Chem Exam (chapter 2,3,4,5,6,7,8,9,10,11, and 12)
An imaginary element Xq consists of two isotopes having masses of 100.0 amu and 102.0 amu. A sample of Xq was found to contain 20.0% of the Xq isotope and 80.0% of the Xq. Calculate the atomic weight of Xq.
101.6 amu
What is the concentration of a phosphoric acid solution of a 25.00 mL sample of the acid requires 42.24 mL of 0.135 M NaOH for neutralization?
0.0760 M
Which has the highest boiling point?
0.1 M Al(NO3)3
What is the specific heat of a metal if it takes 26.5 calories to raise the temperature of a piece weighing 50.0 g by 5.00 Celsius degrees?
0.106 cal/g °C
How many g in 10.0 mEq of Mg2+?
0.122 g
What is the specific heat of a metal if it takes 48.4 calories to raise the temperature of a 45.0 g sample by 5.0°C?
0.215 cal/g °C
A 20.0 mL sample of CuSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution?
0.303 M
What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization?
0.422 M
How many moles of gas are present in a 10.0 liter sample at STP?
0.446 moles
How many quarts are contained in 450.0 mL?
0.475 quarts
A 250 mL sample of gas at 1.00 atm and has the temperature increased to and the volume increased to 500 mL. What is the new pressure?
0.534 atm
An imaginary element Xz consists of two isotopes having masses of 100.0 amu and 102.0 amu. A sample of Xz was found to contain 75.0% of the 100Xz isotope and 25.0% of the 102Xz. Calculate the atomic weight of Xz.
100.5 amu
The molar mass of Fe(OH)3 is ________ g.
106.87
An atom containing 47 protons, 47 electrons, and 60 neutrons has a mass number of
107
How much Ca(NO3)2 should be weighed out to have 0.650 mol?
107 g
The value for A for an atom containing 47 protons, 47 electrons, and 60 neutrons is
107.
When the prefix centi is used in the metric system, a fundamental unit of measurement is multiplied by what factor?
10^-2
When the prefix milli is used in the metric or SI system, a fundamental unit of measurement is multiplied by what factor?
10^-3
How many meters are there in one kilometer?
10^3
Which of the following pH's corresponds to a strongly basic solution?
11.5
What is the total length of two pieces of rubber tubing which are 7.69 cm and 4.028 cm in length? Express this answer to the correct number of significant figures.
11.72 cm
What is the total pressure of a mixture of He and H2 if the partial pressures are 320 mm Hg and 800 mm Hg respectively?
1120 mm Hg
What is the volume of a gold nugget that weighs 2.20 kg? The density of gold is
116 cm3
What is the volume of a gold nugget that weighs 2.20 kg? The density of gold is 19 g/cm^3
116 cm3
How many hydrogen atoms are present in the molecule shown? I----I---CH3 I----I---CH3
12
How many hydrogens are present in a molecule composed of a six membered ring of carbon atoms and no double or triple bonds?
12
How much NaOH is present in a 250 mL sample of a 5.00% (w/v) solution?
12.5 g
The half-life of nickel-65 is 2.5 days. How much of a 100-g sample remains after 7.5 days?
12.5 g
125 cL is the same as all of these except
125 cubic liter.
How many g of C6H12O6 are needed to prepare 2.5 L of a 5.00% (w/v) solution?
125 g
How many mL of 16 M NH3 are needed to prepare 2.0 L of a 2.0 M solution?
125 mL
In the reaction shown, what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C4H10? 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
13 moles O2 / 2 moles C4H10
Which of the following isotopes can be used to monitor thyroid function?
131 I
The formula weight of copper(II) chloride is ________ g.
134.45
What will be the new volume when 128 mL of gas at 20.0° C is heated to 40.0° C while pressure remains unchanged?
137 mL
The molecular weight of PCl3 is ________ amu.
137.33
Normal saline is 0.92% (w/v) NaCl in water. How many grams of NaCl are needed to prepare of normal saline?
138 g
How many grams of N2 are contained in an 11.2 liter sample at STP?
14.0
What other product is formed when one neutron interacts with uranium-235 to form bromine-87 and 3 neutrons?
146 / 57 La
What temperature is -10°C on the Fahrenheit scale?
14°F
How many mL of 0.360 M HNO3 are needed to neutralize a 22.5 mL sample of 0.240 M KOH?
15.0 mL
The pH of a solution with [H+] = 5.9 × 10-3 M, to the correct number of significant figures, is ________.
2.23
What is the molarity of a solution prepared by dissolving 3.50 mol NaCl in enough water to make of solution?
2.33 M
In the reaction 2 C + O2 → 2 CO, how many moles of carbon are needed to produce 66.0 g of carbon monoxide?
2.36
How many moles of NaHCO3 are present in a 2.00 g sample?
2.38 x 10^-2 mol
What is the IUPAC name of the compound shown? CH3-CH2-CH2-CH-CH2-CH-CH3 CH3 CH2 CH3
3,5-dimethyloctane
What is the % (w/v) concentration of a solution containing 12 grams of solute in 400 mL of solution?
3.0%
How much NaCl is present in 25.0 mL of a 12.0% (w/v) solution?
3.00 g
The pH of a cup of coffee is measured as 5.45. Express this measurement as [H+], using the correct number of significant figures.
3.5 × 10-6 M
42.0 g Cl2 contains ________ molecules Cl2 and ________ atoms of Cl.
3.57 × 10^23; 7.13 × 10^23
How much NaOH is present in a 75.0 mL sample of a 5.00% (w/v) solution?
3.75 g
The number of mm Hg in one atmosphere is ________.
760
What is the missing reactant in the reaction shown? 27 / 13 Al + ________ → 30 / 15 P + 1 / 0 n
4 / 2 He
What is the IUPAC name of the compound shown? CH3-(CH2)2-CH-(CH2)5-CH3 I CH3-CH-CH3
4-isopropyldecane
A sealed container with gas at 2.00 atm is heated from 20.0 K to 40.0 K. The new pressure is
4.00 atm.
Calculate the hydrogen ion concentration in a solution with pH = 6.35.
4.5 × 10-7 M
Consider the reaction shown: N2 + O2 → 2 NO ΔH = 43.2 kcal When 50.0 g of N2 react, ________ kcal will be ________.
77.1; consumed
How many mL of a 0.200 M HNO3 solution contains 10.0 g of HNO3?
793 mL
Which column of the periodic table contains only nonmetals?
7A
How many carbon atoms are there in the longest continuous chain of the molecule shown?
8
How many electrons can occupy the shell having n = 2?
8
How much NaCl is needed to make 50.0 mL of a 16% (w/v) solution?
8.0 g
The number of grams in 0.350 mol of Na is ________.
8.05
What is the hydrogen ion concentration in a solution with pH = 2.34?
4.57 × 10-3 M
In scientific notation, the number 0.0046 is expressed as 4.6 × 10-1.
4.6 × 10-3.
How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H2SO4?
80.00 mL
Calculate the volume of 5.00 mol of helium at 120°C and 1520 mm Hg.
80.7 liters
The mass number of Br-81 is
81
S + O2 → SO2 ΔH = -70.8 kcal Based on the reaction shown, which statement is true?
70.8 kcal are produced when 32.1 g of sulfur reacts.
Which product is formed by beta emission from arsenic-75? The atomic number of arsenic is 33.
75 / 34 Se
How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of CH3CO2H, a monoprotic acid?
75.00 mL
All of the water in a 0.200 M solution of NaCl was evaporated and 0.150 mole of NaCl was obtained. What was the original volume of the sample?
750. mL
Which compound has a very large value of Ka in aqueous solution?
HNO3
Which of the following is a strong acid?
HNO3
All of the reactions shown are oxidation-reduction reactions except
K2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 KCl(aq).
Which of the following compounds is a salt?
KNO3
Which group contains only noble gases?
Kr, Xe, Rn
What is the formula for the ionic compound formed between lithium and bromide?
LiBr
What is the formula of a compound formed by the ions M+ and X3-?
M3X
Which of the following elements is most likely to form an ion with a +2 charge?
Mg
Which is the correct equation for the reaction of magnesium with hydrochloric acid to produce hydrogen and magnesium chloride?
Mg + 2 HCl → H2 + MgCl2
Which of the following formulas represents a compound that is a base?
Mg(OH)2
Which substance produces carbon dioxide and water upon reaction with an acid?
MgCO3
What is the formula of the ammonium ion?
NH4+
Which of the following cannot act as a Bronsted base?
NH4+
Which compound produces an acidic solution when dissolved in water?
NH4Cl
Which of the following compounds is a salt?
NH4NO3
The formula for ammonium hydroxide is ________.
