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Physical Science Unit 4- Bonding and Reactions

Total questions: 215

Worksheet time: 4hrs 48mins

Name
Class
Date
1.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
2.
How many atoms of carbon (C) are in  C6H12O6?
a)
3
b)
6
c)
12
d)
24
3.
Which is the correct formula for:
one carbon (C)
two oxygen (O)
a)
CO2
b)
CO
c)
C2O
d)
2CO
4.
Metals tend to 
a)
gain electrons
b)
lose electrons
5.

Atoms that gain electrons become

a)

positively charged

b)

neutrally charged

c)

negatively charged

6.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
7.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
8.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
9.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
10.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
11.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
12.
An ion with a positive charge is a/an 
a)
anion
b)
cation
13.
An ion with a negative charge is a/an
a)
anion
b)
cation
14.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
15.

Name the following compound: CaCl2

a)

calcium dichloride

b)

calcium chloride

c)

calcium (II) chloride

d)

carbon chloride

e)

None of these.

16.

Name the following compound: Na2S

a)

sodium sulfide

b)

disodium sulfide

c)

sodium sulfur

d)

sodium monosulfide

e)

None of these.

17.

What is the formula for: magnesium sulfide

a)

MgS

b)

Mg2S2

c)

MnS

d)

MgS2

e)

None of these.

18.

What is the formula for: aluminum phosphide

a)

AlP

b)

AlP3

c)

Al3P3

d)

Al3P2

e)

None of these.

19.
What is the correct formula for potassium oxide?
a)
KO
b)
KO2
c)
K2O
d)
KO3
20.
Name the following ionic compound: Cs2S
a)
cesium sulfide
b)
cesium sulfate
c)
cesium II sulfate
d)
cesium II sulfide
21.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
22.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
23.

Hexaboron monosilicide

a)

B5S

b)

B6S

c)

B6Si

d)

Br6Si2

e)

Br6Si

24.

Iodine pentafluoride

a)

I1P6

b)

I1F5

c)

IF5

d)

IFl5

25.

Dinitrogen trioxide

a)

NO3

b)

N2O3

c)

N4O6

d)

2N3O

26.

P4S5

a)

phosphorus sulfide

b)

quadphosphorus hexasulfide

c)

tetraphosphorus pentasulfur

d)

tetraphosphorus pentasulfide

27.

SeF6

a)

silicon fluoride

b)

selenium fluoride

c)

selenium hexafluoride

d)

selenium heptafluoride

28.

CCl4

a)

Methane

b)

carbon tetrachloride

c)

carbon quadchloride

d)

monocarbon tetrachloride

29.
Elements combine to form __________.
a)
compounds
b)
atoms
c)
positive ions
d)
negative ions
30.
What part of an atom is involved in chemical bonding?
a)
protons
b)
neutrons
c)
electrons
d)
nucleus
31.
How many valence electrons does nitrogen have?
a)
3
b)

2

c)
5
d)
1
32.
Where are the non-metals located on the periodic table?
a)
All over
b)
On the left side of the "staircase"
c)
On the right side of the "staircase"
33.

Which is the correct name for the ionic compound, LiCl?

a)

monolithium monochloride

b)

lithium chloride

c)

lithium monochloride

d)

lithium (I) chloride

34.
A covalent bond is formed when two atoms ____ electrons
a)
share
b)
lose
c)
transfer
d)
gain
35.
How does a calcium atom form a bond with an oxygen atom?
a)
They form a bond by sharing two pairs of electrons, both of which come from the calcium atoms.
b)
They form a bond by sharing two pairs of electrons, both of which come from the calcium atoms.
c)
They form a bond by transferring two electrons from the calcium atom to the oxygen atom.
d)
They form a bond by transferring two electrons from the oxygen atom to the calcium atom.
36.
Which of the following statements about ionic compounds in solid state is true?
a)
A cation is only bonded to the anion(s) that it donates its electron(s) to.
b)
They can conduct electricity due to the presence of free-moving ions.
c)
Its structure is a giant lattice in which ions are held by electrostatic attraction.
d)
They have a simple molecular structure as a result of the transfer of electron(s) between the metal and non-metal.
37.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

38.

