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AP review-2019

Total questions: 111

Worksheet time: 4hrs 22mins

Name
Class
Date
1.

What is the name of the precipitate formed in the reaction of sodium sulfide and aluminum nitrate (write the net ionic equation)

a)

calcium nitrate

b)

aluminum sulfide

c)

no ppt is formed

d)

aluminum nitrate

2.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?
a)
4.88 M
b)
4.880 M
c)
2.440 M
d)
2.44 M
3.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.074 mol
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
4.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
5.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
6.
Which of the letters (A-D) represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
7.
What kind of reaction is this?
a)
endothermic
b)
exothermic
8.
A sample of iron receives 50J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?
a)
25g
b)
30g
c)
20g
d)
50g
9.
žDetermine the energy (in J) required to raise the temperature of 100.0 g of water from 20.0 C to 85.0 C? The specific heat of water is 4.184 J/g°C
a)
500 J
b)
4,182 J
c)
27,196 J
d)
27200 J
10.
The Law of _______________ states that energy cannot be created nor destroyed only transferred 
a)
Specific Heat
b)
Conservation of Energy
c)
Exothermic Reaction
d)
Potential Energy
11.

Refer the the following question:

2N2 + 3H2 --> 2NH3 ΔH= 46 kJ/mol rxn

How much energy would be produced if only 1 mol of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

12.
permanganate
a)
MnO41-
b)
MnO32-
c)
MnO21-
d)
MnO1-
13.
carbonate
a)
CO32-
b)
CO22-
c)
CO3
d)
CO2
14.
CN1-
a)
cyanide
b)
cyanate
c)
carbon nitride
d)
cyanite
15.
perchlorate
a)
ClO41-
b)
ClO31-
c)
ClO21-
d)
ClO1-
16.
Which of the following is not a strong acid?
a)
HCl
b)
HF
c)
HBr
d)
HNO3
17.
What is the oxidation number of Br in NaBrO3?
a)
-1
b)
+1
c)
+3
d)
+5
18.
Which of the following would be a weak electrolyte in a solution?
a)
HBr
b)
KCl
c)
KOH
d)
HC2H3O2
19.
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
20.
Find the percentage composition of  Mg in Mg3(PO4)2.
   

a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
21.
What is the name of this compound?  Na2CO3
a)
Disodium carbonate
b)
Sodium III carbonate
c)
Sodium II carbonate
d)
Sodium carbonate
22.
What is the name of CaSO4
a)
Calcium sulfide
b)
Calcium sulfate
c)
Calcium sulfite
d)
Calcium II sulfate
23.
What is the name of PbS
a)
Lead sulfate
b)
Lead II sulfate
c)
Lead sulfide
d)
Lead II sulfide
24.
What is the formula for Iron II phosphide
a)
Fe3P2
b)
Fe2P3
c)
Fe3(PO4)4
d)
Fe2(PO4)3
25.
What is the name of FeCl3
a)
Iron chloride
b)
Iron chloride III 
c)
Iron III chloride
d)
Iron II chloride
26.
What is the name of Al2(SO4)3
a)
Aluminum oxide
b)
Aluminum II sulfate
c)
Aluminum sulfate 
d)
Aluminum III sufate
27.
What is the formula for  Barium nitrate
a)
BaNO3
b)
Ba(NO3)2
c)
Be(NO3)2
d)
Be2NO3
28.
What is the formula for Copper I carbonate
a)
Cu2CO3 
b)
CuC
c)
CuCO3
d)
Cu(CO3)2
29.
What is the chemical formula for Aluminum hydroxide
a)
AlOH
b)
AlOH3
c)
Al(OH)3 
d)
AlHO
30.
Name the following in order:
HCl, HBr, HI
a)
hydrochloric acid, hydrobromic acid, hydroiodic acid
b)
chloric acid, bromic acid, iodic acid
c)
chlorous acid, bromous acid, iodous acid
d)
hydrochlorous acid, hydrobromous acid, hydroiodous acid
31.
When using water as a solvent which type of molecule is likely  to have the highest  Rf value
a)
polar
b)
non-polar
32.
chromatography separate the mixture of dyes on the basis of their ----------------------------
a)
density
b)
solubility
c)
gravity
d)
boiling point
33.

Distillation is used to separate mixtures on the basis of what physical property?

a)

Freezing point

b)

Boiling point

c)

Cooling point

d)

Heating point

34.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
35.

Real gas behavior deviates from ideal gas behavior because real gas particles have

a)

no volume and no attraction for each other

b)

no volume but some attraction for each other

c)

volume but no attraction for each other

d)

volume and some attraction for each other

36.
This electrode in a voltaic cell gains mass
a)
anode
b)
cathode
37.
Reactions in voltaic cells are
a)
spontaneous, redox reactions
b)
non-spontaneous, redox reactions
c)
spontaneous, non-redox reactions
d)
non-spontaneous, non-redox reactions
38.
In a voltaic cell, the half cell that receives anions from the salt bridge is
a)
cathode
b)
anode
39.
Consider the following numbered processes:
1. A -> 2B
2. B -> C + D
3. E -> 2D
ΔH for the process A -> 2C + E is
a)
ΔH1 + ΔH2 + ΔH3
b)
ΔH1 + ΔH2 
c)
ΔH1 + ΔH2 - ΔH3
d)
ΔH1 + 2ΔH2 - ΔH3
40.
Consider the following processes:
I.  condensation of a liquid
II. increasing volume of an ideal gas at constant temp
III. dissolving sugar in water
IV. heating 1.0 mol of an ideal gas at constant volume
For how many of these is ΔS positive?
a)
0
b)
1
c)
2
d)
3
41.
For the reaction A + B -> C + D, ΔHₒ = +40 kJ and ΔSₒ = +50 J/K. Therefore, the reaction under standard conditions is
a)
spontaneous at temps > 10K
b)
spontaneous at temps > 800K
c)
spontaneous at temps between 10K and 800K
d)
spontaneous at all temperatures
42.
Which is most acidic?
a)
pH = 8.5
b)
[H3O+] = 1 x  10-13
c)
[H3O+] = 1 x  10-2
d)
pH = 3
43.
step 1: O3 → O2 + O
step 2: O3 + O → 2 O2