NH4OH
What is the formula of the nitrate ion?
NOv3-
Which of the following is an alkali metal?
Na
Which nuclear reaction is an example of positron emission?
Na → Ne + β
Which of the following is always a spectator ion in a chemical reaction?
Na+
Which compound produces a basic solution when dissolved in water?
NaF
Which is the best description of a beta particle?
charge -1; mass of 0 amu; medium penetrating power
Which is the best description of gamma radiation?
charge 0; mass of 0 amu; high penetrating power
The name of Cl- is
chloride ion.
Which element listed is the most electronegative?
chlorine
The element with the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^5 is
chlorine.
A buffer solution
closely maintains its original pH.
In gas chromatography, the concentration of a substance can be determined by ...
comparison of the area under the peak produced by the substance with the areas under the peaks produced by standard solutions.
The various shapes taken on by an organic molecule are known as ________
conformations
The net ionic equation for the reaction of formic acid, a weak acid,with potassium hydroxide, a strong base, is
HCO2H (aq) + OH- (aq) → HCO2- (aq) + H2O (l)
CH3NH2 + HCl CH3NH3+ + Cl- A conjugate acid-base pair in the reaction shown is ________ and ________.
HCl and Cl-
Two or more compounds with the same molecular formula but with the atoms connected differently are referred to as
constitutional isomers.
The name of Cu2+ is ________ ion or ________ ion.
copper(II); cupric
A process which is unfavorable with respect to enthalpy, but favorable with respect to entropy
could occur at high temperatures, but not at lower temperatures.
A reaction which is unfavorable with respect to entropy, but favorable with respect to enthalpy
could occur at low temperatures but not at higher temperatures.
A chemical bond formed between two identical atoms is a(an) ________ bond.
covalent
The base forms a new ________ bond in a Bronsted-Lowry acid-base reaction.
covalent
The amount of a radioactive substance that undergoes 3.7 × 1010 disintegrations per second is known as a
curie.
Which process is not likely to be considered reversible?
cutting down a tree
When a radioactive isotope decays into a nucleus which is also unstable and undergoes decay, and this process is repeated several times, the succession of reactions is called a
decay series.
The solubility of gases in liquids
decreases as temperature increases and increases as pressure increases
A chemical bond formed when two atoms share four electrons is a ________ bond; it is best described as ________.
double; covalent
A chemical bond formed when two atoms share two pairs of electrons is a ________ bond; it is best described as ________.
double; covalent
Transition metals can also be called
d-block elements.
Another name for atomic mass unit (amu) is the
dalton.
All of the following are properties typical of ionic compounds except
form distinct molecules by interaction of specific particles.
The abbreviation for the metric unit used to measure mass is
g
Main group elements that are non-metals usually ________ one or more electrons to form ________, which have a ________ charge.
gain; anions; negative
Which transformation is condensation?
gas → liquid
A student weighed a solid sample. The units for this measurement are most likely to be recorded as
grams.
In an aqueous solution that is acidic, [H3O+] is ________ than 1.0 x 10-7 and ________ than
greater; greater
In comparing gases with liquids, gases have ________ compressibility and ________ density.
greater; smaller
A formula unit of the ionic compound copper(II) carbonate consists of ________ copper(II) ions and ________ carbonate ions.
one, one
The formula Ca(NO3)2 tells us that one formula unit of this compound is composed of ________ calcium atoms, ________ nitrogen atoms, and ________ oxygen atoms.
one; two; six
Acetic acid is a weak acid in water because it is
only slightly dissociated into ions.
The passage of a solvent across a semipermeable membrane because of concentration differences is called
osmosis.
When a substance loses electrons it is ________; the substance itself is acting as a(an) ________ agent.
oxidized, reducing
The element chlorine is very reactive as a(an) ________ agent because it readily ________ electrons to form the chloride ion.
oxidizing, gains
Which element is most likely to be "X" in the diatomic molecule shown? .. .. :X=X:
oxygen
For the structure shown, the most likely elements are X = ________ and Y = ________. .. .. x=y=x .. ..
oxygen; carbon
To prepare a buffer using sodium phosphate, which of the following would also be needed?
phosphoric acid
A molecule in which the central atom forms one double bond and two single bonds is said to have a ________ shape.
planar triangular
Consider the molecule SiCl4. The electronegativity values for Si and Cl are 1.8 and 3.0, respectively. Based on these values and on consideration of molecular geometry, the Si-Cl bond is ________ and the molecule is ________.
polar; non-polar
The carbon dioxide molecule is linear. The electronegativities of C and O are 2.5 and 3.5, respectively. Based on these values and on consideration of molecular geometry, the is ________ and the molecule is ________.
polar; non-polar
Protons possess a ________ charge, and electrons possess a ________ charge.
positive, negative
Protons possess a ________ charge, and neutrons possess a ________ charge.
positive, zero
In the process of dissolving sugar in water, the entropy increases. This means that the sign of ΔS is ________, and that the randomness of the system ________.
positive; increases
2 AgNO3(aq) + K2SO4(aq) → 2 KNO3(aq) + Ag2SO4(s)The spectator ions in the reaction shown are
potassium ion and nitrate ion.
What is the name of K2S?
potassium sulfide
The reaction 2 AgNO3(aq) + K2SO4(aq) → 2 KNO3(aq) + Ag2SO4(s) is an example of a(an) ________ reaction.
precipitation
A reaction that is spontaneous can be described as
proceeding without external influence once it has begun.
The name of the hydrocarbon with three carbon atoms and having only single bonds between carbon atoms is
propane.
According to Bronsted-Lowry theory, acid-base reactions can be described as ________ reactions.
proton transfer
In a neutral atom the number of ________ is equal to the number of ________.
protons, electrons
A molecule in which the central atom forms three single bonds and has one lone pair is said to have a ________ shape.
pyramidal
The carbon atom marked with * is a ________ carbon atom. C C C-C*-C-C-C-C C
quaternary
A unit used to measure the amount of radiation absorbed per gram of tissue is the
rad.
At a high altitude water boils at 95°C instead of 100°C as at sea level because
the atmospheric pressure is less.
Activation energy can best be described as
the difference in energy between reactants and the maximum energy.
In a covalent compound the bond length can be defined as
the distance between two nuclei when repulsion and attraction are balanced.
The number of valence electrons in a main group element is given by ________.
the elements group number
The dissolving process is exothermic when
the energy released in solvation exceeds the energy used in breaking up solute-solute and solvent-solvent interactions.
A characteristic feature of any form of chromatography is the
use of a mobile and a stationary phase.
Which example is not basic?
vinegar
Which list includes all the pieces of lab equipment needed to prepare 0.100 M H3PO4 from a 5.00 M solution of H3PO4?
volumetric pipet and bulb; volumetric flask
Consider the following four liquids: 1.water: highly polar; H-bonding 2.hexanol: slightly polar; some H-bonding 3.chloroform: slightly polar; no H-bonding 4.octane: non-polar; no H-bonding Which pair of liquids is immiscible?
water and octane
All of the statements regarding redox reactions are true except
when a substance is oxidized its charge (or oxidation number) decreases.
Thin layer chromatography can be used to distinguish between different amino acids. If a particular amino acid has low solubility in the mobile phase used, then the amino acid ...
will have a low Rf value.
Although noble gases do not normally form covalent compounds, XeO3 has been prepared. The systematic name of this compound is
xenon trioxide.
Which choice best describes the degree of uncertainty in the measurement 16.30 g?
±0.01 g
Which type of radiation is attracted toward a negative plate?
α
Which type of radiation is attracted toward a positive plate?
β
Which form of radiation is generally considered the most dangerous?
γ
Magnesium is an example of a(an)
alkaline earth.
Which family of organic compounds does not contain any multiple bonds?
alkyl halides
All of the families below include functional groups which contain oxygen except
alkyl halides.
Which of the following cannot serve as the solvent in a solution?
all of the above
Reduction is the process of ________
all of the above.
Which of the properties of radioisotopes make them useful as tracers in medical or agricultural applications? i.Their chemical behavior is the same as nonradioactive isotopes. ii.They emit various types of radiation. iii.The nuclear reaction is unaffected by the chemical state of the isotope.
all of these
What is the name of AlCl3?
aluminum chloride
The functional group illustrated below is an O=C-NH2-R
amide.
Which functional group does not contain oxygen?
amine
A solid compound which has no definite crystalline structure and a poorly defined melting point is referred to as a(an) ________ solid.
amorphous
The percentage yield of a reaction can best be described as the ________ times 100%.
amount of product obtained divided by the maximum possible amount of product
Water and HSO4- can either accept protons or donate protons. Such substances are said to be
amphoteric.