Which of the following is NOT TRUE about covalent compounds?

a)

They have low melting and boiling points.

b)

They are formed from 2 nonmetals.

c)

They can conduct electricity when dissolved in water (aqueous).

39.

What property is describing an ionic compound?

a)

shares electrons

b)

high melting point

c)

weak bonds

d)

made up of nonmetals.

40.

Select all the true statements about the compound shown above.

a)

It is covalent

b)

It will conduct electricity when dissolved in water

c)

It is ionic

d)

It will dissolve in water

e)

It has a low melting point

41.
When Aluminum forms an ionic compound then it will ________________ electron(s).
a)
gain 1
b)
gain 2 
c)
gain 3
d)
lose 3 
42.
What is the charge for the halogens when they become ions?
a)
1+
b)
2+
c)
1-
d)
2-
43.
What type of bond is this? Lithium with Fluorine?
a)
ionic
b)
covalent
44.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

45.

A sodium ion has a charge of

a)

-1

b)

-2

c)

+1

d)

+2

46.

True or False: Sodium and Chloride ions have equal but opposite charges

a)

True

b)

False

47.

True or False: An ionic bond forms when atoms of a non-metal give up electrons to atoms of a metal

a)

True

b)

False

48.

An example of a covalent compound is

a)

sodium floride

b)

calcium chloride

c)

carbon dioxide

d)

all of the above

49.

In all covalent bonds, valence electrons are

a)

lost

b)

gained

c)

shared equally

d)

shared

50.

What is the chemical formula for the compound containing one nitrogen atom and two oxygen atoms?

a)

O2N

b)

N2O

c)

NO

d)

NO2

51.

Chemical bonds always involve

a)

ions

b)

protons

c)

metals

d)

electrons

52.

True or False: An oxygen atom has eight valence electrons

a)

True

b)

False

53.

The chemical formula for carbon dioxide is

a)

CO

b)

C2O

c)

CO2

d)

C2O2

54.

Chemical bonds form when atoms

a)

gain protons

b)

combine nuclei

c)

give up neutrons

d)

share or transfer electrons

55.
An ionic compound of calcium and chlorine would be named
a)
calcium chlorine.
b)
calcium chlorite.
c)
calcium chloride.
d)
chlorine calcium.
56.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

57.

Metals tend to

a)

gain electrons

b)

lose electrons

58.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
59.

What is the name of the following compound: CS2?

a)

Carbon Sulfide

b)

Monocarbon Sulfide

c)

Monocarbon disulfide

d)

Carbon disulfide

60.

What is the name of the following compound: CO2?

a)

Carbon Dioxide

b)

Monocarbon dioxide

c)

Dicarbon monoxide

d)

Carbon oxide

61.

What is the name of the following compound: NaCl?

a)

Monosodium monochloride

b)

Sodium chlorine

c)

Sodium chloride

d)

Sodium monochloride

62.

What is the chemical formula of the following compound: potassium chloride

a)

PCl

b)

KCl

c)

KCl2

d)

K2Cl

63.

A covalent bond is made of the 2 following kinds of elements:

a)

Metal and metal

b)

Nonmetal and nonmetal

c)

Metalloid and Metalloid

d)

Metal and nonmetal

64.

Ionic compounds are made of the two following kinds of elements:

a)

Metal and metal

b)

Nonmetal and nonmetal

c)

Metalloid and metalloid

d)

Nonmetal and metal

65.

What is the name of the following compound: Ag3PO4?

a)

Silver potassium

b)

Silver phophate

c)

Gold potassium

d)

Gold phosphate

66.

What is the formula for the compound carbon tetrachloride?

a)

CF

b)

CF3

c)

C2F4

d)

CF4

67.

What is the name of the following formula: Li2O?

a)

Lithium oxide

b)

Dilithium monoxide

c)

Lithium monoxide

d)

Lithium oxygen

68.

What is the name of the following chemical compound: SF6?

a)

Sulfur fluoride

b)

Monosulfur hexafluoride

c)

Sulfur hexafluoride

d)

Sulfur fluorine

69.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
70.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
71.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
72.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
73.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
74.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
75.

