Chemistry 1 Final

According to the balanced reaction below, calculate the moles of NO₂ that form when 5.20 × 10⁻³ mol of N₂O₅ completely reacts: 2N₂O₅(g)→4NO₂(g)+O₂(g)

0.0104 mol NO2

100.0 mL of a 0.500 M solution of KBr is diluted to 500.0 mL. What is the new concentration of the solution?

0.1M

How many orbitals are in the n=4 shell? Select one: a. 8 b. 16 c. 4 d. 32

16

If 2.00 moles of H₂ and 1.55 moles of O₂ react how many moles of H₂O can be produced in the reaction below? 2 H₂(g) + O₂(g) → 2 H₂O(g)

2 mol

Convert 287 kPA to atm

2.83 atm

The mineral gibbsite has the formula Al(OH)3 . What mass, in kg, of Al is present in 9.0 kg of gibbsite?

3.11 kg

Convert 3.20 bar to atm

3.16 ATM

What is the atomic number for an element whose mass number is 78, which contains 40 neutrons per atom?

38

How many miles can you drive, if your car gets 32.60 miles per gallon and you have 12.0 gallons of gas?

391 miles

A sample of 2.00 mol of gas in a 10.00 L container is at 45.0 °C. What is the pressure (in atm) of the gas?

5.22 atm

What is the frequency of green light that has a wavelength of 531 nm? (c = 3.00 x 10⁸ m/s)

5.65 x10^14 1/s (use: C=Y*V)

The molar mass of a compound is 133.2. How many moles are present in a 9.07 kg sample of this compound?

68.1

The formula for barium nitrate is: Select one: a. Ba(NO3)2 b. BaNO3 c. Ba(NO2)2 d. Ba3N2

A

What is the formal charge on nitrogen in NH3? Select one: a. +1 b. -3 c. 0 d. +3

A

What is the shape of NF3 ? Select one: a. Pyramidal b. Planar c. Tetrahedral d. Linear

A

How many valence electrons are in PF6-1 ? Select one: a. 48 b. 46 c. 42 d. 36

A. 48

The cation, 134Ba+2, has how many protons, electrons, and neutrons?

A. 56 protons, 54 electrons, and 78 neutrons.

What is the correct IUPAC name for Al(NO₂)₃?

Aluminum Nitrite

A sample contains 3.23 x 1025 molecules of CO2. What would be the mass of that sample, in grams? Select one: a. 5.36 x 101 grams b. 2.36 x 103 grams c. 1.95 x 1049 grams d. 1.22 grams

B

What is the identity of a 100. g sample of metal that, upon absorbing 4680 J of heat, increases in temperature by 52.0°C? A) Mg B) Al C) Ti D) Fe

B) Al

Which of the following is a transition metal? A) Strontium B) Silver C) Sulfur D) Samarium E) Sodium

B) Silver

Draw the Lewis structure of CH₂NH and then choose the appropriate pair of hybridization states for the two central atoms. Your answer choice is independent of the orientation of your drawn structure. Click to edit molecule A) sp / sp² B) sp² / sp² C) sp² / sp³ D) sp³ / sp³ E) sp³ / sp

B) sp² / sp²

Which hydrocarbon has all of its atoms in the same plane? A) C₂H₆ B) CH₄ C) C₂H₄ D) C₃H₄

C) C₂H₄

Which of the following is a lanthanide element? A) Lithium B) Molybdenum C) Europium D) Plutonium E) Astatine

C) Europium

Which of the following ions has the electron configuration 1s²2s²2p⁶? A) Mg⁺ B) N²⁻ C) N³⁻ D) O⁻ E) F⁺

C) N³⁻

Which of the following states that no two electrons can have the same set of four quantum numbers? A) Hund's rule B) de Broglie wave equation C) Pauli exclusion principle D) Bohr equation E) Schrödinger equation

C) Pauli exclusion principle

Which of the following is NOT an alkali or alkaline earth element? A) Ra B) Cs C) Sc D) Be E) Rb

C) Sc

What is the correct IUPAC name for CaBr₂?

