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AP Chemistry Unit 1 Thou Shall Not Forget

Total questions: 112

Worksheet time: 56mins

Name
Class
Date
1.

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

a)

interstitial

b)

substitutional

2.

Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

3.

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

4.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

5.

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

a)

increases

b)

decreases

6.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

7.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

8.

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

a)

12

b)

6

c)

4

d)

8

9.

What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

10.

What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

104.5

11.

Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

12.

What is the bond angle in NH3

a)

120

b)

107.3

c)

180

d)

90

13.

What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

14.

What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

15.

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

16.

Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

17.

What is the hybridization for an oxygen in CO2

a)

sp3

b)

sp

c)

sp2

18.

When a molecular solid melts or boils, which breaks?

a)

Intermolecular forces

b)

Intramolecular bonds

19.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
20.

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

a)

12

b)

6

c)

4

d)

8

21.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

22.

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

23.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

24.

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

25.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

26.

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

27.

The dashed line is a representation of a hydrogen bond.

a)

True

b)

False

28.

The dotted line is a representation of a hydrogen bond.

a)

True

b)

False

29.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

30.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

31.

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

32.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

33.

What type of solid always conducts electricity?

a)

Ionic Solid

b)

Metallic Solid

c)

Covalent Network Solid

d)

Molecular Solid

34.

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

a)

Intermolecular

b)

Intramolecular

35.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

36.

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

37.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

38.

P and V are ___________________ related?

a)

inversely

b)

directly

39.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

40.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

41.

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

42.

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

43.

What is the formula for calculating % yield?

a)

actual/theoretical *100

b)

theoretical/actual *100

44.

1.What type of reaction is this?

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

a)

Single Displacement

b)

Decomposition

c)

Double Displacement

d)

Combustion

45.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

46.

Acids

a)

donate electrons

b)

donate protons

c)

accept protons

d)

donate protons

47.

Bases

a)

donate electrons

b)

accept electrons

c)

donate protons

d)

accept protons

48.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

49.

Losing electrons is ________________, gaining electrons is ________________

a)

oxidation, reduction

b)

reduction, oxidation

50.

What is the oxidation number of N in NO21-?

a)

0

b)

-1

c)

2

d)

3

51.

What is the oxidation number of P in PO43-?

a)

0

b)

4

c)

5

d)

-2

52.

Chose the salts that are soluble:

a)

sodium

b)

potassium

c)

nitrates

d)

ammonium

53.

The ______ the acid, the ______ its conjugate base.

a)

stronger, weaker

b)

stronger, stronger

54.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

55.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

56.

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

a)

zero

b)

first

c)

second

57.

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

a)

True

b)

False

58.

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

59.

What order is the half life of Carbon14?

a)

Zero

b)

First

c)

Second

60.

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

a)

s-1

b)

M/s

c)

M-1s-1

61.

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

62.

___________ 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

63.

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

a)

Faster

b)

Slower

64.

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

65.

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]

66.

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]

67.

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]

68.

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

69.

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

70.

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

71.

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

72.

In an exothermic reaction, the sign of ΔH is ____ and the reaction feels ______

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

73.

Freezing is an _________________________ process

a)

Endothermic

b)

Exothermic

74.

Vaporizing is an _________________________ process

a)

Endothermic

b)

Exothermic

75.

Breaking bonds is _________________. Forming bonds is ______________________

a)

endothermic, exothermic

b)

exothermic, endothermic

76.

ΔHrxn = ΔH_________________ − ΔH_________________

a)

products, reactants

b)

reactants, products

77.

If a reaction is exothermic, then the bonds formed in the products are ___________________ than the reactant bonds.

a)

stronger/more stable

b)

weaker/less stable

78.

If a reaction is endothermic, then the bonds formed in the products are ___________________ than the reactant bonds.

a)

stronger/more stable

b)

weaker/less stable

79.

According to Hess' Law, if you double the coefficients of a reaction, ΔH will ________________________

a)

Stay the same

b)

Double

c)

Quadruple

d)

Halve

80.

According to Hess' Law, if you reverse a reaction, ΔH will ________________________

a)

Change signs

b)

Double

c)

Be inversed

d)

Halve

81.

_____ Hydrogen-Hydrogen single bond/s are broken and _____ Carbon-Hydrogen single bond/s formed

a)

6; 8

b)

2; 8

c)

2; 10

d)

6; 10

82.

_____ Carbon-Carbon single bond/s are formed

a)

6

b)

2

c)

3

d)

10

83.

Bond enthalpy is the amount of energy is takes to break __________ of a bond.

a)

one mole

b)

one gram

c)

the activation energy

d)

the binding energy

84.

