Chem Final Review Packet 2

deci= 10

For which pair is the SI prefix not matched correctly with its meaning?
A) mega = 10^6
B) kilo = 1000
C) deci = 10
D) nano = 10^-9
E) centi = 0.01

2.1 x 10^4 m

The distance of 21 km equals
A) 0.021 m
B) 0.21 m
C) 210 m
D) 2100 m
E) 2.1 x 10 ^4 m

All of these are equally probable

Which of the following is the least probable concerning five measurements taken in the lab?
A) The measurements are accurate and precise
B) The measurements are accurate but not precise
C) The measurements are precise but not accurate
D) The measurements

0.00649

Express the number 6.49 x 10^-3 in common decimal form.
A) 0.00649
B) 6.49
C) 6490
D) 0.0649
E) 0.000649

$200

For spring break you and some friends plan a road trip to a sunny destination that is 2105 miles away. If you drive a car that gets 33 miles per gallon and gas costs $3.199/gal, about how much will it cost to get to your destination?
A) $410
B) $220
C) $2

17 lbs

Convert 7.9 kg to lb. (1 kg = 2.205 lb)

At 323F, the indium is partially solid and partially liquid; there is an equilibrium between the two states

The melting point of indium is 156.2C. At 323F, what is the physical state of indium?
A) solid
B) liquid
C) gas
D) not enough information
E) at 323F, the indium is partially solid and partially liquid; there is an equilibrium between the two states

It will float on top

The density of gasoline is 0.7025 g/mL at 20C. When gasoline is added to water:
A) It will float on top
B) It will sink to the bottom
C) It will mix so, you can't see it
D) The mixture will improve the running of the motor
E) None of these things will hap

The y, or vertical, intercept is the weight of the empty beaker

If volume of liquid is plotted along the horizontal axis, and total mass of beaker plus liquid is plotted on the vertical axis:
A) The x, or horizontal, intercept is the negative value of the weight of the beaker
B) The y, or vertical, intercept is the we

1.52 x 10^6 g

Suppose that you purchased a water bed with the dimensions 2.55 m x 2.53 dm x 235 cm. What mass of water does this bed contain?
A) 1.52 x 10^3 g
B) 1.52 x 10^4 g
C) 1.52 x 10^5 g
D) 1.52 x 10^8 g
E) 1.52 x 10^6 g

all of these

An example of a pure substance is
A) elements
B) compounds
C) pure water
D) carbon dioxide
E) all of these

homogeneous mixture

A solution is also called a
A) homogeneous mixture
B) heterogeneous mixture
C) pure mixture
D) compound
E) distilled mixture

1 microliter/ 1000 nL

Which of the following unit factors is incorrect?
A) 1 microliter/ 1000 nL
B) 1 cg/ 100 g
C) 1 L/ 1000 mL
D) 1000 m/ 1 km

gram

Which of the following is not a fundamental metric unit?
A) meter
B) second
C) gram
D) mole

liter

Which of the following is not a fundamental metric unit?
A) meter
B) second
C) kilogram
D) liter

1230.

How should the number 1.230 x 10^3 be properly expressed as a decimal?
A) 1230
B) 0.001230
C) 1230.0
D) 1230.

3, 3

When 87.7 is added to 73.841, the result should be reported with ___ significant figures. And when 87.7 is divided by 73.841 the result should be reported with ___ significant figures.
A) 3, 3
B) 3, 5
C) 4, 3
D) 4, 4

SO and SO2

Which of the following pairs can be used to illustrate the law of multiple proportions?
A) SO and SO2
B) CO and CaCO3
C) H2O and C12H22O11
D) H2SO4 and H2S
E) KCl and KClO2

A, B, and C

Alpha particles beamed at thin metal foil may
A) pass directly through without changing direction
B) be slightly diverted by attraction to electrons
C) be reflected by direct contact with nuclei
D) A and C
E) A, B, and C

All of the above statements (A-D) are true

Which of the following statements about atomic structure is false?
A) An atom is mostly empty space
B) Almost all of the mass of the atom is concentrated in the nucleus
C) The protons and neutrons in the nucleus are very tightly packed
D) The number of pr

There are only three types of radioactivity known to scientists today

Which statement is not correct?
A) The mass of an alpha particle is 7300 times that of the electron
B) An alpha particle has a 2+ charge
C) Three types of radioactivity emission are gamma rays, beta rays, and alpha particles
D) A gamma ray is high energy

