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Chem final exam review

Total questions: 70

Worksheet time: 18hrs 30mins

Name
Class
Date
1.

A combination of sand, salt, and water is an example of a _____

a)

heterogeneous mixture

b)

compound

c)

solid

d)

homogeneous mixture

e)

pure substance

2.

which one of the following has the element name and symbol correctly matched?

a)

Tn, tin

b)

S, sodium

c)

Fe, iron

d)

B, bromine

e)

N, neon

3.

in the following list, only ____ is not an example of a chemical reaction

a)

the condensation of water vapor

b)

a burning candle

c)

dissolution of a penny in the nitric acid

d)

the formation of polyethylene from ethylene

e)

the rusting of iron

4.

which one of the following is an intensive property?

a)

amount

b)

volume

c)

temperature

d)

mass

e)

heat content

5.

there should be _____ significant figures in the answer to the following computation

a)

1

b)

2

c)

3

d)

4

e)

5

6.

which one of the following is the highest temperature

a)

302 K

b)

38 ⁰C

c)

96 ⁰F

d)

none of the above

e)

the freezing point of water

7.

the density of a gold nugget is 19.3 g/cm³. If the volume of the gold nugget is 0.00369 L, the mass of the nugget is ____g.

a)

5.23

b)

19.3

c)

71.2

d)

0.191

e)

none of the above

8.

an atom of the most common isotope of gold, ¹⁹⁷ Au, has _____ protons,______ neutrons, and _______ electrons

a)

197, 79, 118

b)

79,118,118

c)

79,197,197

d)

79,118,79

e)

118,79,39

9.

which pair of atoms constitutes a pair of isotopes of the same element?

a)

b)

c)

d)

e)

10.

there are _____protons, _____neutrons, and _____ electrons in 238U⁺5

a)

92,146,92

b)

146,92,146

c)

92,146,87

d)

92,92,87

e)

146,92,92

11.

the element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ____amu

a)

219.7

b)

221.0

c)

220.4

d)

220.42

e)

218.5

12.

which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?

a)

Cs,Ba

b)

Ga,Ge

c)

H,Li

d)

C,O

e)

Ca,Sr

13.

the elements in group 1A, 6A, and 7A are called _____, respectively

a)

halogens, transition, and alkali metal

b)

alkaline earth metal, halogen, and chalcogens

c)

alkaline earth metal, transition metal, and halogen

d)

alkali metal, halogen, and noble gases

e)

alkali metals, chalcogens and halogen

14.

an element in the upper right corner of the periodic table _____

a)

is definitely a nonmetal

b)

is either a metal or metalloid

c)

is definitely a metal

d)

is definitely a metaloid

e)

is either a metalloid or nonmetal

15.

which one of the following molecular formulas is also an empirical formula?

a)

C6H6O2

b)

C6H6

c)

H2O2

d)

H2P4O6

e)

C2H6SO

16.

which formula/name pair is incorrect?

a)

FeSO3 iron (II) sulfite

b)

fe2(SO4)3 iron (III) sulfide

c)

FeSO4 iron (II) sulfate

d)

FeS iron (II) sulfide

e)

Fe2(SO3)3 iron (III) sulfite

17.

which one of the following is the formula of hydrochloric acid?

a)

HClO4

b)

HClO

c)

HCl

d)

HClO2

e)

HClO3

18.

which of the following compounds is copper (I) chloride?

a)

CuCl2

b)

Cu2Cl3

c)

CuCl

d)

Cu3Cl2

e)

Cu2Cl

19.

the correct name for HBrO4 is ____

a)

hydrobromic acid

b)

perbromic acid

c)

bromic acid

d)

bromous acid

e)

hydrobromous acid

20.

when a metal and a nonmetal react, _____ tends to lose electrons and the ______ tends to gain electrons

a)

nonmetal, nonmetal

b)

metal, nonmetal

c)

metal, metal

d)

nonmetal, metal

e)

none of the above; these elements share electrons

21.

which of the following are combination reactions?

