name

Oxide

Which of the following is the conjugate base of HPO₄²⁻? a. H₃PO₄ b. H₂PO₄⁻ c. PO₄³⁻ d. OH⁻

PO₄³⁻

MnO4 -

Permanganate

PO4 3-

Phosphate

K+

Potassium ion

Which of the following must we know in order to write the equilibrium constant for a chemical reaction? a. The balanced chemical equation for the reaction b. The rate at which the reaction occurs c. Both a and b d. Neither a nor b

The balanced chemical equation for the reaction

valence electrons

The electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds.

In an energy diagram for an exothermic chemical reaction which of the following is true?

The energy of the products is lower than that of the reactants and the energy of the transition state is higher than that of the reactants.

Which of the following is true of the rates of most chemical reactions?

The initial rate is faster than the rate later in time

Which of the following will occur if the temperature of a gas is increased from 20°C to 40°C at constant pressure?

The volume will increase slightly

Why will increasing the temperature of a reaction speed up the reaction?

There are more effective collisions between molecules.

A particular reaction has an equilibrium constant of 1 x 10⁻¹⁵. Which of the following best describes the relationship between the equilibrium constant and the reaction rate? a. because the equilibrium constant is small the reaction proceeds slowly b. there is no relationship between the size of the equilibrium constant and the rate of the reaction c. both a. and b. are true d. Neither a. nor b. is true

There is no relationship between the size of the equilibrium constant and the rate of the reaction

. A particular reaction has an equilibrium constant of 1 × 1020. Which of the following best describes the relationship between the equilibrium constant and the reaction rate?

There is no relationship between the size of the equilibrium constant and the rate of the reaction.

Naming Polyatomic Ions

Those that contain oxygen usually end with -ite or -ate -ate has one more oxygen atom -ite has one less oxygen atom

Sn2+

Tin (II) ion

Sn4+

Tin (IV) ion

A double bond is treated as a single region of electron density in the

VSEPR model

VSEPR Model

Valance Electron Pair Repulsion model / Unshared electron pairs around the central atom

Which of the following statements is true about a reversible reaction?

When we mix the reactants together none of the reactants will be completely used up.

Binary ionic compounds from four metals that form two different positive cations

Write name of metal, then Roman numeral (enclosed in parentheses), immediately following (with no space), then write ion.

The notation [A]⁴ is equivalent to which of the following? a. [A] + [A] + [A] + [A] b. 1/([A] + [A] + [A] + [A]) c. [A] x [A] x [A] x [A] d. 1/([A] x [A] x [A] x [A])

[A] x [A] x [A] x [A]

Hydrofluoric acid, HF, is a weak acid. Which of the following is the correct expression for the Ka of hydrofluoric acid? a. [H₃O⁺][HF]/[F⁻] b. [HF]/[ H₃O⁺][F⁻] c. [H₃O⁺][F⁻]/[HF] d. [HF][F⁻]/[ H₃O⁺]

[H₃O⁺][F⁻]/[HF]

Which of the following is the correct expression for Kw of water? a. [H₃O⁺][OH⁻]/[H₂O] b. [H₃O⁺][OH⁻] C. [H₂O]/[H₃O⁺][OH⁻] d. [H₃O⁺][OH⁻]/[H₂O]²

[H₃O⁺][OH⁻]

Which of the following exerts the greatest pressure? a. a 20 gram object on a surface of 0.50 cm² b. a 40 gram object on a surface of 2.0 cm² c. a 60 gram object on a surface of 3.0 cm² d. none, they all exert the same pressure

a 20 gram object on a surface of 0.50 cm²

Which of the following instruments is used to measure atmospheric pressure? a.an altimeter b.a barometer c.a manometer d.an odometer

a barometer

which of the following is the best definition of a catalyst

a catalyst is a material which speeds up the rate of a chemical reaction without being consumed during the reaction

Le Chatelier's Principle

a chemical system at equilibrium responds to a change in conditions by adjusting the relative concentrations of the reaction components

indicator

a compound that changes color at the titration equivalence point

nonpolar covalent bond

a covalent bond in which the electrons are shared equally by the two atoms

reducing potential

a greater tendency fo accept electrons than another ion

Which of the following instruments is used to measure the pressure of a gas sample? a. an altimeter b. a barometer c. a manometer d. an odometer

a manometer

Fracking is NOT

a new technology

rate constant

a proportionality constant that varies only when the reaction temperature changes

Which of the following buffers will have the highest pH? a. a solution containing 0.20 M HC₂H₃O₂ and 0.20 M NaC2H3O2 (acetic acid and sodium acetate) b. a solution containing 0.25 M HC₂H₃O₂ and 0.15 M NaC₂H₃O₂ c. a solution containing 0.15 M HC₂H₃O₂ and 0.25 M NaC₂H₃O₂ d. they all have the same pH

a solution containing 0.15 M HC₂H₃O₂ and 0.25 M NaC₂H₃O₂

Which of the following solutions can function as a buffer? a. a solution containing HCl and NaCl b. a solution containing NaOH and NaCl c. a solution containing HC₂H₃O₂ and NaC₂H₃O₂ (acetic acid and sodium acetate) d. all of the above

a solution containing HC₂H₃O₂ and NaC₂H₃O₂ (acetic acid and sodium acetate)

electrochemical cell

a system that utilizes a spontaneous oxidation-reduction reaction to pump electrons through an electrical curcuit

