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Chemistry Final

Total questions: 156

Worksheet time: 2hrs 1mins

Name
Class
Date
1.
There are more metals than non metals in the periodic table.
a)
True
b)
False
2.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
3.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
4.

Metals are hard because metals have a

a)

sea of electrons that tightly hold the nuclei together

b)

they form triple bonds

c)

low melting point

d)

high luster

5.

Alloys are important because

a)

their properties are often superior to the component elements

b)

their properties are a blend of the component elements

c)

they never corrode

d)

they are less expensive than their component elements.

6.

In metallic bonds electrons are:

a)

shared

b)

move around the nuclei randomly

c)

transferred

7.

Why does copper wire conduct electricity when a potential difference is applied?

a)

The crystal lattice breaks down

b)

Copper (II) ions move to the cathode

c)

The atoms of copper become ionised

d)

Bonding electrons in the crystal lattice move

8.

Why are metals malleable?

a)

The metal ions can easily slide past one another

b)

The metal ions cannot easily slide past one another

c)

The metal ions repel one another

d)

The metal ions attract one another

9.

Metals conduct electricity because

a)

the metal ions are free to travel

b)

their electrons are free to travel

c)

the bonds between metal atoms can easily be broken

d)

of witchcraft

10.

The structure of metals includes

a)

metal atoms sharing electrons

b)

metal ions bonded to non-metal ions

c)

cations surrounded by free-floating electrons

d)

metal atoms giving electrons to other metal atomes

11.

Which of the following would be held together by the metallic bond?

a)

Atoms of iron (Fe)

b)

Molecules of CH4

c)

Atoms of sulfur (S)

d)

Units of NaCl

12.

True or False: Gold reacts easily with other elements like oxygen.

a)

True

b)

False

13.

What property of metals is being shown in figure 1(b) in the image?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

14.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

15.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
16.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
17.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
18.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
19.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
20.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
21.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
22.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
23.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

24.

If Bromine bonds with Hydrogen, a ____________ bond forms.

Bromine EN = 2.96, Hydrogen EN = 2.20

a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
25.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

26.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

27.

What kind of reaction is this?

a)

Synthesis

b)

Decomposition

c)

Electrolysis

28.

What kind of reaction is this?

a)

Synthesis

b)

Decomposition

c)

Electrolysis

29.

Which of the following describes a chemical change?

a)

Atoms are rearranged, forming a new substance

b)

Reactants yield products

c)

New substance or substances are produced

d)

All of the above!

30.

How many hydrogen (H) atoms are there on the reactant side of this chemical change?

a)

3

b)

2

c)

6

31.

How many total carbon atoms are there on the product side of this chemical change?

a)

4

b)

2

c)

1

32.

What does the arrow mean in this chemical equation?

a)

Reactants

b)

Products

c)

Yield

33.

In the electrolysis of water, why did we observe more bubbles (gas) produced at the end of one pencil compared to the other?

a)

Because twice as much hydrogen gas was produced compared to oxygen gas

b)

Because twice as much oxygen gas was produced compared to hydrogen gas

c)

There was an equal amount of hydrogen and oxygen gas produced

34.

What does this chemical equation represent?

a)

Decomposition of water

b)

Synthesis of water

35.

What is one way that we may be able to produce hydrogen gas to power cars?

a)

The synthesis of water

b)

Burning coal

c)

Using oil and gasoline

d)

Electrolysis of water

36.
If fluorine is stronger then carbon, what charge will the fluorine receive?
a)
negative
b)
slight negative
c)
positive
d)
slight positive
37.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
38.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
39.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
40.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
41.

The stronger the intermolecular forces of a substance, the _____________ the melting point.

a)

higher

b)

lower

42.

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

a)

higher

b)

lower

43.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
44.

Which of the following explains the very high melting and boiling point of water?

a)

Strong dipole-dipole attractions between water molecules

b)

Strong hydrogen bonds between water molecules

c)

London dispersion forces between water molecules

d)

Dipole-induced dipole attractions between water molecules

45.
Which of the following molecules would have the lowest boiling point?
a)
CH4
b)
C2H6
c)
C3H8
d)
C4H10
46.

Propane is a gas at room temperature, while bromine is a liquid at room temperature. Which statement correctly explains these observations?

a)

Bromine has weaker intermolecular forces than propane does

b)

Bromine has greater molecular polarity than propane does

c)

Bromine has weaker molecular polarity than propane does

d)

Bromine has stronger intermolecular forces than propane does

47.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
48.
Cations are
a)
positive
b)
negative
c)
neutral
d)
nonmetals
49.
If an atom gains an electron to become an ion, it is a(n)....
a)
cation
b)
anion
c)
noble gas
d)
metal
50.
Name that Ion
Li+
a)
copper (III)
b)
lithium
c)
ladmium
d)
iodine
51.
Name the ion...  P3-
a)
Phosphorous
b)
Phosphide
c)
Phosphorous (III)
d)
Potassium 
52.
Will Magnesium gain or lose electrons to become stable?
a)
gain
b)
lose
c)
neither
53.
Name the ion....  Ca2+
a)
Calcium
b)
Calcide
c)
Calcium (II)
d)
Calciumide
54.
Ionic bonds consist of the ____ of valence electrons.
a)
sharing
b)
transfer
55.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
56.
Br-
a)
bromide
b)
bromine
c)
boron
d)
barium
57.
What is the charge does a sodium ion have?
a)
+2
b)
+1
c)
-1
d)
-2
58.