Calcium Bromide

What is the correct IUPAC name for Ca(NO₃)₂?

Calcium Nitrate

What is the correct IUPAC name for CsHSO₄?

Cesium Hydrogen Sulfate

Rank the following atoms in order of increasing first ionization energies (i.e., lowest to highest): Rb, F, Mg, B, N. A) F < N < B < Mg < Rb B) Rb < Mg < F < N < B C) Mg < Rb < F < N < B D) Rb < Mg < B < N < F E) Rb > B > N > F > Mg

D) Rb < Mg < B < N < F

A π bond could be formed from the overlap of which two orbitals? A) two sp² hybrid orbitals B) a 1s and a sp² hybrid orbital C) a sp and a sp² hybrid orbitals D) two unhybridized p orbitals

D) two unhybridized p orbitals

Which particles make up Cathode Rays? Select one: a. alpha particles b. neutrons c. protons d. electrons e. jumbotrons

D. Electrons

Which of the following is a halogen? A) Sodium B) Copper C) Neodymium D) Selenium E) Iodine

E) Iodine

Write the chemical formula for iron(III) oxide

Fe2O3

Predict the chemical formula for the ionic compound formed by the elements K and S

K₂S

Write the chemical formula for lithium hydroxide

LiOH

Rank the following compounds in order of increasing mass percentage of nitrogen: NO, NO₂, N₂O.

Mass percentage can be calculated by finding the ratio of the mass of atoms of an element to the total mass in a molecule. One could calculate the value for each compound using the molar masses of 14.01 g for N and 16.00 g for O, but the relative mass percentages can determined just by inspection of the formula, recognizing that the molar masses of N and O are very similar.N₂O contains 2 nitrogen atoms for every three atoms in the molecule, so a mass fraction of approximately 2/3 or ~67%.NO contains 1 nitrogen atom for every two atoms in the molecule, or a mass fraction of approximately 1/2 or ~50%.NO₂ contains 1 nitrogen atom for every three atoms in the molecule, or a mass fraction of approximately 1/3 or ~33%.

Which of the following metric prefixes corresponds to 10⁻⁶? A) centi- B) kilo- C) mega- D) micro- E) milli-

Micro

Write the chemical formula for lead(II) nitrate

Pb(NO3)2

Write the chemical formula for lead(II) nitrate

Pb(NO₃)₂

Which of these has the lowest first ionization energy? Select one: a. Sr b. K c. Rb d. Mg e. Br

Rb

Determine the correct number of valence electrons and draw the correct electron dot structure for CH3CH2OH and upload a good photo of your work.

20 Valence Electrons

What is the molar mass of potassium phosphate, K3PO4? Enter the numeric value very carefully below, rounding to one decimal place only. Do not put the units in, but think about what the units are!

212.2

A compound containing a metal atom, M, with atomic mass 93.47 combines with oxygen to form the compound M2O2. What is the molar mass of this compound?

218.94 g/mol

Gasoline in Iceland costs approximately 220 ISK (Icelandic Krona) per liter. Assume 12000 ISK = $100 (US) and 1 gallon = 3.785 L and convert the price of gasoline to dollars (and cents) per gallon.

220 ISK/L * 3.785L/gal = 832.79 ISK/gal 832.79 ISK/gal * $100/12000ISK = $6.94/gal

Determine the formula weight of Al₂(SO₄)₃. Provide an answer to two decimal places.

340 amu

A mythical element, idontexistium (Id) has two stable isotopes. 394Id (393.427amu) and 397Id (396.513amu). If the abundance of 394Id is 13.57 and 397Id is the remainder, what is the average atomic mass of Id?

396.1 Average atomic mass= m1*p1+m2*p2

What is the energy of a photon with a frequency of 7.00 × 10¹⁴ s⁻¹? (h = 6.626 × 10⁻³⁴ J • s)

4.64 x10^-19 J (use E=HV)

What is the mass of a compound with molar mass 142.5 if there are 31.632 moles present? Make sure to include your units.