Le Chateliers principle applies to which of the following systems

a system which has reached equilibrium

Le Châtelier's Principle applies to which of the following systems?

a system which has reached equilibrium

Which of the following occurs when the weak base ammonia, NH₃, is dissolved in water? a. a very small number of ammonia molecules break up b. a very small number of ammonia molecules take an H⁺ from the water c. a very small number of molecules of NH₄OH are formed d. a very small number of water molecules take an H⁺ from ammonia

a very small number of ammonia molecules take an H⁺ from the water

Which of the following can be characterized as a strong acid? a. 0.001 M HCl b. 3.0 M CH3COOH c. both a and b d. neither a nor b

a. 0.001 M HCl

Which of the following can be characterized as a strong electrolyte? a. 0.001 M HCl b. 3.0 M CH3COOH c. both a and b d. neither a nor b

a. 0.001 M HCl

a. 0.22 L/min

A particular chemical reaction carried out at 20°C takes 2 hours. Approximately how long will it take to carry out the reaction at 40°C? a. 0.5 hour b. 1 hour c. 4 hours d. 8 hours

a. 0.5 hour

For which of the following reactions is it important that the species collide with the correct orientation?

a. 2 NO(g) + O2(g) → 2 NO2(g) b. +-HCl(g) + H2O(l) → H3O (aq) + Cl (aq)

For the reaction 2C → A + B, 0.01 mol of A is formed during the first 15 seconds of the reaction. Assuming that the rate of reaction remains constant for two minutes, which of the following statements is true? a. After 2 minutes 0.08 moles of B were produced. b. After 2 minutes 0.08 moles of C were consumed. c. both a and b d. neither a nor b

a. After 2 minutes 0.08 moles of B were produced.

The temperature effect on reaction rate is the result of which of the following? a. At higher temperatures there are more collisions. b. At higher temperatures a larger fraction of the collisions are effective collisions. c. both a and b d. neither a nor b

a. At higher temperatures there are more collisions .b. At higher temperatures a larger fraction of the collisions are effective collisions.

For the reaction A + B → 2 C, which of the following statements is true? a. B is consumed at the same rate that A is consumed. b. C is produced at the same rate A is consumed. c. both a and b d. neither a nor b

a. B is consumed at the same rate that A is consumed.

According to Arrhenius which species is associated with all acids? a. H3O+ b. OH- c. H2O d. none of these

a. H3O+

When hydrogen chloride gas is dissolved in water which of the following species is not present in the solution? a. HCl(aq) b. H2O(l) c. Cl-(aq) d. None, they are all present.

a. HCl(aq)

When acetic acid is dissolved in water which of the following is true of the equilibrium which is established as represented below? a. It lies very far to the left. b. It lies slightly to the left. c. It lies very far to the right. d. It lies slightly to the right.

a. It lies very far to the left

When solid sodium hydroxide is dissolved in water which of the following species is not present in the solution? a. NaOH(aq) b. H2O(l) c. OH-(aq) d. None, they are all present.

a. NaOH(aq)

Which of the following is true? a. Reactions with low activation energies are rapid. b. The activation energy for an exothermic reaction is negative. c. both a and b d. neither a nor b

a. Reactions with low activation energies are rapid

Many molecular collisions do not result in chemical reaction. Why is this?

a. The colliding molecules are not the correct chemicals .b. The colliding molecules do not have sufficient energy. c. The colliding molecules do not have the correct orientations.

In an energy diagram for an exothermic chemical reaction which of the following is true? a. The energy of the products is lower than that of the reactants. b. The energy of the transition state is higher than that of the reactants. c. both a and b d. neither a nor b

a. The energy of the products is lower than that of the reactants .b. The energy of the transition state is higher than that of the reactants.

Which of the following is true of effective collisions?

a. The number of effective collisions determines the reaction rate .b. The number of effective collisions increases as the temperature is increased.

What is the effect of adding C2H5OH(g) to a container in which the reaction has reached equilibrium? a. The reaction will shift left to right. b. The reaction will shift right to left. c. There will be no effect. d. What happens depends on the temperature.

a. The reaction will shift left to right.

What is the effect of adding CH3COOH(g) to a container in which the reaction has reached equilibrium? a. The reaction will shift left to right. b. The reaction will shift right to left. c. There will be no effect. d. What happens depends on the temperature.

a. The reaction will shift left to right.

