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Secondary SummerAP Chem Topics

Total questions: 106

Worksheet time: 5hrs 1mins

Name
Class
Date
1.

What would be the pH of a solution with an [H+] of 0.001?

a)

3

b)

1

c)

-3

d)

-1

2.

What would be the pH of a solution with an [H+] of 0.010?

a)

2

b)

12

c)

-2

d)

0.98

3.

What would be the pOH of a solution with [H+] of 0.024?

a)

1.6

b)

-1.6

c)

12.4

d)

0.95

4.

What would be the pOH of a solution with [H+] of 0.00034?

a)

1.0

b)

-3.47

c)

10.53

d)

3.47

5.

What would be the pOH of a solution with [OH-] of 0.00054?

a)

3.26

b)

-3.26

c)

10.74

6.

What would be the pOH of a solution with [OH-] of 0.06?

a)

1.22

b)

-1.22

c)

12.78

d)

0.06

7.

What is the pH if the pOH is 5.3?

(a)  

8.

What is the pH if the pOH is 10.0?

(a)  

9.

What is the pOH if the pH is 11.0?

(a)  

10.

What is the [H+] if the pH is 6.5?

a)

3.16 x 107

b)

3.16 x 10-7

c)

8.13 x 10-1

11.

What is the [OH-] if the pH is 1.0?

a)

0.1

b)

0

c)

1 x 10-13

d)

13

12.

What is the [OH-] if the pOH is 8.2

a)

6.3 x 10-9

b)

1.6 x 108

c)

9.1 x 10-1

13.

What is the [OH-] if the [H+] is 8.5 x 10-4?

a)

3.07

b)

9.9 x 10-1

c)

1.2 x 10-11

14.

What is the pH if the [OH-] is 7.5 x 10-5?

a)

4.12

b)

9.88

c)

9.9 x 10-1

15.

What is the pH if the [OH-] is 1.3 x 10-3?

a)

11.1

b)

2.89

c)

9.9 x 10-1

16.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

polar covalent bonding

c)

London dispersion forces

d)

dipole-dipole interaction

17.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

18.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
19.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
20.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
21.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

22.

What kind of force is the arrow pointing to?

a)

Intramolecular Force

b)

Intermolecular Force

23.

What kind of force is the arrow pointing to?

a)

Intramolecular force

b)

Intermolecular force

24.

Which sample has hydrogen bonding?

a)

H2S

b)

CH4

c)

NH3

d)

HI

25.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
26.

What type of intermolecular forces do nonpolar molecules exhibit?

a)

Hydrogen bonding

b)

Dipole-dipole interactions

c)

Only London dispersion forces.

d)

Ionic bonding

27.

What type of intermolecular forces does a polar molecule exhibit?

a)

Hydrogen bonding and ionic interactions.

b)

Dipole-dipole interactions and London dispersion forces.

c)

Covalent bonding and metallic bonding.

d)

Van der Waals forces and hydrogen bonding.

28.

Define electronegativity.

a)

The ability of an atom to lose electrons easily.

b)

The tendency of an atom to attract shared electrons to itself.

c)

The measure of an atom's size in a molecule.

d)

The energy required to remove an electron from an atom.

29.

What is the relationship between molecular weight and London dispersion forces?

a)

London dispersion forces decrease with molecular weight.

b)

London dispersion forces remain constant regardless of molecular weight.

c)

London dispersion forces increase with molecular weight.

d)

London dispersion forces are unrelated to molecular weight.

30.

Which molecule has the strongest London forces: F2, Br2, I2, or Cl2?

a)

F2

b)

Br2

c)

I2

d)

Cl2

31.

Which of the following has the highest boiling point: H2, NH3, N2, or O2?

a)

H2

b)

N2

c)

O2

d)

NH3

32.

What is the difference between ionic bonding and covalent bonding?

a)

Ionic bonding involves the sharing of electrons, while covalent bonding involves the transfer of electrons.

b)

Ionic bonding involves the transfer of protons, while covalent bonding involves the sharing of neutrons.

c)

Ionic bonding involves the transfer of electrons, while covalent bonding involves the sharing of electrons.

d)

Ionic bonding occurs only in metals, while covalent bonding occurs only in non-metals.

33.

What is hydrogen bonding?

a)

A weak interaction between nonpolar molecules.

b)

A strong type of dipole-dipole interaction that occurs between molecules containing hydrogen bonded to highly electronegative atoms like N, O, or F.

c)

A type of covalent bond formed between hydrogen and carbon.

d)

An ionic bond formed between hydrogen and metals.

34.

What is the effect of intermolecular forces on boiling points?

a)

Stronger intermolecular forces result in higher boiling points.

b)

Weaker intermolecular forces result in higher boiling points.

c)

Intermolecular forces have no effect on boiling points.

d)

Stronger intermolecular forces result in lower boiling points.

35.

What are dipole-dipole interactions?

a)

Attractive forces between the positive end of one polar molecule and the negative end of another.

b)

Repulsive forces between two non-polar molecules.

c)

Attractive forces between two identical non-polar molecules.

d)

Interactions that occur between ions and polar molecules.

36.

What is the role of intermolecular forces in solubility?

a)

Intermolecular forces have no effect on solubility.

b)

Intermolecular forces determine how well substances dissolve in each other, with similar forces promoting solubility.

c)

Intermolecular forces only affect the boiling point of substances.

d)

Intermolecular forces are irrelevant in the context of solubility.

