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AP Chemistry Midterm Practice

Total questions: 143

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

Which has a larger atomic radius?

a)

Both same

b)

K

c)

Ca

d)

Cannot determine

2.

What happens to ionization energy moving across period 2?

a)

Random

b)

Stays the same

c)

Decreases

d)

Increases

3.

An element has 60% isotope A (10 amu) and 40% isotope B (12 amu). Average atomic mass?

a)

10.0 amu

b)

12.0 amu

c)

11.2 amu

d)

10.8 amu

4.

Which element has the highest electronegativity?

a)

K

b)

Na

c)

Li

d)

F

5.

How many protons, neutrons, and electrons are in Se-80?

a)

34 p, 46 n, 34 e

b)

34 p, 46 n, 36 e

c)

34 p, 46 n, 35 e

d)

35 p, 45 n, 34 e

6.

Which molecule is nonpolar despite polar bonds?

a)

H2O

b)

HF

c)

NH3

d)

CO2

7.

Draw Lewis structures for H2O and NH3; identify bond angles.

a)

180°, 107°

b)

90°, 120°

c)

109.5°, 120°

d)

104°, 107°

8.

A compound contains 40 g C, 6.7 g H, 53.3 g O. Empirical formula?

a)

CHO

b)

C4HO

c)

CH2O

d)

C4H2O2

9.

Which type of bond involves electron sharing?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Hydrogen

10.

Which is a property of ionic compounds?

a)

Nonpolar

b)

Soft solids

c)

Poor conductor when melted

d)

High melting point

11.

Which has the strongest hydrogen bonding?

a)

CH4

b)

NH3

c)

HF

d)

H2O

12.

Explain why I2 has a higher boiling point than Cl2.

a)

Cl2 is ionic

b)

I2 has stronger London dispersion

c)

I2 is polar

d)

Cl2 is heavier

13.

A 20 g sample occupies 25 mL. Calculate density.

a)

1.25 g/mL

b)

0.80 g/mL

c)

0.60 g/mL

d)

0.50 g/mL

14.

Which IMF is weakest?

a)

Ionic

b)

Dipole-dipole

c)

London dispersion

d)

Hydrogen bonding

15.

Which molecule has dipole-dipole interactions?

a)

HCl

b)

CH4

c)

Ne

d)

O2

16.

Identify oxidation and reduction in 2Al + 3Br2 → 2AlBr3.

a)

Al reduced, Br2 oxidized

b)

Both oxidized

c)

Both reduced

d)

Al oxidized, Br2 reduced

17.

Predict products of Zn + HCl → ?

a)

ZnCl2 + H2

b)

Zn + Cl2 + H2

c)

ZnH + Cl2

d)

ZnCl + H2O

18.

If 5.0 g Na reacts with water, moles of H2 gas?

a)

0.109 mol

b)

0.217 mol

c)

0.054 mol

d)

0.500 mol

19.

Which is a single replacement reaction?

a)

BaCl2 + Na2SO4 → BaSO4 + 2NaCl

b)

H2 + O2 → H2O

c)

Zn + CuSO4 → ZnSO4 + Cu

d)

2Na + Cl2 → 2NaCl

20.

Spectator ions are:

a)

Catalysts

b)

Oxidized

c)

Reduced

d)

Not involved in reaction

21.

Which factor increases reaction rate?

a)

Smaller surface area

b)

Higher temperature

c)

Less concentration

d)

Lower temperature

22.

Reaction is first order in A; if [A] doubles, rate?

a)

Doubles

b)

Quadruples

c)

Stays same

d)

Halves

23.

Rate = k[A][B]; if [A] and [B] double, how much does rate change?

a)

2×

b)

8×

c)

4×

d)

1×

24.

For 2NO2→2NO+O2, if rate of NO2 consumption = 0.50 M/s, moles O2 in 2 s?

a)

0.75 mol

b)

0.25 mol

c)

1.0 mol

d)

0.50 mol

25.