Which of the following buffers will have the best buffer capacity? a. a solution containing 0.1 M HC2H3O2 and 0.1 M NaC2H3O2 b. a solution containing 0.05 M HC2H3O2 and 0.15 M NaC2H3O2 c. a solution containing 0.15 M HC2H3O2 and 0.05 M NaC2H3O2 d. They all have the same buffer capacity.

a. a solution containing 0.1 M HC2H3O2 and 0.1 M NaC2H3O2

Drug manufacturers use which of the following when making time release drugs? a. control of the thickness of a drug coating b. control of the size c. both a and b d. neither a nor b

a. control of the thickness of a drug coating b. control of the size

Which of the following is the study of the rates of chemical reactions? a. kinetics b. stoichiometry c. thermodynamics d. none of these

a. kinetics

Which of the following is generally not included when writing an equilibrium constant expression? a. liquids b. solids c. both a and b d. neither a nor b

a. liquids b. solids

Fossil fuel use is directly linked to food production through nitrogen fertilizer production. a. true b. false

a. true

C2H3O2-

acetate ion

HC2H3O2

acetic acid

strong acids

acids that dissociate completely in water

weak acids

acids that only partially dissociate in water

Naming Monatomic Anions

add -ide to the base name.

standard NaOH solution

adding a NaOH solution of known concentration

acid-base titration

adding a base to an acid

When considering the effect of a catalyst on a system to which LeChatelier's Principle can be applied, which of the following is true?

addition of a catalyst speeds up both the forward and reverse reaction by the same amount

Which of the following molecules can engage in hydrogen bonding? a. NH₃ b. H₂O c. HF d. all of them

all of them

which of the following compounds has the largest formula weight?

aluminum acetate

Name binary ionic compound AlCl3

aluminum chloride

NH4Cl

ammonium chloride

standard acid solution

an acid solution of known concentration

which of the following is true of fevers

an increase of above 3 degrees C is potentially fatal

neon is least likely to form

an ion

electrons are transferred from the less electronegative element to the more electronegative element when

an ionic bond is formed

K+ snd Ca^2+ have the same configuration as

argon

Which of the following statements best describes the acid/base relationship? a. as acid strengths increase conjugate base strengths increase b. as base strengths increase conjugate acid strengths decrease c. both a. and b. d. Neither a. nor b.

as base strengths increase conjugate acid strengths decrease

Air pressure can be expressed in which of the following units?

atmospheres, millimeters of Hg, and torr

Which of the following units can used to describe the rate of a chemical reaction? a. (mol·L)/min b. (mol/L)/min c. 1/(mol·L·min) d. none of these

b. (mol/L)/min

How many protons can be lost by citric acid, H3C6H5O6? a. 1 b. 3 c. 5 d. 8

b. 3

Which of the following is true of fevers? a. An increase in body temperature never has beneficial effects. b. A 1°C increase in temperature can be protective. c. A 3°C increase in temperature is invariably fatal. d. None of the above is true.

b. A 1°C increase in temperature can be protective.

Which of the following occurs when the weak base ammonia, NH3, is dissolved in water? a. A very small number of ammonia molecules break up. b. A very small number of ammonia molecules take an H+ from the water. c. A very small number of molecules of NH4OH are formed. d. A very small number of water molecules take an H+ from ammonia.

b. A very small number of ammonia molecules take an H+ from the water

b. As base strengths increase conjugate acid strengths decrease.

Human blood contains which of the following buffers? a. HC2H3O2/C2H3O2- b. H2PO4-/HPO42- c. both a and b d. neither a nor b

b. H2PO4-/HPO42-

Which base is sometimes used as a laxative? a. LiOH b. Mg(OH)2 c. NaOH d. NH3

b. Mg(OH)2

In an energy diagram for an endothermic chemical reaction which of the following is true? a. The energy of the products is lower than that of the reactants. b. The energy of the transition state is higher than that of the reactants. c. both a and b d. neither a nor b

b. The energy of the transition state is higher than that of the reactants

Which of the following is true of the rates of most chemical reactions? a. The initial rate is cannot be measured. b. The initial rate is faster than the rate later in time. c. The initial rate is the same as the rate later in time. d. The initial rate is slower than the rate later in time.

b. The initial rate is faster than the rate later in time

Consider the following hypothetical acid-base reaction. A(aq) + B(aq) C(aq) + D(aq) weaker acid weaker base stronger acid stronger base a. The position of the equilibrium favors the forward reaction. b. The position of the equilibrium favors the reverse reaction. c. Neither the forward nor the reverse reaction are favored at equilibrium. d. The position of equilibrium cannot be predicted from the given data.

b. The position of the equilibrium favors the reverse reaction.