A small negatively charged particle formed when an atom gains one or more electrons is called a(an)
anion.
Which characteristics correctly describe a proton?
approximate mass 1 amu; charge +1; inside nucleus
Which characteristics correctly describe a neutron?
approximate mass 1 amu; charge 0; inside nucleus
Which characteristics correctly describe an electron?
approximate mass 5 × 10-4 amu; charge -1; outside nucleus
Which family of organic molecules is a hydrocarbon?
aromatic
The number of components in a solution is ________
at least 2.
The smallest amount of an element that retains that element's characteristics is the
atom.
Elements in the Periodic Table are arranged according to
atomic number.
The smallest possible unit of a covalent compound is a(an)
molecule.
Which of the following measurements has three significant figures?
0.0250 g
What is the molarity of a solution prepared by dissolving 1.25 mol of AgNO3 in enough water to make of solution?
2.00 M
The number of valence electrons in the acetic acid molecule (CH3CO2H) is ________.
24
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns^2 np^1?
3+
The shell having n = 3 contains ________ subshells, ________ orbitals, and up to ________ electrons.
3, 9, 18
What is the IUPAC name of the compound shown? CH3 I CH3-CH2-C-CH3 I CH2Ch2CH3
3,3-dimethylhexane
How many neutrons will be produced in the reaction shown? Cm + C → No + ________ n
4
What is the final concentration of a solution prepared by adding water to 50.0 mL of 1.5 M to make 1.00 L of solution?
0.075 M
Which solution will have the highest boiling point?
0.075 M CaCl2
If gasoline sells for 95.4 cents per liter, what is its cost on a per gallon basis?1 L = 1.06 q
$3.60
All of the choices listed are representations of the same molecule except
(CH3)2CHCH2CH3.
The balanced equation for the reaction between aqueous ammonium sulfate and aqueous barium acetate is
(NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) → BaSO4 (s) + 2 NH4C2H3O2 (aq).
In a precipitation reaction the insoluble product can be identified by the symbol ________.
(s)
The oxidation number of iron in the compound FeBr3 is ________.
+3
The oxidation number of sulfur in calcium sulfate, CaSO4, is ________.
+6
The oxidation number of chlorine in the compound FeCl3 is ________.
-1
When the volume of a gas is plotted against the Celsius temperature while holding pressure and the number of moles constant, the x-intercept will occur at what temperature?
-273°C
What temperature do the celsius and fahrenheit scales read the same?
-40
Which description best fits a gas? -Volume and shape of container; no intermolecular attractions -Definite shape and volume; strong intermolecular attractions -Volume and shape of container; strong intermolecular attractions -Definite volume; shape of container; weak intermolecular attractions -Definite volume; shape of container; moderate intermolecular attractions
-Volume and shape of container; no intermolecular attractions
The process of sublimation is ________ and involves a(an) ________ in entropy. -endothermic; increase -endothermic; decrease -exothermic; decrease -exothermic; increase -endothermic; no change
-endothermic; increase
Which process is exothermic? -gas → liquid -none of the above -solid → gas -liquid → gas -solid → liquid
-gas → liquid
In comparing liquids and gases, liquids have ________ compressibility and ________ density. -greater; smaller -smaller; greater -smaller; smaller -none of the above -greater, greater
-smaller; greater
Which representation of a methane molecule is not correct? (A methane molecule is composed of one carbon atom and four hydrogen atoms.)
.. :H: .. I .. :H- C - H: '' I '' :H: ''
The carbon skeleton of an alkane is shown below. How many hydrogen atoms are bonded to the carbon marked with a *? C C C-C*-C-C-C-C C
0
As a pure element the oxidation number of zinc is ________, but in compounds such as ZnCO3 its oxidation number is ________.
0, +2
What is 2.1 × 10-5 written in decimal notation?
0.000021
Which of the following numbers contains four significant figures?
0.002301
How many moles of HCl are present in 35.5 mL of a 0.200 M solution?
0.00710 mol
A sample of CO2 gas at 100°C has a volume of 250 mL at 760 mm Hg. How many moles of CO2 are present?
0.00816 mol
A student weighed 0.550 g of lithium chloride, LiCl, to use in a reaction. How many moles is this?
0.0130
How many moles of HCl are present in 75.0 mL of a 0.200 M solution?
0.0150 mol
Which solution will have the lowest boiling point?
0.025 M NH4NO3
What is the molarity of a solution prepared by dissolving 36.0 g of NaOH in enough water to make 1.50 L of solution?
0.600 M
What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by of 0.105 M H3PO4?
0.609 M
What is the molarity of a solution prepared by dissolving 1.25 mol AgNO3 in enough water to make 2.00 × 103 mL of solution?
0.625 M
What is the molarity of a solution prepared by dissolving 10.0 g of acetone, C3H6O, in enough water to make 250. mL of solution?
0.689 M
50.0 g of Cl2 contains ________ mol Cl2.
0.705
What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?
0.75 M
Calculate the density of cyclohexane if a 50.0 g sample has a volume of 64.3 mL.
0.778 g/mL
What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make of solution?
0.800 M
The carbon skeleton of an alkane is shown below. How many hydrogen atoms are bonded to the carbon marked with a *? C C C-C-C-C-C-C
1
The conversion factor used to convert 198 cm to inches is
1 in/2.54cm
Which value is closest to the mass of a 2-pound box of laundry detergent?
1 kg
In the balanced reaction shown, the mole ratio of Fe2S3 to O2 is Fe2S3 + 4 O2 → 2 FeO + 3 SO2
1 to 4.
If the [H+] of a water sample is 1 × 10-4 M, the [OH-] is
1 × 10-10 M.
If the concentration of OH- is 1 × 10-2 M, the concentration of H3O+ is ________ M.
1 × 10-12
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns1?
1+
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns^1?
1+
When the reaction shown is correctly balanced, the coefficients are HNO3 + KOH → KNO3 + H2O
1, 1, 1, 1
What is the IUPAC name of the molecule shown?
1,1-dimethylcyclobutane
What is the IUPAC name of the molecule shown? I-----I-CH3 I-----I-CH3
1,2-dimethylcyclobutane
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns^2 np^5?
1-
How many grams of FeSO4 are present in a 20 mL sample of a 0.500 M solution?
1.52 g
At 25°C, the value of Kw is ________.
1.00 × 10-14
105 g of MgCl2 contains ________ mol MgCl2.
1.10
What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?
1.2 M
What is the numerical value of 1.50/1.222 x 10^3? Express your answer using the correct number of significant figures.
1.23 × 10-3
What is the numerical value of ? Express your answer using the correct number of significant figures.
1.23 × 10-3
What is the numerical value of 1.00x10^5/8.00 ?
1.25 × 10^4
If the concentration of H3O+ in an aqueous solution is 7.6 × 10-9 M, the concentration of OH- is ________.
1.3 × 10-6 M
What is the molarity of a solution prepared by dissolving 10.0 g of acetone, in enough water to make 125 mL of solution?
1.38 M
What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?
1.39
What is the numerical value of 1.2 × 1.222? Express your answer using the correct number of significant figures.
1.5
Which sample contains the largest number of ions?
1.5 mol SnCl2
What is the value of [H3O+] in a solution with pH = 10.82?
1.5 × 10-11 M
Determine the number of moles of water produced when one mole of NH3 reacts according to the balanced reaction shown. 4 NH3 + 5 O2 → 4 NO + 6 H2O
1.50
A 50.0 mL sample of a 6.0 M solution of HCl is diluted to 200 mL. What is the new concentration?
1.50 M
What is the molarity of a solution prepared by dissolving 0.750 mol CaCl2 in enough water to make 0.500 L of solution?
1.50 M
What is the numerical value of (8.0 × 10^3)(2.0 × 10^2)?
1.6 × 10^6
If the temperature of a 1.75 liter sample of gas is changed from 30.0° C to 20.0° C at constant pressure, what will be the new volume?
1.69 L
105 g of NaCl contains ________ moles?
1.76
How much NaCl is present in a 15.0 mL sample of a 12.0% (w/v) solution?
1.80 g
How many molecules are there in 3.00 moles of NH3?
1.81 × 10^24
In scientific notation, the number 185,000,000 is
1.85 × 10^8.
How many molecules are present in 3.25 mol of C2H6O?
1.96 × 10^24
How many electrons can occupy the 4d subshell?
10
What is the maximum number of electrons that can occupy the 4d orbitals?
10
Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?
10 mL of alcohol is mixed with enough water to make 250 mL of solution.
A student sets up a paper chromatogram and places a spot of green food dye on the origin. After six minutes the solvent has moved 12 cm and a blue spot has advanced 9 cm. After fourteen minutes the solvent has advanced a further 8 cm. How many cm from the origin is the blue spot likely to be?