CH4 (g) + O2 (g) -> CO2 (g) + H2O (I)

CaO (s) + CO2 (g) -> CaCO3 (s)

Mg (s) + O2 (g) -> MgO (s)

PbCO3 (s) -> PbO (s) + CO2 (g)

a)

1,2,3

b)

1,2,3,4

c)

2,3

d)

2,3,4

e)

4 only

22.

the formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is ____amu

a)

123.11

b)

42.03

c)

3.06

d)

109.10

e)

107.11

23.

the formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is ____amu

a)

118

b)

116

c)

100

d)

132

e)

264

24.

calculate the percentage by mass of lead in Pb (NO3)2

a)

44.5

b)

62.6

c)

71.2

d)

38.6

e)

65.3

25.

one mole ____ contains the largest number of atoms

a)

S8

b)

Al2(SO4)3

c)

Na3PO4

d)

C10H8

e)

Cl2

26.

how many molecules of CH4 are in 48.2 g of this compound?

a)

4.00

b)

  1. 5.00 x 1024

c)

1.81 x 1024

d)

3.00

e)

2.90 x 1025

27.

a sample of CH2F2 with a mass of 19 g contains ___ atoms of F

a)

38

b)

2.2 x 1023

c)

3.3 x 1024

d)

9.5

e)

4.4 x 1023

28.

a sulfur oxide is 50.0% by mass sulfur. This molecular formula could be_______

a)

S2O

b)

SO

c)

S2O4

d)

SO2

e)

either SO2 or S2O4

29.

when the following equation is balanced, the coefficient of HNO3 is _____

HNO3 (aq) + CaCO3 (s) -> Ca(NO3)2 (aq) + CO2 (g) + H2O (I)

a)

2

b)

1

c)

4

d)

5

e)

3

30.

what is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass?

a)

K2SO4

b)

KSO2

c)

KSO4

d)

K2SO3

e)

KSO3

31.

the combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:

C3H8 (g) + 5O2 (g) -> 2CO2 (g) +4H2O (g)

when 2.5 mol of O2 are connected in their reaction, ______ mol of CO2 are produced

a)

2.5

b)

1.5

c)

6.0

d)

5.0

e)

3.0

32.

under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:

N2 (g) + 3H2 (g) -> 2NH3 (g)

a_____ g sample of N2 requires 3.0 g of H2 for complete reactions

a)

1.2

b)

0.51

c)

17.2

d)

0.76

e)

14.0

33.

the combustion of propane (C3H8) produces CO2 and H2O:

C3H8 (g) +5O2 -> 3CO2 (g) +4H2O (g)

the reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce ______mol of H2O

a)

4.0

b)

3.0

c)

2.5

d)

2.0

e)

1.0

34.

under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:

N2 (g) + 3H2 (g) -> 2NH3 (g)

if the reaction yield is 87.5%, how many moles of N2 are needed to produce 3.00 mol of NH3

a)

1.5

b)

2.32

c)

0.166

d)

1.71

e)

1.00

35.

the net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is ______

a)

Al(OH)3 (s) + 3NO3- (aq) -> 3OH- (aq) + Al(NO3)3 (aq)

b)

Al(OH)3 (s) + 3HNO3 (aq) -> 3H2O (I) + Al3+(aq)+ NO3- (aq)

c)

Al(OH)3 (s) + 3HNO3 (aq) -> 3H2O (I) + Al(NO3)3 (aq)

d)

Al(OH)3 (s) + 3NO3- (aq) -> 3OH- (aq) + Al(NO3)3 (s)

e)

Al(OH)3 (s) + 3H+ (aq) -> 3H2O (I) + Al3+ (aq)

36.

which of the following is insoluble in water at 25 ⁰C?

a)

Ba(C2H3O2)2

b)