The oxygen atom (O) is considered to be a(n)...
a)
reactant
b)
catalyst
c)
reaction intermediate
d)
activated complex
44.
a)
rate = k[CO]2[O2]2
b)
rate = k[CO]2[O2]
c)
rate = k[CO][O2]2
d)
rate = k[CO][O2]1/2
45.
Which one of the following elements has the greatest ionization energy?
a)
Al
b)
Cl
c)
Br
d)
S
46.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
47.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
48.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
49.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
50.

What is the shape of an s orbital?

a)

sphere

b)

dumbbell

c)

pear

51.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
52.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
53.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
54.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
55.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
56.
Which is a correct orbital box diagram?  
a)
a
b)
b
c)
d
d)
e
57.
How many valence electrons does an element with the following electron configuration have?
1s22s22p63s23p64s23d104p2
a)
2
b)
4
c)
14
d)
32
58.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
59.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
60.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
61.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
62.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
63.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
64.
The element bromine is a -
a)
Period 3 alkali metal.
b)
Period 4 halogen.
c)
Period 3 noble gas.
d)
Period 4 transition metal.
65.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
66.
The greater the speed of gas particles in a container, the:
a)
greater the pressure
b)
fewer collisions there will be
c)
lower the temperature
d)
lower the pressure
67.

Atoms with the same number of protons & different numbers of neutrons are known as ____.

a)

isotopes

b)

isomers

c)

ions

d)

sister elements

68.

Which of the following subshells has the lowest energy?

a)

4d

b)

5s

c)

5p

d)

5f

69.

What is ionization energy?

a)

How well an atom attracts electrons in a chemical bond

b)

The relative size of an atom

c)

An atom that has gained or lost an electron

d)

The amount of energy it takes to remove an electron from the valence shell of an atom

70.

Which Lewis dot structure shows exactly two unshared pairs of valence electrons?

a)

H2S

b)

CO2

c)

NH3

d)

CBr4

71.

What is the shape of PCl5?

a)

Tetrahedral

b)

Octahedral

c)

Trigonal pyramidal

d)

Trigonal bipyramidal

72.

What type of hybridization does C have in CH2OH?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

73.

How many sigma and pi bonds are in C2H2?

a)

3 sigma and 1 pi

b)

3 sigma, 2 pi

c)

4 sigma, 1 pi

d)

4 sigma, 2 pi

74.

Which of the following would require resonance structures to satisfactorily describe the bonding?

a)

H2O

b)

NO3-

c)

CO2

d)

OH-

75.

What is the oxidation state of S in Na2SO4?

a)

-2

b)

+2

c)

+4

d)

+6

76.

A reaction will be thermodynamically favorable at all temperatures if

a)

it is exothermic with an increase in entropy

b)

it is endothermic with an increase in entropy

c)

it is exothermic with an decrease in entropy

d)

it is endothermic with a decrease in entropy

77.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
78.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
79.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
80.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
81.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
82.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
83.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
84.

The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

85.

The geometry of a molecule with 3 bonded pairs of electrons and 0 lone pairs of electrons, AB3

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

86.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
87.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
88.

Determine the molecular geometry of the given structure.

a)

Octahedral

b)

Square Pyramidal

c)

Trigonal Bipyramidal

d)

See Saw

89.

Determine the hybridization of the given structure.

a)

sp

b)

sp2

c)

sp3

d)

sp3d

90.

What IMF would exist between molecules of BrF5?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

LDF and Dipole-Dipole Forces

d)

None

91.

Determine the VSEPR shape and hybridization of the given structure.

a)

tetrahedral; sp3

b)

tetrahedral; sp3d

c)

trigonal pyramidal; sp3

d)

trigonal pyramidal; sp3d

92.

Determine the VSEPR shape and intermolecular forces of the given structure.

a)

T-Shape; LDF

b)

T-Shape; LDF and Dipole-Dipole

c)

See Saw; LDF and Dipole-Dipole

d)

See Saw; LDF

93.

Identify the hybridization and IMF of the given structure.

a)

sp3d; LDF

b)

sp3d; LDF and Dipole-Dipole

c)

sp3d2; LDF

d)

sp3d2; LDF and Dipole-Dipole

94.

Determine the VSEPR shape and intermolecular forces that exist between molecules of the given structure.

a)

Square Pyramidal; LDF

b)

Square Pyramidal; LDF and Dipole-Dipole

c)

Octahedral; LDF

d)

Octahedral; LDF and Dipole-Dipole

95.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
96.

Which of the following linear molecules would be considered polar?

a)
b)
c)
d)
97.

For which of the following would hydrogen bonding occur between molecules?

a)
b)
c)
d)
98.

Which of the following linear molecules would be considered polar?

a)
b)
c)
d)
99.

Which of the following has T-shape molecular geometry?

a)
b)
c)
d)
100.
If fluorine is stronger then carbon, what charge will the fluorine receive?
a)
negative
b)
slight negative
c)
positive
d)
slight positive
101.
Hydrocarbons will have which type of intermolecular forces?
a)
Dispersion
b)
dipole
c)
hydrogen bonds
102.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
103.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
104.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
105.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
106.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
107.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
108.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
109.

This picture most likely depicts the arrangement of atoms in a

a)

diamond

b)

salt

c)

metal

d)

gas

110.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
111.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above

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