37.

How do intermolecular forces affect the state of matter?

a)

Stronger intermolecular forces generally lead to gases, while weaker forces lead to solids.

b)

Stronger intermolecular forces generally lead to liquids, while weaker forces lead to gases.

c)

Stronger intermolecular forces generally lead to solids, while weaker forces lead to gases.

d)

Intermolecular forces do not affect the state of matter.

38.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
39.

Hydrogen being an exception to the octet rule, needs _____ electrons in its outer energy level to be stable.

a)

4

b)

6

c)

8

d)

2

40.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
41.

Draw the lewis dot structure for F2. Which of the following is the correct Lewis dot structure for the molecule F2?

a)

A

b)

B

c)

C

d)

D

42.

How many electrons are shared in each bonding line?

a)

1

b)

2

c)

3

d)

4

43.

How many valence electrons does phosphorus have?

a)

15

b)

4

c)

5

d)

31

44.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
45.

Which of these is the correct Lewis structure for NH3?

a)
b)
c)
d)
46.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

47.

When drawing Lewis structures, only __________ electrons are used.

a)

inner shell

b)

core

c)

valence

d)

stable

48.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
49.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

50.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

51.

CH2O has which of the following?

a)

Multiple double bonds

b)

Multiple single bonds

c)

One double bond

d)

One single bond

e)

A lone pair

52.

Look at the picture and determine if it is accurate

a)

The structure is correct because Nitrogen has 8 electrons

b)

The structure is correct because Nitrogen needs 8 Valence electrons to fulfill octet

c)

The structure is incorrect because Nitrogen needs 10 valence electrons and the image has 8 valence electrons

d)

The structure is incorrect because there is no lone pairs on nitrogen

53.

Which of the following elements can have an incomplete octet?

a)

B

b)

P

c)

N

d)

O

54.

Which atom will never be in the middle of a Lewis Dot structure?

a)

N

b)

C

c)

H

55.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
56.
A molecule of water has what shape?
a)
Linear
b)
Tetrahedral
c)
Bent
d)
Triangular
57.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

58.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

59.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

60.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

61.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

62.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

63.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

64.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

65.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

66.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

67.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

68.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

69.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

70.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

71.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

72.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

73.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

74.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

75.

Is this molecule polar or nonpolar?

a)

Polar

b)

Nonpolar

76.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
77.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
78.
What will happen to the volume of a gas if the pressure increases, with constant temperature ?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
79.

Gas Laws involve what three factors?

a)

Solid, Liquid, and Gas

b)

Speed, Velocity, and Acceleration

c)

Elements, Compounds, and Mixtures

d)

Pressure, Temperature, and Volume

80.

Directly proportional means that as one value increases ...

a)

the other stays the same

b)

the other increases as well

c)

the other decereases

d)

the other goes to zero

81.

Inversely proportional means as one value increases the other...

a)

increases

b)

decreases

c)

stays the same

d)

goes to zero

82.
The word inverse means.......
a)
the same
b)
opposite 
83.
Temperature describes  the ______________ of particles.
a)
volume
b)
mass
c)
motion
d)
conductivity
84.

If the temperature of a gas increase, the pressure... (volume is constant)

a)

Decreases

b)

Increases

c)

Does not change

85.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
86.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
87.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

88.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

89.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

90.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
91.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
92.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
93.

Metals have the largest...

a)

atomic radius and electronegativity

b)

electronegativity and ionization energy

c)

ionization and atomic radius

d)

atomic radius only

94.

Which has a lower ionization energy: Lithium or Potassium?

a)

Lithium

b)

Potassium

95.

Which atom has the most valence electrons

a)

Ca

b)

C

c)

Cl

d)

Si

96.

Which atom has the largest radius

a)

Mg

b)

B

c)

S

d)

Br

97.

Vertical columns of elements (families) on the periodic table with similar properties

a)

period

b)

row

c)

groups

d)

quadrants

98.

What does molarity (M) measure in a solution?

a)

The volume of solute

b)

The number of moles of solute per liter of solution

c)

The mass of solvent per liter

d)

The density of the solution

99.

What must you do *before* adding a solute when preparing a solution from a solid?

a)

Heat the container

b)

Measure the total mass of the container

c)

Zero the balance and measure the correct mass of solute

d)

Add solvent

100.

When making a solution by dilution, what is being changed?

a)

The total mass of solute

b)

The identity of the solute

c)

The concentration of the solution

d)

The temperature of the solvent

101.

What happens to the concentration of a solution if you add more solvent without adding solute?

a)

The concentration increases

b)

The concentration decreases

c)

The concentration stays the same

d)

The solution becomes saturated

102.

What does it mean if a solution is *saturated*?

a)

No solute is present

b)

No more solute can dissolve at that temperature

c)

The solution has evaporated

d)

Only a small amount of solute has been added

103.

Why must you stir or swirl a solution after adding solute?

a)

To cool the solution

b)

To increase the pressure

c)

To evenly distribute the solute particles

d)

To change the identity of the solute

104.
State whether the following compound is soluble or insoluble. potassiun bromide KBr
a)
Soluble
b)
Insoluble
105.
State whether the following compound is soluble or insoluble.Potassium hydroxide KOH
a)
Soluble 
b)
Insoluble
106.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

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