Which of these is NOT a property of most metals?

a)

Good conductor of electricity

b)

Malleable

c)

Low melting point

d)

Ductile

76.

Most SIMPLE covalent molecules are (a)   at room temperature

77.

When would you find ionic bonding?

a)

Between metal and non-metal

b)

In metals

c)

Between two or more non-metals

78.

When would you find covalent bonding?

a)

Between metal and non-metal

b)

In metals

c)

Between two or more non-metals

79.

What type of bonds hold together the carbon atoms in diamond?

a)

covalent

b)

ionic

c)

metallic

80.

Ionic substances can conduct electricity only when (a)   or dissolved in water

81.

Which bonds hold together the atoms in a molecule of carbon dioxide?

a)

ionic

b)

covalent

c)

metallic

82.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
83.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
84.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
85.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
86.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
87.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
88.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
89.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
90.
usually soft
a)
ionic compounds
b)
covalent compounds
91.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
92.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

93.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
94.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

95.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

96.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

97.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

98.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

99.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
100.

To form the nitride ion, the nitrogen atom needs to _____ electrons and will have a ______ charge.

a)

gain 3; 3−\text{gain }3;\ 3-  

b)

gain 3; −3\text{gain }3;\ -3  

c)

lose 5; 5−\text{lose }5;\ 5-  

d)

lose 5; 5+\text{lose }5;\ 5+  

101.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

102.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

103.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
104.

When electrons are lost by one atom and gained by another, so that they both get full outer shells.

a)

Covalent bond

b)

Ionic bond

c)

Pairing

d)

Compound

105.

When atoms share electrons so that they both get a full outer shell.

a)

Covalent bond

b)

Ionic bond

c)

Compound

d)

Pairing

106.

What type of reaction involves the breaking down of a substance into simpler substances?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

107.

What type of reaction involves 2 substances combining to form 1 new compound?

a)

Decomposition Reaction

b)

Single Displacement Reaction

c)

Double Displacement Reaction

d)

Synthesis Reaction

108.

What type of reaction involves one element replacing another element in a compound?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

109.

What type of reaction involves ions from 2 compounds exchanging places to form 2 completely new compounds?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

110.

What type of reaction involves one element replacing another element in a compound?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

111.

What are the reactants in the chemical equation pictured?

a)

CH4 and CO2

b)

CH4 and O2

c)

CO2 and H2O

d)

O2 and H2O

112.

What are the products of the chemical reaction pictured?

a)

CH4 and CO2

b)

CH4 and O2

c)

CO2 and H2O

d)

O2 and H2O

113.

What type of chemical reaction is this one?

Al(OH)3 --> Al2O3 + H2O

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

114.

What type of chemical reaction is this one?

CUO + CO2 --> CuCO3

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

115.

What type of chemical reaction is this one?

Ca + MgCl2 --> CaCl2 + Mg

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

116.

What type of reaction is illustrated below?

2HI --> H2 + I2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

117.

What type of reaction is illustrated below?

Zn + H2S --> ZnS + H2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

118.

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Combination

b)

Decomposition

c)

Single replacement

d)

Double replacement

119.

2Na +S → Na2S

a)

Double Replacement

b)

Decomposition

c)

Combustion

d)

Synthesis

120.

2 NO2 ---> 2 O2 + N2

a)

Synthesis

b)

Single Replacement

c)

Decomposition

d)

Combustion

121.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

122.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

123.

What reaction has the following general formula:

AB + CD --> CB + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

124.

What reaction has the following general formula:

A + B --> AB

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

125.

What type of reaction is the following:
BaCl2+2KI −> 2KCl + BaI2BaCl_2+2KI\ ->\ 2KCl\ +\ BaI_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

126.

What type of reaction is the following:
2KI −> 2K + I22KI\ ->\ 2K\ +\ I_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

127.

What type of reaction is the following:
2NaHCO3−> Na2CO3+CO2+H2O2NaHCO_3->\ Na_2CO_3+CO_2+H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

128.

What type of reaction is the following:
Zn + 2HCl −> ZnCl2+H2Zn\ +\ 2HCl\ ->\ ZnCl_2+H_2

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

129.

