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Worksheets

END OF SEMESTER 2 REVIEW PACKET

Total questions: 200

Worksheet time: 5hrs 45mins

Name
Class
Date
1.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

2.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

3.

A bond between two atoms that share one pair of electrons.

a)

Double covalent bonds

b)

Triple covalent bonds

c)

Covalent bonds

d)

Single covalent bond

4.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
5.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
6.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
7.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
8.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
9.

What is the term used for the substances that are formed when 2 or more atoms from differing elements come together?

a)

atoms

b)

elements

c)

molecules

d)

compounds

10.

What is sugar? (C6H12O6)

a)

element

b)

compound

c)

mixture

11.

This picture represents a type of substance known as a ....

a)

mixture

b)

homogeneous mixture

c)

compound

d)

heterogeneous mixture

12.

Which vocabulary combination represents substances that are pure?

a)

elements & mixtures

b)

compounds & elements

c)

mixtures & compounds

d)

solutions & elements

13.

Grape juice is classified as a ....

a)

Element

b)

Compound

c)

Heterogenous mixture

d)

Homogeneous mixture (solution)

14.
Carbon is considered an element while carbon dioxide is considered a compound. This is because carbon dioxide is –
a)
a gas at room temperature.
b)
made of two different elements.
c)
given off by green plants.
15.

This picture represents which of the following?

a)

molecules of an element

b)

molecules of a compound

c)

particles of a mixture

16.

This picture represents which of the following?

a)

molecules of an element

b)

molecules of an compound

c)

particles of a solution

17.

The phrase "blended so well you just cannot tell" refers to which type of mixture

a)

heterogeneous

b)

homogeneous

c)

compound

d)

element

18.

What does this picture portray?

a)

atom of an element

b)

element

c)

molecule of an element

d)

compound

e)

molecule of a compound

19.

What does this picture portray?

a)

atom of an element

b)

elemental substance

c)

molecule of a compound

d)

compound

20.

What is the binary molecular name for water (H2O).

a)

dihydrogen oxide

b)

dihydroxide

c)

hydrogen monoxide

d)

dihydrogen monoxide

21.

What is the molecular formula of hydrochloric acid

a)

HCl

b)

H2Cl

c)

HBr

d)

HCl2

22.

What is the name of CCl4

a)

monocarbon chloride

b)

carbon tetrachloride

c)

tetracarbon chloride

d)

carbon chloride

23.

What is the name of binary acid HF

a)

hydrofluoric acid

b)

hydrogen fluoric acid

c)

fluoric acid

d)

hydroflouride acid

24.

Antimony tribromide

a)

AnBr3

b)

AtBr3

c)

Sb1Br3

d)

SbBr3

25.

Hexaboron monosilicide

a)

B5S

b)

B6S

c)

B6Si

d)

Br6Si1

e)

Br6Si

26.

Chlorine dioxide

a)

Cl1O2

b)

CO2

c)

ClO2

d)

CrO2

27.

Dinitrogen trioxide

a)

NO3

b)

N2O3

c)

N4O6

d)

2N3O

28.

Pentaphosphorus hexasulfide

a)

K5S6

b)

P5S6

c)

P6S5

d)

6P5S

29.
If an atom becomes an ion with a 2+ charge, what does that mean?
a)
It has lost 2 electrons
b)
It has gained 2 electrons
c)
The atom is in period 2
d)
The atom has an atomic # of 2
30.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
31.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
32.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
33.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
34.

Hydrogen nitrite (nitrous acid)

a)
H2NO3
b)
HNO3
c)
HNO2
d)
H2NO2
35.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
36.
Name this compound: 
Ca(CO3)
a)
Calcium carbon oxide
b)
Calcium (II) carbonate
c)
Calcium carbonate
d)
Carbonate (I) calcide
37.
What is the compound made between Chlorate and Magnesium
a)
Cl2Mg
b)
(ClO3)2Mg
c)
MgCl2
d)
Mg(ClO3)2
38.
How do the following two elements bond together?
Pb4+  O2-       
a)
PbO
b)
Pb4O2
c)
PbO2
d)
Pb2O4
39.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
40.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
41.
Whats the formula
Sr+2  +  (CO3)-2
a)
Sr(CO3)
b)
Sr2 (CO3)2
c)
Sr1(CO)5
d)
Sr(CO5)
42.

