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Worksheets

Semester 1 Review

Total questions: 265

Worksheet time: 5hrs 55mins

Name
Class
Date
1.

Which of the following is a correct lab safety rule?

a)

Eating during experiments is allowed

b)

Always wear safety goggles when handling chemicals

c)

Smell chemicals directly from the container

d)

Use broken glassware if it looks clean

2.

Oil and Water

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

3.

Copper - Cu

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

4.

Chalk - CaCO3

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

5.

Rocks and Sand

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

6.

Water - H2O

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

7.

Aluminum - Al

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

8.

Air

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

9.

Sugar (sucrose) ----C6H22O11

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

10.

Is melting butter for popcorn a chemical or physical change?

a)

chemical

b)

physical

11.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
rust
12.
Freezing Juice?
a)
Physical Change
b)
Chemical Change
13.
Fizzing, foaming, and burning are all examples of
a)
Chemical change
b)
Physical change
14.
Dissolving sugar in water is an example of a 
a)
physical change
b)
chemical change
15.
Digesting your food is an example of 
a)
chemical change
b)
physical change
16.
Rotting bananas?
a)
Physical Change
b)
Chemical Change
17.

What kind of change is it most likely if there is a color change?

a)

Physical change

b)

Chemical change

18.

An ice cube is placed in the sun. Later there is a puddle of water. Later still the puddle is gone.

a)

Physical Change

b)

Chemical Change

19.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

20.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
21.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
22.
Atoms of the same element but with different numbers of neutrons.
a)
Ion
b)
Isotope
c)
Mass Number
d)
electron
23.

Carbon has how many protons?

a)

12

b)

6

c)

7

d)

4

24.

What is Oxygen's atomic number?

a)

8

b)

16

c)

15

d)

6

25.

Iodine has ______ electrons

a)

127

b)

53

c)

74

d)

7

26.

How many protons are in Gold

a)

79

b)

197

c)

118

d)

276

27.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

28.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

29.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
30.

Positively charged atoms with electrons. "Plum pudding"

a)

Democritus

b)

Bohr

c)

Thomson

d)

Dalton

31.

conducted gold foil experiment

a)

Schrodinger

b)

Dalton

c)

Heisenberg

d)

Rutherford

32.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
33.

Which one of these is Dalton's Model?

a)
b)
c)
d)
34.

The two subatomic particles found in the nucleus are ____________________.

a)

protons and electrons

b)

protons and neutrons

c)

neutrons and electrons

d)

protons, neutrons, and electrons

35.

Electrons are found in _____________.

a)

the nucleus

b)

the center

c)

the electron cloud

36.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
37.
What is the mass number?
a)
the number of protons
b)
the sum of the number of protons and the number of neutrons in the nucleus of an atom 
c)
the number of electrons
d)
the number of neutrons
38.
an atom with atomic number 6 would have how many protons 
a)
6
b)
12
c)
3
d)
cannot be determined 
39.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
40.
An atom has 5 protons and 7 neutrons. What is the mass number of the atom?
a)
5
b)
7
c)
2
d)
12
41.
An atom has an atomic number of 19 and a mass number of 29. How many neutrons are in the atom?
a)
30
b)
19
c)
10
d)
38
42.
Outside the nucleus of an atom are these
a)
protons
b)
neutrons
c)
quarks
d)
electrons
43.

An atom has 12 protons and 13 neutrons in its nucleus. Which is the correct symbol?

a)
b)
c)
d)
44.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
45.

Anions are...

a)

Positive

b)

Negative

c)

Neutral

46.

An element has 25 protons and 22 electrons. It has a charge of...

a)

3+

b)

3-

c)

2+

d)

1-

47.
How is carbon-12 different from carbon-14?
a)
They have a different number of protons
b)
they have a different number of electrons
c)
they have a different number of neutrons
48.

What is atomic mass?

a)

The average mass that is weighted based on the abundance of the isotopes of the element

b)

The mass that is weighted based on the abundance of the isotopes of the element

c)

The average mass that is weighted based on the abundance of the protons of the element

d)

The average mass that is weighted based on the abundance of the neutrons of the element

49.