What type of reaction is the following:
3CuS +2Al −> Al2S3+3Cu3CuS\ +2Al\ ->\ Al_2S_3+3Cu

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

130.

What type of reaction is the following:
Na2S +2HCl −> H2S+2NaClNa_2S\ +2HCl\ ->\ H_2S+2NaCl

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

131.

What type of reaction is the following:
Na2S +2HCl −> H2S+2NaClNa_2S\ +2HCl\ ->\ H_2S+2NaCl

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

132.

What type of reaction is the following:
Ag3N + 3HBr−>3AgBr+H3NAg_3N\ +\ 3HBr->3AgBr+H_3N

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

133.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
134.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
135.
The following reaction is an example of what reaction type? 
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
136.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
137.

What type of reaction is shown in all four models?

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

138.
Ca + AlCl3→ CaCl2 + Al
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
139.
Si + S8 →Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
140.
Mg + N2 →Mg3N2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
141.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
142.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

143.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

144.

a different way to say Law of Conservation of Matter

a)

Law of Conservation of Volume

b)

Law of Conservation of Energy

c)

Law of Conservation of Mass

d)

Law of Conservation of Environment

145.

a way to describe a chemical reaction using chemical formulas and other symbols

a)

mathematical formula

b)

mathematical equation

c)

chemical formula

d)

chemical equation

146.

a substance that takes part in and undergoes change during a reaction

a)

coefficient

b)

subscript

c)

reactant

d)

product

147.

a new material formed in a chemical reaction

a)

coefficient

b)

subscript

c)

reactant

d)

product

148.

a reaction in which energy is absorbed

a)

exothermic reaction

b)

endothermic reaction

c)

red hot reaction

d)

cool reaction

149.

a reaction that releases energy, usually in the form of heat.

a)

exothermic reaction

b)

endothermic reaction

c)

red hot reaction

d)

cool reaction

150.

Suppose you have 15g of baking soda and mix it with 15g of vinegar. When they are combined they bubble and fizz a lot. The final solution has a mass of 25g. What happened to the "lost" 5g?

a)

it dissappears

b)

it is still there just not weighted

c)

it is in the gas that is formed

d)

nothing happened

151.

Balance this equation:

MgCl2 --> Mg4 + Cl2

a)

It's already balanced.

b)

4 MgCl2 --> Mg4 + 4 Cl2

c)

4 MgCl2 --> Mg4 + 5 Cl2

152.

How many atoms of aluminum are on each side of the following equation?

4Al + 3O2 --> 2Al2 O3

a)

2

b)

6

c)

4

d)

1

153.
A precipitate is a 
a)
liquid that forms when two solids are reacted
b)
a solid that forms when two liquids are mixed
c)
a gas that forms when vinegar and baking soda react
d)
a change of color in a solution
154.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
155.

The Law of Conservation of Mass States

a)

Energy cannot be created nor destroyed, it can only change form.

b)

Mass cannot be created nor destroyed, it can only change form.

c)

Mass can be created or destroyed, it cannot change form.

156.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
157.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

158.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

159.

A student pours hydrochloric acid (HCl) into an open beaker that contains a piece of magnesium (Mg). A chemical reaction occurs, and the data for the reaction is shown in the image. Which of the following answer choices best identifies a possible explanation for the change in mass? SELECT TWO.

a)

There was a increase in mass.

b)

There was a decrease in mass.

c)

There was no change in mass.

d)

Because the reaction occurred in an open container, a gas that was produced was able to escape

e)

Because the reaction occurred in an open container, a gas in the air was able to react with the other chemicals

160.

A student heated a 10 gram sample of a chemical in an open container. A chemical reaction occurred, and the mass of the sample was measured again. The mass of the sample was found to be less than before the reaction. Which of the following best explains the decrease in mass of the sample?

a)

The heat caused the chemical to become less dense.

b)

The reaction gave off more heat than was added.

c)

Some of the lighter particles were destroyed.

d)

Some of the particles escaped as a gas formed.

161.