What is the formula for phosphorous acid?

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

43.

What is the formula for nitric acid?

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

44.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

45.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
46.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
47.

carbonic acid

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

48.

Binary acids start with the prefix "____________"

a)

acid

b)

nitric

c)

hydraulic

d)

hydro

49.

When naming binary acids, the ending always changes to:

a)

-ate

b)

-ite

c)

-ic

d)

-ous

50.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

51.

Name the acid that uses an acetate ion: HC2H3O2

a)

Acetic acid

b)

Acetous acid

c)

Hydrogen Acetate acid

d)

Hydrogen Acetatic acid

52.

Name this acid: H2SO4

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

53.

There are no lone pairs and _ shared pairs of electrons surrounding the boron atom in the borane (BH3) molecule shown.

a)

4

b)

2

c)

3

d)

1

54.

What is the shape of the BH3 molecule?

a)

trigonal planar

b)

octahedral

c)

tetrahedral

d)

linear

55.

How many lone pairs and how many shared pairs of electrons surround the carbon atom in methane (CH4)?

a)
2 shared pairs, 2 lone pairs
b)
3 shared pairs, 1 lone pair
c)
1 shared pair, 3 lone pairs
d)
4 shared pairs, 0 lone pairs
56.

What is the shape of the methane molecule?

a)

linear

b)

planar

c)

tetrahedral

d)

octahedral

57.

How many lone pairs and how many shared pairs of electrons surround the nitrogen atom in ammonia (NH3)?

a)
1 shared pair and 3 lone pairs
b)
2 shared pairs and 2 lone pairs
c)
3 shared pairs and 1 lone pair
d)
4 shared pairs and 0 lone pairs
58.

What is the shape of the ammonia molecule?

a)

linear

b)

planar

c)

tetrahedral

d)

trigonal pyramidal

59.

How many lone pairs and how many shared pairs of electrons surround the oxygen atom in water (H2O)?

a)
1 lone pair and 3 shared pairs
b)
3 lone pairs and 1 shared pair
c)
4 lone pairs and 0 shared pairs
d)
2 lone pairs and 2 shared pairs
60.

What is the shape of the water molecule?

a)

bent

b)

planar

c)

tetrahedral

d)

trigonal pyramidal

61.

... bond happens when electrons are shared EVENLY between the two bonded atoms.

a)

Covalent polar

b)

Covalent nonpolar

c)

Ionic

d)

Metallic

62.

A polar bond happens between ...

a)

metal/ non metal

b)

Two non metals of the same strength

c)

Two non metals, one is stronger than the other

d)

Two metals

63.

The bond between two chlorine atoms in Cl2 molecule is ...

a)

Ionic

b)

Covalent polar

c)

Covalent nonpolar

d)

metallic

64.

The bonds between atoms in this molecule are NH3 is

a)

ionic polar

b)

ionic non-polar

c)

covalent polar

d)

covalent non-polar

65.

NH3 is a ... molecule

a)

Polar

b)

Nonpolar

66.

Chloroform (CHCl3) is a .... molecule.

a)

polar

b)

nonpolar

c)

ionic

67.

CCl4 is a ... molecule.

a)

polar

b)

nonpolar

c)

ionic

68.

Classify the following molecule.

a)

polar

b)

nonpolar

69.

CH4 is a nonpolar molecule because ...

a)

It is NOT symmetrical

b)

It is symmetrical

c)

It has polar bond between its atoms

d)

It dissolves in water

70.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
71.

What does the law of conservation of mass state?

a)

Matter can transform into energy

b)

Matter can be created and destroyed

c)

Matter can neither be created nor destroyed

d)

Only energy can be conserved, not matter

72.

What must remain the same on both sides of a balanced chemical equation?

a)

Type of molecules only

b)

Number of molecules only

c)

Number and type of atoms

d)

Energy content of the molecules

73.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
74.

How many HCl molecules do you need to balance this equation?