14/8 N

Which of the following atomic symbols is incorrect?
A) 14/6 C
B) 37/17 Cl
C) 32/15 P
D) 39/19 K
E) 14/8 N

75 protons, 110 neutrons

The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. Rhenium-185 has in its nucleus
A) 75 protons, 75 neutrons
B) 75 protons, 130 neutrons
C) 130 protons, 75 neutrons
D) 75 protons, 110 neutrons
E) not enough information

I, IV and II, V

Which among the following represent a set of isotopes? Atomic nuclei containing:
I. 20 protons and 20 neutrons
II. 21 protons and 19 neutrons
III. 22 neutrons and 18 protons
IV. 20 protons and 22 neutrons
V. 21 protons and 20 neutrons
A) I, II, III
B) III

I, II, IV

Which of the following statements are true of unanium-238?
I. Its chemical properties will be exactly like those of uranium-235
II. Its mass will be slightly different from that of an atom of uranium-235
III. It will contain a different number of protons

A, B, and C

An isotope, X, of a particular element has an atomic number of 15 and a mass number of 31. Therefore:
A) X is an isotope of phosphorus
B) X has 16 neutrons per atom
C) X has an atomic mass of 30.973
D) A and B
E) A, B and C

Scientists believe that solids are mostly open space

Which of the following statements are true?
A) Ions are formed by adding or removing protons or electrons
B) Scientists believe that solids are mostly open space
C) Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases
D

A and C

Which of the following statements is (are) true?
A)18/8 O and 19/9 F have the same number of neutrons
B) 14/6 C and 14/7 N are isotopes of each other because their mass numbers are the same
C) 18/8 O^-2 has the same number of electrons as 20/10 Ne
D) A an

Cesium, Ce

Which of the following are incorrectly paired?
A) Copper, Cu
B) Carbon, C
C) Cobalt, Co
D) Calcium, Ca
E) Cesium, Ce

tend to gain electrons in chemical reactions

All of the following are characteristics of metals except:
A) good conductors of heat
B) malleable
C) ductile
D) often lustrous
E) tend to gain electrons in chemical reactions

phosphorous pentoxide, P2O5

Which of the following pairs is incorrect?
A) iodine trichloride, ICl3
B) phosphorous pentoxide, P2O5
C) ammonia, NH3
D) sulfur hexafluoride, SF6
E) all of the above pairs are correct

8

How many oxygen atoms are there in one formula unit of Ca3(PO4)2?
A) 2
B) 4
C) 6
D) 8
E) none of these

BaPO4, barium phosphate

Which of the following pairs is incorrect?
A) NH4Br, ammonium bromide
B) K2CO3, potassium carbonate
C) BaPO4, barium phosphate
D) CuCl, copper(I) chloride
E) MnO2, manganese(IV) oxide

all

Which of the following name(s) is(are) correct?
1. sulfide, S^-2
2. ammonium chloride, NH4Cl
3. acetic acid, HC2H3O2
4. barium oxide, BaO
A) all
B) none
C) 1, 2
D) 3, 4
E) 1, 3, 4

transition metals

Which metals form cations with varying positive charges?
A) transition metals
B) Group 1 metals
C) Group 2 metals
D) Group 3 metals
E) metalloids

The 5 lead by mass in the compound galena is the same for all pure samples obtained from any source

Which of these statements is a consequence (follows from) the Law of Multiple Proportions?
A) All samples of chlorine contain 35Cl and 37Cl in the same (definite) ratio
B) The mass of oxygen that is combined with a fixed mass of nitrogen in each of the bi

34, 45, 36

How many protons, neutrons, and electrons, in that order are present in the anion formed by one atom of 79Se?
A) 34, 34, 45
B) 34, 45, 34
C) 32, 45, 34
D) 34, 45, 36
E) 36, 45, 36

An atom of 18O has an equal number of protons and neutrons

Which statement is INCORRECT?
A) An atom of 60ZN has an equal number of protons and neutrons
B) An atom of 50Mn has an equal number of protons and neutrons
C) An atom of 18O has an equal number of protons and neutrons
D) An atom of 41K has an equal number

Mg(OH)2 is magnesium dihydroxide

Which of the following compounds is incorrectly named?
A) Mg(OH)2 is magnesium dihydroxide
B) CaO is calcium oxide
C) NH4NO3 is ammonium nitrate
D) K3PO4 is potassium phsphate
E) MgSO3 is magnesium sulfite