15cm
How many grams of O2 are contained in a 25.0 L sample at 5.2 atm and 28.0°C?
168 g
Atoms of Cl contain ________ protons and ________ electrons.
17, 17
Atoms of 35/17 Cl contain ________ protons and ________ neutrons.
17, 18
Atoms of 35/17 Cl contain ________ protons and ________ electrons.
17,18
The electron capacity of the third shell is ________.
18
The value of Z for the element 37^Ar is
18
Which product is formed by alpha emission from gold-185? The atomic number of gold is 79.
181 / 77 Ir
Consider the reaction shown: P4 (s) + 10 Cl2 (g) → 4 PCl5 (s) + 452 kcal When 50.00 g of P4 react, ________ kcal will be ________.
182.4; produced
How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v) solution?
19 g
How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of KOH?
19.8 mL
What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change in temperature?
190 mm Hg
Which sample contains the largest number of atoms?
2.0 mol CH4
The number of grams in 7.00 moles of N2 is ________.
196
The correct order for filling orbitals with electrons is ________.
1s2s2p3s3p4s3d
Which of the following electron configurations is most stable?
1s^2 2s^2 2p^6
What is the electron configuration of Mg?
1s^2 2s^2 2p^6 3s^2
The electron configuration for phosphorus is
1s^2 2s^2 2p^6 3s^2 3p^3.
What is the electron configuration of S?
1s^2 2s^2 2p^6 3s^2 3p^4
What is the electron configuration of Fe?
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6
How many electrons can occupy the 4s subshell?
2
How many structural isomers are possible for the molecular formula, C4H10?
2
The maximum number of electrons in any orbital is ________.
2
Which reaction is not an example of a redox reaction?
2 (NH4)3PO4 (aq) + 3 Ba(NO3)2 (aq) → Ba3(PO4)2 (s) + 6 NH4NO3 (aq)
Which equation correctly represents the neutralization of aluminum hydroxide by sulfuric acid?
2 Al(OH)3 + 3 H2SO4 → Al2(SO4)3 + 6 H2O
The balanced equation for the reaction occurring when iron(III) oxide, a solid, is reduced with pure carbon to produce carbon dioxide and molten iron is
2 Fe2O3 + 3 C (s) → 4 Fe (l) + 3 CO2 (g).
Consider the balanced equation shown, and identify the statement that Na2SO4 (aq) + BaCl2 (aq) → 2 NaCl (aq) + BaSO4 (s)
2 NaCl (aq) could also be correctly written as Na2Cl2 (aq).
Consider the balanced equation shown, and identify the statement that Na2SO4 (aq) + BaCl2 (aq) → 2 NaCl (aq) + BaSO4 (s)
2 NaCl (aq) could also be correctly written as Na2Cl2 (aq).
When the reaction shown is correctly balanced, the coefficients are HBr + Ca(OH)2 → CaBr2 + H2O
2, 1, 1, 2
When the reaction shown is correctly balanced, the coefficients are Li + Br2 → LiBr
2, 1, 2
When the reaction shown is correctly balanced, the coefficients are C6H14 (l) + O2 (g) → CO2 (g) + H2O (g)
2, 19, 12, 14
When the reaction shown is correctly balanced, the coefficients areKClO3 → KCl + O2
2, 2, 3
The shell having n = 2 contains ________ subshells, ________ orbitals, and up to ________ electrons.
2, 4, 8
What is the IUPAC name of the compound shown? CH3 CH3-CH2-C-CH3 CH3
2,2-dimethylbutane
What is the IUPAC name of the compound shown? (CH3)3—C—CH2—CH2—CH3
2,2-dimethylpentane
What is the IUPAC name of the compound shown? CH3-CH-CH-Ch2-CH-CH3 Ch2 CH3 CH3 CH3
2,4,5-trimethylheptane
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns2np4?
2-
What is the most likely charge on an ion formed by an element with a valence electron configuration of ns^2 np^4?
2-
A 50.0 mL sample of a 12.0 M solution of HCl is diluted to 250. mL. What is the new concentration?
2.40 M
How many g of Fe(NO3)3 are present in a 20.0 mL sample of a 0.500 M solution?
2.42 g
What is the [H3O+] in a solution with pH = 11.61?
2.45 × 10-12 M
Which sample contains the smallest number of atoms?
2.5 mol Au
What is the concentration of an acetic acid solution if a 10.0 mL sample required 26.4 mL of KOH for neutralization?
2.51 M
The conversion factor used to convert 15.0 inches to cm is
2.54 cm/1 in
This question was deleted.
2.54 cm/1 in
If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH- is ________ M.
2.9 × 10-12
What is the pH of a solution in which [H3O+] = 1.2 × 10-3 M?
2.92
How many g of CaCl2 are needed to prepare 500. mL of a 0.375 M solution?
20.8 g
How many grams of CaCl2 are needed to prepare 125 mL of a 1.50 M solution?
20.8 g
Which product is formed by alpha emission from polonium-208? The atomic number of polonium is 84.
204 / 82 Pb
Which measurement represents the largest value of pressure?
22.0 psi
Which product is formed by alpha emission from uranium-235? The atomic number of uranium is 92.
231 / 90 Th
Which nuclear reaction is an example of alpha emission?
235 / 92 U → 4 / 2 He + 231 / 90 Th
How many grams of water are needed to prepare 250 g of a solution that is 5.00% by mass NaCl?
238 g
How many neutrons does an atom of 46/22 Ti have?
24
Which nuclear reaction is an example of alpha emission?
242 / 96 Cm → 238 / 94 Pu + 4 / 2 He
Which reaction is an example of an alpha emission?
242 / 96 Cm → 238 / 94 Pu + 4 / 2 He
An atom with a mass number of 58 and with 32 neutrons will have ________ protons.
26
An atom with Z = 26 and A = 58 contains ________ protons, ________ electrons, and ________ neutrons.
26; 26; 32
An atom with Z = 26 and A = 58 contains ________ protons and ________ neutrons.
26; 32
Consider the reaction shown: 304.0 kcal + 4 PCl3 (l) → P4 (s) + 6 Cl2 (g) When 50.00 g of PCl3 react, ________ kcal will be ________.
27.67; consumed
How many mL of 14.5 M NH3 are needed to prepare 2.0 L of a 1.0 M solution?
276 mL
The atomic number of an atom containing 29 protons, 29 electrons, and 34 neutrons is
29.
The value of Z for an atom containing 29 protons, 29 electrons, and 34 neutrons, is
29.
Which measurement represents the smallest quantity?
2950 ng
What temperature is 75°F on the Kelvin scale?
297 K
The main group element E reacts with chlorine to form an ionic compound with the formula ECl2. The element E is a member of what group in the Periodic Table?
2A
Monochlorination of Pentane, C5 H12 , leads to formation of how many different products?
3
The carbon skeleton of an alkane is shown below. How many hydrogen atoms are bonded to the carbon marked with a *?
3
The volume of a gas sample is recorded as 0.0970 L. How many significant figures is this?
3
What is the minimum number of carbons that must be present in a molecule to have a secondary carbon?
3
The balanced equation for the reaction occurring when calcium nitrate solution is mixed with sodium phosphate solution is
3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) → Ca3(PO4)2 (s) + 6 NaNO3 (aq).
In the reaction shown, what is the mole ratio that would be used to determine the number of moles of H2 that would be produced when 3.5 moles of AlCl3 are produced? 2 Al + 6 HCl → 2 AlCl3 + 3 H2
3 moles H2 / 2 moles AlCl3
Calculate the concentration in ppm of a pollutant that has been measured at 450 mg per 150 kg of sample.
3 ppm
Which solution is the least concentrated? Each choice refers to the same solute and solvent.
30 g solute in 150 mL solution
How many moles of solute are present in 5.00 L of 6.00 M HCl?
30.0 mol
How many centimeters are contained in 12.5 inches?
31.8 cm
An atom with Z = 31 and A = 69 contains ________ protons and ________ neutrons.
31; 38
For the isotope 71Ga, Z = ________ and A = ________.
31; 71
For the isotope 71^Ga, Z = ________ and A = ________.
31; 71
How many electrons can occupy the shell having n = 4?
32
Which product is formed by beta emission from phosphorus-32? The atomic number of phosphorus is 15.
32 / 16 S
An isotope with 15 protons and 17 neutrons will have which symbol?
32/15 P
In an introductory laboratory exercise, a student was asked to measure the volume of soda in a partially filled can in metric units. Which value below is most likely to be correct?
