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AP Chemistry Semester

Total questions: 70

Worksheet time: 5hrs 3mins

Name
Class
Date
1.

The amount of heat needed to raise the temperature of 1g of a substance by 1C is called:

a)

Melting Point

b)

Boiling Point

c)

Specific Heat

d)

Heat of Vaporization

2.

What are the products of a combustion reaction (select all that apply)?

a)

CO2

b)

O2

c)

H2O

d)

H2

3.

Which of the following is an example of a physical property of a substance?

a)

Shape

b)

Color

c)

Malleability

d)

All of the above

4.

A substance that is made up of only the same molecules is known as a:

a)

Pure substance

b)

Mixture

c)

Bad idea

d)

Compound

5.

What is the periodic trend for INCREASING electronegativity? (Select all that apply)

a)

Left to right

b)

Right to left

c)

Bottom to top

d)

Top to bottom

6.

What is the periodic trend for INCREASING ionization energy? (Select all that apply)

a)

Left to right

b)

Right to left

c)

Bottom to top

d)

Top to bottom

7.

What is the periodic trend for INCREASING atomic radius? (Select all that apply)

a)

Left to right

b)

Right to left

c)

Bottom to top

d)

Top to bottom

8.

What is ionization energy?

a)

The amount of energy required to remove electrons

b)

The amount of energy required to remove protons

c)

The amount of energy needed to create new bonds

d)

The amount of energy needed to cancel out ions

9.

If 7.00 grams of nitrogen gas are contained in a 5.00 L flask at 4.62 kPa. What is the temperature of the gas?

a)

11.1 K

b)

1.00 K

c)

4.12 K

d)

9.07 K

10.

If 2.00 L of a gas in a container at room temperature exerts a pressure of 4.00 atm. If the pressure doubles and the temperature remains the same, the volume would become ________.

a)

16.0 L

b)

2.00 L

c)

4.00 L

d)

1.00 L

11.

What are the coefficients that will balance the skeleton equation below?

AlCl3 + NaOH → Al(OH)3 + NaCl

a)

1,3,1,3

b)

3,1,3,1

c)

1,1,1,3

d)

1,3,3,1

12.

Order the elements S, Cl, and F in terms of increasing ionization energy.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

13.

Which of the following atoms would have the largest second ionization energy?

a)

Mg

b)

Cl

c)

S

d)

Ca

e)

Na

14.

Which of the following statements is true?

a)

The first ionization potential of H is greather than that of He.

b)

The ionic radius of Fe+ is larger than that of F3+.

c)

The ionization energy of S2- is greater than that of Cl-.

d)

The atomic radius of Li is larger than that of Cs.

e)

All are false.

15.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
16.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
17.

What is the empirical formula of a compound that is 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

18.
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
19.
63Cu is 69% of the naturally occurring isotope of Cu.  If only one other isotope is present for natural copper, what is it?
a)
59Cu
b)
65Cu
c)
61Cu
d)
62Cu
20.

According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?

a)

SF6

b)

H2O

c)

HCl

d)

Cl2

e)

None, the molecules of all gases have the same root mean square speed at any given temperature.

21.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

22.

The density of N2O at 1.52 atm and 45.2ºC is ____ g/L.

a)

0.388 g/L

b)

2.58 g/L

c)

9.99 g/L

d)

1.76 g/L

e)

18.2 g/L

23.

The volume of a sample of gas (2.49 g) is 752 mL at 1.98 atm and 62ºC. What is the gas?

a)

NO2

b)

SO3

c)

SO2

d)

Ne

e)

NH3

24.

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

a)

H2

b)

He

c)

Ne

d)

O2

e)

All have the same volume.

25.

In a chromatography experiment using water as the solvent, the solute that would have the highest Rf value would be:

a)

polar

b)

nonpolar

26.

Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.

a)

IMFs; solubility

b)

solubility; conductivity

c)

IMFs; boiling point

d)

boiling point; solubility

27.
According to the table which solute is nonpolar.
a)
ammonium chloride
b)
naphthalene
c)
ethanol
d)
urea
28.
Which salt is LEAST soluble at 0 ºC?
a)
K2Cr2O7
b)
KNO3
c)
 KClO3
d)
Ce2(SO4)3
29.

NO CALCULATOR! What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH - molar mass 40 g/mol)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

e)

You are evil for making me do this in my head.

30.

How can you increase the solubility of a gas in a liquid?

a)

Decrease the IMFs between the gas the and the liquid.

b)

Increase the temperature of the solution.

c)

Increase the pressure of the solution.

d)

All of these would work.

31.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
32.

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

33.

