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Worksheets(H) Semester (II) Review
Total questions: 150
Worksheet time: 4hrs 54mins
Name
Class
Date
1.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
2.
Draw the Lewis structure for OF2 and determine the number of lone pairs on the central atom.
a)
none
b)
1
c)
2
d)
it's ionic
3.
How many unpaired electrons are in the Lewis dot symbol of a chlorine atom?
a)
7
b)
3
c)
5
d)
1
4.
Which of these has a double bond?
a)
Cl2
b)
H2
c)
N2
d)
O2
5.
How many lone pairs are on the central atom in ammonia (NH3)?
a)
0
b)
1
c)
2
d)
3
6.
What is the structure of an ammonia (NH3) molecule?
a)
Tetrahedral
b)
Trigonal planar
c)
Trigonal pyramidal
d)
Octahedral
7.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
8.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
9.
Which of the following is octahedral?
a)
SCl6
b)
XeI4
c)
NBr5
d)
CH4
10.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
11.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
12.
*
a)
tetrahedral
b)
trigonal pyramid
c)
angular or bent
d)
trigonal plane
13.
The basic fact that determines molecular shapes is that
a)
nuclei attract each other.
b)
electron pairs attract each other.
c)
electron pairs repel each other.
d)
nuclei repel each other.
14.
Lone pairs around the oxygen atom of a water molecule play no role in determining its molecular geometry which has what shape?
a)
True;
bent
bent
b)
False;
bent
bent
c)
True;
linear
linear
d)
False;
linear
linear
15.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces
16.
Which of these is the strongest?
a)
hydrogen bonding
b)
dipole-dipole forces
c)
London dispersion forces
d)
ionic bonding
17.
The shape of Carbon Dioxide is called ______.
a)
tetrahedral
b)
square
c)
planar
d)
linear
18.
What is the name of pairs of electrons that do not participate in bonding?
a)
outer pair
b)
unvalenced pair
c)
unshared pair
d)
inner pair
19.
What is the hybridization of a linear molecule?
a)
sp
b)
sp2
c)
sp3
d)
sp3d
20.
Which of the following images represents a Trigonal Planar molecular geometry?
a)
b)
c)
d)
21.
What is the hybridization of this molecule shown above
a)
sp
b)
sp2
c)
sp3
d)
sp4
22.
What is the bond angle for the CH4 molecule?
a)
120°
b)
107°
c)
109.5°
d)
90°
23.
What is the hybridization of the central atom of a bent molecule? (AB2E2)
a)
sp
b)
sp2
c)
sp3
d)
sp3d
24.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
25.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
26.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
27.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
28.
Which of the following is octahedral?
a)
SCl6
b)
XeI4
c)
NBr5
d)
CH4
29.
The molecule shown in the diagram can best be classified as a
a)
polar covalent molecule
b)
nonpolar covalent molecule
c)
ionic compound
d)
nonpolar ionic compound
30.
The polarity of a bond between two elements can be best determined by
a)
The difference in electronegativity between the elements
b)
The difference in first ionization energy between the elements
c)
The number of electrons shared in the bond
d)
The difference in atomic radius between the elements
31.
Which bond is most polar?
a)
H-F
b)
H-Cl
c)
H-Br
d)
H-I
32.
What kind of bond do you have: Li and Cl
a)
Non-polar covalent
b)
Polar covalent
c)
ionic
d)
James Bond
33.
What are the hybridization and the approximate bond angles in CS2?
a)
sp2, 1070
b)
sp3, 1200
c)
sp2, 1200
d)
sp, 1800
34.
Which molecule exhibits resonance?
a)
O3
b)
BeCl2
c)
CO2
d)
NF3
35.
What are the formal charges on the boron and nitrogen in the compounds BF3 and NH3?
a)
-2 and +2
b)
+2 and –2
c)
0 and 0
d)
+1 and –1
36.
Which of the following is a covalent compound?
a)
SrI2
b)
P4O10
c)
LiOH
d)
ZnS
37.
Which of the following molecules has Π bonds?
a)
CO2
b)
BF3
c)
NH3
d)
H2O
38.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
39.
2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
40.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
41.
2H2 + O2 → 2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
42.
How many grams are in one mole of Oxygen
a)
16
b)
32
c)
15.99
d)
31.98
43.
In the reaction 2 H2 + O2 → 2 H2O what is the mole ratio of oxygen to water
a)
1:2
b)
2:1
c)
3:4
d)
4:3
44.