4508 g

How much heat is required to heat 1.8 kg of water from 3.6oC to 14.8oC? The heat capacity of water is 4.1813 J/g*oC

84000 J

A 5.7 L balloon is filled with He at 1.00bar pressure and 298 K. How many He atoms are in the balloon?

?

Calculate the mass of oxygen that will be prepared through the decomposition of 50 kg of potassium chlorate ( KClO3 , Molar mass= 122.55 g/mol)2 KClO3 → 2 KCl + 3 O2 Select one: a. 19.6 kg b. 612 kg c. 9.8 kg d. 12.25 kg

A

Choose the correct ratio of C3H6 : O2 in the balanced version of the following chemical equation: C3H6 + O2 → CO2 + H2O Select one: a. 2:9 b. 6:2 c. 5:2 d. 2:3

A

Which is the balanced equation for combustion of n-butanol (C4H9OH)? Select one: a. C4H9OH + 6 O2 → 4 CO2 + 5 H2O b. 2 C4H9OH + 16 O2 → 4CO + 5H2O c. C4H9OH + 5 O2 → 4CO2 + 5H2O d. 2 C4H9OH + 13 O2 → 8CO2 + 10 H2O

A

Which of the following does NOT describe the element bromine (Br)? A) A metalloid B) A nonmetal C) A main group element D) A halogen

A) A Metalloid Bromine (Br) is in group 7A (17) making it a halogen. This also means it is a main group element as well as a nonmetal.

rue or false: two electrons can simultaneously occupy the same (n,ℓ,mℓ) orbital. A) True B) False

A) True Correct! The fourth quantum number, the spin number (ms), allows for two electrons to have the same n, ℓ, mℓ quantum numbers, but different values for ms.

Equal amounts of heat are added to equal masses of substances A and B at the same temperature, but substance B gets hotter. What is true of their heat capacities (c)? A) c(A) > c(B) B) c(B) > c(A) C) c(a) = c(B) D) Not enough info

A) c(A) > c(B)

The reactant in a chemical reaction that is the first to be used up is called _________.

A) limiting reactant

A ground state atom of Mg could not have any electrons with which of the following configurations? A) n = 3, ℓ = 1, mℓ = 0, ms = +½ B) n = 2, ℓ = 1, mℓ = 0, ms = +½ C) n = 3, ℓ = 0, mℓ = 0, ms = +½ D) n = 2, ℓ = 0, mℓ = 0, ms = +½ E) n = 1, ℓ = 0, mℓ = 0, ms = +½

A) n = 3, ℓ = 1, mℓ = 0, ms = +½

Draw the Lewis structure of CH₂CCH₂ and then choose the appropriate set of pair hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure. Click to edit molecule A) sp² / sp / sp² B) sp² / sp² / sp³ C) sp³ / sp² / sp D) sp² / sp² / sp² E) sp / sp³ / sp³

A) sp² / sp / sp²

Draw the Lewis structure of glycine (NH₃⁺CH₂COO⁻) and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure. Click to edit molecule A) sp³ / sp³ / sp² B) sp / sp² / sp² C) sp² / sp / sp³ D) sp / sp / sp² E) sp³ / sp³ / sp

A) sp³ / sp³ / sp²

When molecules absorb heat, there is an increase in A) the kinetic energy of the molecules. B) The potential energy of the molecules. C) The mass of the molecules. D) The bond energy of the molecules.

A) the kinetic energy of the molecules.