Hydrocyanic acid, HCN, is a weak acid. Which of the following is the correct expression for the Ka of hydrocyanic acid? a. [H3O+][HCN]/[CN-] b. [H3O+][CN-]/[HCN] c. [HCN]/[ H3O+][CN-] d. [HCN][CN-]/[ H3O+]

b. [H3O+][CN-]/[HCN]

Which of the following is the Brønsted-Lowry definition of a base? a. a hydroxide ion acceptor b. a proton acceptor c. a proton donor d. none of these

b. a proton acceptor

Which of the following is true of a buffer prepared with equal concentrations of an acid and its conjugate base? a. pH = 7 b. pH = pKa c. The pH depends on the concentration of the buffer. d. none of the above

b. pH = pKa

b. the number of effective collisions determines the reaction rate

If a particular reactant is involved in the slowest step of a multi-step reaction what will be the effect of increasing its concentration? a. The reaction rate will decrease. b. The reaction rate will increase. c. The reaction rate will be unaffected.

b. the reaction will increase

What is the effect of adding H2O(g) to a container in which the reaction has reached equilibrium? a. The reaction will shift left to right. b. The reaction will shift right to left. c. There will be no effect. d. What happens depends on the temperature.

b. the reaction will shift right to left

Which of the following can be characterized as a strong base? a. 0.001 M KOH b. 3.0 M KOH c. both a. and b. d. Neither a. nor b.

both a. and b.

Which of the following can be characterized as a strong electrolyte? a. 0.001 M HCl b. 3.0 M HCl c. both a. and b. d. Neither a nor b

both a. and b.

Which of the following occurs when an acid reacts with an active metal? a. H⁺ is reduced b. the metal is oxidized c. both a. and b. d. Neither a. nor b.

both a. and b.

ionic compounds are solids in which

both cations and anions are present

Which of the following symbols is used to denote a reversible reaction?

It has been estimated that the production of nitrogen fertilizer, by the Huber-Bosch process, has resulted in being able to feed approximately how many additional people in the world? a. 1 billion b. 2 billion c. 3 billion d. 4 billion

c. 3 billion

Which of the following is the best definition of a catalyst? a. A catalyst is a material which speeds up the rate of a chemical reaction. b. A catalyst is a material which speeds up the rate of a chemical reaction without participating in the reaction. c. A catalyst is a material which speeds up the rate of a chemical reaction without being consumed during the reaction. d. All of the above are equally good definitions.

c. A catalyst is a material which speeds up the rate of a chemical reaction without being consumed during the reactions

For the reaction A + B → 2 C, which of the following best describes how we can measure the reaction rate? a. The rate can be measured by measuring how fast A is consumed. b. The rate can be measured by measuring how fast C is produced. c. Either of the above procedures can be used. d. Neither of the above procedures can be used.

c. Either of the above procedures can be used.

Which of the following is a diprotic acid? a. HCl b. HNO3 c. H2SO4 d. H3PO4

c. H2SO4

When HCl is dissolved in water which of the following is true of the equilibrium which is established? a. It lies virtually completely to the left. b. It lies slightly to the left. c. It lies virtually completely to the right. d. It lies slightly to the right.

c. It lies virtually completely to the right

If the reaction below is at equilibrium and if H2O(g) is added the equilibrium will shift. What happens to the value of the equilibrium constant? a. It will increase b. It will decrease c. It will stay the same d. It will be decreased by 2

c. It will stay the same

Given that the reaction 2 H2(g) + O2(g) → 2 H2O(g) is exothermic, which of the following is true of the reaction 2 H2O(g) → 2 H2(g) + O2(g) ? a. Its activation energy is lower than that of 2 H2(g) + O2(g ) → 2 H2O(g). b. Its activation energy is the same as that of 2 H2(g) + O2(g ) → 2 H2O(g). c. Its activation energy is higher than that of 2 H2(g) + O2(g ) → 2 H2O(g). d. There is no relationship between its activation energy and that of 2 H2(g) + O2(g ) → 2 H2O(g).

c. Its activation energy is higher than that of 2 H2(g) + O2(g) --> 2 H2O (g)

Which of the following is the conjugate base of water? a. H3O+ b. NaOH c. OH- d. O2-

c. OH-

If a reaction occurs very rapidly, even at a relatively low temperature, which of the following is probably true? a. The reaction is endothermic. b. The reaction is exothermic. c. The reaction has a low activation energy. d. The reaction occurs as a single step.

c. The reaction has a low activation energy.

Then notation [A]4 is equivalent to which of the following?

c. [A] × [A] × [A] × [A]

For the reaction 2C → A + B, 0.01 mol of A is formed during the first 15 seconds of the reaction. Assuming that the rate of reaction remains constant for two minutes, which of the following statements is true? a. After 2 minutes 0.08 moles of B were produced. b. After 2 minutes 0.16 moles of C were consumed. c. both a and b d. neither a nor b

c. both a and b

Which of the following can be characterized as a strong acid? a. HNO3 b. H2SO4 c. both a and b d. neither a nor b

c. both a and b

For which of the following reactions is it important that the species collide with the correct orientation? a. 2 NO(g) + O2(g) → 2 NO2(g) b. HCl(g) + H2O(l) → H3O+(aq) + Cl-(aq) c. both of them d. neither of them

c. both of them

When comparing the strength of two weak acids which factor(s) do we use to determine which is the stronger of the two? a. the size of the acid dissociation constants b. the values of the pKa's of the acids c. either a or b d. neither a nor b