Resonance structures differ by __________.

a)

number and placement of electrons

b)

number of electrons only

c)

placement of atoms only

d)

number of atoms only

e)

placement of electrons only

34.

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

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

35.

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

36.

Of the possible bonds between carbon atoms (single, double, and triple), _____.

a)

a triple bond is longer than a single bond

b)

a double bond is stronger than a triple bond

c)

a single bond is stronger than a triple bond

d)

a double bond is longer than a triple bond

e)

a single bond is stronger than a double bond

37.

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

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

38.

In the Lewis structure of ClF, the formal charge on Cl is _______ and the formal charge on F is _______.

a)

0,0

b)

-1, -1

c)

0, -1

d)

-1, 0

e)

+1, -1

39.

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

40.
What is the the shape of this molecule according to VSPER theory?
a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
41.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
42.

Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

43.

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

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

44.
Bond angle for bent
a)
120o
b)
109.5o
c)
104.5o
d)
107o
45.
How many sigma and pi bonds does this have?
a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
46.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
47.
Nitrogen atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
48.

The wavelength of a photon that has an energy of 5.25 x 10-19 J is __________ m

a)

4.21 x 10-24

b)

2.38 x 1023

c)

2.64 x 106

d)

3.79 x 10-7

49.

The lines in the emission spectrum of hydrogen result from __________.

a)

electrons given off by hydrogen as it cools

b)

decomposing hydrogen atoms

c)

electrons given off by hydrogen when it burns

d)

energy given off in the form of visible light when an electron moves from a higher energy state to a lower energy state

50.

Which ion in the isoelectronic series below has the smallest radius in a crystal?

a)

O2-

b)

N3-

c)

Na+

d)

Al3+

e)

F-

51.

__________-orbitals are spherically symmetrical

a)

d

b)

p

c)

s

d)

f

52.

An example of an electron configuration of a transition metal is __________.

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

b)

1s2 2s2 2p6 3s2 3p5

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

e)

1s2 2s2 2p4 3s1

53.
Which of the following type of electromagnetic radiation has the most energy
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
54.
What is the average atomic mass for this element?
a)
10 amu
b)
10.8 amu
c)
19.9 amu
d)
11 amu
55.
What do the heights of the peaks represent in the mass spectrum?
a)
number of isotopes
b)
relative abundance of each isotope
c)
average atomic mass
d)
charge:mass ratio
56.
Which is larger... P or P3- ?
a)
P3- because it gains an energy level
b)
P3- due to extra electron repulsion
c)
P because it loses an energy level
d)
P because of extra electron repulsion
57.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
58.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
59.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
60.

What are the spectator ions in the reaction of sodium chloride with silver nitrate?

a)

silver and nitrate

b)

sodium and chlorine

c)

sodium and nitrate

d)

silver and chlorine

61.
Consider an atom with the electron configuration 1s22s22p63s23p6.  Which of the following is an accurate statement concerning this atom?
a)
This atom would probably be very reactive
b)
This element is diamagnetic
c)
This atom is in an excited state
d)
The atomic number Z = 11
62.
Which principle states that only two electrons can occupy an orbital?
a)
Pauli Exclusion Principle
b)
Hund's Rule
c)
Heisenberg's Uncertainty Principle
d)
Newton's Principle
63.
Which of the following molecules is polar?
a)
SO3
b)
SO2
c)
CO2
d)
CH4
64.
Which of the following compounds will have the lowest boiling point?
a)
CH4
b)
CHCl3
c)
CH3CH2OH
d)
NH3
65.
Under which conditions does a real gas behave most nearly like an ideal gas?
a)
High Temperature and High Pressure
b)
High Temperature and Low Pressure
c)
Low Temperature and Low Pressure
d)
Low temperature and High Pressure
66.
Which of the following compounds does NOT exhibit hydrogen bonding?
a)
CH4
b)
HF
c)
NH3
d)
H2O
67.
Which substance listed below is the strongest oxidizing agent given the following spontaneous redox reaction?
Mg + Sn+2 --> Mg+2 + Sn
a)
Mg+2
b)
Sn
c)
Mg
d)
Sn+2
68.
What is the oxidation number of Br in NaBrO3?
a)
-1
b)
+1
c)
+3
d)
+5
69.
When a substance loses electrons, it is _____.  This substance is known as the _____ agent.
a)
reduced; reducing
b)
oxidized; reducing
c)
reduced; oxidizing
d)
oxidized; oxidizing
70.
Under acidic conditions, what is the coefficient in front of the Fe+2 once the reaction below is balanced?
          Fe+2 + Cr2O7-2 --> Fe+3 + Cr+3
a)
1
b)
2
c)
3
d)
6

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