70%

Naturally occurring copper exists in two isotopic forms: 63Cu and 65Cu. The atomic mass of copper is 63.55 amu. What is the approximate natural abundance of 63Cu?
A) 63%
B) 90%
C) 70%
D) 50%
E) 30%

28.09 amu

Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate the atomic weight of X.
A) 28.09 amu
B) 48.63 amu
C) 27.63 amu
D) 28.9

4.22 x 10^-22 g

What is the mass of 4 atom(s) of copper in grams?
A) 254.2 g
B) 2.37 x 10^21 g
C) 9.57 x 10^-24 g
D) 6.022 x 10^23 g
E) 4.22 x 10^-22 g

2

A given sample of a xenon fluoride compound contains molecules of a single type XeFn, where n is some whole number. Given that 8.06 x 10^20 molecules of XeFn weigh 0.227 g, calculate n.
A) 1
B) 6
C) 4
D) 3
E) 2

176 g/mol

One molecule of a compound weights 2.93 x 10^-22 g. The molar mass of this compound is:
A) 2.06 g/mol
B) 567 g/mol
C) 168 g/mol
D) 176 g/mol
E) none of these

C

A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X?
A) He
B) C
C) F
D) S
E) none of these

8.98 g

How many grams of potassium are in 27.8 g of K2CrO7?
A) 4.49 g
B) 1.422 g
C) 8.98 g
D) 78.2 g
E) 55.6 g

40%

A mixture of KCl and KNO3 is 44.20% potassium by mass. The percentage of KCl in the mixture is closest to
A) 40%
B) 50%
C) 60%
D) 70%
E) 80%

85.05%

The molar mass of an insecticide, dibromoethane, is 187.9 g/mol. Its molecular formula is C2H4Br2. What percent by mass of bromine does dibromoethane contain?
A) 42.52%
B) 2.14%
C) 85.05%
D) 12.78%
E) 6.39%

69.9%

Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed for skin problems. Its molecular formula is C26H38O6. What is the percent by mass of carbon in hydrocortisone valerate?
A) 69.9%
B) 43.6%
C) 54.2%
D) 76.9%
E) 60.1%

You must convert percent by mass to relative numbers of atoms

Suppose you are given the percent by mass of the elements in a compound and you wish to determine the empirical formula. Which of the following is true?
A) You must convert percent by mass to relative numbers of atoms
B) You must assume exactly 100.0 g of

2KClO3 --> 2KCl + 3/2 O2

Which of the following equations is not balanced?
A) 4Al + 3O2 --> 2Al2O3
B) C2H6 + 7/2 O2 --> 2CO2 + 3H2O
C) 2KClO3 --> 2KCl + 3/2 O2
D) 4P4 + 5S8 --> 4P4S10
E) P4 + 5O2 --> P4O10

none of these

wPCl5 + xH2O --> yPOCl3 + zHCl
The above equation if properly balanced when:
A) w= 1, x=2, y=2, z=4
B) w= 2, x=2, y=2, z=2
C) w= 2, x=2, y=2, z=1
D) w= 1, x=1, y=1, z=2
E) none of these

1, 2, 1, 6

Give (in order) the correct coefficients to balance the following reaction:
H2SnCl6 + H2S --> SnS2 + HCl
A) 1, 2, 1, 6
B) 1, 2, 2, 2
C) 1, 1, 1, 6
D) 6, 2, 1, 1
E) 2, 4, 2 6

29.1 g P4O10

For the reaction P4O10(s) + 6H2O(l) --> 4H3PO4(aq), what mass of P4O10 must be consumed if 3.71 x 10^23 molecules of H2O are also consumed?
A) 1.05 x 10^3 g P4O10
B) 29.1 g P4O10
C) 175 g P4O10
D) 1.85 g P4O10
E) 66.6 g P4O10

has the lowest ratio of moles available/ coefficients in the balance equation

The limiting reactant in a reaction
A) has the lowest coefficient in a balanced equation
B) is the reactant for which you have the fewest number of moles
C) has the lowest ratio of moles available/ coefficients in the balance equation
D) has the lowest ra