What is the molar mass of Ba(CN)2
a)
189.37
b)
189.33
c)
189
d)
189.35
45.
The amount of a product this is produced during a chemical reaction
a)
Percent Composition
b)
Actual yield
c)
Theoretical yield
d)
Percent Yield
46.
The calculated amount of a product that is going to be produced
a)
Percent Composition
b)
Actual yield
c)
Theoretical yield
d)
Percent Yield
47.
The reactant this is not completely used up during the reaction.
a)
Mole ratio
b)
Excess reactant
c)
Limiting Reactant
d)
Stoichiometry
48.
An efficient experiment might have which of the following percent yields?
a)
Less than 50%
b)
About 50%
c)
Greater than 50%
d)
Greater than 100%
49.
What is the first thing you must do to solve a stoichiometric problem?
a)
Find the excess reactant
b)
Find the limiting reactant
c)
Write the balanced chemical equation
d)
Find the molecular formula
50.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
51.
What is 0.00 degrees Kelvin known as
a)
No such thing
b)
Very cold
c)
Freezing point of Water
d)
Absolute Zero
52.
What about gasses can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
53.
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
54.
What is the device that measures atmospheric pressure?
a)
Aerometer
b)
Annemeter
c)
Barometer
d)
Humidity Detector
55.
What law combines all 3 factors (pressure, temperature, and volume)
a)
Combined Gas Law
b)
Charle's Law
c)
Boyle's Law
d)
Avagadros Ideal Gas Law
56.
If temperature goes up, then pressure
a)
goes up
b)
goes down
c)
stays the same
d)
goes down then up
57.
•If volume is decreased, then the pressure ____________
a)
decreases
b)
increases
c)
stays the same
d)
lowers
58.
•More collisions on the wall of the container causes more ____________
a)
volume
b)
temperature
c)
pressure
d)
space between particles
59.
As a gas is compressed, the distance between gas molecules ____________
a)
increases
b)
stays the same
c)
decreases
d)
goes up
60.
As a gas is compressed, the number of gas molecules ____________
a)
goes up
b)
goes down
c)
stays the same
d)
decreases
61.
Standard pressure is _____ atm
a)
101.3
b)
2
c)
760
d)
1
62.
Standard pressure is _____ torr
a)
101.3
b)
1
c)
760
d)
2
63.
•If the pressure of 2 L of a gas at STP doubles, its new volume would be ____ L.
a)
4
b)
1
c)
2
d)
.5
64.
If the Kelvin temperature of a sample of 2L of gas at STP doubles, the new volume is
a)
2 L
b)
.5 L
c)
1 L
d)
4 L
65.
•The gas constant, R, is equal to 0.0821 when the pressure is expressed in kilopascals.
a)
TRUE, pressure needs to be expressed in kilopascals
b)
FALSE, pressure needs to be in atmospheres.
66.
At a constant temperature, the pressure exerted by one mole of a gas decreases if the volume increases.
a)
TRUE, P and V are inversely proportional.
b)
FALSE, P and V are directly proportional.
67.
•The ideal gas equation will only give correct values if the temperature is expressed in degrees Celsius.
a)
TRUE, temp. is in Celsius
b)
FALSE, temp. in Kelvins
68.
•If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?
a)
2.96 L
b)
20.3 L
c)
29.6 L
d)
3.0 L
69.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
70.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
71.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
2
c)
8
d)
24
72.
Decomposition occurs when...
a)
Two formulas combine.
b)
A formula breaks apart.
c)
An atom is replaced during a reaction.
73.
Which problem is balanced?
a)
PbO2 + 2H2
b)
So2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
74.
A synthesis occurs when...
a)
Two formulas combine.
b)
A formula breaks apart.
c)
An atom is replaced during a reaction.
75.
Which of the Following Correctly Balances this Equation?
_H2+_Cl2 --> _HCl
_H2+_Cl2 --> _HCl
a)
2H2 + Cl2 --> 4HCl
b)
H2+Cl2 --> 2HCl
c)
3H2 + 3Cl2 --> HCl
d)
H + Cl --> HCl
76.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
77.
C2H6 + O2 --> CO2 + H2O
What coefficient would go in front of C2H6?
What coefficient would go in front of C2H6?
a)
1
b)
2
c)
3
d)
4
78.
Classify
HI → H2 + I2
HI → H2 + I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
79.
Classify
CH4 + O2 → CO2 + H2O
CH4 + O2 → CO2 + H2O
a)
single replacement
b)
double replacement
c)
synthesis
d)
combustion
80.