Catalyst affects reaction by:

a)

Raising activation energy

b)

Lowering activation energy

c)

Being consumed

d)

Changing ΔH

26.

Which element is most likely to form a cation?

a)

F

b)

Na

c)

O

d)

Cl

27.

How many valence electrons does oxygen have?

a)

8

b)

6

c)

4

d)

2

28.

Empirical formula of a compound with 70% Fe and 30% O?

a)

Fe3O4

b)

FeO2

c)

FeO

d)

Fe2O3

29.

Average atomic mass of 75% X (12 amu) and 25% Y (16 amu)?

a)

15 amu

b)

13 amu

c)

14 amu

d)

12 amu

30.

Density of 10 g sample occupying 4 mL?

a)

6 g/mL

b)

2.5 g/mL

c)

14 g/mL

d)

0.4 g/mL

31.

Mole ratio in 2H2+O2→2H2O for H:O?

a)

1:1

b)

2:2

c)

2:1

d)

1:2

32.

Which is a combustion reaction?

a)

Zn + HCl → ZnCl2 + H2

b)

C4H10 + O2 → CO2 + H2O

c)

HCl + NaOH → NaCl + H2O

d)

AgNO3 + NaCl → AgCl + NaNO3

33.

Which bond is polar covalent?

a)

O=O

b)

N≡N

c)

H–H

d)

H–Cl

34.

Electron configuration of Ca?

a)

1s2 2s2 2p6 3s2 3p6 4p2

b)

1s2 2s2 2p6 3s2 3p4

c)

1s2 2s2 2p6 3s2 3p6 3d2

d)

1s2 2s2 2p6 3s2 3p6 4s2

35.

Maximum electrons in n=3?

a)

32

b)

18

c)

16

d)

8

36.

Identify IMF in CH3OH?

a)

Dipole–dipole

b)

Ionic

c)

Hydrogen bonding

d)

London dispersion

37.

Reaction rate increases when:

a)

Concentration increases

b)

Catalyst removed

c)

Temperature decreases

d)

Surface area decreases

38.

Which is a polar molecule?

a)

CH4

b)

Ne

c)

CO2

d)

H2O

39.

Oxidation state of S in H2SO4?

a)

+4

b)

+6

c)

0

d)

-2

40.

Which is an exothermic reaction?

a)

Evaporation

b)

Combustion of methane

c)

Boiling water

d)

Melting ice

41.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
42.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
43.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
44.

Which order is correct from largest to smallest atomic radius?

a)

Thallium, Indium, Gallium, Boron

b)

Boron, Thallium, Indium, Gallium

c)

Boron, Gallium, Indium, Thallium

d)

Thallium, Gallium, Indium, Boron

45.
Rank the following elements by increasing atomic radius:
carbon, aluminum, oxygen, phosphorus.
Not sure? check out page 151 in your textbook
a)
O, C, P, Al
b)
Al, P, C, O
c)
O,P, C, Al
d)
O, P, Al, C
46.

In the alkali metals, which element has a larger atomic radius?

a)

lithium, Li

b)

sodium, Na

c)

potassium, K

d)

cesium, Cs

47.

Looking at period 3, which element has the smallest atomic radius?

a)

Mg

b)

Cl

c)

Al

48.

Which of these halogens has the largest atomic radius?

a)

fluorine, F

b)

chlorine, Cl

c)

bromine, Br

d)

iodine, I

49.

Which atom would have the largest atomic radius?

a)

Potassium (K)

b)

Calcium (Ca)

c)

Selenium (Se)

d)

Bromine (Br)

50.

Which element has the smallest atomic radius?

a)

Lithium (Li)

b)

Francium (Fr)

c)

Fluorine (F)

d)

Radon (Rn)

51.