H2SO4

Phosphoric acid can be prepared by reaction of sulfuric acid with "phosphate rock" according to the equation:
Ca3(PO4)2 + 3H2SO4 --> 3CaSO4 + 2H3PO4
Suppose the reaction is carried out starting with 129 g of Ca3(PO4)2 and 97.4 g of H2SO4. Which substance

42.7 g

Consider the following reaction:
Ch4(g) + 4Cl2(g) --> CCl4(g) + 4HCl(g)
What mass of CCl4 will be formed if 1.20 moles of methane react with 1.11 moles of chlorine?
A) 185 g
B) 171 g
C) 683 g
D) 42.7 g
E) 19.7 g

none of the above

The limiting reactant in a reaction
A) is the reactant for which there is the least amount in grams
B) is the reactant which has the lowest coefficient in a balanced equation
C) is the reactant for which there is the most amount in grams
D) is the reactan

If we have more mass of C2H6, then O2 must be limiting

Which of the following statements is always true concerning a reaction represented by the following balanced chemical equations?
2C2H6(g) + 7O2(g) --> 6H2O(l) + 4CO2(g)
A) If we have equal masses of C2H6 and O2, there is no limiting reactant
B) It we have

Oxygen gas is limiting

Equal masses (in grams) of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting?
A) Oxygen gas is limiting
B) Hydrogen gas is limiting
C) Water is limiting
D) Nothing is limiting
E) More information is needed to answer this q

6.4 kg NH3

Ammonia can be made by reaction of water with magnesium nitride as shown by the following unblanaced equation:
Mg3N2(s) + H2O(l) --> Mg(OH)2(s) + NH3(g)
If this process is 80% efficient, what mass of ammonia can be prepared from 19.0 kg magnesium nitride?

1.81 x 10^24 nitrogen atoms

Calculate the number of nitrogen atoms in 240. g of ammonium nitrate
A) 2.01 x 10^23 nitrogen atoms
B) 6.02 x 10^23 nitrogen atoms
C) 1.20 x 10^24 nitrogen atoms
D) 1.81 x 10^24 nitrogen atoms
E) 3.61 x 10^24 nitrogen atoms

HClO4

Which of the following is a strong acid?
A) HF
B) KOH
C) HClO4
D) HClO
E) HBrO

HNO3- weak acid

Which of the following is paired incorrectly?
A) H2SO4- strong acid
B) HNO3- weak acid
C) Ba(OH)2- strong base
D) HCl- strong acid
E) NH3- weak base

0.00028 mol

Diabetics often need injections of insulin to help maintain the proper blood glucose levels in their bodies. How many moles of insulin are needed to make up 45 mL of 0.0062 M insulin solution?
A) 0.00056 mol
B) 0.14 mol
C) 7.3 mol
D) 0.28 mol
E) 0.00028 m

3.50 M

You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have more of the 4.00 M solution and you add the solutions together. Which of the following could be the concentration of the final solution?
A) 2.70

No reaction will occur

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statements is correct?
A) Both KNO3 and NH4SO4 precipitate from solution
B) A gas is released
C) NH4SO4 will precipitate from solution
D) KNO3 will precipitate from solu

All of these are soluble in water

Which of the following salts is insoluble in water?
A) Na2S
B) K2CO3
C) Pb(NO3)2
D) CaCl2
E) All of these are soluble in water

Ca2+

Which of the following ions is most likely to form an insoluble sulfate?
A) K+
B) Li+
C) Ca2+
D) S2-
E) Cl-

Mg2+, SO4^2-

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?
A) Al3+, S2-
B) Pb2+, Cl-
C) Ba2+, PO2^3-
D) Pb^2+, OH-
E) Mg2+, SO4^2-

3Ca2+ (aq)

The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?
A) 2Br- (aq)
B) PO4^3- (aq)
C) 2Ca3(PO4)2(s)
D) 6NaBr(aq)
E) 3Ca2+ (aq)

CaCO3(s)

When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms will be present in the net ionic equation?
A) CoCO3(s)
B) H+(aq)
C) 2CoCO3(s)
D) 2Cl-(aq)
E) two of these

3OH-(aq)

The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?
A) 3Al3+ (aq)
B) OH- (aq)
C) 3OH- (aq)
D) 2Al3+ (aq)
E) 2Al(OH)3(s)

All are true

You mix 275.0 mL of 1.20 M lead(II)nitrate with 300.0 mL of 1.85 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false?
A) The final concentration of Pb2+ ions is 0.0913 M
B) You form 128 g of lead(II) iodide
C) The final c