325 mL
For the following reaction, if 11.2 L of Nitrogen are reacted to form NH3 at STP, How many liters of Hydrogen will be required to completely consume all of the nitrogen.N2 + 3H2 ——→ 2NH3
33.6 L
The formula weight of Al2(SO4)3 is ________ grams.
342.14
Consider the isotope 79/35 Br. The atomic number is ________, and the mass number is
35, 79
Consider the isotope 79/35 Br. The atomic number is ________, and the mass number is ________.
35, 79
95.0°F is the same as
35°C.
How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl?
36.0 mL
How many moles of solute are present in 12.0 L of 3.00 M HCl?
36.0 mol
A sample of an experimental medication was calculated to contain 0.392 g of active drug. How many milligrams is this?
392 mg
In straight-chain alkanes, the carbon atoms on each end of the molecule always form bonds with ________ atoms of hydrogen; the carbons within the molecule always form bonds with ________ hydrogen atoms.
3; 2
An analysis showed a sample to contain 0.00471 grams of lead. How many micrograms is this?
4.71 × 10^3 μg
Which of the following numbers contains five significant figures?
4.9100
How many mL of a 5.00% (w/v) glucose solution are needed to provide 20.0 g of glucose?
400 mL
A mixture of the gases N2, O2, and He has a total pressure of 760 mm Hg. If the partial pressure of N2 is 90 mm Hg and of O2 is 270 mm Hg, What is the partial pressure of He?
400 mm Hg
A sample of gas has a volume of 135 mL at 0.600 atm. What would be the volume if the pressure is decreased to 0.200 atm while temperature is held constant?
405 mL
If 75.0 g of water at 30.0°C absorbs 900 calories, the new temperature will be
42.0°C.
If a 0.614 g sample of a gas maintains a pressure of 238 mm Hg when contained in a 1.0L flask at 0.0 C, what is the gases molecular weight?
44 g/mol
The atomic number of an atom containing 47 protons, 47 electrons, and 60 neutrons is
47
The value for Z for an atom containing 47 protons, 47 electrons, and 60 neutrons is
47.
Which measurement represents the largest quantity?
47.3 mg
What is the mass of 30.0 mL of a solution with a density of 1.60 g/mL?
48.0 g
How many mL of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of
48.6 mL
If the [H+] of a water sample is 1 × 10-4 M, the pH of the sample is ________, and the sample is ________.
4; acidic
Which of the following subshells consists of five orbitals?
4d
Which of the following subshells consists of three orbitals?
4p
Which of the following pH's corresponds to a weakly acidic solution?
5.3
What volume will be occupied by 8.00 g of oxygen, O2, at STP?
5.60 L
Which value is closest to the amount of gasoline in a small car with a full tank (which contains about 13 gallons)?
50 L
The measurement most likely to describe the amount of pain reliever in a headache tablet is
500 mg.
In a gas mixture of 35% He and 65% O2 the total pressure is 800 mm Hg. What is the partial pressure of O2?
520 mm Hg
A sample of helium has a volume of 480 mL at 47.0°C and 740 mm Hg. The temperature is lowered to 22.0°C and the pressure to 625 mm Hg. What is the new volume?
524 mL
What temperature is 325 K on the Celsius scale?
52°C
How many grams are contained in 1.20 pounds?
545 g
How many carbon atoms are there in the longest continuous chain of the molecule shown? (CH3)3C—(CH2)3—CH3
6
How many electrons can occupy the 4p subshell?
6
The number of valence electrons in an element with electron configuration 1s^2 2s^2 2p^6 3s^2 3p^4 is ________.
6
What is the maximum number of electrons that can occupy the 4p orbitals?
6
The half-life of sodium-24 is 15.0 hours. What percentage of a sample of sodium-24 remains after 60.0 hours?
6.25%
What is the % (w/v) concentration of a solution containing 25.0 g of solute in 400. mL of solution?
6.25%
What percentage of a radioactive sample remains after four half-lives have passed?
6.25%
The solubility of nitrogen in water exposed to the atmosphere, where the partial pressure of nitrogen is 593 mm, is 5.3 × 10-4 M. At the same temperature, what would be the solubility of pure nitrogen, at a pressure of 760 mm?
6.8 × 10-4 M
What is the pressure in a 1.00 liter container of methane, CH4, that contains 40.0 g of the gas at
61.0 atm
An atom containing 29 protons, 29 electrons, and 34 neutrons has a mass number of
63.
The value of A for an atom containing 29 protons, 29 electrons, and 34 neutrons is
63.
Which group in the Periodic Table is most likely to contain the element X in the molecule whose dot structure is shown? .. .. :X=X:
6A
Which of the following pH's corresponds to a neutral solution?
7.0
If the concentration of OH- in an aqueous solution is 1.4 × 10-7 M, the concentration of H3O+ is ________.
7.1 × 10-8 M
In the reaction shown, how many moles of HCl are needed to react with 2.4 moles of Al? 2 Al + 6 HCl → 2 AlCl3 + 3 H2
7.2
What is the pH of a solution in which the hydrogen ion concentration is
7.29
What is the pH of a solution in which [H3O+] = 3.8 × 10-8 M?
7.42
What is the total length of two pieces of tubing which measure 4.5 cm and 3.222 cm? Express the answer to the correct number of significant figures.
7.7 cm
An extra-strength aspirin contains 0.500 g of aspirin. How many grains is this?
7.72 grains
A 2.36 cm3 sample of an unknown metal weighs 18.5 g. What is the sample's density?
7.84 g/cm3
S + O2 → SO2 + 70.8 kcal Based on the reaction shown, which statement is true?
70.8 kcal are produced when 32.1 g of sulfur reacts.
Which product is formed by beta decay of krypton-87? The atomic number of krypton is 36.
87 / 37 Rb
The half-life of nickel-65 is 2.5 days. How much of a 100-g sample has decayed after 7.5 days?
87.5 g
When the reaction shown is balanced, there are ________ atoms of oxygen and ________ atoms of hydrogen on each side. (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) → BaSO4 (s) + NH4C2H3O2 (aq)
8; 14
Which column of the periodic table contains only nonmetals?
8A
How much NaCl is needed to make 75 mL of a 12% (w/v) solution?
9.0 g
The pH of a 250. mL sample of a buffer solution is 9.85. If 1.0 mL of 6 M HCl is added, the pH of the resulting mixture is closest to
9.70
What is 0.0970 written in scientific notation?
9.70 × 10-2
Which product is formed by gamma emission from niobium-94? The atomic number of niobium is 41.
94 / 41 Nb
Calculate the volume of a 3.50 mol sample of carbon dioxide at 30.0° C and 0.90 atm.
96.7 L
Which product is formed by gamma emission from technetium-99? The atomic number of technetium is 43.
99 / 43 Tc
Which of the following isotopes can be used to monitor spleen function?
99Tc
The balanced equation given below means? CH4 + 2O2 → CO2 + 2H2O
A and C are correct
Which of the following statements about paper and gas chromatography is correct?
A long retention time in gas chromatography is indicative of a substance with a strong adsorption on to the stationary phase.
Which statement concerning the mole is not correct?
A mole of any compound contains one mole of each kind of atom found in that compound.
An atom that contains 47 protons, 47 electrons, and 60 neutrons is an isotope of
Ag.
Which element is not a semimetal?
Al
Which element will for an ion with the greatest positive charge?
Al
Which is a correct statement of Gay-Lussac's Law describing the behavior of a fixed amount of gas?
As temperature increases, pressure increases at constant volume.
What fourth period element is represented by the dot structure shown? .. :x: '
Br
Which formula is least likely to represent a molecular compound that really exists?
Br3Cl5
Which list includes all the elements that would be found in an alkane with an amine group?
C, H, N
Which group of elements contains only non-metals?
C, S, I
C5H5N + H2CO3 C5H6N+ + HCO3-In the reaction shown, the conjugate acid of C5H5N is ________.
C5H6N+
Which of the following equations is not balanced?
C7H16 + O2 → 7 CO2 + 8 H2O
All of the following are representations of the same molecule except ________.
CH2CH2CH2CH2
Which molecule is an isomer of the molecule shown?
CH3 CH3 CH2 CH2 CH2 CHCH3
The condensed structure of 2,2,4,4-tetramethyl-heptane is
CH3 CH3 CH3 CHCH2 CHCH2 CH2 CH3 CH3 CH3
The condensed structure of 2,4-dimethyl-octane is
CH3 CHCH2 CHCH2 CH2 CH2 CH3 CH3 CH3
The condensed structure of 2,4-dimethyl-heptane is
CH3 CHCH2 CHCH2 CH2 CH3 CH3 CH3
The condensed structure of 2,4-dimethyl-hexane is
CH3 CHCH2 CHCH2 CH3 CH3 CH3
Which compound has a value of Ka that is close to 10-5?