2Mg + ​ (a)   HCl ---> 2MgCl2 + 2H2

Choose from the below words
4
1
2
3
75.
Select the correct coefficients that will balance this equation:
__Zn + __HCl --> __ZnCl2 + __H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
76.

What are the products in the following chemical equation?

a)

CH4 and 2O2

b)

CO2 and 2H2O

77.

Octane, C8H18, is burned in the presence of oxygen gas. What are the products?

a)

Burnt Octane C8H10 and oxygen

b)

Water and Hydrogen Gas

c)

Water and Carbon Dioxide

d)

H30 + CO3

78.

What are the different types of chemical reactions?

a)

Synthesis, decomposition, single displacement, double displacement, and combustion

b)

Solid, liquid, gas, plasma

c)

Acidic, basic, neutral, alkaline

d)

Addition, subtraction, multiplication, division

79.

Given the reaction 2H2 + O2 --> 2H2O. What type of reaction is this?

a)

single replacement

b)

double replacement

c)

synthesis

d)

combustion

80.

Which one shows a single replacement reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + BC --> B + AC

d)

AB + CD --> CB + AD

81.
Cu + 2Ag(NO3) → 2Ag + Cu(NO3)
a)
Decomposition Reaction
b)
Single Displacement Reaction
c)
Double Displacement Reaction
82.
2 NH3+ 1 H2SO4 ----> 1 (NH4)2SO4
a)
Synthesis (or combination)
b)
Single displacement
c)
Double displacement
83.

Which of the following is an example of Decomposition?

a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
84.
What type of chemical reaction is this one?
C2H2 + O2 --> CO2 + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
85.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Double displacement
86.

Which of the following is a double replacement reaction?

a)

NaCl + AgNO3 > NaNO3 + AgCl

b)

Fe + CuSO4 > FeSO4 + Cu

c)

Cu + SO4 > CuSO4

87.

If the molar mass of magnesium (Mg) is 24.305 g/mol, how many grams are in 5 moles of Mg?

a)

121.525 g

b)

24.305 g

c)

121.5 g

d)

122 g

88.

How many moles is in 25.0 g of calcium?

a)

25.0 moles

b)

0.62 moles

c)

1.60 moles

d)

40.0 moles

89.

Determine the number of moles in 25.0 grams of potassium sulfide (K2S).

a)

0.23 moles

b)

4.41 moles

c)

110.3 moles

d)

25.0 moles

90.

What is the mass of 0.25 moles of rubidium bromide (RbBr)?

a)

165.34 g

b)

0.25 g

c)

41.3 g

d)

0.024 g

91.

What is the molar mass of copper sulfate (CuSO4)?

a)

159.6 g/mole

b)

111.6 g/mol

c)

77.0 g/mol

d)

none of these

92.

What is the mass of 1 mole of Co(NO3)2 cobalt(II) nitrate

a)

182.9 g/mol

b)

168.9 g/mol

c)

88.9 g/mol

d)

134.9 g/mol

e)

238.9 g/mol

93.

How many moles is in 8.40 grams of cobalt(II) nitrate, Co(NO3)2.

a)

182.9 moles

b)

8.40 moles

c)

0.0459moles

d)

21.77 moles

94.

How many molecules are in 27.5 grams of NaOH

a)

41.4 molecules

b)

4.14 x 1023 molecules

c)

4.14 x 1025 molecules

d)

1.83 x 10-21 molecules

95.

How many moles are in 2.85 x 1018 atoms of iron, Fe?

a)

41.4 moles

b)

4.14 x 1023 moles

c)

4.14 x 1025 moles

d)

4.73 x 10-06 moles

96.

For the compound Fe2O3, if we had 4 moles of Iron (Fe), how many moles of oxygen would we have?

a)

6 moles O

b)

3 moles O

c)

4 moles O

d)

9 moles O

97.

For the compound MgF2, if we had 6 moles of fluoride, how many moles of the entire compound would we have?

a)

3 moles MgF2

b)

6 moles MgF2

c)

1 mole MgF2

d)

2 moles MgF2

98.