Classify
FeS + HCl → H2S + FeCl2
FeS + HCl → H2S + FeCl2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
81.
Classify
Fe + O2 → Fe2O3
Fe + O2 → Fe2O3
a)
synthesis
b)
decomposition
c)
double replacement
d)
single replacement
82.
AB + X --> XB + A
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
83.
XY --> X + Y
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
84.
A + B --> AB
a)
synthesis
b)
decomposition
c)
single replacment
d)
double replacement
85.
Pb(NO3)2 + KI --> KNO3 + PbI2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
86.
C12H22O11 + O2 --> CO2 + H20
a)
synthesis
b)
acid base
c)
combustion
d)
acid base
87.
Mg + HCl --> MgCl2 + H2
a)
combustion
b)
synthesis
c)
decomposition
d)
single replacement
88.
Fe + O2 --> Fe2O3
a)
synthesis
b)
decomposition
c)
combustion
d)
acid base
89.
According to the activity series, which of the following single replacement reactions can occur?
a)
Ca + Al2(SO4)3
b)
Fe + NaOH
c)
Ni + MgSO4
d)
Al + KOH
90.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)
Fe + 3 O2 → Fe2O3
b)
3 Fe + 3 O2 → 2 Fe2O3
c)
2 Fe + O2 → Fe2O3
d)
4 Fe + 3 O2 → 2 Fe2O3
91.
Which of the following would create a precipitate according to the solubility table?
a)
Ba(NO3)2
b)
K3PO4
c)
Cu(OH)2
d)
NH4Cl
92.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
93.
How many molecules are there in 0.04 moles of CaF?
a)
2.4 x 1023
b)
2.4 x 1022
c)
2.36
d)
1450
94.
How many moles are there in 64 grams of O2?
a)
0.5
b)
1
c)
2
d)
4
95.
What is the percent composition in NaOH of Na?
a)
19.55%
b)
45.16%
c)
25%
d)
76.45%
96.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements. (keep two decimal places throughout calculations)
a)
SO
b)
SO2
c)
SO3
d)
SO4
97.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
98.
Which one is empirical?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
99.
What is a substance that is dissolved in another substance?
a)
solution
b)
solute
c)
solvent
d)
compound
100.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
101.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?
a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
102.
Force of attraction between similar molecules is called
a)
Cohesive force
b)
Adhesive force
c)
Magnetic force
d)
gravitational force
103.
When water molecules stick to other substances.
a)
Cohesion
b)
Polarity
c)
Adhesion
d)
Capillary Action
104.
The tightness across the top of water - causes polar molecules to pull together.
a)
Capillary Action
b)
Cohesion
c)
Density
d)
Surface Tension
105.
The energy required to change water from liquid to vapor.
a)
Buoyancy
b)
Temperature
c)
Density
d)
Specific Heat
106.
_______ causes water to form DROPS, _______ causes water to look SPHERICAL (oval) and _______ causes water to STAY IN PLACE.
a)
cohesion, surface tension, adhesion
b)
surface tension, cohesion, adhesion
c)
adhesion, cohesion, surface tension
d)
adhesion, surface tension, cohesion
107.
The mobility of ______________________within a metal lattice explains some of the properties of metals.
a)
Protons
b)
Electrons
c)
Metalloids
d)
Transition metals
108.
The properties of an ______________ can be explained by the strong attractions among ions within a crystal lattice.
a)
Chemical bond
b)
Covalent bond
c)
Ionic compound
d)
Periodic table
109.
Which of the following compounds exhibits the greater lattice energy?
a)
NaCl
b)
LiCl
110.
Which of the following compounds exhibits the greater lattice energy?
a)
MgS
b)
CaS
c)
BeO
111.
Compound 'A' has a lattice energy of -1378 kJ/mol while compound 'B' has a lattice energy of -1062 kJ/mol. Which compound has the higher melting point?
a)
A
b)
B
112.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
113.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
e)
Is a base or Neutral Solution
114.
Which of the following statements is correct?
a)
Blue litmus paper turns red when placed in a base.
b)
Red litmus paper turns blue when placed in a base.
c)
Blue litmus paper stays blue when placed in an acid.
d)
Red litmus paper stays red when placed in a base.
115.
Carrie's teacher hands out test tubes filled with different chemicals and tells the students to identify their liquid as an acid, base, or neutral chemical. Carrie's test tube contains a clear chemical. She adds phenolpthalein to her test tube and gently moves the tube from side to side. A few moments later, the chemical in the test tube turns bright pink.
What type of chemical does Carrie have?