CH3CH2CO2H
The condensed structure of n-octane is
CH3CH3CH2CH3CH2CH2CH2CH3
When hydrocarbons undergo complete combustion, the product(s) is(are)
CO2 and H2O.
What is the formula of the carbonate ion?
CO3^2-
The formula for carbon disulfide is ________.
CS2
What fourth period element is represented by the dot structure shown? X:
Ca
What is the formula for the ionic compound formed between calcium and sulfur?
CaS
Which group contains only f-block elements?
Ce, Pr, Nd
Which of the following elements is most likely to form an ion with a -1 charge?
Cl
The formula for the compound chromium(II) nitrate is ________.
Cr(NO3)2
In the reaction shown, ________ is the oxidizing agent because it ________.Ni (s) + CuCl2 (aq) → Cu (s) + NiCl2 (aq)
CuCl2; gets reduced
Which description best fits a solid?
Definite shape and volume; strong intermolecular attractions
Which description best fits a liquid?
Definite volume; shape of container; moderate intermolecular attractions
Hydrogen cyanide, HCN, is a weak acid. Which equation best represents its aqueous chemistry?
HCN (aq) + H2O (l) CN- (aq) + H3O+(aq)
Consider a sample of helium and a sample of neon, both at 30.0°C and 1.5 atm. Both samples have a volume of 5.0 liters. Which statement concerning these samples is not true?
Each sample weighs the same amount.
The statement that best describes the formation of an ionic compound is:
Electrons are transferred from a metal to a non-metal, and the resulting charged particles form a crystalline network.
All of the statements concerning free energy and spontaneity are true except
Enthalpy and entropy are of equal importance in determining the spontaneity of a reaction.
All of the statements regarding equivalents of acids and bases are true except
Equivalents are the same as moles.
The element with the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 is
K.
Which elements all belong in the same group?
F, Cl, Br
Fe(s) + CuCl2(aq) → Cu(s) + FeCl2(aq)In the redox reaction shown, ________ is oxidized and becomes ________.
Fe, Fe2+
The element in the list given that is most likely to form a coordinate covalent bond is
Fe.
The combination of ions most likely to produce a precipitate is
Fe3+ and OH-.
Which reaction is an example of a precipitation reaction?
FeCl3 (aq) + KOH (aq) → Fe(OH)3 (s) + 3 KCl (aq)
Which is not a correct statement of Charles' Law?
For a gas sample at constant pressure, temperature and volume are inversely proportional.
Which assumption of Kinetic Molecular Theory is not followed when a real gas shows non-ideal behavior?
Gas molecules move at random with no attractive forces between them
Which of the assumptions of the kinetic-molecular theory best explains Dalton's law of partial pressures?
Gas molecules move at random with no attractive forces between them.
Which process is endothermic?
Gasoline spilled on the ground evaporates very quickly.
Which atom is least likely to form a polar covalent bond with carbon?
H
Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?
H+ + OH- → H2O
Which substance is not reactive with respect to alkanes?
H2
Which reaction best illustrates the behaviour of the weak base H2PO4- in aqueous solution?
H2PO4- (aq) + H2O (l) H3PO4 (aq) + OH- (aq)
What is the conjugate acid of HSO4-?
H2SO4
Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
H2SO4
Which reaction is an example of both a precipitation and a neutralization?
H2SO4 (aq) + Ba(OH)2 (aq) → BaSO4 (s) + 2 H2O (l)
Which reaction is an example of an acid-base reaction?
H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O(l)
What is the conjugate acid of water?
H3O+ (aq)
Which of the following is a triprotic acid?
H3PO4
Which of the following is a weak acid?
H3PO4
Which representation of a hydrogen molecule is not correct?
H=H
Which of the following molecules has a CCH bond angle of 180°?
HCCH
Which element is most likely to have chemical properties similar to those of bromine (atomic number 35)?
I (atomic number 53)
Which combination of characteristics is most likely to be associated with molecules having strong dipole-dipole interactions? I.polar bond II.asymmetric shape III.relatively low boiling point IV.large surface area
I and II
Which combination of characteristics is most likely to be associated with molecules having strong dipole-dipole interactions? I. polar bond II. asymmetric shape III. relatively low boiling point IV. large surface area
I and II
Which factors would decrease the rate of a reaction? I.Lowering the temperature II.Increasing the concentration of reactants III.Adding a catalyst
I only
Which factors would increase the rate of a chemical reaction? I.Increasing the temperature II.Removing products as they are formed III.Adding a catalyst
I, II, and III
Which of the following processes involve an increase in entropy? I.Mothballs vaporize in a closet. II.Blocks are assembled into a house. III.Crystals grow from a sugar solution. IV.Recyclable plastics are sorted. V.Cake mix is manufactured from five basic ingredients.
I, V
Which set of properties would identify a unknown white solid as a molecular compound? I.Contains a metal. II.Has a definite crystal structure. III.Dissolves in water, but not in organic liquids. IV.Melts at 80 degrees Celsius. V.Does not conduct electricity when melted.
II, IV, V
Which of the following statements is correct?
In an acidic solution, [H3O+] > 10-7; [OH-] < 10-7.
Which of the following is not an example of ionizing radiation?
Infrared rays
All of the statements regarding the symbol ΔG are true except
It allows us to identify an exothermic reaction.
All of the statements regarding the symbol "ΔH" are correct except
It can be called entropy change.
Which statement best describes the way a catalyst works?
It decreases the value of Eact.
Which physical property is most closely associated with covalent molecules?
It is a gas at room temperature.
Which property could describe a covalent compound?
It is a gas at room temperature.
How will the volume of a fixed sample of gas change if its pressure is doubled and the Kelvin temperature is doubled?
It will increase by a factor of 4.
As the temperature of a liquid is lowered, what happens to its vapor pressure?
Its vapor pressure drops.
Which pair of elements is most likely to form an ionic compound if allowed to react together?
K and Br
Which of the following elements is a noble gas?
Ne
Which nuclear reaction is an example of beta emission?
Ni → Cu + β
Which group contains only d-block elements?
Ni, Pd, Pt
The element with the electron configuration 1s^2 2s^2 2p^4 is ________.
O
Which atom is most likely to form a polar covalent bond with carbon?
O
The functional group which illustrates an ester is ________.
O R-C-O-R'
One definition of a base is a substance that produces which ion in water solution?
OH-
What is the conjugate base of water?
OH- (aq)
Which represents the largest pressure?
One atmosphere
Which statement concerning the mole concept is not true?
One mole of any compound contains one mole of atoms.
Which statement based on the mole concept is not correct?
One mole of methane, CH4, contains the same number of atoms as one mole of carbon dioxide, CO2.
Interpret in words the equation: P4O10 (s) + 6 H2O (l) → 4 H3PO4 (aq)
One mole of solid tetraphosphorus decaoxide reacts with six moles of liquid water to produce four moles of phosphoric acid solution.
Which element is most likely to form three covalent bonds?
P
The formula for phosphorus pentafluoride is ________.
PF5
Which of the following statements about chromatography is correct?
Paper chromatography is usually considered to be qualitative only, while gas chromatography can be qualitative or quantitative.
Consider the reaction: A + 2 B 2 C + D The equilibrium expression for this reaction is
[C]^2 [D] ---------- [A][B]^2
The carbon atom marked with * is a ________ carbon atom. C C* C-C-C-C-C
Primary
Which statement is correct for pure water?
Pure water contains equal amounts of hydroxide, [OH-], and hydronium, [H3O+], ions.
Which element is most likely to have chemical properties similar to those of potassium (atomic number 19)?
Rb (atomic number 37)
Which of the following elements is most likely to form an ion with a -2 charge?
S
The formula for sulfur hexabromide is ________.
SBr6
The covalent bonding model is most useful in describing which of the following compounds?
SCl2
Which of the following equations is not balanced?
SO2 + O2 → SO3
What is the conjugate base of HSO4-?
SO42-
The element which has four valence electrons is ________.
Si
Which group contains only metalloids?
Si, Ge, As
Which statement about solubility is not true?
Solubility of ionic solids increases greatly with temperature.
All of the following statements describing solutions are true except
Solutions are colorless.
Which statement is incorrect according to modern atomic theory?
Some sugars have the formula C3.5H7O3.5.
Which of the following statements is true of specific gravity?
Specific gravity is unitless because it is the density of one substance divided by the density of water
An s-block element in the 5th Period is
Sr.
Which statement regarding balanced chemical equations is not true?
Subscripts may be changed to make an equation simpler to balance.