If I had 17.0 grams of Hydrogen (H) in the compound HCl, how many grams of Chloride (Cl) would we have?

a)

597.9 g Cl

b)

0.4757 g Cl

c)

46.23 g Cl

d)

2.563 g Cl

99.

For the compound AgNO3, it took

5.873⋅10245.873\cdot10^{24}   atoms of oxygen (O) to make the compound. How many grams of silver (Ag) was needed to make the compound?
Hint: If you need help setting up the problem, check the image.

a)

350.8 g Ag

b)

1052.3 g Ag

c)

107.9 g Ag

d)

2.11⋅10262.11\cdot10^{26}  g Ag

100.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
101.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
102.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
103.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
104.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
105.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
106.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
107.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
108.

What is the molecular formula of a compound with an empirical formula of C2OH4 and a molecular mass of 88 grams per mole?

a)

C2O4H8

b)

C8O2H4

c)

C4O2H8

d)

C4O8H2

109.

Na2CO3 · 10H2O is known as sodium carbonate ______

a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
110.
Name the following hydrate:  NaCl * 5H2O
a)
sodium chloride 
b)
sodium monochloride pentahydrate
c)
sodium chloride pentahydrate
d)
pentahydrate
111.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)

contains water in the compound

d)
repels water from the compound
112.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
113.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
114.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
115.
If you predicted that 1.5 moles of Magnessium are used in a reaction, and you have 2.0 moles of Magnessium, what type of reactant is Magnessium?
a)
Limiting Reactant
b)
Excess Reactant
c)
Fast Reacter
d)
Non-Reactant
116.
If you predicted that 1.5 moles of Magnesium are used in a reaction, and you have 1.0 mole of Magnesium, how much Magnesium is in Excess?
a)
0.5 moles Mg
b)
1.5 moles Mg
c)
1.0 mole Mg
d)
0.0 Moles Mg
117.
Carbon and Oxygen combine to form CO2. If 10g of Carbon combines with Oxygen to produce 20g of CO2 and 10g of Oxygen combines with Carbon to produce 15g of CO2, How many grams of CO2 are produced from 10g of Carbon and 10g of Oxygen?
a)
20g of CO2
b)
15g of CO2
c)
17.5g of CO2
d)
25g of CO2
118.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
119.

In the equation 2 Al2O3 → 4 Al + 3 O2, what is the mole ratio of Al to O2?

a)

10 mol Al/ 6 mol O2

b)

3 mol Al/ 2 mol O2

c)

4 mol Al/ 3 mol O2

d)

2 mol Al / 3 mol O2

120.

1 N2 + 3H2 → 2NH3

How many grams of H2 are needed to react with 2.00 moles of N2?

2 mol N2mol N2×g H2\frac{2\ mol\ N_2}{mol\ N_2}\times g\ H_2

What should you put in the denominator?

a)

moles of N2

b)

moles of H2

c)

molar mass of H2

d)

molar mass of N2

121.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

122.

What mass of Carbon Dioxide, in grams, is needed to react with 3.00 mol H2O in the photosynthetic reaction described in Sample Problem B?

a)

44

b)

120

c)

40

d)

132

123.

Suppose you have two gases numbered 1 and 2.

The total pressure can be calculated to be the ____ of the pressure of each individual gas.

a)

sum (+)

b)

difference (–)

c)

product (×)

d)

quotient (÷)

e)

average

124.

Suppose you have two gases numbered 1 and 2.

Which equation represents make the most sense to calculate the total pressure exerted by both gases?

a)

Multiply their pressures :

Ptotal = P1 × P2

b)

Divide their pressures :

Ptotal = P1 ÷ P2

c)

Add their pressures :

Ptotal = P1 + P2

d)

Subtract their pressures :

Ptotal = P1 – P2

e)

Average their pressure :

Ptotal = (P1 + P2)/2

125.

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

a)

900 atm

b)

0.90 atm

c)

9.00 atm

d)

920 atm

126.

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

a)

200 mmHg

b)

80 mmHg

c)

40 mmHg

d)

120 mmHg

127.