A student measures the mass of an iron nail to be 25 grams. The student heats the nail over a bunsen burner and measures the mass of the nail afterwards. The mass of the nail is found to be greater after burning. Which of the following best explains the increase in mass of the nail?

a)

The heat caused the compound to become more dense.

b)

The reaction gave off less heat than was added.

c)

Some of the heavier particles multiplied inside the nail.

d)

Extra particles from the air were added to the nail during burning.

162.

How many oxygen atoms are in the products for the chemical reaction below?
4Fe + 3O2 → 2Fe2O34Fe\ +\ 3O_{2\ }\rightarrow\ 2Fe_2O_3  

a)

2

b)

3

c)

5

d)

6

163.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
164.
Is this equation balanced or unbalanced? 
H2 + O2 --> H2O
a)
balanced
b)
unbalanced
165.

When sodium and chlorine combine to form sodium chloride, sodium chloride is the:

a)

Originator

b)

Reactant

c)

Product

d)

Produce

166.
Anthony is performing an experiment. He adds 0.25 grams of baking soda to 5 grams of water and stirs. Anthony watches as the baking soda dissolves in the water. If Anthony weighs the water and baking soda solution, what will its mass be?
a)
4.75 grams
b)
5.0 grams
c)
5.25 grams
d)
7.5 grams
167.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

168.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
169.

1. Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the most exothermic?

a)

A. temperature rises by 3 °C\degree C    

b)

B. temperature falls by 5 °C\degree C   

c)

C. temperature falls by 3 °C\degree C    

d)

D. temperature rises by 5 °C\degree C  

170.

4. Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the least endothermic?

a)

A. temperature falls by 3 °C\degree C    

b)

B. temperature rises by 5 °C\degree C

c)

C. temperature falls by 5 °C\degree C

d)

D. temperature rises by 3 °C\degree C

171.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
172.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
173.
Baking bread and cooking an egg are examples of....?
a)
Endothermic processes
b)
Exothermic processess
c)
None of these 
174.
What type of reaction is shown in the photo?
a)
Exothermic
b)
Isothermic
c)
Endothermic
d)
None of the  above
175.

What type of reaction occurs in a hand warmer?

a)

exothermic

b)

endothermic

176.

5. When ammonium chloride dissolves in water the temperature falls. The type of energy change is described as?

a)

A. exothermic    

b)

 B. activated  

c)

C. decomposition            

d)

D. endothermic

177.

O2(g) + 2 H2 (g) → 2 H2O (g) + EnergyO_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy  

a)

endothermic

b)

exothermic

178.

6 CO2+ 6 H2O + Energy → C6H12O6 + 6 O26\ CO_2+\ 6\ H_2O\ +\ Energy\ \rightarrow\ C_6H_{12}O_6\ +\ 6\ O_2

a)

endothermic reaction

b)

exothermic reaction

179.

A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true?

a)

It is an exothermic reaction

b)

It is an endothermic reaction

180.

Fire is an example of

a)

exothermic reaction

b)

endothermic reaction

c)

none

d)

both

181.

Fireworks are an example of

a)

exothermic

b)

endothermic

c)

both

d)

none

182.

Your hands get cold outside from not wearing gloves

a)

exothermic

b)

endothermic

c)

both

d)

none

183.

An ice pack in an example of

a)

exothermic

b)

endothermic

c)

both

d)

none

184.

A melting ice cube is an example of

a)

exothermic

b)

endothermic

c)

none

d)

both

185.

What coefficients are needed to balance the equation?

__ SiCl4 + __ H2O → __ H4SiO4 + __ HCl

write the numbers in order like this: #, #, #, #

(a)  

186.

What coefficients are needed to balance the equation?

__ Al + __ HCl → __ AlCl3 + __ H2

write the numbers in order like this: #, #, #, #

(a)  

187.

What coefficients are needed to balance the equation?

__ C7H6O2 + __ O2 → __ CO2 + __ H2O

write the numbers in order like this: #, #, #, #



(a)  

188.

KClO3 → KClO4 + KCl

(a)  

189.

H2SO4 + HI → H2S + I2 + H2O

(a)  

190.

What is the left part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical equation

191.

What is the right part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical Equation

192.

What is the total number of atoms present in 5Na3PO4?

a)

5

b)

55

c)

40

d)

8

193.