A neutral atom always has the same number of protons and ______.

a)

electrons

b)

neutrons

c)

ions

d)

nuclei

50.

The nucleus of which atom is represented below?

a)

Mg

b)

Br

c)

Al

d)

Na

51.

How many neutrons are in the given atom?

a)

92

b)

143

c)

235

d)

327

52.

Elements are known (named) based on the number of ____________ in their atom.

a)

electrons

b)

neutrons

c)

ions

d)

protons

53.
These particles have a mass of 1 amu
a)
protons and neutrons
b)
protons and electrons
c)
neutrons and electrons
54.
What are the 3 subatomic particles that make-up the atom?
a)
protons, neutrons, and isotopes
b)
neutrons, isotopes, and electrons
c)
positives, negatives, and electrons
d)
protons, neutrons, and electrons
55.
This subatomic particle has basically no mass
a)
protons
b)
neutrons
c)
electrons
d)
protons and neutrons
56.

If Carbon-14 has 6 protons, how many neutrons does it have?

a)

6

b)

7

c)

8

d)

14

57.

Which of the following is true about isotopes?

a)

They have different atomic numbers.

b)

They have the same number of neutrons.

c)

They have the same number of protons.

d)

They are different elements.

58.

How can you find the number of neutrons in an isotope?

a)

Subtract the atomic number from the mass number.

b)

Add the atomic number to the mass number.

c)

Multiply the atomic number by 2.

d)

Divide the mass number by the atomic number.

59.

What is the mass number of an isotope with 20 protons and 22 neutrons?

a)

20

b)

22

c)

40

d)

42

60.

If an isotope has an atomic number of 15 and a mass number of 31, how many neutrons does it have?

a)

15

b)

16

c)

31

d)

46

61.

Which of the following isotopes has the most neutrons?

a)

Oxygen-16

b)

Oxygen-17

c)

Oxygen-18

d)

They all have the same number of neutrons.

62.

A nuclear reaction involves what two parts of the atom? (that are in the nucleus)

a)

electrons and protons

b)

protons and neutrons

c)

neutrons and electrons

d)

nucleus and protons

63.

The splitting of a nucleus into smaller, lighter nuclei is called what?

(taking a large marshmallow and tearing it into two smaller pieces)

a)

fusion

b)

fission

c)

hydrogen bomb

64.

What process occurs when two sets of nuclei merge to form one singe, large nuclei

(many small marshmallows smash together to form one big sticky marshmallow)

a)

fission

b)

fusion

c)

atomic bomb

65.

What is the process in which an unstable atomic nucleus emits charged particles or energy or both?

a)

radioactivity

b)

oxidation

c)

decomposition

d)

synthesis

66.

The stability of an isotope nucleus depends on the ____.

a)

atomic number

b)

atomic mass

c)

number of neutrons

d)

neutron-to-proton ratio

67.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
68.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
69.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
70.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
71.

How many valence Electrons does Copper Have?

1s2 2s2 2p6 3s2 3p6 4s2 3d9

a)

6

b)

9

c)

17

d)

2

72.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
73.
What atom matches this electron configuration?
[Xe] 6s25d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
74.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
75.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
76.
Magnesium's ion
a)
Mg+
b)
Mg2+
c)
Mg-
d)
Mg2-
77.
What is this element? 
[Ar]4s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
78.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
79.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

80.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
81.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

82.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
83.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
84.

What does the 1 in "1s" stand for?

a)

energy level

b)

number of orbitals

c)

shape of orbitala

d)

the number of electrons

85.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
86.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
87.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
88.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
89.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
90.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
91.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
92.
Question Image

Match the parts of the electron configuration to what it represents.

a)

1

1.

energy level

b)

s

2.

sublevel

c)

2

3.

number of electrons

93.

What subatomic particle is responsible for the spectral lines seen in emission spectra diagrams? (a)  

Choose from the below words
electrons
protons
neutrons
94.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

wiggle

95.

When an electron returns to ground state from an excited state, the atom will (a)  

Choose from the below words
emit energy
absorb energy
rotate
wiggle
96.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
97.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
98.