How many valence electrons are in XeF4? (Assume that the s and p electrons count for Xe, but not the d electrons since that shell is filled.) Select one: a. 36 b. 38 c. 24 d. 28

A. 36

If 65 grams of Zn are reacted with excess HCl, approximately what volume of H2 gas will be produced at 298K and 1 bar pressure?Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) Select one: a. 12.5L b. 25 L c. 50L d. 33L

B

Which molecule does not have more than one resonance form? Select one: a. C6H6 b. BF3 c. NO3-1 d. SO2

B

Which molecule in bent? Select one: a. NO3-1 b. H2S c. HCN d. PH4+1

B

Which of the following metric prefixes corresponds to 10³? A) centi- B) kilo- C) mega- D) micro- E) milli-

B

Which set of quantum numbers (n, l, ml, ms ) is not allowed? Select one: a. (2,1,0,-1/2) b. (3,1,2,-1/2) c. (4,0,0,+1/2) d. (3,1,-1,+1/2)

B

Which molecule(s) have at least one double bond? Select one or more: a. N2 b. CO2 c. NO3- d. CO

B & C

The ground state electron configuration of an Al atom is A)1s²2s²2p⁶3s²3d¹ B) 1s²2s²2p⁶3s²3p¹ C) 1s²2s²2p⁶3s²3p⁶4s²4p¹ D) 1s²2s²2p⁶3s²3p² E)1s²2s²2p¹

B) 1s²2s²2p⁶3s²3p¹

Which atomic orbitals from carbon hybridize to form the bonds in CH₄? A) 1s, 2p_x, 2p_y, 2p_z B) 2s, 2p_x, 2p_y, 2p_z C) 3s, 3p_x, 2p_y, 2p_z D) 2s, 2p_x, 2p_y Time's

B) 2s, 2p_x, 2p_y, 2p_z

An atom has nine protons and ten electrons. This makes it: A) Nonstoichiometric B) An ion C) A cathode ray D) An alpha particle E) Neutrally charged

B) An ion

Balance the following reaction and select the correct values of I, J, K AND L. IC5H12O2 + JO2 --> KCO2 + LH2O Select one: a.1, 8, 5, 6 b.1, 7, 6, 5 c.1, 7, 5, 6 d.1, 16, 5, 6

C

CO2 gas with a volume of 25.0L was collected at 25 degrees Celsius and 0.982 atm. Calculate the pressure of the gas if it compressed to a volume of 0.150 L and heated to 350 degrees Celsius. Select one: a. 0.0001215 atm b. Cannot be determined c. 342 atm d. 1.54 atm

C

Calculate the volume of a balloon that can be filled at 1.00 atm with the helium in a 2.50-L compressed gas cylinder in which the pressure is 200 atm at 298K. Select one: a. 5,525 L b. 2.50 L c. 500 L d. 0.002 L

C

How many moles of P4O10 are in 1.11 grams of P4O10?[The Molar Mass of P4O10 is 283.886 g/mol.] Select one: a. 315.12 moles b. 1.11 moles c. 3.91 x 10 -3 moles d. 9.42 x 10 21 moles e. 2.36 x 10 21 moles

C

There are two naturally occurring isotopes of europium, ¹⁵¹Eu (151.0 amu) and ¹⁵³Eu (153.0 amu). If the atomic mass of Eu is 151.96, what is the approximate natural abundance of ¹⁵¹Eu? A) 20% B) 40% C) 50% D) 60% E) 80%

C

What is the name of Fe2O3? Select one: a. Iron (II) Oxide b. Diron (III) Trioxide c. Iron (III) Oxide d. Iron Trioxide

C

What is the name of MgS? Select one: a. magnesium sulfate b. magnesium sulfite c. magnesium sulfide d. magnesium monosulfide

C

What pressure is required to allow 1.5L of He at 1 bar pressure to expand to 5.8L? Select one: a. 7.30 b. 8.70 c. 0.26 d. 3.87

C

Why does BrF5 have a square pyramidal shape? Select one: a. There are 5 electron domains around the Br. b. None of the above, the molecule is not square pyramidal. c. There are 5 bonding electron domains and one non-bonding domain around the Br atom. d. Bromine can have an expanded octet.