What is the little number after an element in a chemical equation called?

Example: H2

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

194.

Is the following equation balanced?

Al + O2 ---> 2Al2O3

a)

YES

b)

NO

195.

What is the number before a chemical formula called?

Example: 2H2 + O2 ---> 2H2O

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

196.

Which of the following equations are correctly balanced?

a)

12CO2 + H2O ---> C6H12O6 + O2

b)

CO2 + H2O ---> 3C6H12O6 + O2

c)

CO2 + 9H2O ---> C6H12O6 + O2

d)

6CO2 + 6H2O ---> C6H12O6 + 6O2

197.

Balance this equation:

H2 + Cl2 ---> HCl

a)

It is balanced.

b)

H2 + Cl2 ---> 2HCl

c)

3H2 + Cl2 ---> 6HCl

d)

H2 + 3Cl2 ---> 6HCl

198.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
199.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
200.
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
201.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
202.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
203.

Fill in the blanks with coefficient:

PCl5+_ H2O→_ HCl+H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

204.
Balance this equation:
P4+O2  -->  P2O3
a)
3 P4+ O2 --> 2 P2O3
b)
 P4+ O2 --> 2 P2O3
c)
 P4+ 3 O2 --> 2 P2O3
d)
 P4+ 2 O2 --> 3 P2O3
205.

Balance the following equation:

___ Mg+ ___ O2→___ MgO

a)

1, 1, 3

b)

2, 1, 2

c)

1, 2, 1

d)

2, 2, 2

206.

Select all of the reactants in the following reaction:

Hydrogen + Oxygen --> Water

a)

Hydrogen

b)

Oxygen

c)

Water

207.

Select all of the reactants in the following reaction:

Barium carbonate + Nitric acid --> Barium nitrate + Water + Carbon dioxide

a)

Barium carbonate

b)

Nitric acid

c)

Barium nitrate

d)

Water

e)

Carbon dioxide

208.

Select all of the reactants in the following reaction:

Sodium hydroxide + Hydrochloric acid --> Sodium chloride + Water

a)

Sodium hydroxide

b)

Hydrochloric acid

c)

Sodium chloride

d)

Water

209.
Magnesium can be burned in air to produce solid magnesium oxide.
a)
2Mg(s) + O2(g)→ 2MgO(s)
b)
Mg(s) + O(g) → MgO(s)
c)
2Mg(s) + CO2(g) → 2MgO(s) + C(s)
d)
2Mg(s) + O2(g) → Mg2O2(s)
210.
Sodium reacts with chlorine to produce sodium chloride.
a)
NaCl(s) → Cl(g) + Na(s)
b)
Na(s) + CO2(g) → NaCO2(s)
c)
2Na(s) + Cl2(g) → 2NaCl(s)
d)
Na(s) + Cl(g) → NaCl
211.

When hydrogen reacts with sulfur, a smelly gas, dihydrogen monosulfide, is produced.

a)

H2 + S → HS

b)

H2 + S → H2S

c)

H + S→ HS

d)

H + S→ H2S

212.

Hydrogen gas and nitrogen monoxide gas forms water and nitrogen gas.

a)

H2 + NO --> H2O + N2

b)

H + NO --> H2O + N

c)

H2 + N2O3 --> H2O + N2

d)

H + NO --> H2O + N2

213.

Aluminum bromide and chlorine gas produce aluminum chloride and bromine gas.

a)

AlBr3 + Cl2 --> AlCl3 + Br2

b)

AlBr3 + Cl --> AlCl3 + Br

c)

Al3Br + Cl --> Al3Cl + Br2

d)

AlBr3 + Cl2 --> AlCl3 + Br

214.

Hydrogen gas and chlorine gas produce hydrogen chloride

a)

H2 + Cl2 --> HCl

b)

H + Cl --> HCl

c)

H2 + Cl2 --> H2Cl2

d)

H + Cl --> H2Cl

215.

Aluminum and oxygen produces aluminum oxide

a)

Al + O2 --> Al2O3

b)

Al + O --> Al2O3

c)

Al3 + O2 --> Al2O3

d)

Al + O --> AlO

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