13.53%

If all the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample?
A) 50.52%
B) 13.53%
C) 1.425%
D) 7.391%
E) none of the above

0.538 M

You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.72 M solution of AgNO3(aq). Calculate the concentration of Ag+ after the two solutions are mixed together.
A) 0.00 M
B) 0.538 M
C) 1.08 M
D) 0.088 M
E) 0.215 M

hydrogen ion

When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in the complete ionic equation?
A) hydrogen ion
B) carbonate ion
C) potassium ion
D) hydroxide ion
E) water

none of these

When solutions of carbonic acid and copper(II) hydroxide react, which of the following are spectator ions?
A) hydrogen ion
B) carbonate ion
C) copper(II) ion
D) hydroxide ion
E) none of these

5.4 g

What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H2SO4?
A) 2.7 g
B) 0.7 g
C) 5.4 g
D) 135 g
E) none of these

0.0876 M

Sulfamic acid, HSO3NH2 (molar mass =(7.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base:
HSO3NH2(aq) + KOH(aq) --> KSO2NH2 (aq) + H2O(l)
A 0.165-g sample of HSO2NH2 required 19.4 mL of an aqueous solution of KOH for a co

NO2

In which of the following does nitrogen have an oxidation state of +4?
A) HNO3
B) NO2
C) N2O
D) NH4Cl
E) NaNO2

NH4+

Which of the following ions forms the fewest insoluble salts?
A) Al3+
B) Cl
C) NH4+
D) OH-
E) Mg2+

N2O

In which of the following does nitrogen have the lowest oxidation state?
A) HNO3
B) NO2
C) N2O
D) NH4Cl
E) NaNO2

I2

In which of the following does iodine have the lowest oxidation state?
A) LiIO3
B) IO2
C) I2O
D) NH4I
E) I2

11.4 psi

Which of the following would represent the greatest pressure?
A) 0.680 atm
B) 517 mmHg
C) 11.4 psi
D) 62106 Pa
E) 14.1 in Hg

all have the same volume

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?
A) H2
B) He
C) Ne
D) O2
E) All have the same volume

Cl2

Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0C and 1 atm pressure.
Which gas has the highest density?
A) He
B) Cl2
C) CH4
D) NH3
E) all gases the same

Cl2

For which gas are the molecules diatomic?
A) He
B) Cl2
C) CH4
D) NH3
E) all gases the same

The full bag contains fewer molecules of each bag than it did at 0.0C

A plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered:
Temperature: 0.0C (273 K)
Pressure: 1.00 atm
Mass of empty bag: 20.77 g
Mass of 1.12 liters of air at conditions given: 1.30 g
Volume of bag: 1

\

Which of the following is the best qualitative graph of P versus molar mass of a 1-g sample of different gases at constant volume and temperature?
A) /
B) / (starts higher)
C) ----
D) \
E) none of these

0.67

Given reaction N2 + 3H2 --> 2NH3, you mix 1 mol of each of nitrogen and hydrogen gases under the same conditions in a container fitted with a piston. Calculate the ratio of volumes of the container (Vf/Vi)
A) 0.67
B) 1.00
C) 1.33
D) 1.50
E) none of these

0.260 atm

A 3.31-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 2.37 L. The salt decomposes when heated, according to the equation:
2Pb(NO3)2(s) --> 2PbO(s) + 4NO2(g) + O2 (g)
Assuming complete decomp

B2H6

A 1.00-g sample of a gaseous compound of boron and hydrogen occupies 0.820 L at 1.00 atm and 3C. What could be the molecular formula for the compound?
A) BH3
B) B2H6
C) B4H10
D) B3H12
E) B5H14

0.056 mol

Zinc metal is added to hydrochloric acid to generate hydrogen gas, which is collected over a liquid whose vapor pressure is the same as pure water at 20.0C (18 torr). the volume of the gas mixture is 1.7 L and its total pressure is 0.810 atm
Determine the

2.52 atm

The valve between the 2.00-L bulb, in which the gas pressure is 1.80 atm, and the 3.00-L bulb, in which the gas pressure is 3.00 atm, is opened. What is the final pressure in the two bulbs, the temperature remaining constant?
A) 0.720 atm
B) 2.28 atm
C) 2

The mean square velocity of molecules in sample A is twice as large as the mean square velocity of molecules in sample B