C

If you have 1 mol Xe and 1 mol F₂, how many moles of XeF₄ can you create in the following chemical reaction? Xe (g) + 2 F₂ (g) → XeF₄ (g) A) 2 mol B) 1 mol C) 0.5 mol D) 0.25 mol

C) 0.5 mol

Which one of the following changes would cause the pressure of a gas to double assuming volume and moles were held constant? A) Increasing the temperature from 20.0 °C to 40.0 °C. B) Decreasing the temperature from 400 K to 200 K. C) Increasing the temperature from 200K to 400K. D) Decreasing the temperature from 40.0 °C to 20.0 °C.

C) Increasing the temperature from 200K to 400K.

For which atomic orbital does n = 3 and ℓ = 1? A) 2s B) 3s C) 3p D) 3d E) 4d

C. 3P

What is Molar Mass of C6H16Cl2N4? Select one: a. 62.479 g/mol b. 72.066 g/mol c. 158.11 g/mol d. 342.23 g/mol e. 215.124 g/mol

E

What is the noble gas core in the electron configuration for U? A) Ne B) Ar C) Kr D) Xe E) Rn

E) Rn

The nucleus of an atom contains: A) Protons and electrons B) Protons and neutrons C) Electrons and neutrons D) Protons, neutrons and electrons E) Electrons only

Protons and Neutrons

Predict the chemical formula for the ionic compound formed by NH₄⁺ and PO₄³⁻

(NH₄)₃PO₄

Determine the mass in grams of 1.6 × 10⁻³ mol glucose, C₆H₁₂O₆

0.29 g C6H12O6

In a 4.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.20 atm, how many moles of steam are in the cooker?

0.41 mol

How many moles of propylene (C₃H₆) are in 25.0g of the substance?

0.594 mol C3H6

If n = 2, what is the maximum allowed value for ℓ?

1

Identify each of the following ions as having the correct or incorrect charge. 1. F2- 2. Se2- 3.Na2+ 4. Cu2-

1. Incorrect- F 1- 2. Correct 3. Incorrect Na 1+ 4. Incorrect Cu

Identify each of the following ions as having the correct or incorrect charge. 1. SE2- 2. NA2+ 3. F2- 4. CU2-

1. correct 2. Incorrect. Na +1 3. Incorrect. F -1 4. Incorrect. Cu +1

Determine the number of grams of HCl that can react with 0.750g of Al(OH)₃ according to the following reaction Al(OH)₃(s) + 3HCl(aq)→ AlCl₃(aq) +3H₂O(aq)

1.05 g HCL

Convert 1.30 atm to Pa 1.30 atm

1.32 x 10^ 5 PA

Convert 1050 mmHg to bar.

1.4 bar

A sample of argon has a volume of 1.2 L at STP. If the temperature is increased to 22°C and the pressure is lowered to 0.80 atm, what will the new volume be, in L?

1.6 L

How many milliliters are in a liter?

1000 mL

Deci

10^-1 (0.1)

Centi

10^-2 (0.01)

Milli

10^-3 (0.001)

Tetra

10^12

Kilo

10^3 (1000)

Mega

10^6 (1,000,000)

Giga

10^9

Determine the formula weight of KBr.

119 amu

What is the mass of one mole of carbon atoms?

12

How many calories are in 5401 J ? (1 cal = 4.184 J)

1291 Cal

Determine the correct number of valence electrons and draw the electron dot structure of NO2- ion. Upload a good photo of your work.

18 Valence electrons

An irregularly-shaped piece of aluminum (Al) has a mass of 50.6 grams. What is the volume in cm³ of this piece of aluminum if its density is 2.70 g/cm³?

18.7 cm³

What is the final temperature (in °C) of 150.1 g of water (specific heat = 4.184 J/g･°C) at 24.20°C that absorbed 950.0 J of heat?

25.71 degrees celcius

Determine the number of valence electrons in TeOF₂ and draw the correct electron dot structure. Make sure to follow the octet rule on all atoms.

26 VE

Draw the correct electron dot structure for the chlorate ion ClO3-1 with the lowest possible formal charges.