What is the symbol for Oxide?

a)

O-2

b)

HO-

c)

O2-

d)

O

59.

The positive ion changes the ending of the name.

a)

TRUE

b)

FALSE

60.

If the negative ion ends with -ate/ -ite that is means that ion is a polyatomic ion.

a)

TRUE

b)

FALSE

61.

Select ALL of the polyatomic ions.

a)

CO3-2

b)

O-2

c)

NO3-1

d)

HO-

e)

Li+

62.

What is the formula for Hydroxide?

a)

OH-1

b)

O2-2

c)

H+

d)

OH

63.

What is the correct symbol of an iron (III) ion?

a)

Fe2+

b)

Fe3+

c)

Fe2-

d)

Fe3-

64.

What is the correct symbol of a mercury (I) ion?

a)

Hg1+

b)

Hg2+

c)

Hg1-

d)

Hg2-

65.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

66.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

67.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

68.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

69.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

70.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

71.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

72.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

73.

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

74.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
75.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
76.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
77.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
78.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
79.
What is the chemical formula for Tetraphosphorous Pentachloride ?
a)
4P5Cl
b)
PCl
c)
P4Cl5
d)
none of the above
80.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
81.
What is the chemical formula for Fluorine trisulfide ?
a)
S3F
b)
FS3
c)
FS
d)
none of the above
82.
What is the chemical formula for CP ?
a)
Carbon phosphide
b)
Monocarbon phosphide
c)
Carbon monophosphide
d)
none of the above
83.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
84.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Metal and 1 Nonmetal

c)

2 Metals

d)

2 Noble Gases

85.

What is the name of the compound with the formula BrO3?

a)

bromine oxide

b)

monobromine trioxide

c)

bromine trioxide

d)

bromine (III) oxide

86.

N4O10

a)

Dinitrogen pentoxide

b)

Tetranitrogen decoxide

c)

Nitric acid

d)

Nitrogen oxide

87.

What is the correct formula for sodium oxide?

a)
b)
c)
d)
88.

What is the correct formula for magnesium fluoride?

a)
b)
c)
d)
89.

What is the charge on a lithium ion when it is bonded to a calcium ion?

a)

+3

b)

+1

c)

-1

d)

lithium will not bond with calcium

90.
Definite shape and a definite volume.
a)
Gas
b)
Liquid
c)
Solid
91.
No Definite Shape and No Definite Volume
a)
Gas
b)
Liquid
c)
Solid
92.

All matter is made of _____ that are constantly moving.

a)

insulators

b)

particles

c)

convection

d)

pieces of plastic

93.
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
94.

What happens to the average kinetic energy of matter when it is heated?

a)

It increases

b)

It stays the same

c)

It decreases

d)

It cannot be determined

95.
The amount of energy needed to change a material from a solid to a liquid state.
a)
Heat of Solids
b)
Heat of Liquids
c)
Heat of Fusion
d)
Heat of Vaporization
96.
As a material is heated, it's particles....
a)
get smaller
b)
slow down
c)
get cooler
d)
move more quickly
97.

Two flasks each contain water at 25 degrees Celsius. Which one has more heat energy?

a)

They have the same heat energy because they are the same temperature.

b)

The one on the right has more heat energy because it has less water.

c)

The one on the left has more heat energy because it has more water.

98.

This diagram represents particles in a __________ state.

a)

solid

b)

liquid

c)

gas

d)

plasma

99.

When a substance changes directly from a gas to a solid, it is called :

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Vaporization

100.

Thermal energy always moves from :

a)

Warm object to cool object

b)

Object with low KE to object with high KE

c)

Cool object o warm object

d)

Object with high mass to object with low mass

101.

What phase change occurs between points B and C if heat is added?

a)

Freezing

b)

Melting

c)

Boiling

d)

Condensing

102.

Which phase change occurs between points D and E if heat is removed?

a)

Freezing

b)

Melting

c)

Boiling

d)

Condensation

103.

A substance Y has a melting point of -7 degrees Celsius and a boiling point of 63 degrees Celsius. At which temperature is Y a liquid?

a)

-25

b)

25

c)

75

d)

150

104.

An inflated balloon is placed in a refrigerator. Which statement the movement of the gas particles in the balloon?

a)

The particles move faster and become further apart.

b)

The particles move more slowly and become further apart.

c)

The particles move faster and become closer together.

d)

The particles move more slowly and become closer together.

105.

Which of the following statements about the particles of a gas is true?

a)

The particles vibrate about a fixed position.

b)

The particles are far apart and move freely.

c)

The particles are packed close together, but in a disorderly arrangement.

d)

The particles are stationary and orderly.