Which of the assumptions of the kinetic-molecular theory best explains the observation that a gas can be compressed?
The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.
The family of organic compounds with functional groups that do not consist only of hydrocarbons is
aldehydes.
Which is the best description of hydrogen bonding?
The association between a hydrogen atom which is somewhat positive because it is bonded to a small electronegative atom and an atom of O, N or F on another molecule
How will the volume of a fixed sample of gas change if the pressure is doubled and its Celsius temperature is halved?
The change cannot be determined without more specific information.
All of the statements about molarity are correct except
The interpretation of the symbol is "moles of solute per mole of solvent."
Which choice best describes the degree of uncertainty in the measurement 4.0032 g?
The measurement is between 4.0031 and 4.0033 g.
All of the statements about nuclear reactions are true except
The rate of a nuclear reaction is increased by the addition of a catalyst.
In the common nomenclature of ions, ous and ic are used as endings for the ions. In this system, which species is named with the ous ending?
The species with the lower positive charge.
Which of the assumptions of the kinetic-molecular theory best explains the observation that a balloon collapses when exposed to liquid nitrogen (which is much colder than a cold winter day!!)?
The velocity of gas molecules is proportional to their Kelvin temperature.
In a chemical reaction ________
There are equal numbers of atoms on each side of the reaction arrow.
Which solution is basic?
[H3O+] = 1.0 × 10-10
Which of the following statements about alkyl groups is incorrect?
They are derived from alkenes.
Which of the following properties is not characteristic of alkanes?
They form strong hydrogen bonds.
All of the following statements are general properties of organic compounds except
They usually behave as electrolytes in solution.
Which reaction is an example of a beta emission?
Ti → V + e
Which nuclear reaction is not balanced?
U + He → Am + n
Which reaction is an example of a neutron bombardment?
U + n → Te + Zr + 2 n
Which reaction illustrates artificial transmutation by alpha bombardment?
U + n → Te + Zr + 3 n
Which reaction is an example of a chain reaction?
U + n → Te + Zr + 3 n
The symbol of the element with 23 protons is
V
If the elements W, X, Y, and Z have electronegativity values of 1.0, 2.0, 2.5, and 3.5, respectively, which bond is ionic?
WZ
Consider the reaction shown and identify the statement that CaCO3 (s) CaO (s) + CO2 (g)
Water must be present for this reaction to occur.
4 PCl3 (l) → P4 (s) + 6 Cl2 (g) ΔH = 304.0 kcal Based on the reaction shown, which statement is true?
When 1 mol P4 (s) is produced, 304.0 kcal are consumed.
P4 (s) + 10 Cl2 (g) → 4 PCl5 (s) ΔH = -435.2 kcal Based on the reaction shown, which statement is true?
When 1 mol P4 (s) reacts, 435.2 kcal are released.
Which of the statements about the behavior of the element carbon in organic molecules is incorrect?
When carbon forms four single bonds, the bond angles are 90°.
If the elements W, X, Y, and Z have electronegativity values of 1.0, 2.0, 2.5, and 3.5, respectively, which bond is the least polar?
XY
Consider the reaction: 2 CO (g) + O2 (g) 2 CO2 (g) The equilibrium expression for this reaction is
[CO2]^2 --------- [CO]^2[O2]
The functional group illustrated below is an R-C=O-H
aldehyde.
The alkyne functional group is
a carbon-carbon triple bond.
The alcohol functional group is
a carbon-oxygen-hydrogen group.
For a chemical reaction to occur, all of the following must happen except
a large enough number of collisions must occur.
A necessary requirement for a Bronsted base is
a lone pair of electrons in its Lewis dot structure.
The arene or aromatic functional group is often represented as
a six-membered ring with three double bonds.
Which example is not acidic?
a solution in which [H3O+] = 1.00 x 10-7
Which of the following solutions is a buffer?
a solution of acetic acid and sodium acetate
A rem is
a unit that that measures both the energy and the penetrating power of different types of radiation.
A rad is
a unit used to measure the amount of radiation absorbed per gram of tissue.
In a mixture of 5 mL water, 10 mL alcohol, and 50 mL acetone the solvent(s) is(are) ________.
acetone
If the half-life of vanadium-48 is 16 days, it is true that
after 16 days 50% of a sample of vanadium-48 would have decayed.
A new youth drink contains sugar, salt, alcohol and vitamin C. A gas chromatogram could be used to determine the
alcohol, sugar and vitamin C content only.
The functional group illustrated by R—OH is an
alcohol.
The functional group illustrated below is an O R-C H
aldehyde.
According to VSEPR theory, a molecule with three charge clouds including one lone pair would have a ________ shape.
bent
The water molecule has a ________ geometry because its central atom has ________ bonds and ________ lone pairs of electrons.
bent; two; two
The element least likely to obey the octet rule in forming chemical bonds is
boron.
The term nucleon refers to
both protons and neutrons.
The compound BrF3 would be called
bromine trifluoride.
Elements in Period 3 or below don't always "obey" the octet rule because they
can use s, p, and d orbitals for bonding.
A section of the Periodic Table containing representative elements is shown. Which bond would be least polar? W I X ------ Y I Z
cannot be determined without more specific information
For the dot structure shown the most likely elements are X =________ and Y = ________. .. :Y: .. I .. :Y-X-Y: '' I '' :Y: ''
carbon; fluorine
A positively charged particle formed by loss of one or more electrons from an atom is called a(an)
cation.
A positively charged particle formed by loss of one or more electrons from an atom is called a(an) anion.
cation.
Which is the best description of an alpha particle?
charge +2; mass of 4 amu; low penetrating power
A curie is
the amount of radioactive substance that undergoes 3.7 × 1010 disintegrations per second.
The property defined as the energy released on adding an electron to an isolated gas phase atom is
electron affinity.
Which list includes all the pieces of lab equipment needed to prepare a 0.500 M solution of NaCl from the pure salt and water?
electronic balance; volumetric flask
In the reaction energy diagrams shown, reaction B is ________, and it occurs ________ reaction A.
endergonic; faster than
The concept of free energy allows prediction of spontaneity of a process by considering the changes in ________ and ________ during the process.
enthalpy; entropy
The functional group illustrated by R—O—R' is an
ether.
In the reaction energy diagrams shown, reaction A is ________, and it occurs ________ reaction B.
exergonic; slower than
A process or reaction which releases heat to the surroundings is said to be
exothermic.
Consider the reaction shown: C3H8 + 5 O2 → 3 CO2 + 4 H2O + 488 kcal We can say that this reaction is ________ and that the sign of ΔH is ________.
exothermic; negative
When a nucleus is bombarded with particles and breaks into two similarly sized nuclei plus one or more small particles, the process is called
fission.
Which group is the best description of the properties of alkanes?
flammable, non-reactive, insoluble in water
When an alkane reacts with an element from group 7A, the reaction is referred to as
halogenation.
A rapid reaction is distinguished by
having a small value of activation energy.
The amount of energy involved in melting a substance without changing its temperature is called the
heat of fusion.
The amount of energy associated with changing a liquid into a gas is called the
heat of vaporization.
Which of the following is the most suitable gas to use as a carrier gas in a gas chromatogram?
helium
The molecule shown is named as a substituted ________ because ________.
hexane; it contains six atoms of carbon in its longest chain.
Most gases show variations from ideality at ________ pressure and ________ temperature.
high, low
Ionizing radiation is
high-energy radiation that removes electrons from atoms or molecules.
Which element listed is the least electronegative?
hydrogen
Which intermolecular force is characteristic of compounds which are liquids at room temperature and have relatively high boiling points?
hydrogen bonds
The HCO3- ion is called ________
hydrogen carbonate
The H3O+ ion is called the ________ ion.
hydronium
An ionic compounded that attracts atmospheric water strongly is said to be
hygroscopic.
According to Avogadro's Law, the volume of a gas will ________ as the ________ is increased while the ________ are held constant.
increase; number of moles; pressure and temperature
What is the systematic name of ICl3?
iodine trichloride
An element with the same number of valence electrons as the element with the electron configuration 1s22s22p63s23p5 is
iodine.
An element with the same number of valence electrons as the element with the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^5 is
iodine.
The term which best describes the crystalline substance that results when a large number of metal atoms transfer electrons to a large number of non-metal atoms is
ionic solid.
The property that describes the ease with which an atom gives up an electron to form a positive ion is
ionization energy.
When a solution of iron(III) nitrate is mixed with a solution of sodium hydroxide, a rust colored precipitate forms. This precipitate is probably
iron(III) hydroxide.
What is the name of Fe2S3?
iron(III) sulfide
When an atom donates an electron, that electron
is acquired by another atom which becomes an anion.