What type of chemical does Carrie have?
a)
Carrie has a neutral chemical.
b)
Carrie has an acidic chemical.
c)
Carrie has a basic chemical.
d)
The type of chemical Carrie has cannot be determined.
116.
What would be considered the weakest base?
a)
8
b)
14
c)
7.8
d)
11.6
117.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
118.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
119.
Calculate the molarity of the following solution: 1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
120.
a)
Substance A because HCl is a strong acid, therefore, a strong electrolyte
b)
Substance A because HCl is a weak acid, therefore, a nonelectrolyte
c)
Substance B because HCl is a strong acid, therefore a nonelectrolyte
d)
Substance B because HCl is a weak acid, therefore a strong electrolyte
121.
Solvation is a process in which the _____ pulls apart the _____.
a)
solvent & solute
b)
solute & solvent
c)
solution & solvent
d)
solvent & solution
122.
An exothermic reaction:
a)
Produces heat when the reaction occurs
b)
Absorbs heat when a reaction occurs
123.
Which sample has hydrogen bonding?
a)
H2S
b)
CH4
c)
NH3
d)
HI
124.
Water has an unusually high boiling point for a molecular compound because it has
a)
hydrogen bonding
b)
ion-ion attractions
c)
a high density
d)
a large gram formula mass
125.
Which substance has the weakest intermolecular forces?
a)
Substance A, boiling point of 75 °C
b)
Substance B, boiling point of 105 °C
c)
Substance C, boiling point of 25 °C
d)
Substance d, boiling point of 45 °C
126.
________________________ have the strongest intermolecular forces of attraction.
a)
Dipole- Dipole
b)
Dispersion
c)
Hydrogen Bonds
127.
Which of these has dispersion forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
128.
Intermolecular forces for: NH3
a)
Dispersion Force
b)
Dipole dipole
c)
Hydrogen bonding
129.
When the temperature of matter decreases the particles ...
a)
speed up and move farther apart
b)
speed up and move closer together
c)
slow down and move farther apart
d)
slow down and move closer together
130.
Which two phases changes takes away energy?
a)
Freezing, Melting
b)
Condensation, Evaporation
c)
Freezing, Condensation
d)
Melting, Evaporation
131.
Which two phases changes add energy?
a)
Freezing, Melting
b)
Condensation, Evaporation
c)
Freezing, Condensation
d)
Melting, Evaporation
132.
Gas pressure is caused by
a)
gas molecules colliding with surfaces
b)
gas molecules condensing to a liquid
c)
gas molecules hitting other gas molecule
d)
barometers
133.
a)
Gas particles are elastic and do not attract each other.
b)
The kinetic energy of gas is dependent on temperature
c)
Energy is not lost when gas particles collide with each other or with the walls of the container.
d)
All of the above
134.
Movement of gas through a tiny opening
a)
Diffusion
b)
Effusion
135.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
136.
Use Graham’s Law to calculate fast O2 gas will effuse compared to Cl2.
a)
O2 effuses 1.5x faster than Cl2
b)
O2 effuses 0.11x as fast as Cl2
c)
O2 effuses 1.1x faster than Cl2
d)
O2 effuses 0.15x as fast as Cl2
137.
In order to calculate the rate of effusion of a gas, you must compare it to that of another gas and
a)
take the square root of the molar mass of the lighter gas divided by the square root of the molar mass of the heavier gas.
b)
take the square root of the molar mass of the heavier gas.
c)
take the square root of the molar mass of the lighter gas.
d)
take the square root of the molar mass of the heavier gas divided by the square root of the molar mass of the lighter gas.
138.
Heavier gases have a __________________ rate of effusion.
a)
Faster
b)
Slower
c)
Rate of effusion does not depend on mass.
139.
What line segment represents only the solid state?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
140.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
141.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
142.
Between which points is the temperature of the substance increasing?
a)
A-B only.
b)
A-B, C-D, E-F
c)
B-C only.
d)
B-C, D-E
143.
What state of matter is segment 5?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
144.
True or false: melting and freezing occur at the same temperature!
a)
True
b)
False
c)
I don't know
145.
Water exists as a _____________ at 3 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
146.
At 10 atm, dry ice is heated from -100 °C to 30 °C. What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
147.
What state of matter is X?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
148.
What state of matter is Y?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
149.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
150.
Which of these conditions is always true for an exothermic process?
a)
They leave the surroundings feeling cold
b)
They release energy into the surroundings.
c)
They absorb energy from the surroundings
d)
The reactants gain energy as they form the products
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