106.

Particles are always moving.

a)

True

b)

False

107.

Which gas "explodes" and gives you a squeaky pop?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

108.

Which gas(es) could I test for with a glowing splint?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

109.

Which gas can relight a glowing splint?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

110.

Which gas can suffocate a lit splint?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

111.

Which of the following is the most likely clue that a reaction has created a gas?

a)

you can smell it

b)

the container gets hot

c)

the container gets cold

d)

bubbles form in liquid solution

112.

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

113.
Of these three states of matter, which one has the most kinetic energy? 
a)
Solid 
b)
Liquid 
c)
Gas
114.

What phase change is occurring when substances like dry ice turn straight from a solid to a gas?

a)

sublimation

b)

deposition

c)

evaporation

d)

freezing

115.

A substance's heating curve is shown in the graph. What is its boiling point? (Diagram B)

a)

100 C

b)

60 C

c)

80 C

d)

20 C

116.

Match the following phase changes

a)

Melting

1.

Solid -> Liquid

b)

Evaporation

2.

Liquid -> Gas

c)

Deposition

3.

Gas -> Solid

117.

Match the following phase changes

a)

Freezing

1.

Liquid -> Solid

b)

Condensation

2.

Gas -> Liquid

c)

Sublimation

3.

Solid -> Gas

118.

Water bugs can walk on water because of _______ tension.

a)

surface

b)

Santa Claus

c)

San Diego

119.

Surface tension is the property of water in which...

a)

water molecules at the surface tend to stick together.

b)

water spills easily.

c)

water tends to be see-through.

120.
molecule in which opposite ends have opposite electric charges
a)
cohesion
b)
polar molecule
c)
hydrogen bond
d)
solution
121.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
122.

Which solution contains an electrolyte?

a)

A

b)

B

123.

Oil is a nonpolar substance. Why can't it dissolve in water?

a)

water is nonpolar

b)

water is polar

c)

oil is an electrolyte

d)

oil is a colloid

124.

In this solution, what is the solute?

a)

water

b)

koolaid

125.

If water contains dissolved substances, it is known as ___.

a)

an organic solvent

b)

a nonelectrolyte

c)

an aqueous solution

d)

a nonpolar solution

126.

Which substances dissolve best in water?

a)

gasoline and kerosene

b)

ionic compounds

c)

nonelectrolytes

d)

colloids

127.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
128.

Under which conditions would carbon dioxide be most soluble in water?

a)

20 degrees Celsius and 1 atm

b)

20 degrees Celsius and 2 atm

c)

10 degrees Celsius and 1 atm

d)

10 degrees Celsius and 2 atm

129.

At which temperature would 100 g of liquid water contain the most dissolved nitrogen?

a)

20 degrees Celsius

b)

15 degrees Celsius

c)

10 degrees Celsius

d)

5 degrees Celsius

130.
a)

solvent

b)

solute

c)

solution

131.
a)

solvent

b)

solute

132.
a)

solute

b)

solvent

133.
a)

solute

b)

solvent

134.
a)

solvent

b)

solution

c)

solute

135.
a)

solution

b)

solute

c)

solvent

136.
In this mixture, which of the following will be the solute?
a)
The water in the glass
b)
The glass that holds the final mixture
c)
The solution containing both powder and water
d)
The powder on the spoon
137.

In which beaker does salt dissolves faster?

a)

Hot water

b)

Room temperature

c)

Ice watet

138.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg + O2→ MgO

b)

Mg+ O→ MgO

c)

Mg + CO2 → MgO + C

d)

Mg + O2→ Mg2O2

139.

Sodium reacts with chlorine gas to produce sodium chloride.

a)

NaCl→ Cl + Na

b)

Na+ CO2 → NaCO2

c)

Na + Cl2→ NaCl

d)

Na + Cl → NaCl

140.

Magnesium + ________ --> magnesium oxide


What is missing?

a)

Hydrogen

b)

Sulphur

c)

Oxygen

d)

Oxide

141.

What are the reactants in this word equation?

a)

Carbon dioxide and oxygen

b)

Carbon dioxide and water

c)

Oxygen and glucose

d)

Oxygen and water

142.

In this chemical reaction zinc is a...

a)

Product

b)

Reactant

c)

Neither

143.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

144.
 Mg  +  ___ HCl  →   MgCl2  +   H2
a)
1
b)
2
c)
3
d)
4
145.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
146.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
147.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
148.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
149.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
150.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
151.

A reaction that gives out energy to the surroundings causes the surroundings ....

a)

temperature to drop

b)

temperature to rise

c)

temperature to remain constant

d)

temperature to vary

152.

In the reaction picture, the energy will be on product or reactant

a)

Product

b)

Reactant

153.
What type of reaction is shown in the reaction pathway?
a)

endothermic reaction

b)

exothermic reaction

154.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

155.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

156.

CaO(s) + H2O(l) ⟶ Ca(OH)2(s)     ΔH = −65.2 kJ

Is the above reaction exothermic or endothermic?

a)

Exothermic

b)

Endothermic

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