26 VE

There are 14.5 psi per bar. Calculate the pressure in psi at 1.8 bar.

26 psi

A popular car has an engine that is reported to have a volume of 4320 cm^3 what is the size in cubic inches?

264 in^3

A parsec is a unit of length equal to about 3.10X1013 km. How long will it take light, moving at 3.00X108 m/s to travel 1.00 parsec. (3.154X107 seconds = 1 yr)

3.27 years

At what pressure in atm does ethane (C₂H₆) have a density of 37.2 g/L at 40.0 °C?

31.9 atm

If 75J of heat are applied to 6.1 L of a gas at 732 mmHg and 298K, what is the final temperature, in K, of the gas? Cp for an ideal gas is 20.79 J/mol*K.

310 K

Determine the molar mass of CH₃OH.

32 g/mol

Convert 3.20x10^4 J to KJ

32.0 KJ

A small sample of a pharmaceutical named Placebin contains 0.00937 moles of the active ingredient, (2R,3R,4S,5S,6R)-2-[(2S,3S,4S,5R)-3,4-dihydroxy-2,5-bis(hydroxymethyl)oxolan-2-yl]oxy-6-(hydroxymethyl)oxane-3,4,5-triol which has a molar mass of 342.2965 g/mol. How many mg are in this sample?

3210mg

Determine the molar mass of CH₃OCH₃.

46 g/mol

.Convert 3.2 ft^2 to square inches

460 in^2

A photon has a frequency of 8.63 × 10⁸ Hz. What is the energy of this photon? (h = 6.626 × 10⁻³⁴ J • s)

5.72 × 10⁻²⁵ J

An unknown element X has the following isotopes: ⁵²X (85.50% abundant), ⁴⁹X (8.00% abundant), ⁵⁰X (6.50% abundant). What is the average atomic mass in amu of X?

52 AMU

How many mg in 5.6 kg? Make sure to include units in your answer

5600000 mg

What is the mass percentage of Na in Na₂S?

59%

What is the value of Avogadro's number?

6.00x10^23

A compound containing a metal atom, M, with atomic mass 56.47 combines with oxygen to form the compound M1O2. What is the percentage of M in this compound?

64

How many mmHg are in 89.6 kPa?

672 mmHg

Determine the molar mass of LiNO₃. Provide an answer to two decimal places.

69 g/mol

An atom of a particular element has a volume of 7.8x10^-31 m^3. What is the volume in cubic nanometers?

7.8x10^-4 nm^3

Determine the molar mass of Ca(OH)₂. Provide an answer to two decimal places.

73 g/mol

Determine the mass, in grams, of 0.400 moles of Pb (1 mol of Pb has a mass of 207.2 g).

83 g

What is the mass (in grams) of 5.00 L of propane vapor (C₃H₈) at STP?

9.8 g

Which of the following is an assumption of the ideal gas law? Select one: a. All collisions are elastic b. Molecules occupy space. c. All collisions are not elastic. d. The distance between collisions is very short.

A

Which atom and/or ion is (are) isoelectronic with Br+ (note that this ion IS NOT A COMMON ION). Pick ALL that are correct. Select one or more: a. Se b. Cl- c. S2+ d. Kr e. Se2+ f. As- g. Ga3+

A + F Isoelectronic: having the same numbers of electrons or the same electronic structure.

Which of the following groups of elements tend to form cations? A) Metals B) Metalloids C) Nonmetals D) Noble gases E) Radioactive elements

A) Metals

Which of the following electron configurations is incorrect? A) Ca [Ar]4s² B) Mn [Ar]4s²4d⁵ C) Cu [Ar]4s¹3d¹⁰ D) Ga [Ar]4s²3d¹⁰4p¹ E) Br [Ar]4s²3d¹⁰4p⁵

B) Mn [Ar]4s²4d⁵ Mn is in the third d block, not the fourth.