Red blood cells are placed in a solution and neither hemolysis nor crenation occurs. Therefore the solution is
isotonic.
Ionizing radiation is dangerous to living things because
it alters the chemical structure of atoms or molecules.
Ammonia reacts with acids because
it contains a lone pair of electrons
One characteristic of a cation is ________
it has more protons than electrons.
To simplify comparisons, the energy value of fuels is expressed in units of
kcal/g.
An element belonging to the halogen family would be expected to have a ________ ionization energy and a ________ electron affinity.
large, large
In a radioactive decay series , a radioisotope decays into another radioisotope successively until a stable nucleus is produced. Th begins a decay series that consists of six alpha decays and four beta decays. What is the final stable isotope produced in this series?
lead-208
The bond angle in the molecule H2S is ________ because the ________.
less than 109.5°; lone pairs force the hydrogen atoms closer together
Diatomic nitrogen is added to the equilibrium system: N2 (g) + H2 (g) 2 NH3(g) + heat When a new equilibrium is established the concentration of H2 will be ________ the amount at the original equilibrium, and the amount of NH3 will be ________ the amount at the original equilibrium.
less than; greater than
In an aqueous solution that is basic, [H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].
less; less
Which transformation is evaporation?
liquid → gas
Which transformation is freezing?
liquid → solid
The term miscable is used to describe which type of solution
liquid/liquid
The metric unit used to measure volume is the
liter.
In a Lewis dot structure the electrons which complete an octet but are not located between two atoms are referred to as
lone pairs.
An atom with 3 valence electrons will most likely ________
lose three electrons.
An atom with 3 valence electrons will most likely ________ gain three electrons.
lose three electrons.
Main group elements that are metals usually ________ one or more electrons to form ________, which have a ________ charge.
lose; cations; positive
Which change to this reaction system would cause the equilibrium to shift to the right? N2 (g) + 3 H2 (g) 2 NH3 (g) + heat
lowering the temperature
The SI unit for volume is ________ and the metric unit for volume is ________.
m3; L
The units most likely to be used to measure the amount of alcohol to be added to a small test tube are
mL.
The amount of matter in an object is its
mass.
Which of the following represents the largest unit?
megaliter
According to a geologist, a mineral is a(an)
naturally occurring, crystalline chemical compound.
The element least likely to obey the octet rule in forming chemical bonds is
neon.
Which particle has a mass approximately equal to the mass of a proton?
neutron
Hydrogen exists as three isotopes. These isotopes differ by the number of ________ contained in the atom.
neutrons
Which group contains only elements which normally exist as diatomic molecules?
nitrogen, oxygen, fluorine
Consider a bent molecule, such as H2Se, in which the central atom has two lone pairs of electrons. The electronegativities of H and Se are 2.1 and 2.4, respectively. Based on these values and on consideration of molecular geometry, the H-Se bond can be considered ________ and the molecule is ________.
non-polar; polar
2 Al2O3 (s) → 4 Al (s) + 3 O2 (g) ΔG = +138 kcal Consider the contribution of entropy to the spontaneity of this reaction. As written, the reaction is ________, and the entropy of the system ________.
non-spontaneous; increases
All of the following species are involved in the blood buffer system except ________.
none of the above
Which is not a correct statement of Boyle's Law?
none of the above
Which is not an example of a solution?
none of the above
Which of the following statements about the solubility of gases in liquids is not correct?
none of the above
Which statement concerning Arrhenius acid-base theory is not correct?
none of the above
A molecule that contains three identical polar bonds to the central atom will be ________.
nonpolar if the geometry is planer triangular.
What is the valence shell electron configuration of the ion formed from an atom of the halogen family?
ns^2 np^6
The emission of a particle from an unstable nucleus is called
nuclear decay.
Radioactivity is generally associated with which part of the atom?
nucleus
Where is most of the mass of an atom concentrated?
nucleus
In terms of atomic structure, the common characteristic of elements in the same group is
number of electrons in the outermost shell.
The permanganate ion is composed of
one atom of manganese, four atoms of oxygen, and one extra electron.
The formula PO4^3- means that this ion is composed of
one atom of phosphorus, four atoms of oxygen, and three extra electrons.
The most important unit for measure biological doses of radiation is?
rem
The unit of radiation exposure which allows for the energy and penetrating power of different types of radiation is the
rem.
The amount of radiation that produces 2.1 × 109 units of charge in 1 cm3 of air is the
roentgen.
Valence electrons in the main group elements are contained in which type(s) of orbitals?
s and p
When acids and bases react the product other than water is a
salt.
In the molecule 3,3-dimethylhexane, carbon number two is
secondary.
For the following reaction, increasing the pressure will cause the equilibrium ________ 2 SO2 (g) + O2 (g) 2 SO3 (g) + heat
shift to the right, towards products.
If SiCl4 is named as a covalent compound, what would it be called?
silicon tetrachloride
A chemical bond formed when two atoms share one pair of electrons is a ________ bond; it is best described as ________.
single; covalent
A chemical bond formed when two atoms share two electrons is a ________ bond; it is best described as ________.
single; covalent
An element belonging to the alkaline earth family would be expected to have a ________ ionization energy and a ________ electron affinity.
small; small
The name of the compound with formula NaMnO4 is
sodium permanganate.
A substance represented by a formula written as MxLOy ∙ zH2O is called a
solid hydrate.
Which transformation is sublimation?
solid → gas
Which transformation is melting?
solid → liquid
Which is not a property of most alkanes?
soluble in water
The name of S^2- is
sulfide ion.
The element least likely to obey the octet rule in forming chemical bonds is
sulfur.
Which of the following is a diprotic acid?
sulfuric acid
Which homogeneous mixture is opaque and has particles large enough to be filtered?
suspension
The carbon atom marked with * is a ________ carbon atom. C C C-C-C-C-C-C
tertiary
A molecule in which the central atom has no lone pairs and forms four single bonds is said to have a ________ shape.
tetrahedral
The molecule SiCl4 has a ________ shape.
tetrahedral
The scientific principle which is the basis for balancing chemical equations is
the Law of Conservation of Mass.
A sievert is
the SI unit for radiation absorbed.
Entropy can be defined as
the amount of disorder in a system.
A roentgen is
the amount of radiation that produces 2.1 × 10^9 units of charge in one cubic centimeter of air.
Which factor is most important in determining the chemistry of an organic molecule?
the functional groups
The basis of the technique of chromatography for separating components of a mixture is ...
the interaction of the components with both stationary and mobile phases.
The position of the equilibrium for a system where K = 4.6 × 10-15 can be described as being favored to ________; the concentration of products is relatively ________.
the left; small
Which information is necessary to determine the molarity of a solution if the chemical formula of the solute is known?
the mass of solute dissolved and the final volume of the solution
Acetone is an organic molecule with a semi-structural formula of CH3COCH3. A student runs a sample of acetone through a gas chromatogram at 50°C. The acetone produces a peak after 4.2 minutes. The student then injects a mixture of unknown organic substances into the same column at the same temperature. There are peaks after 3.1, 4.2 and 7.4 minutes. From this information, it can be concluded that ...
the mixture has at least three components, one of which must be acetone.
The VSEPR model or molecular structure requires a knowledge of ________ to predict the geometry of an atom in a molecule.
the number of atoms bonded to the atom of interest
When a reaction system is at equilibrium
the rates of the reaction in the forward and reverse directions are exactly equal.
All of the statements are true for spontaneous reactions except
the reaction rate is determined by the value of ΔG.
Reaction rates are determined by all of the following factors except
the spontaneity of the reaction.
The formula (NH4)3PO4 indicates that one formula unit of this compound is composed of
three atoms of nitrogen, twelve atoms of hydrogen, one atom of phosphorus, and four atoms of oxygen.
What is the name of Mg3(PO4)2?
three atoms of nitrogen, twelve atoms of hydrogen, one atom of phosphorus, and four atoms of oxygen.
What is the name of SnCl2?
tin(II) chloride
A chemical bond formed when two atoms share six electrons is a ________ bond; it is best described as ________.
triple; covalent
A chemical bond formed when two atoms share three pairs of electrons is a ________ bond; it is best described as ________.
triple; covalent
A formula unit of ammonium sulfate consists of ________ ammonium ions and ________ sulfate ions.
two, one
In forming covalent bonds where the octet rule is obeyed, sulfur usually forms ________ bonds and chlorine usually forms ________ bonds.
two; one
Consider the endothermic reaction: N2 (g) + 2 H2 (g) → N2H4 (l) The entropy change of this reaction is ________ and the enthalpy change is ________, so at a very high temperature, this reaction is probably ________.
unfavorable; unfavorable; nonspontaneous