What is the LOWEST possible energy level that an electron can occupy?

a)

Excited State

b)

Fundamental State

c)

Ground State

d)

Outermost State

99.

What is the light that you can see called?

a)

invisible light

b)

ultraviolet light

c)

visible light

d)

infrared light

100.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

101.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
102.

The color of emitted light with the LONGEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

103.

The color of emitted light with the SHORTEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

104.

The color of emitted light with the LOWEST frequency is

a)

violet

b)

green

c)

red

d)

indigo

105.

The color of emitted light with the HIGHEST energy is

a)

orange

b)

green

c)

blue

d)

yellow

106.

The color of emitted light with the HIGHEST frequency is

a)

orange

b)

green

c)

blue

d)

yellow

107.

The color of emitted light with the LOWEST energy is

a)

orange

b)

green

c)

blue

d)

yellow

108.

Which form of radiation has the highest frequency?

a)

radio waves

b)

ultraviolet

c)

x-ray

d)

gamma

109.

A wave with a long wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

110.
Based on the picture, choose the best description of how wavelength and frequency are related
a)
As wavelength increases, frequency increases
b)
As frequency increases, wavelength remains the same
c)
As frequency increases, wavelength decreases
d)
frequency and wavelength mean the same thing
111.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
112.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
113.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
114.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
115.

A row on the periodic table is a _______.

a)

group

b)

period

c)

range

116.

About 3⁄4 of the elements on the periodic table are ________.

a)

metalloids

b)

nonmetals

c)

metals

d)

gases

117.

All _________ are semiconductors.

a)

metals

b)

metalloids

c)

nonmetals

d)

gases

118.

All _________ share properties that include luster, conductivity, malleability, and ductility.

a)

gases

b)

nonmetals

c)

metalloids

d)

metals

119.

Elements on the periodic table are arranged in columns according to their _________.

a)

properties

b)

categories

c)

atomic number

d)

boiling point

120.

Group 1 metals that react quickly with other elements are ___________.

a)

metals

b)

alkaline earth metals

c)

alkali metals

d)

nonmetals

121.

Group 2 metals that are soft and silvery are _______________.

a)

metals

b)

alkali metals

c)

alkaline earth metals

d)

gases

122.

What determines the order of elements on today's periodic table?

a)

increasing atomic mass

b)

decreasing atomic mass

c)

increasing atomic number

d)

decreasing atomic number

123.

Look at the periodic table. Which list of elements forms a group on the periodic table?

a)

Li, Be, B, C, N, O, F, and Ne

b)

He, Ne, Ar, Kr, Xe, and Rn

c)

B, Si, As, Te, and At

d)

Sc, Ti, V, Cr, Mn, Fe, Co, Cu, Ni, and Zd

124.

Using the periodic table, which element is a metalloid?

a)

carbon

b)

silicon

c)

oxygen

d)

aluminum

125.

What is one similarity among elements in a group?

a)

atomic mass

b)

atomic weight

c)

chemical properties

d)

practical uses

126.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
127.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
128.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

129.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

130.
___________ is the only metal that is a liquid at room temperature.
a)
Platinum
b)
Water
c)
Tin
d)
Mercury
131.

Which scientist created the Periodic Table and arranged elements in increasing atomic mass?

a)

Rutherford

b)

Thomson

c)

Mendeleev

d)

Moseley

132.

What is the term of an atom that will lose electron(s) and have a positive change?

a)

cation

b)

anion

c)

electronegativity

d)

ionic radius

133.

What is the term of an atom that will gain electron(s) and have a negative change?

a)

cation

b)

anion

c)

electronegativity

d)

ionic radius

134.

What element is in period 6 and group 14?

a)

Ar (Argon)

b)

O (Oxygen)

c)

Pb (Lead)

d)

Fe (Iron)

135.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
136.
What family is Cadmium a part of?
a)
Noble Gases
b)
Metalloids
c)
Transition Metals
d)
Actinoids
137.

What period contains the element Plutonium (Pu)?

a)

8

b)

6

c)

7

d)

Plutonium doesn't exist

138.