Which of the following elements would be chemically similar to calcium (Ca)? A) K B) Sr C) Sc D) S E) Ga

B) Sr

What is the atomic symbol and mass number for an atom containing 50 protons and 64 neutrons? A) ⁵⁰Sn B) ¹¹⁴Sn C) ⁶⁴Sn D) ⁶⁴Gd E) ¹¹⁴Gd

B) ¹¹⁴Sn

Which of the following quantities is equivalent to 3.7 cm? A) 3.7×10⁻³ m B) 3.7×10⁻⁵ km C) 3.7×10⁻² mm D) 3.7×10⁵ μm E) 3.7×10² mm

B.

Which molecule has the longest N-N bond? Select one: a. HNNH b. H2NNH2 c. N2 d. NO3-1

B. H2NNH2

What is the correct IUPAC name for BaHPO₄?

Barium Hydrogen Phosphate

What is the correct IUPAC name for BaS?

Barium Sulfide

A molecule has an empirical formula of CH, and its molar mass is known to be 26 g/mol. What is its molecular formula? A) CH B) CH₂ C) C₂H₂ D) C₂H E) C₃H₃

C2H2

Glucose is an important biological molecule with the molecular formula C₆H₁₂O₆. What is its empirical formula? A) CHO B) CH₂O C) C₂HO₂ D) C₆H₁₂O₆ E) Not enough info

CH2O

Predict the chemical formula for the ionic compound formed by the elements Ca and Br

CaBr₂

What is the correct IUPAC name for CrBr₃?

Chromium (111) bromide

Write the chemical formula for cobalt(II) hydrogen carbonate

Co(HCO3)2

Write the chemical formula for cobalt(II) oxide

CoO

Write the chemical formula for cesium carbonate

Cs2CO3

Write the chemical formula for copper(I) chlorite

CuClO2

Columns on the periodic table are known as A) Periods B) Halogens C) Metals D) Groups E) Metalloids

D

The formula for barium nitrate is: Select one: a. Ba3N2 b. Ba(NO2)2 c. BaNO3 d. Ba(NO3)2

D

When 10 Joules of heat are transferred into 30 g of Copper at 18.20oC, the final temperature is 19.07oC. What is the specific heat of copper? Select one: a. 10 b. 11.49 c. 30 d. .383

D

Which molecule contains sp hybridized orbitals? A) C₂H₆ B) CH₄ C) C₂H₄ D) C₃H₄

D) C₃H₄

Under what conditions are gases most likely to behave ideally? A) High pressures B) Low temperatures C) Polar molecules D) Low pressures E) Large molecules

D) Low pressures

Which of the following statements concerning the periodic table is NOT correct? Select one: a. The columns of the periodic table are called periods and the horizontal rows are called groups. b. Dmitri Mendeleev invented the periodic table in 1869. c. Alkali metals and alkaline earth metals are never found as a metallic element in nature. d. The least reactive elements are the noble gasses, which are in group 8A.

a. The columns of the periodic table are called periods and the horizontal rows are called groups.

Looking at the Table of First Ionization Energies, if the n=1 shell held 3 electrons max (instead of two) then the 1st Ionization Energy for Li(g) would be around ______ MJ/mol. a. ~3100 MJ/mol b. ~3.3 MJ/mol c. ~0.510 MJ/mol d. ~1.9 MJ/mol

b. ~3.3 MJ/mol

The element neon is ... Select one: a. A member of group 1, alkali metals b. A member of group 2, alkaline earth metals c. A member of group 17, halogens d. A member of group 18, noble gases e. A transition metal

d. A member of group 18, noble gases

What is the electron configuration that best represents the ground state of I(g)? Select one: a. [Kr]5s14d105p6 b. [Kr]5s24d95p6 c. [Kr]5s24d105p36s2 d. [Kr]5s24d105p5

d. [Kr]5s24d105p5

Which pair of ions will form a compound of formula M2X? Select one: a. sodium and fluoride b. potassium and cyanide c. magnesium and chloride d. ammonium and sulfate

d. ammonium and sulfate

What is the mass percentage of C in C₂H₄O₂?