(NH4)2CO3

c)

Na2S

d)

Mg3(PO4)2

e)

Ca(OH)2

37.

which compound has the atom with the highest oxidation number?

a)

NH4Cl

b)

CaS

c)

MgSO3

d)

AL(NO2)3

e)

Ma3N

38.

a 0.100 M solution _____ will contain the highest concentration of potassium ions

a)

potassium phosphate

b)

potassium hydrogen carbonate

c)

potassium oxide

d)

potassium iodide

e)

potassium hypochlorite

39.

what volume (mL) of a concentrated solution hydrogen (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?

a)

26.4

b)

176

c)

2.64

d)

50.0

e)

29.3

40.

which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

a)

10.0 mL of 0.0500 M perchloric acid

b)

15.0 mL of 0.0500 M hydrobromic acid

c)

10.0 mL of 0.0500 M phosphoric acid

d)

20.0 mL of 0.0500 M nitric acid

e)

5.0 mL of 0.0100 M sulfuric acid

41.

__________ is an oxidation reaction

a)

table salt dissolving in water for cooking vegetables

b)

rusting of iron

c)

neutralization of HCl by NaOH

d)

the reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate

e)

ice melting in a soft drink

42.

what are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?

a)

K+ and NO3-

b)

Ag+ and Cl-

c)

K+ only

d)

K+ and Ag+

e)

Ag+ and NO3-

43.

which one of the following is an exothermic process?

a)

water evaporating

b)

ice melting

c)

boiling soup

d)

condensation of water vapor

e)

ammonium thiocyanate and barium hydroxide are mixed at 25 ⁰C: the temperature drops

44.

for which one of the following reactions is ΔH⁰rxn equal to the heat of formation of the product?

a)

12C (g) + 11H2 (g) +11O (g) -> C6H22O11 (g)

b)

6C (s) +6H (g) -> C6H6 (I)

c)

(1/2)N2 (g) + O2 (g) -> NO2 (g)

d)

N2 (g) + 3H2 (g) -> 2NH3 (g)

e)

P (g) +4H (g) + Br (g) -> PH4Br (I)

45.

consider the following two reactions:

A -> 2B Δ⁰rxn= 456.7 kj/mol

A -> C Δ⁰rxn= -22.1kj/mol

determine the enthalpy change for the process:

2B -> C

a)

478.8 kj/mol

b)

-478.8 kj/mol

c)

-434.6 kj/mol

d)

434.6 kj/mol

46.

the value of ΔH⁰ for the reaction below is -790 kj. The enthalpy change accompanying the reaction of 0.95 g of S is _______kj

2S (s) + 3O2 (g) -> 2SO3 (g)

a)

-790

b)

-23

c)

12

d)

-12

e)

23

47.

given the data in the table below, ΔH⁰rxn for the reaction

Ca(OH)2 + 2H3AsO4 -> Ca(H2AsO4)2 + 2H2O

is ________kj

a)

-4519

b)

-744.9

c)

-130.4

d)

-4219

e)

-76.4

48.

a sample of iron absorbs 81.0 j of heat, upon which temperature of the sample increases from 19.7 ⁰C to 28.2 ⁰C. If the specific heat of iron is 0.450 j/g-K, what is the mass (in grams) of the sample?

a)

4.29 g

b)

-21.2 g

c)

0.0472 g

d)

3.83 g

e)

21.2 g

49.

which of the following is not a valid set of quantum numbers? (n,l,ml,ms)

a)

3,1,-1,-1/2

b)

1,1,0,+1/2

c)

2,0,0,+1/2

d)

1,0,0,+1/2

e)

2,1,0,-1/2

50.

the ground state electron configuration of Ga is_______.

a)

1s22s22p63s23p64s23d104d1

b)

1s22s22p63s23p64s23d104p1

c)

1s22s22p63s23p64s24d104p1

d)

[Ar]4s23d11

e)

