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AP Chem ST Unit 0-4

Total questions: 98

Worksheet time: 16hrs 20mins

Name
Class
Date
1.

What is a titration?

a)

when the moles of hydrogen ions is equal to the moles of hydroxide ions

b)

adding a known amount of solution of known concentration to determine the concentration of an unknown

c)

reaction in which an acid and a base react in an aqueous solution to produce a salt and water

d)

the extent of ionization of an acid or base

2.
In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
3.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
4.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
5.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
6.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

7.
Neutralization reactions
a)
formed from joining positive and negative ions 
b)
increases OH ions
c)
froms a salt and water
d)
increases H2O ions
8.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
9.
Is calcium oxidized or reduced in the following reaction? 
2 CaO--> 2 Ca + O2
a)
Oxidized
b)
Reduced
10.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
11.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
12.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

13.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
14.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
15.

In the equation below, what is the Bronsted Lowry base (accepts H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

16.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
17.

30mL of NaOH is neutralised by 12.3mL of 0.2mol/l HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

18.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
19.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
20.
If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of sulfuric acid, what is the concentration of the acid?
a)
0.2 M
b)
5 M
c)
0.5 M
21.

Which element is represented by this PES graph?

a)

argon

b)

potassium

c)

calcium

d)

scandium

22.

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum?

a)

Nitrogen atoms have a half-filled p subshell.

b)

There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.

c)

Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p sub shell of nitrogen atoms.

d)

Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

23.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
24.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
25.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
26.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
27.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
28.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
29.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
30.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

31.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
32.
EF = CF2 
Molecular formula mass = 192
MF =
a)
C4F8
b)
C4F
c)
CF8
d)
C2F4
33.

What is the charge of a proton?

a)

Negative

b)

Positive

c)

Neutral

34.

What is the center of an atom containing protons and neutrons?

a)

nucleus

b)

neutron

c)

proton

d)

electron cloud

35.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
36.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

37.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

38.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

39.
How many protons are in Cadmium?
a)
112.411
b)
170
c)
64
d)
48
40.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

41.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
42.

The Lewis structure of N2H2 shows __________.

a)

a nitrogen-nitrogen triple bond

b)

a nitrogen-nitrogen single bond

c)

each nitrogen has one lone pair

d)

each nitrogen has two lone pairs

e)

each hydrogen has one lone pair

43.

In the nitrite ion (NO2-), __________.

a)

both bonds are single bonds

b)

both bonds are double bonds

c)

both bonds are the same because of resonance

d)

there are 20 valence electrons

e)

there is one single and one double bond

44.

The ability of an atom in a molecule to attract electrons is best quantified by the ______.

a)

electronegativity

b)

paramagnetism

c)

diamagnetism

d)

electron change-to-mass ratio

e)

first ionization energy

45.

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

46.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

47.

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

48.

Bond enthalpy is __________.

a)

always negative

b)

always positive

c)

sometimes positive and sometimes negative

d)

always zero

e)

unpredictable

49.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

50.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
51.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

52.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

53.

Potassium iodide, KI,has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

54.

The formal charge on carbon in the molecule shown is _______.

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

55.

Choose the correct shape for H2S

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

56.
The electronegativity of C is 2.5, F is 4.0.  predict the character of a C-F bond.
a)
polar covalent
b)
nonpolar covalent
c)
ionic
d)
metallic
57.
The following molecules all contain polar bonds however only one is a polar molecule.  Which one?
a)
CCl4
b)
CO2
c)
NH3
d)
CH4
58.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
59.
How are compounds with metallic bonds similar to ionic compounds? 
a)
Both tend to have double and triple bonds
b)
Both tend to have low boiling points 
c)
Both tend to have poor conductivity
d)
Both tend to have high melting points 
60.
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .
a)
eg = tetrahedral, mg = tetrahedral
b)
eg = linear, mg = linear
c)
eg = octahedral, mg = square planar
d)
eg = trigonal bipyramidal, mg = tetrahedral
61.

How many sigma and pi bonds are there in C2H2? (the structure will be ordered HCCH)

a)

1 sigma and 1 pi

b)

3 sigma and 1 pi

c)

3 sigma and 2 pi

d)

2 sigma and 3 pi

62.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
63.
The interaction energy of two hydrogen atoms is shown on the graph above. Which of the answer choices displayed on the graph best represents the bond length of the H2 molecule?
a)
A
b)
B
c)
C
d)
D
64.
Of the following molecules, which has the largest dipole moment?
a)
CO
b)
CO2
c)
O2
d)
HF
65.
CCl4, CO2, PCl3, PCl5, SF6
Which of the following does not describe any of the molecules above?
a)
Trigonal pyramidal
b)
Octahedral
c)
Square planar
d)
Tetrahedral
66.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
67.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

68.

In paper chromatography, if water is the mobile phase, what kind of substance will move up the farthest?

a)

polar substance

b)

non polar substance

69.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

70.

List the 4 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, ion-dipole, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, ion-dipole, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding, ion-dipole

d)

dipole dipole, hydrogen bonding, ion-dipole, london dispersion

71.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

72.

List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

73.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

74.

The dotted line is a representation of a hydrogen bond.

a)

True

b)

False

75.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

76.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

77.

What type of solid will not conduct electricity until it is liquid or aqueous?

a)

Ionic Solid

b)

Covalent Network Solid

c)

Molecular Solid

d)

Metallic Solid

78.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

79.

What type of solid always conducts electricity?

a)

Ionic Solid

b)

Metallic Solid

c)

Covalent Network Solid

d)

Molecular Solid

80.

When a molecular solid melts or boils, which bonds break?

a)

Intermolecular

b)

Intramolecular

81.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

82.

What type of alloy is made when the radii of one element are similar in size with the other element making up the alloy?

a)

interstitial

b)

substitutional

83.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

84.

P and V are ___________________ related?

a)

inversely

b)

directly

85.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

86.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

87.

Real gases behave most like an ideal gas at what conditions of temperature and pressure?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

88.

Compounds can be separated into elements by ______.

a)

chemical changes

b)

physical changes

c)

paper chromatography

89.

_______ separates mixtures based on differences in particle size.

a)

filtering

b)

distillation

c)

chromatography

90.

_______ separates mixtures based on differences in boiling point.

a)

filtering

b)

distillation

c)

chromatography

91.

_______ separates mixtures based on differences in polarity.

a)

filtering

b)

distillation

c)

chromatography

92.

Which type of change conserves masss?

a)

chemical

b)

physical

c)

both

d)

neither

93.

Rank the following from least precise to most precise.

a)

beaker

b)

graduated cylinder

c)

volumetric flask

d)

burette

1)
2)
3)
4)
94.

density =

a)

mass * volume

b)

mass / volume

c)

volume / mass

95.

The simplest whole # ratio of the atoms in a compound is called the

a)

molecular formula

b)

empirical formula

c)

density

d)

percent yield

96.

Percent yield =

a)

experimental / theoretical

b)

theoretical / experimental

c)

theoretical * experimental

97.

Percent error =

a)

(experimental - theoretical) / theoretical

b)

(experimental + theoretical) / theoretical

c)

(experimental - theoretical) * theoretical

d)

(experimental * theoretical) / theoretical

98.

The amount of product for a reaction is determined by the...

a)

limiting reactant

b)

percent error

c)

molecular formula

d)

excess reactant

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