A gas container contains hydrogen gas and water vapor. The pressure of the water is 20 torr. If the total pressure is measured to be 750 torr, what is the pressure of only the hydrogen gas?

a)

770 torr

b)

730 torr

c)

37.5 torr

d)

15,000 torr

128.
The rate of effusion is _______________ proportional to the square root of its' molar mass. 
a)
Directly
b)
Inversely 
129.
Lighter gases have a ________________ rate of effusion.
a)
faster 
b)
slower
c)
rate of effusion does not depend on mass.
130.
Which of the following would have a faster rate of effusion: 15g of Kr or 15g of N2?
a)
Kyrpton
b)
Nitrogen
c)
Both would have the same rate of effusion
131.
Effusion is
a)
used to describe the combustibility of a gas.
b)
ability of a gas to escape through a tiny opening
c)
what occurs after diffusion.
d)
the ability of a gas to mix with other gases.
132.
The rate of effusion of water vapor is 0.391 and the rate of effusion of propane is 0.251 at the same temperature and pressure.  What is the molar mass of propane? (write the formula and show your work)
a)
44.0 g/mol
b)
6.63 g/mol
c)
0.37 g/mol
d)
28.2 g/mol
133.

Identify the factor that determines rates of diffusion and effusion for different molecules at a given temperature.

a)

Size of the molecules

b)

Polarity of the molecules

c)

Temperature of the gas

d)

Molar mass of the gas

134.

Grahams law refers specifically to

a)

the rate of diffusion

b)

the rate of effusion

c)

the temperature of gases

d)

the partial and total pressures of gases in a sample.

135.

why would O2 effuse faster than CO2 in the same room

a)

because O2 has more energy

b)

because CO2 has a greater molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

136.
Which of the following gases will effuse most slowly under the same physical conditions?
Don't forget to check for diatomics!
a)
Hydrogen
b)
Chlorine
c)
Ammonia (NH3)
d)
Bromine
137.

Use Graham’s Law to calculate how 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
138.

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

a)

real gas

b)

ideal gas

c)

imaginary gas

d)

perfect gas

139.

Which condition is necessary for most gases to behave nearly ideally?

a)

high pressure

b)

high temperature

c)

low compressibility

d)

low expansion

140.

For a fixed amount of gas at a constant temperature, the volume increases as the pressure...

a)

remains steady.

b)

increases.

c)

decreases.

d)

fluctuates.

141.

The pressure exerted by a gas does not depend on

a)

temperature.

b)

volume.

c)

number of moles present.

d)

the identity of the gas.

142.
The movement of gas molecules is greatly affected by _________.
a)
the shape of the container
b)
size of the container
c)
temperature of the container
143.

Gas pressure is caused by ______.

a)

gravity.

b)

gas molecules colliding with each other.

c)

gas molecules colliding with surfaces of the container.

d)

gas molecules reacting with each other.

144.
True or false: melting and freezing occur at the same temperature!
a)
True
b)
False
c)
I don't know
145.

What happens to matter as its temperature increases?

a)

The average kinetic energy of its particles decreases

b)

The average thermal energy of its particles decreases

c)

The particles gain kinetic energy

d)

The particles lose potential energy

146.

Which among the following is NOT true regarding the Kinetic Molecular Theory of gases?

a)

Gases particles move in straight lines.

b)

Gas particles are closely packed and their motion is orderly.

c)

Gas particles are in constant motion.

d)

Gas particles do not attract or repel each other.

147.
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.
148.
Does HCl have hydrogen bonding?
a)
yes
b)
no
149.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

150.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
151.

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

152.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

153.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
154.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
155.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
156.

In a polar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom equally

d)

Only the atom with the greatest electronegativity

157.

In a nonpolar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom Equally

d)

Only the atom with the greatest electronegativity

158.

Which letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

159.

Which letter on the diagram represents a liquid?

a)

A

b)

B

c)

C

d)

D

160.

What does point B represent?

a)

Triple point

b)

Critical point

c)

Equilibrium point

d)

Normal melting point

161.

The temperature and pressure conditions at which the solid, liquid, and gas phases of a substance exist at the same time is called the

a)

Critical point

b)

Triple point

c)

Melting point

d)

Boiling point

162.