Consider the following gas samples:
Sample A Sample B
Which of the following statements is false?
A) The volume of sample A is twice the volume of Sample B
B) The average kinetic energy of the molecules in sample A is twice the average kinetic energy of t

The average velocity of the gas particles is directly proportional to the absolute temperature

Which of the following is not an assumption of the kinetic molecular theory for a gas?
A) Gases are made up of tiny particles in constant chaotic motion
B) Gas particles are very small compared to the average distance between the particles
C) Gas particle

All collisions between molecules are elastic

Which of the following is included as a postulate in the kinetic molecular theory of an ideal gas?
A) The distance between gas molecules is small compared with the size of the molecule
B) All collisions between molecules are elastic
C) In an average colli

CH4

Which of the following would have a higher rate of effusion than C2H2?
A) N2
B) O2
C) Cl2
D) CH4
E) CO2

CO2

The rate of effusion of an unknown gas was measured and found to be 11.9 mL/min. Under identical conditions, the rate of effusion of pure oxygen (O2) gas is 14.0 mL/min. Based on this information, the identity of the unknown gas could be:
A) F2
B) NO
C) C

the finite volume of molecules

The van der Waals equation, nRT = [P +a(n/V^2](V-nb), incorporates corrections to the ideal gas law in order to account for the properties of real gases. One of the corrections account for law in order to account for the properties of real gases. One of t

Real gases consist of molecules or atoms that have volume

Which of the following properties of a real gas is related to the b coefficient in the van der Waals equation?
A) Real gases consist of molecules or atoms that have volume
B) The average speed of the molecules of a real gas increases with temperature
C) T

The gas molecules have a very low molar mass

Which of the following statements is least likely to be true of a sample of nitrogen gas?
A) The gas molecules are large enough to occupy a substantial amount of space
B) A large number of molecules have speeds greater than the average speed
C) The gas mo

The volume of the sample would be zero at -273C

Which of the following statements is least likely to be true of a sample of nitrogen gas?
A) Molecules of gaseous nitrogen are in constant random motion
B) The pressure exerted by gaseous nitrogen is proportional to the absolute temperature of the gas
C)

H2

Of the following real gases, which would be expected to have the lowest van der Waals correction for inter molecular attractions?
A) H2
B) Cl2
C) NH3
D) O2
E) not enough information to determine

O3

Which of the following pollutant gases is not produced directly in a combustion engine?
A) CO
B) CO2
C) O3
D) NO
E) NO2

1.42 liters

A sample of a gas occupies a volume of 2.62 liters at 25C and 1.00 atm. What will be the volume at 50.0C and 2.00 atm?
A) 1.42 liters
B) 2.62 liters
C) 4.83 liters
D) 5.68 liters
E) 10.5 liters

The system does work on the surroundings when an ideal gas expands against a constant external pressure

Which of the following statements is correct?
A) The internal energy of a system increases when more work is done by the system than heat was flowing into the system
B) The internal energy of a system decreases when work is done on the system and heat is

None of the above is false

For a particular process q=-17 kJ and w= 21 kJ. Which of the following statements is false?
A) Heat flows from the system to the surroundings
B) The system does work on the surroundings
C) E= +4 kJ
D) The process is exothermic
E) None of the above is fals

11.4 L

A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.310-L. When the mixture is ignited, gases are produced and 935 J of energy is released. To what volume will the gases expand a constant pressure of 635 mmHg, if all

The amount of heat released in the process will depend on the path taken

Which statement is true of a process in which one mole of a gas is expanded from state A to state B?
A) When the gas expands from state A to state B, the surroundings are doing work on the system
B) The amount of work done in the process must be the same,

2

Of energy, work, enthalpy, and heat, how many are state functions?
A) 0
B) 1
C) 2
D) 3
E) 4

The chemical reaction is absorbing energy

In the lab, you mix two solutions (each originally at the same temperature) and the temperature of the resulting solution decreases. Which of the following is true?
A) The chemical reaction is releasing energy
B) The energy released is equal to s x m x ^T

283 J/g*C

What is the specific heat capacity of a metal if it requires 178.1 J to change the temperature of 15.0 g of the metal from 25.00 C to 32.00 C
A) 0.590 J/g*C
B) 11.9 J/g*C
C) 25.4 J/g*C
D) 29.6 J/g*C
E) 283 J/g*C