c. either a or b

The species H3O+ can be called which of the following? a. heavy water b. hydrogen ion c. hydronium ion d. all of these

c. hydronium ion

Given the following information determine which of these acids is the strongest? Ka for boric acid is 7.3 × 10-10 pKa of acetic acid is 4.75 Ka for lactic acid is 8.4 × 10-4 pKa of phenol is 9.89 a. acetic acid b. formic acid c. lactic acid d. phenol

c. lactic acid

Which of the following solutions can function as a buffer? a. a solution containing HCl and NaCl b. a solution containing NaOH and NaCl c. a solution containing H2SO4 and NaHSO4 d. none of the above

d. none of the above

Ions produced from which of the following acids play an important role in biochemistry? a. acetic b. Boric c. nitric d. Phosphoric

d. phosphoric

Which of the following will determine the pH of a buffer made using acetic acid and sodium acetate? a. the amount of water present b. the [C2H3O2-] c. the [HC2H3O2] d. the ratio [C2H3O2-]/[HC2H3O2]

d. the ratio [C2H3O2-]/[HC2H3O2]

In an energy diagram for a chemical reaction what species represents the highest energy? a. the catalyst b. the products c. the reactants d. the transition state

d. the transition state

H2PO4 -

dihydrogen phosphate

OF2 has a nearly tetrahedral

distribution of electron density

What symbol is used to denote that two or more representations of a species are resonance structures?

double headed arrow

either a. or b.

oxidation reduction (redox)

electron-transfer reactions

all cations have more protons than

electrons

Consider the reversible reaction: PCl3(g) + Cl2(g) PCl5(g), where K = 0.5. Since K < 1, the reaction must be exothermic.

false

Consider the following exothermic reversible reaction at equilibrium: CO(g) + Cl2(g) COCl2(g) When the temperature of the reaction vessel decreases, the system responds by

forming more COCl2

percent =

g/ theoretical x 100

an atom with two valance electrons will most likely

gain two electrons

If a chemist wishes to carry out a reaction in which one reactant is a solid and one is a liquid, which of the following will be most effective in speeding up the reaction?

grinding the solid to a form a powder

Which of the following is associated with cells in a hypotonic solution? a. crenation b. hemolysis c. reverse osmosis d. none of these

hemolysis

The term solution is synonymous with which of the following?

homogeneous mixture

group in periodic table shows

how many acetates

Which of the following acids is the acid found in gastric fluid? a. acetic b. hydrochloric c. nitric d. Sulfuric

hydrochloric

HCO 3-

hydrogen carbonate (bicarbonate)

H+

hydrogen ion

HPO4 2-

hydrogen phosphate

HSO4 -

hydrogen sulfate (bisulfate)

HSO3 -

hydrogen sulfite (bisulfite)

The species H₃O⁺ can be called which of the following? a. heavy water b. hydrogen ion c. hydronium ion d. all of these

hydronium ion

metals give up electrons when

in contact with nonmetals

In the reaction: 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g), increasing the concentration of C2H6(g) will

increase the reaction rate

Electronegativity on the periodic table

increases from left to right, decreases from top to bottom

Which of the following will change the numerical value of the equilibrium constant of a particular reaction?

increasing the temperature

Which of the following will change the numerical value of the equilibrium constant of a particular reaction? a. increasing the concentration of reactants b. increasing the concentration of products c. increasing the temperature d. all of the above

increasing the temperature

Which of the following will change the numerical value of the equilibrium constant of a particular reaction? a. increasing the concentration of the products b. increasing the temperature c. both a. and b. d. Neither a. nor b.

increasing the temperature

Water, which is a polar solvent, is generally a good solvent for which of the following types of compounds?

ionic compounds and polar compounds

activation energy

is the minimum energy necessary for a reaction to start

What happens when an atom gains an electron?

it becomes a negative ion

What happens when an atom loses an electron?

it becomes a positive ion

What is the expression for the equilibrium constant for the reaction: 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)?

k = right side / left side

Which of the following is the study of the rates of chemical reactions?

kinetics

aluminum acetate has the

largest formula weight

PbCl2

lead chloride

Electronegativity increases as we move

left to right

C2H2 has a

linear disribution

https://ourworldindata.org/how-many-people-does-synthetic-fertilizer-feed

link for fertilizer

Name binary ionic compound LiBr

lithium bromide

Name binary ionic compound MgO

magnesium oxide

In a chemical reaction, the mass of the products always equals the

mass of the starting materials

method of initial rates

measuring and comparing the initial reaction rates when the initial reactant concentrations are independently changed

low electronegativities are associated with which type of elements?