What are the units of ΔHrxn?

a)

kJ

b)

J

c)

kJ/mol

d)

J/mol

85.

Endothermic

a)

absorb energy

b)

release energy

86.

Exothermic

a)

absorb energy

b)

release energy

87.

In the dissolution process, the increase in separation between ions in the solute is

a)

endothermic

b)

exothermic

88.

In a system, the energy lost by the reacting species must be ________________ the energy gained by the surrouding

a)

greater than

b)

less than

c)

equal to

89.

On a potential energy diagram for an endothermic reaction,

a)

the potential energy of the reactants is greater than the potential energy of the products

b)

the potential energy of the reactants is less than the potential energy of the products

c)

the potential energy of the reactants is equal to the potential energy of the products

90.

A temperature is placed in a calorimeter. A solid is dissolved in water in the calorimeter and the temperature of the thermometer increases. The dissolution reaction must be

a)

endothermic

b)

exothermic

91.

Using bond energies to solve for enthalpy, 

a)

ΔH\Delta H  =  Bond broken - bonds formed

b)

 \Delta H  =  Bond formed- bonds broken

c)

 \Delta H  =  products - reactants

d)

 \Delta H  =  reactants- products

92.

The enthalpy of formation for a lone element is

a)

a number

b)

zero

93.

At equilibrium, rates of the forward and reverse reaction are...

a)

The same

b)

Not the same

94.

A system at equilibrium

a)

Must have reactants and products

b)

Must have products only

c)

Must have reactants only

95.

At equilibrium, concentrations of reactants and products are

a)

equal

b)

constant

96.

At what time does the system first reach equilibrium?

a)

24s

b)

40s

c)

60s

d)

80s

97.

The equilibrium constant expression, Kc, given aA + bB ⇄ cC + dD, is...

a)

Kc = [C]c[D]d[A]a[B]bK_c\ =\ \frac{\left[C\right]^c\left[D\right]^d}{\left[A\right]^a\left[B\right]^b}  

b)

Kc = [A]a[B]b[C]c[D]dK_c\ =\ \frac{\left[A\right]^a\left[B\right]^b}{\left[C\right]^c\left[D\right]^d}  

98.

Which substance(s) would not be included in a equilibrium constant expression?

a)

NaCl(s)

b)

NaCl(aq)

c)

NaCl(l)

d)

NaCl(g)

99.

If a K value is greater than 1,

a)

more products are present at equilibrium

b)

more reactants are present at equilibrium

100.

If a K value is VERY large,

a)

the reaction has essentially gone to completion

b)

there are more reactants present at equilibrium

101.

If K < Q, the reaction will proceed in the...

a)

reverse direction to reach equilibrium

b)

forward direction to reach equilibrium

102.

When a reaction at equilibrium is reversed,

a)

the K value's sign is flipped

b)

the K value is divided by 2

c)

the K value is inverted

103.

To calculate the K of an overall reaction from individual reaction K values, the individual K values are

a)

added

b)

subtracted

c)

multiplied

d)

divided

104.

When the coefficient of a reaction is multiplied by a factor x,

a)

the K value is multipled by x

b)

the K value is divided by x

c)

the K value is raised to the power x

105.

Given the following equilibrium equation,

A (g) + 2B (g) ⇄ AB2 (g) ΔH > 0, which of the following changes will increase the amount of AB2 in the vessel?

a)

Decreasing the temperature

b)

Increasing the concentration of A

c)

Removing a small amount of B

d)

Decreasing the pressure

106.

Given the following equilibrium equation,

A (g) + 2B (g) ⇄ AB2 (g) ΔH < 0, which of the following changes will decrease the amount of AB2 in the vessel?

a)

Increasing the temperature

b)

Increasing the concentration of A

c)

Increasing the pressure

d)

Adding a catalyst

107.

The following system at equilibrium is exothermic. If the temperature is increased...

A (g) + 2B (g) ⇄ AB2 (g)

a)

[A] will increase the most

b)

[B] will increase the most

c)

[AB2] will increase the most

108.

For an exothermic system at equilibrium, if the temperature is increased, the equilibrium will shift towards the...

a)

reactants

b)

products

109.

For an endothermic system at equilibrium, if the temperature is decreased, the equilibrium will shift towards the...

a)

reactants

b)

products

110.

In a Ksp expression, we always assume that the reactant is made up of

a)

the solid precipitate

b)

the aqueous ions

111.

If Ksp >1, we say the salt is...

a)

soluble

b)

insoluble

112.

If a common ion is present, the solubility of a salt

a)

is increased

b)

is decreased

c)

will remain the same

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