Which has the LARGER radius?

a)

F

b)

Br

52.
Which of the following statements is true about the atomic radii of magnesium and sulfur?
a)
Magnesium has a smaller atomic radius than sulfur
b)
Magnesium has a larger atomic radius than sulfur
c)
Magnesium has the same atomic radius as sulfur
53.

Which of the following has the greatest atomic radius?

a)

K

b)

Ca

c)

Zn

d)

Kr

54.

Use the image to determine which of the following choices has the largest atomic radius.

a)

Ne

b)

F

c)

N

d)

Be

55.

Which of the following has the greatest atomic radius?

a)

H

b)

Li

c)

K

d)

Na

56.

Which of the following has the greatest atomic radius?

a)

H

b)

Li

c)

K

d)

Na

57.

Atomic radius is the SIZE of an atom. Atomic radius __________ as we go ACROSS a periodic table and ___________ as we go DOWN a group

a)

Increases, Decreases

b)

Decreases, Increases

c)

Decreases, Stays the same

d)

Stays the same, Increases

58.

Atomic radius is the SIZE of an atom. Atomic radius __________ as we go ACROSS a periodic table and ___________ as we go DOWN a group

a)

Increases, Decreases

b)

Decreases, Increases

c)

Decreases, Stays the same

d)

Stays the same, Increases

59.

Which atom has the biggest Atomic Radius?

a)

Li

b)

Ba

c)

Br

d)

Rn

60.

What trend in atomic radius occurs across a period on the periodic table? 

a)

Increasing

b)

Decreasing

c)

Going to Space

d)

Random

61.

Why does sulfur have a smaller atomic radius than phosphorus?

a)

Sulfur has more protons and a more effective nuclear charge

b)

Sulfur has fewer protons and a less effective nuclear charge

c)

Sulfur has more occupied energy levels

d)

Sulfur has fewer occupied energy levels

62.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

63.
The average atomic mass rhenium, Re, is 186.21 amu. If 37.1% of rhenium has mass# = 185, what is the other stable isotope?
a)
Rhenium-183
b)
Rhenium-181
c)
Rhenium-187
d)
Rhenium-189
64.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
65.

A 5.00 g sample of a compound consisting of calcium and chlorine contains 1.82 g of calcium and 3.23 g of chlorine. What is the empirical formula?

a)

CaCl2

b)

Ca2Cl4

c)

Ca2Cl2

d)

Ca4Cl2

66.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

67.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
68.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
69.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
70.
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
71.
Which of the following properties uniquely identifies every element?
a)
Number of valence electrons
b)
Phase at room temperature
c)
Number of protons
d)
Charge of the atom
72.
Which element would have similar properties to Sulfur?
a)
Nitrogen
b)
Oxygen
c)
Flourine
d)
Chlorine
73.

What type of alloy is made when the radii of the atoms are similar in size?

a)

interstitial

b)

substitutional

74.

Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

75.

In this molecule, Carbon has a formal charge of ____ and Nitrogen has a formal charge of _____.

a)

0, 0

b)

1, 0

c)

0, -1

d)

-1, 0

76.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

77.

As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________

a)

increases

b)

decreases

78.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

79.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

80.

What is the total # of covalent bonds carbon can form when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

81.

What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

82.

What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

104.5

83.

Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

84.

What is the bond angle in NH3

a)

120

b)

107.3

c)

180

d)

90

85.

What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

86.

What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

87.

Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

88.

Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

89.

What is the hybridization for an oxygen in CO2

a)

sp3

b)

sp

c)

sp2

90.

When a molecular solid melts or boils, which breaks?

a)

Intermolecular forces

b)

Intramolecular bonds

91.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
92.

What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

93.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

94.

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

95.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

96.

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

97.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

98.

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

99.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

100.

The dotted line is a representation of a hydrogen bond.

a)

True

b)

False

101.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

102.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

103.

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

104.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

105.

What type of solid always conducts electricity?

a)

Ionic Solid

b)

Metallic Solid

c)

Covalent Network Solid

d)

Molecular Solid

106.