metals

CO3^2-

might be found in the solution if an acid is added

fluorine

most electronegative element

in resonance structures you can

move electrons from one location to another

the octet rule does not apply to

nickel

Which of the following solutions can function as a buffer? a. a solution containing HCl and NaCl b. a solution containing NaOH and NaCl c. a solution containing H₂SO₄ and NaHSO₄ d. none of the above

none of the above

which is true about carbonate ion,

none of the above

A student has three gas samples with equal volumes of each gas. All the gases are at the same temperature and pressure. If the three gases are O₂, CO₂, NH₃, which sample contains the largest number of molecules? a. O₂ b. CO2 c. NH3 d. none, they all contain the same number of molecules

none, they all contain the same number of molecules

Which of the following is not an acid? a. H₃O⁺ b. H₂CO₃ c. HPO₄²⁻ d. none, they are all acids

none, they are all acids

Which of the following is not a base? a. HPO₄²⁻ b. OH⁻ c. NH₃ d. none, they are all bases

none, they are all bases

Which of the following is not a unit of pressure? a. mm of Hg b.pascals c. torr d. none, they are all units of pressure

none, they are all units of pressure

high electronegativities are associated with which type of elements?

nonmetals

the valance shell electron configuration of all noble gases except helium is

ns^2np^6

lithium is in group one so it can lose

one electron and gain a positive charge

oxidized

one reactant loses electrons

Hydrogen cyanide has

one single bond and one triple bond

Acetylene has

one triple bond

H2C2O4

oxalic acid

loss of electrons, loss of hydrogen, gain of oxygen

oxidation

reducing agent

oxidized species

Which of the following is the correct relationship between pH and pOH? a. pH+pOH =14 b. (pH) x (pOH) = 14 c. pH/pOH= 14 d. pH-pOH= 14

pH+pOH =14

phenolphthalein in base

pink

CH2CI2 and CH3CI are

polar

CH2CI2 is

polar

NH3 is

polar

Name binary ionic compound KCl

potassium chloride

KMnO4

potassium permanganate

reduced

reactant gains electrons

oxidizing agent

reduced species

gain of electrons, gain of hydrogen, loss of oxygen

reduction

standard reduction potentials

relative reduction potentials

deliquescent

salts that absorb so much water that they form solutions

efflorescent

salts that lose water under normal conditions of temperature and pressure

A polar covalent bond is formed when the electrons of a bond are

shared unequally by the two atoms

If, in the reaction S + O2 SO2 the SO2 is constantly removed by allowing it to react with water, the removal of SO2 will

shift the equilibrium to the right

Consider the reaction: 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g). Decreasing the pressure on the system will cause the equalibrium to

shift to the right

Carbonic acid has 4

single covalent bonds

Which of the following can pass through a dialysis membrane? a. colloidal particles b. macromolecules c. small molecules d. all of them

small molecules

Na+

sodium ion

What is the name of the species formed when a sodium atom loses an electron?

sodium ion

In a solution of a solid in a liquid, the solid is called which of the following?

solute

brackets mean it's not

stable

Each resonance structure is less

stable than is the resonance hybrid

equilibrium

state of most disorder

hydrates

substances that contain water molecules as a part of their crystal structure

electronegativity

tendency of an atom in a bond to attract shared electrons

Which of the following must we know in order to write the equilibrium constant for a chemical reaction?

the balanced chemical equation for the reaction

water of hydration

the bound water molecule attached to a crystal structure

equilibrium

the concentrations of reactants and products stabilize

oxidation number

the difference between the number of valence electrons in the species involved in the reaction and the number present in the atom's uncombined form

in an energy diagram for an exothermic chemical reaction which of the following is true

the energy of the transition state is higher than that of the reactants

what occurs when a magnesium atom is converted to Mg^2+

the magnesium atom loses two electrons

rate equation

the mathematical relationship between the individual reactant concentrations and the reaction rate

In writing the equilibrium constant expression we use square brackets. The notation [A] means which of the following?

the molar concentration of A

if all atoms have filled valance shells

the molecule is stable

which of the following is true of effective collisions

the number of effective collisions determines the reaction rate

second order reaction

the overall reaction order of this reaction is two

Which of the following is characteristic of a buffer? a. the pH will go down significantly when H₃O⁺ is added to the buffer b. the pH will go down very slightly when H₃O⁺ is added to a buffer c. the pH will go up significantly when H₃O⁺ is added to the buffer d. the pH will go up very slightly when H₃O⁺ is added to the buffer

the pH will go down very slightly when H₃O⁺ is added to a buffer

equivalence point

the point at which we have neutralized all of the acid

end point

the point in a titration when the indicator changes color

Which of the following describes the effect of raising the temperature of an exothermic reaction which has not yet reached equilibrium? a. the rate of reaction slows and less product is produced b. the rate of reaction slows, but more product is produced c. the rate of reaction speeds up, but less product is produced d. the rate of reaction speeds up and more product is produced

the rate of reaction speeds up, but less product is produced

which of the following is true of a reaction which has reached equilibrium

the rate of the forward reaction is equal to the rate of the reverse reaction

equilibrium constant

the ratio the concentrations of products to the concentrations of reactants at equilibrium

acid dissociation constant

the reaction of an acid with H2O

first order

the reaction order with respect to that reactant is one

reverse/backward reaction

the reaction products begin reacting re-form the original reactants

second order

the reaction rate is quadrupled as a result of doubling the concentration of one of the reactants

forwards reaction

the reaction shown in a typical chemical equation

For the endothermic reaction N2O4(g) 2NO2(g) what is the effect of removing NO2 from the reaction vessel?