1s22s23s23p64s23d104p1

51.

the ground-state electron configuration of the element _______is [Kr}5s14d5

a)

Mn

b)

Tc

c)

Nb

d)

Mo

e)

Cr

52.

the ground-state configuration of fluorine is ________

a)

[He]2s22p4

b)

[He]2s22p3

c)

[He]2s22p2

d)

[He]2s22p6

e)

[He]2s22p5

53.

of the following, which gives the correct order for atomic radius fir Mg, Na, P, Si, and Ar?

a)

Mg>Na>P>Si>Ar

b)

Ar>Si>P>Na>Mg

c)

Si>P>Ar>Na>Mg

d)

Ar>P>Si>Mg>Na

e)

Ba>Mg>Si>P>Ar

54.

Na reacts with element X to form an ionic compound with formula ZNa3X. Ca will react with X to form ________

a)

Ca2X3

b)

Ca3X2

c)

CaX2

d)

CaX

e)

Ca3X

55.

which of the following has the largest second ionization energy?

a)

Si

b)

P

c)

Al

d)

Na

e)

Mg

56.

in the ionic bond formation, the lattice energy of ions _______as the magnitude of the ion charges ________and the radii__________

a)

increases, increases, decreases

b)

increases, decreases, decreases

c)

increases, increases, increases

d)

increases, deceases, increases

e)

decreases, increases, increases

57.

in which of the molecules below in the carbon-carbon distance the shortest

a)

H-C=C-H

b)

H3C-CH2-CH3

c)

H3C-CH3

d)

H2C=C=CH2

e)

H2C=CH2

58.

given the electronegativities below, which covalent single bond is most polar?

elements: H C N O

electronegativity: 2.1 2.5 3.0 3.5

a)

O-H

b)

O-N

c)

O-C

d)

C-H

e)

N-H

59.

a valid Lewis structure of ______cannot be drawn without violating the octet rule

a)

SbF3

b)

PF3

c)

IF3

d)

SO42-

e)

NF3

60.

the ion PO43- has ____valence electrons

a)

27

b)

29

c)

32

d)

14

e)

24

61.

how many equivalent resonance structures can be drawn for the molecules of SO3 without having to violate the octet rule on the sulfur atom?

a)

2

b)

3

c)

4

d)

5

e)

1

62.

using the table of average bond energies below, the ΔH for the reaction is ______kJ

H-C=C-H (g) + H-I (g) -> H2C=CHI (g)

a)

-129

b)

-506

c)

-931

d)

+129

e)

+506

63.

of the following species ______will have bond angles of 120⁰

a)

BCl3

b)

PH3

c)

NCl3

d)

ClF3

e)

all of these will have bond angle of 120⁰

64.

PCl5 has _______electron domains and a _______molecular arrangement

a)

5, square pyramidal

b)

5, trigonal bipyramidal

c)

6, trigonal bipyramidal

d)

6, tetrahedral

e)

6, seesaw

65.

of the following molecules, only ________is polar

a)

CBr4

b)

BeCl2

c)

SiH2Cl2

d)

BF3

e)

Cl2

66.

the Sp3d2 atomic hybrid orbital set accommodates _____electron domains

a)

2

b)

3

c)

4

d)

5

e)

6

67.

there are _______σ bonds and ______π bonds in:

a)

14,2

b)

12,2

c)

16,3

d)

13,2

e)

10,3

68.

the volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62 ⁰C. The gas is ________

a)

SO3

b)

SO2

c)

Ne

d)

NH3

e)

NO2

69.

of the following gases, _______will have the greatest rate if effusion at any given temperature

a)

HCl

b)

HBr

c)

NH3

d)

CH4

e)

Ar

70.

at the temperature of ________ ⁰C, 0444 mol of CO gas occupies 11.8L at 839 torr

a)

32.0

b)

83.5

c)

14.0

d)

379

e)

73.0

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