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Unit 8 - Thou Shalt Not Forget AP Chemistry

Total questions: 75

Worksheet time: 35mins

Name
Class
Date
1.
What is the the shape of this molecule according to VSPER theory?
a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
2.

Draw the Lewis Dot structure for PCl5 and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

3.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
4.

Filtering separates mixtures based on differences in what property?

a)

Chemical

b)

Solubility

c)

Particle size

d)

Density

5.

What is the equation for calculating the density of a substance?

a)

D=m/v

b)

m=D/v

c)

D=v*m

d)

D=v/m

6.

When an electron is in a lower energy level, it is ________________ away from the nucleus

a)

Closer

b)

Farther

7.

Isotopes of an element have the same number of __________, but different number of __________.

a)

protons, neutrons

b)

neutrons, protons

c)

protons, electrons

d)

electrons, protons

8.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

9.

What type of change conserves mass?

a)

none

b)

chemical

c)

physical

d)

chemical and physical

10.

When an electron is in a higher energy level, it has ___________ Coulombic attraction to the nucleus

a)

More

b)

Less

11.

What is the measurement of the burette? (in mL)

a)

6.6mL

b)

6.64mL

c)

7.36mL

d)

7.3mL

12.

Which orbital comes after 4s?

a)

3d

b)

5s

c)

4p

d)

4d

13.

Are cations larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

14.

Which piece of glassware is the most precise

a)

beaker

b)

graduated cylinder

c)

burette

d)

test tube

15.

Moving across a row (L to R) on the periodic table, effective nuclear charge, Zeff _________________

a)

Increases

b)

Decreases

c)

Stays the same

16.

What type of change separates a compound into elements?

a)

physical

b)

chemical

c)

chemical and physical

17.

Why do atoms get smaller moving across a period (L to R) on the periodic table?

a)

More protons (q) to attract the electrons

b)

Fewer protons (q) to attract the electrons

c)

More energy shells (r) so it can't attract the electrons

d)

Fewer energy shells (r) so it attracts the electrons closer

18.

Why are anions larger than their neutral atoms?

a)

More electrons that repels each other

b)

Fewer protons to attract electrons

c)

More electrons to attract protons

d)

More Zeff to attract electrons

19.

Which piece of glassware is the least precise?

a)

graduated cylinder

b)

beaker

c)

burette

20.

When an electron is in a lower energy level, it has a ________________ 1st ionization energy

a)

Higher

b)

Lower

c)

Same

21.

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

a)

12

b)

6

c)

4

d)

8

22.

What do mass spectroscopy graphs measure?

a)

Mass of isotopes

b)

Mass of protons

c)

Energy of electrons

d)

Number of electrons

23.

Which orbital comes after 4p?

a)

5s

b)

4s

c)

3d

d)

4p

24.

What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

109.5

25.

Fill in the blanks germanium is a ________________, hydrogen is a _________________ and uranium is a ________________

a)

metal, non-metal, metalloid

b)

metalloid, non-metal, metal

c)

non-metal, metal, metalloid

26.

Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

27.

List the 3 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding

d)

dipole dipole, hydrogen bonding, london dispersion

28.

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

29.

Are anions larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

30.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

31.

P and V are ___________________ related?

a)

inversely

b)

directly

32.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

33.

When an electron is in a lower energy level, it has a ___________ 1st ionization energy

a)

Higher

b)

Lower

34.

Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

35.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

36.

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

a)

Intermolecular

b)

Intramolecular

37.

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

a)

interstitial

b)

substitutional

38.

This is a representation of a hydrogen bond.

a)

True

b)

False

39.

This is a representation of a hydrogen bond.

a)

True

b)

False

40.

Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

41.

What is the formula for calculating % yield?

a)

actual/theoretical *100

b)

theoretical/actual *100

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.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

44.

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

a)

increases

b)

decreases

45.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

46.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

47.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

48.

What is the electron configuration of Phosphorus?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 4p3

d)

1s2 2s2 2p6 3s2 3p5

49.

1.What type of reaction is this?

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

a)

Single Displacement

b)

Decomposition

c)

Double Displacement

d)

Combustion

50.

Losing electrons is ________________, gaining electrons is ________________

a)

oxidation, reduction

b)

reduction, oxidation

51.

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

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

52.

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

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

53.

Freezing is an _________________________ process

a)

Endothermic

b)

Exothermic

54.

Vaporizing is an _________________________ process

a)

Endothermic

b)

Exothermic

55.

What are the coefficients?

a)

1; 2; 1; 2

b)

2; 1; 2; 1

c)

4; 2; 1; 4

d)

1; 4; 2; 2

56.

ΔHrxn = ΔH_________________ − ΔH_________________

a)

products, reactants

b)

reactants, products

57.

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

a)

Stay the same

b)

Double

c)

Quadruple

d)

Halve

58.

This reaction is ____________________ because energy is _____________

a)

endothemic, absorbed

b)

exothermic, released

c)

endothermic, absorbed

d)

endothermic, released

59.

There are two Carbon(graphite) in the final equation. We should ________ the ΔH of the first sub-reaction.

a)

Double

b)

Halve

c)

Take the inverse of

d)

Reverse the sign of

60.

We need to reverse one of the equations.

a)

True

b)

False

61.

Heat is measure in K or °C

a)

True

b)

False

62.

What are the units of ΔHrxn?

a)

kJ

b)

J

c)

kJ/mol

d)

J/mol

63.

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

a)

The same

b)

Not the same

64.

A system at equilibrium

a)

Must have reactants and products

b)

Must have products only

c)

Must have reactants only

65.

At equilibrium, concentrations of reactants and products are

a)

equal

b)

constant

66.

At what time does the system first reach equilibrium?

a)

24s

b)

40s

c)

60s

d)

80s

67.

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}  

68.

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

a)

NaCl(s)

b)

NaCl(aq)

c)

NaCl(l)

d)

NaCl(g)

69.

If a K value is greater than 1,

a)

more products are present at equilibrium

b)

more reactants are present at equilibrium

70.

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

a)

reverse direction to reach equilibrium

b)

forward direction to reach equilibrium

71.

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

72.

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

73.

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

74.

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

75.

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

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