the reaction will shift left to right

If the endothermic reaction N₂O₄(g)⇌2NO₂(g) has reached equilibrium, what is the effect of lowering the temperature of the reaction vessel? a. the reaction will shift left to right b. the reaction will shift right to left c. there will be no further reaction d. what happens depends on the temperature

the reaction will shift right to left

A sample of carbon dioxide occupies 22.4 liters at STP. Which of the following statements apply to the sample? a. the sample contains 6.02 x 1023 atoms b. the sample contains 6.02 x 1023 atoms of oxygen c. the sample contains 6.02 x 1023 molecules d. none of the above

the sample contains 6.02 x 1023 molecules

A sample of carbon dioxide occupies 22.4 liters at STP. Which of the following statements apply to the sample? a. the sample contains 6.02 x 10²³atoms b. the sample contains 6.02 x 10²³ atoms of oxygen c. the sample contains 6.02 x 10²³ molecules d.none of the above

the sample contains 6.02 x 10²³ molecules

titrant

the standard solution

When comparing two acids which of the following is true? a. the stronger acid has the larger Ka c. both a. and b. b. the stronger acid has the larger pKa d. Neither a. nor b.

the stronger acid has the larger Ka

kinetics

the stud of reaction rates and of the mechanisms

overall reaction order

the sum of the orders of the individual reactants

net cell potential

the sum of the reduction potential and the oxidation potential

standard net potential

the sum of the standard reception and oxidation potentials

an ionic bond is associated with

the transfer of electrons

half-cells

the two parts of an electrochemical cell

Which of the following will occur if the temperature of a gas is decreased from 60 K to 30 K? a. the volume will double b. the volume will be halved c. the volume will decrease slightly d. the volume will increase slightly

the volume will be halved

A particular reaction has an equilibrium constant of 1 x 10²⁰. Which of the following best describes the relationship between the equilibrium constant and the reaction rate? a.because the equilibrium constant is large the reaction proceeds rapidly b. there is no relationship between the size of the equilibrium constant and the rate of the reaction c. both a. and b. are true d. Neither a. nor b. is true

there is no relationship between the size of the equilibrium constant and the rate of the reaction

If the reaction H₂(g)+Cl₂(g)⇌2HCl(g) has reached equilibrium, what is the effect of doubling the volume of the reaction vessel? a. the reaction will shift left to right b. the reaction will shift right to left c. there will be no effect d. what happens depends on the temperature

there will be no effect

Which of the following buffers will have the lowest pH? a. a solution containing 0.10 M HC₂H₃O₂ and 0.10 M NaC₂H₃O₂ (acetic acid and sodium acetate) b. a solution containing 0.20 M HC₂H₃O₂ and 0.20 M NaC₂H₃O₂ c. a solution containing 0.30 M HC₂H₃O₂ and 0.30 M NaC₂H₃O₂ d. they all have the same pH

they all have the same pH

What is the purpose of the enteric coating of aspirin?

to insure drug release in the intestine

electronegativity decreases as we move

top to bottom

C2H6 has a nearly tetrahedral distribution

true

Ethane is produced from western Pa wet gas

true

Horizontal drilling is a new tech developed in Texas in 2008

true

Pittsburgh will be a significant global polymer proudcer

true

The Marcellus Shale gas deposit is the largest deposit in the world

true

When the equilibrium constant for a reversible reaction is much greater than one (K > 1), the equilibrium is said to lie to the right.

true

Which pair of species is most likely to form an ionic bond?

two electrically charged species, one positive and one negative

molecular polarity

uneven distribution of molecular charge; determined by polarity of bonds and geometry of molecule

CaCo3 is

unsoluble in water

Carbonic acid has 24

valance electrons

rate

velocity that the reaction occurs at

reversible

when a system at equilibrium is going forward and reverse at the same time

neutralization reaction

when the acid is neutralized by a base

half-reactions

when two reactions constitute half of the overall reaction

Which of the following is an example of a colloid in which a gas is dispersed in a liquid?

whipped cream

organic acids

compounds that contain a carboxyl group

bases

compounds that have an unshared electron pair

acids

compounds that release hydrogen ions

when two nonmetallic elements interact to form a compound the bond formed is

covalent

Which of the following could be the equilibrium constant for a reaction which proceeds very far in the direction of the products?

d. 1 × 10^15

Which of the following is a triprotic acid? a. HCl b. HNO3 c. H2SO4 d. H3PO4

d. H3PO4

For the reaction which of the following is the equilibrium constant expression? a. K = [H2][O2]/[H2O] . b. K = [H2O]/[H2][O2] c. K = [H2O]2/[H2]2[O2] d. K = [H2]2[O2]/[H2O]2

d. K = [H2]2[O2]/[H2O]2

Which base is an important starting material in the manufacture of fertilizers? a. LiOH b. Mg(OH)2 c. NaOH d. NH3

d. NH3

Which of the following is the conjugate acid of ammonia, NH3? a. H+ b. H3O+ c. NH2- d. NH4+

d. NH4+

Which of the following is not a base? a. HPO42- b. OH- c. NH3 d. None, they are all bases.

d. None, they are all bases

Which of the following is true of all multi-step reactions? a. They involve more than two reactant molecules. b. They are endothermic. c. they are exothermic. d. The rate of reaction is determined by the slowest step.

d. The rate of reaction is determined by the slowest step.