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

a)

Intermolecular

b)

Intramolecular

107.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

108.

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

109.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

110.

P and V are ___________________ related?

a)

inversely

b)

directly

111.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

112.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

113.

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

114.

What is a limiting reactant?

a)

The reactant that runs out first

b)

The reactant that has the lowest mass

c)

The reactant with the smallest coefficient

d)

The reactant with the lowest molar mass

115.

What is the formula for calculating % yield?

a)

actual/theoretical *100

b)

theoretical/actual *100

116.

1.What type of reaction is this?

3O2 + 2FeCl3 --> 2Fe2O3 + 3Cl2

a)

Single Displacement

b)

Decomposition

c)

Double Displacement

d)

Combustion

117.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

118.

Acids

a)

accept electrons

b)

donate electrons

c)

accept protons

d)

donate protons

119.

Bases

a)

donate electrons

b)

accept electrons

c)

donate protons

d)

accept protons

120.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

121.

Losing electrons is ________________, gaining electrons is ________________

a)

oxidation, reduction

b)

reduction, oxidation

122.

What is the oxidation number of N in NO21-?

a)

0

b)

-1

c)

2

d)

3

123.

What is the oxidation number of P in PO43-?

a)

0

b)

4

c)

5

d)

-2

124.

Chose the salts that are soluble:

a)

sodium

b)

potassium

c)

nitrates

d)

ammonium

125.

The ______ the acid, the ______ its conjugate base.

a)

stronger, weaker

b)

stronger, stronger

126.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

127.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

128.

If you quadruple the concentration and the rate quadruples, what order is this reaction?

a)

zero

b)

first

c)

second

129.

The particles under the purple curve (middle) have an average Kinetic Energy that is proportional to of 500K

a)

True

b)

False

130.

Which step of a reaction mechanism determines the rate?

a)

the slow step

b)

the fast step

c)

the first step

d)

the second step

131.

What order is the half life of Carbon14?

a)

Zero

b)

First

c)

Second

132.

What is the unit for the rate constant (k) for 2nd order reactions?

a)

s-1

b)

M/s

c)

M-1s-1

133.

How does a catalyst speed up a reaction?

a)

Adding more reactant

b)

Providing a pathway that has a lower activation energy

c)

Increasing the activation energy

d)

Increasing binding energy

134.

___________ are produced in one step and used up in a later step and __________________ are present and unchanged in the reactants and the products

a)

intermediates, catalysts

b)

catalysts, intermediates

135.

If a “reaction profile” has a taller ‘hill’ (or activation energy) then the reaction is ____________________?

a)

Faster

b)

Slower

136.

What are the 2 characteristics that an effective collision must have? SELECT TWO

a)

Enough energy to overcome Ea

b)

Molecules in the correct orientations

c)

High enough temperature

d)

Apporpriate intermediates present

137.

What is the rate law for the reaction with this slow elementary step? A + A --> B + B

a)

rate = k[A]2

b)

rate = k[B]2

c)

rate = k[A][B]

d)

rate = k[A]

138.

What is the rate law for the reaction with this slow elementary step? A --> B + C

a)

rate = k[A]2

b)

rate = k[B]2

c)

rate = k[A][B]

d)

rate = k[A]

139.

What is the rate law for the reaction with this slow elementary step? A + 2B --> D + C

a)

rate = k[A]2

b)

rate = k[A][B]2

c)

rate = k[A][B]

d)

rate = k[A]

140.

What is NOT a way to speed up a reaction

a)

Add a catalyst

b)

Decrease the volume

c)

Increase the concentration of reactants

d)

Increase surface area of the solid

e)

Decrease the pressure

141.

Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

They all have the same number of particles

142.

Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

All particles are moving at the same speed

143.

What order of reaction has a half-life that does not change regardless of the initial concentration?

a)

Zero

b)

First

c)

Second

d)

Third

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