What is the normal melting point of this substance?

a)

150°C

b)

100°C

c)

-50°C

d)

0°C

163.

Which letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

164.

What is true regarding CO2 for temperatures above 31°C?

a)

It does not exist

b)

It decomposes

c)

It cannot be condensed back into a liquid

d)

It is a plasma

165.

What is the normal melting point of this substance?

a)

40°C

b)

60°C

c)

100°C

d)

110°C

166.

What phase change occurs from F to E?

a)

Sublimation

b)

Deposition

c)

Melting

d)

Condensation

167.

The temperature and pressure at which the gas and liquid states of a substance become identical and form one phase is called the

a)

Critical point

b)

Triple point

c)

Melting point

d)

Boiling point

168.

What is the normal boiling point of this substance?

a)

40°C

b)

60°C

c)

100°C

d)

110°C

169.

What phase change occurs from C to D?

a)

Condensation

b)

Vaporization

c)

Melting

d)

Sublimation

170.

What phase would this substance be in at 0.5 atm of pressure and 100°C?

a)

Solid

b)

Liquid

c)

Gas

171.

What phase change occurs from E to C?

a)

Sublimation

b)

Freezing

c)

Melting

d)

Vaporization

172.

What term is given to a reaction which transfers heat energy to the surroundings?

a)

Endothermic

b)

Reversible

c)

Exothermic

d)

Exotermic

173.

When barium hydroxide and ammonium chloride aqueous solutions react, the temperature decreases. What kind of reaction is this?

a)

Endothermic

b)

Decomposition

c)

Exothermic

d)

Indothermic

174.

When calcium reacts with water, the temperature changes from 18°C to 39°C. Which statement is correct?

a)

The solution at the end is acidic

b)

The reaction is reversible

c)

The reaction is exothermic

d)

The reaction is endothermic

175.

photosynthesis is an example of

a)

Exothermic reaction

b)

Endothermic reaction

c)

both

d)

none

176.

A + B-------> C + Heat

a)

Endothermic

b)

Exothermic

177.

What type of reaction occurs in a hand warmer?

a)

exothermic

b)

endothermic

178.

An ice pack in an example of

a)

exothermic

b)

endothermic

c)

both

d)

none

179.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

180.

What type of reaction is shown in this energy profile diagram

a)

Exothermic

b)

Endothermic

181.

What does 'X' represent in the energy profile shown here?

a)

Energy change

b)

Products

c)

Reactants

d)

Reaction progess (time)

182.

The initial temperature was measured to be 20oC and the final temperature was 10oC. The reaction was

a)

exothermic

b)

endothermic

183.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

184.

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

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

185.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

186.

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

187.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
188.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
189.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

190.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
191.
A 7.00 L sample of argon gas at 420. K exerts a pressure of 625 kPa.  If the gas is compressed to 1.25 L and the temperature is lowered to 350 K, what will be its new pressure in atm?
a)
10.4 atm
b)
2920 atm
c)
2916.7 atm
d)
28.8 atm
192.

If I have 4 moles of Argon gas at 560kPa and 0.012m3, what is the temperature?

a)

-68.4K

b)

204.6K

c)

22.1K

d)

295.7K

e)

Other

193.

If I have a gas at 120kPa, at 87oC, and at a volume of 31dm3, how many moles of gas do I have?

a)

5.2 mol

b)

0.8 mol

c)

0.2 mol

d)

1.3 mol

e)

Other

194.

If I have 7.7 moles of chlorine gas at a pressure of 9000Pa and at 56oC, what is the volume?

a)

2310.9 dm3

b)

393.4 dm3

c)

39.0 dm3

d)

2.3 dm3

e)

Other

195.

Concentration is

a)

the amount of solute in the solvent

b)

the amount of solvent in the solute

c)

density

d)

particle size

196.

In order to dilute a solution, you need to

a)

add more of the solid

b)

add more water

c)

find the mass

d)

find the volume

197.

Calculate the mass percent of solution, if there is 100 g of sugar and 400 g of water

a)

30

b)

25

c)

20

d)

15

198.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
199.
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
200.
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

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