Acetic acid, CH3COOH, is a stronger acid than the ammonium ion, NH4+. When acetic acid reacts with ammonia, NH3, what species are present in the solution in the largest amount? a. acetic acid, CH3COOH and ammonia, NH3 b. acetic acid, CH3COOH, and ammonium, NH4+ c. acetate ion, CH3COO-, and ammonia, NH3 d. acetate ion, CH3COO-, and ammonium ion, NH4+

d. acetate ion, CH3COO-, and ammonium ion, NH4+

If the reaction below is at equilibrium and if H2O(g) is added the equilibrium will shift. Why? a. Because Le Chatelier's principle says the stress must be relieved b. Because the addition of water has made the reaction system more ordered (higher water concentration) c. Because the second law of thermodynamics states that the universe moves spontaneously towards disorder (increasing entropy, more disorder) d. All of the above

d. all of the above

Which of the following must we know when we carry out a titration? a. the concentrations of all reactants except one b. the stoichiometric ratio of the reactants c. the volumes all reactants d. all of the above

d. all of the above

monatomic anions end in

-ide

Which of the following units can used to describe the rate of a chemical reaction?

(mol/L)/min

A solution is prepared by dissolving 53.5 grams of ammonium chloride, NH4Cl in 4000 grams of water? What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water] a. -0.37°C b. -0.47°C c. -0.93°C d. -1.86°C

-0.93°C

A solution is prepared by dissolving 104.10 grams of barium chloride, BaCl2 in 1000. grams of water? What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

-2.79 C

In writing the equilibrium constant expression we use square brackets. The notation [A] means which of the following? a. the mass of A b. the number of moles of A c. the molecular concentration of A d. none of the above

The molar concentration of A

Naming Cations for Elements of Groups 1A, 2A, 3A

The name of the cation is the name of the metal followed by the word "ion"

Which of the following is true of effective collisions?

The number of effective collisions determines the reaction rate.

Consider a sample of water in a closed, rigid container. Which of the following would indicate that the reaction has reached equilibrium?

The pressure in the container remains constant.

For the reaction A+B-->2C, which of the following best describes how we an measure the reaction rate?

The rate can be measured by measuring how fast A is consumed and the rate can be measured by measuring how fast C is produced.

Which of the following describes the effect of raising the temperature of an endothermic reaction which has not yet reached equilibrium? a. The rate of reaction slows and less product is produced b. The rate of reaction slows, but more product is produced c. The rate of reaction speeds up, but less product is produced d. The rate of reaction speeds up and more product is produced

The rate of reaction speeds up and more product is produced

Which of the following describes the effect of raising the temperature of an exothermic reaction which has not yet reached equilibrium?

The rate of reaction speeds up, but less product is produced.

When the concentration of a reactant is increased which of the following is true?

The rate of reaction usually increases.

Which of the following is true of a reaction which has reached equilibrium? a. The rate of the forward reaction is equal to the rate of the reverse reaction b. The reactants have been completely converted to products c. The rate of the forward reaction is faster than the rate of the reverse reaction d. The rate of the forward reaction is slower than the reverse reaction

The rate of the forward reaction is equal to the rate of the reverse reaction

Which of the following is true of a reaction which has reached equilibrium?

The rate of the forward reaction is equal to the rate of the reverse reaction.

If a reaction occurs very rapidly, even at a relatively low temperature, which of the following is probably true?

The reaction has a low activation energy.

In a particular chemical reaction 2 bonds are broken and no bonds are formed. Based only on this information, which of the following is true?

The reaction is endothermic

If the endothermic reaction N₂O₄(g)⇌2NO₂(g) has reached equilibrium, what is the effect on doubling the volume of the vessel? a. there will be no further reaction b. the reaction will shift left to right c. the reaction will shift right to left d. what happens depend on the temperature

The reaction will shift left to right

If the endothermic reaction has reached equilibrium, what is the effect of lowering the temperature of the reaction vessel?

The reaction will shift right to left.

What is the effect of adding H2O(g) to a container in which the reaction has reached equilibrium?

The reaction will shift right to left.

Which of the following happens when NaCl, an ionic compound, dissolves in water?

Chem quiz 3, Chem exam 2, Chem exam #4 (chapters 7 & 8), Exam 3 Study Guide, Chem test 3, chem ch 7, CHEM chapter 7, Chemistry 1601 final set, Chem chapter 7, 8, INTRO TO CHEM FINAL STUDY GUIDE

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