40%

A compound has the mass percent data given below. Determine its empirical formula. 32.43 % carbon by mass 8.16 % hydrogen by mass 21.60 % oxygen by mass 37.81 % nitrogen by mass Select one: a. C2H6N2O1 b. C2H8N1O2 c. C3H6N2O2 d. C3H6N3O3

A

The formula for strontium (Sr) nitrate is: Select one: a. SrNO3 b. Sr(NO3)2 c. Sr(NO2)2 d. Sn3N2

B

12oz of water initially at 75oF is mixed with 20oz of water intiially at 140oF. What is the final temperature? a. 140oF b. 116oF c. 108oF d. 59oF

?

Which one of the following is NOT a statement of the Kinetic Molecular Theory? A) Gas particles will be attracted to one another. B) The volume available to the gas particles is equal to the volume of the container. C) The measured pressure is from collisions of the gas particles with the walls of the container. D) The average kinetic energy is proportional to the temperature of the system.

A) Gas particles will be attracted to one another.

Which of the following is an alkaline earth metal? A) Rubidium B) Beryllium C) Iridium D) Americium E) Phosphorous

B) Beryllium

ClF3 has what geometry? Select one: a. See-saw b. Square pyrimdal c. Trigonal bipyramidal d. T-shaped

C

Determine the number of protons (p) and electrons (e) in Mg²⁺. A) 10 p, 12 e B) 12 p, 12 e C) 12 p, 10 e D) 12 p, 14 e E) 10 p, 10 e

C

How many milliliters of 10.0M HCl are needed to make a 350 mL solution of HCl with a Molarity of 0.67M? Select one: a. 19 mL b. 1.9 mL c. 23 mL d. 0.043 mL

C

What pressure is required to allow 2.0L of He at 1 bar pressure to expand to 3.0L? a. 1.5 bar b. 0.5 bar c. 0.66 bar d. 3.0 bar

C

Which of the following sets of quantum numbers can describe a 3p electron? A) n = 1, ℓ = 3, mℓ = 1 B) n = 3, ℓ = 2, mℓ = 1 C) n = 3, ℓ = 1, mℓ = 1 D) n = 3 , ℓ = 0, mℓ = 1 E) n = 2, ℓ = 3, mℓ = 1

C) n = 3, ℓ = 1, mℓ = 1

Draw the Lewis structure of phosphate (PO₄³⁻) by following the octet rule on all atoms and then determine the hybridization of the central atom. Click to edit molecule A) sp³d² B) p C) sp³ D) sp⁵ E) sp³d

C) sp³

Draw the Lewis structure of nitrite (NO₂⁻) and then determine the hybridization of the central atom. Click to edit molecule A) sp³d B) sp³d² C) sp D) sp⁵ E) sp²

E) sp²

Alpha particles are composed of two protons and two neutrons. What is the mass number of an alpha particle? Select one: a. It's not an element so it doesn't have a mass number b. 2 c. 1 d. 3 e. 4

E. 4

How many protons are in an atom of Co?

27

What is the wavelength (in nm) of a photon if the energy is 7.26 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)

273 nm

A thermometer reads 22.7 °C. What is the temperature in Kelvin?

296 K

What is the coefficient in front of the O₂ when the equation below is balanced (using only whole numbers and the lowest whole number ratio)? C₂H₄(g) + O₂ (g) → CO₂(g) + H₂O (g)

3

What ionic compound will form when elemental sulfur reacts with metallic sodium? Select one: a. NaS2 b. NaS c. Na3S8 d. Na2S

Na2S

A red-breasted Merganser (duck) has been observed flying at a speed of 118 ft/s. What is this speed in km/hr? Be sure to include units in your answer.

129 km/hr

If 4.1 kg of Na2CO3 are dissolved to make 3.0 L of solution, what is the concentration of CO32- ?

13 M