0.353 J/g*C

Exactly 123.7 J will raise the temperature of 10.0 g of a metal from 25.0C to 60.0C. What is the specific heat capacity of the metal?
A) 2.83 J/g*C
B) 0.353 J/g*C
C) 24.9 J/g*C
D) 29.6 J/g*C
E) none of these

0.60 J/g*C

What is the specific heat capacity of silver if it requires 86.3 J to raise the temperature of 15 grams of silver by 25C?
A) 4.3 J/g*C
B) 0.23 J/g*C
C) 0.14 J/g*C
D) 0.60 J/g*C
E) none of these

Lead

Consider the following specific heats of metals
Metal Specific Heat
If the same amount of heat is added to 25.0 g of each of the metals, which are all the same initial temperature, which metal will have the highest temperature?
A) Zinc
B) Magnesium
C) Iro

-610.1 kJ

Given the heat of the following reactions:
I. P4(s) + 6Cl2(g) --> 4PCl3(g) -1225.6
II. P4(s) + 5O2(g) --> P4O10(g) -2967.3
III. PCl3(s) + Cl2(g) --> PCl5(g) -84.2
IV. PCl3(g) + 1/2 O2(g) --> Cl3PO(g) -285.7
Calculate the value of ^H for the reaction below

C(gr) + 1/2O2(g) --> CO(g), ^H= -110.5 kJ

Choose the correct equation for the standard enthalpy of formation of CO(g), where ^Hf for CO= -110.5 kJ/mol (gr indicates graphite)
A) 2C(gr) + O2(g) --> 2CO(g), ^H= -110.5 kJ
B) C(gr) + O(g) --> CO(g), ^H= -110.5 kJ
C) C(gr) + 1/2O2(g) --> CO(g), ^H= -1

All of its hydrocarbon chains contain the same number of carbon atoms

The following statements concerning petroleum are all true except:
A) It is a thick, dark liquid composed mostly of hydrocarbons
B) It must be separated into fractions (by boiling) in order to be used efficiently
C) Some of the commercial uses of petroleu

methane

Which of the following is both a greenhouse gas and a fuel?
A) carbon dioxide
B) coal
C) freon
D) methane
E) nitrogen

4.12 x 10^5 s-1

Which of the following frequencies corresponds to light with the longest wavelength?
A) 3.00 x 10^13 s-1
B) 4.12 x 10^5 s-1
C) 8.50 x 10^20 s-1
D) 9.12 x 10^12 s-1
E) 3.20 x 10^9 s-1

n=4 to n=3

Consider the following portion of the energy-level diagram for hydrogen:
n=4 -0.1361 x 10^-18 J
n=3 -0.2420 x 10^-18 J
n=2 -0.5445 x 10^-18 J
n=1 -2.178 x 10^-18 J
For which of the following transitions does the light emitted have the longest wavelength?

It is impossible to accurately know both the exact location and momentum of a particle

Which of the following statements best describes the Heisenberg uncertainty principle?
A) The exact position of an electron is always uncertain
B) The velocity of a particle can only be estimated
C) It is impossible to accurately know both the exact locat

10

How many electrons in an atom can have the quantum numbers n=3, l=2?
A) 2
B) 5
C) 10
D) 18
E) 6

32

How many electrons can be contained in all of the orbitals with n=4?
A) 2
B) 8
C) 10
D) 18
E) 32

4

Which of the following could not be a valid m1 quantum number for a 4d orbital?
A) 2
B) 0
C) -2
D) 1
E) 4

14

It l=3, how many electrons can be contained in all the possible orbitals?
A) 7
B) 6
C) 14
D) 10
E) 5

n=1, l=1, m1=0, ms= 1/2

Which of the following combinations of quantum numbers is not allowed?
A) n=1, l=1, m1=0, ms= 1/2
B) n=3, l=0, m1=0, ms= -1/2
C) n=2, l=1, m1=-1, ms= 1/2
D) n=4, l=3, m1=-2, ms= -1/2
E) n=4, l=2, m1=0, ms= 1/2

1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5p2

The complete electron configuration of tin is
A) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5d10 5p2
B) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d10 4p2
C) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5d10 5p2
D) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5p2
E) none of these

When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital

Which of the following statements about quantum theory is incorrect?
A) The energy and position of an electron cannot be determined simultaneously
B) Lower energy orbitals are filled with electrons before higher energy orbitals
C) When filling orbitals of

An orbital can accommodate at most two electrons

Which of the following statements is false?
A) An orbital can accommodate at most two electrons
B) The electron density at a point is proportional to u2 at that point
C) The spin quantum number of an electron must be either 1/2 or -1/2
D) A 2p orbital is

EF4

An element E has the electron configuration [Kr] 5s2 4d10 5p2. The formula for the fluoride of E is most likely
A) EF14
B) EF4
C) EF
D) EF6
E) EF8

transition elements

An element with the electron configuration [Xe] 6s2 4f14 5d7 would belong to which class on the periodic table?
A) transition elements
B) alkaline earth elements
C) rare earth elements
D) none of the above

P

Of the following elements, which needs three electrons to complete its valence shell?
A) Ba
B) Ca
C) Si
D) P
E) Cl

2

How many of the following electron configurations for the species in their ground state are correct?
I. Ca: 1s2 2s2 2p6 3s2 3p6 4s2
II. Mg: 1s2 2s2 2p6 3s1
III. V: [Ar] 3s2 3d3
IV. As: [Ar] 4s2 3d10 4p3
V. P: 1s2 2s2 2p6 3p5
A) 1
B) 2
C) 3
D) 4
E) 5

Ti

For which of the following elements does the electron configuration for the lowest energy state show a partially filled d orbital?
A) Ti
B) Rb
C) Cu
D) Ga
E) Kr

Cr

Which of the following electron configurations is different from that expected?
A) Ca
B) Sc
C) Ti
D) V
E) Cr

two of the above

Which of the following have 10 electrons in the d orbitals?
A) Mn
B) Fe
C) Cu
D) Zn
E) two of the above

Br(g) ---> Br+(g) +e-

Which of the following processes represents the ionization energy of bromine?
A) Br(s) ---> Br+(g) +e-
B) Br(l) ---> Br+(g) +e-
C) Br(g) ---> Br+(g) +e-
D) Br(s) ---> Br+(s) +e-
E) Br2(g) ---> Br2+(g) +e-

F, Cl, S

Order the elements S, Cl, and F in terms of increasing ionization energy.
A) S, Cl, F
B) Cl, F, S
C) F, S, Cl
D) F, Cl, S
E) S, F, Cl

That of Al is higher than that of Mg because electrons are taken from the same energy level, but the Al atom has one more proton

Which of the following concerning second ionization energies is true?
A) That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to take the second electron away
B) That of Al is higher than that of Mg because el

Ba

Of the following elements, which has the lowest first ionization energy?
A) Ba
B) Ca
C) Si
D) P
E) Cl

Ne

Which of the following atoms has the largest ionization energy?
A) O
B) Li
C) Ne
D) Be
E) K

It will be equal to and opposite in sign to the electron affinity of Mg2+

Which of the following statements is true about the ionization energy of Mg+?
A) It will be equal to the ionization energy of Li
B) It will be equal to and opposite to the electron affinity of Mg
C) It will be equal to and opposite to the electron affinit

The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer

Which of the following statements is true?
A) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer
B) The krypton 1s orbital is larger than the helium 1s orbital because krypton contains

ultraviolet, visible, infrared

Which has these types of electromagnetic radiation arranged in order of decreasing frequency?
A) visible, ultraviolet, x-ray
B) radiowaves, visible, ultraviolet
C) ultraviolet, visible, infrared
D) x-ray, visible, ultraviolet
E) none of these

ultraviolet, visible, infrared

Which has these types of electromagnetic radiation arranged in order of decreasing energy?
A) visible, ultraviolet, x-ray
B) radiowaves, visible, ultraviolet
C) ultraviolet, visible, infrared
D) x-ray, visible, ultraviolet
E) none of these

[Ar] 4s1 3d10

Select the correct electron configuration for Cu.
A) [Ar] 4s2 3d9
B) [Ar] 4s1 3d10
C) [Ar] 4s2 4p6 3d3
D) [Ar] 4s2 4d9
E) [Ar] 3d10

X(g) + e- => X+(g) +e-

Which of the following equations correctly represents the process involved in the electron affinity of X?
A) X+(g) + e- => X(g)
B) X+ (g) + Y-(g) => XY(g)
C) X(g) + e- => X+(g) +e-
D) X(g) => X+(g) + e-
E) X+(g) => X+ (aq)