How many groups are there in modern periodic table?

a)

8

b)

9

c)

18

d)

17

139.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

140.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

141.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

142.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

143.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
144.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
145.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
146.

What are 3 broad classes of elements?

a)

metals, nonmetals, and metalloids

b)

solids, liquids, and gases

c)

small, medium, and large

d)

helium, neon, and argon

147.

atoms that gain or lose electrons are called

a)

ions

b)

isotopes

c)

metals

d)

nonmetals

148.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
149.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
150.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
151.
What is the name for CaS?
a)
calcium sulfate
b)
calcium sulfide
c)
calcium monosulfide
d)
monocalcium monosulfide
152.

What is special about group 14 elements when forming ionic bonds?

a)

They only form +4 ions.

b)

They only form -4 ions.

c)

They may form +4 or -4 ions.

d)

They don't form ions.

153.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

154.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

155.

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

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

156.

What is the charge of all group 17 ions, like Chlorine?

a)
-1
b)

-2

c)
+2
d)
+1
157.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
158.
What is the ionic compound formed between Ca and O?
a)
CaO
b)
Ca2O
c)
Ca2O2
d)
CaO2
159.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
160.

Which atom can Oxygen form an ionic bond with?

a)
Magnesium
b)
Chlorine
c)
Argon
d)
Nitrogen
161.
Boron will ____ valence electrons when forming an ionic bond.
a)
lose three
b)
gain three
c)
lose 5
d)
gain 5
162.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

163.

Ionic bonds form between metals and ____.

a)

metalloids

b)

metals

c)

nonmetals

164.

What is the charge on the iron in: iron (II) oxide

a)

2+

b)

2-

c)

1+

d)

1-

e)

None of these.

165.

PbS2

a)

lead sulfide

b)

lead sulfur

c)

lead (II) sulfide

d)

lead (IV) sulfide

166.

How many valence electrons?

a)

1

b)

2

c)

3

d)

4

167.

How many valence electrons?

a)

1

b)

6

c)

7

d)

8

168.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

169.

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

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

170.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

171.

A Metal + Nonmetal compound is a(n)...

a)

ionic compound

b)

covalent compound

172.

In a(n) ________ electrons are transferred from one atom to another

a)

ionic compound

b)

covalent compound

173.

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

174.
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.
175.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
176.

A Lewis Dot Diagram shows which electrons?

a)

all of them

b)

valence only

c)

all except valence

177.
Na +  and  S -2
a)
Na2S
b)
NaS2
c)
Na2S2
d)
NaS
178.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
179.
 Li2O
a)
Dilithium oxideDilithium oxide
b)
Lithium oxide
c)
Lithium dioxide
180.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
181.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
182.
What is the charge on the simple (single atom) ion that sulfur forms?
a)
1-
b)
2+
c)
3+
d)
2-
183.
What is the formula for the compound formed by magnesium ions and nitrogen ions?
a)
MgN
b)
Mg2N3
c)
Mg3N2
d)
MgN3
184.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
185.

Name the following compound: K2O

a)

Oxygen potasside

b)

Potassium oxide

c)

Potassium II oxide

d)

Potassium dioxide

186.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
187.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
188.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
189.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
190.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
191.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
192.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
193.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
194.

The name for CuSO4

a)

Copper sulfide

b)

Copper (II) sulfate

c)

Copper (I) sulfoxide

d)

Copper (I) sulfide

195.

The name for CrO2

a)

Chromium oxide

b)

Chromium (II) oxide

c)

Chromium (III) oxide

d)

Chromium (IV) oxide

196.

The formula for strontium phosphate

a)

SrPO4

b)

Sr2PO4

c)

Sr(PO4)3

d)

Sr3(PO4)2

197.

What is the overall charge of the ionic compound NaCl

a)

+1

b)

+2

c)

+3

d)

0

198.

What kind of Ion does Aluminum form?

a)

Al+3Al^{+3}  

b)

Al−3Al^{-3}  

c)

Al−1Al^{-1}  

d)

Al+2Al^{+2}  

199.

A sodium ion has a charge of

a)

-1

b)

-2

c)

+1

d)

+2

200.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
201.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
202.

When a neutral atom loses an electron, the atom becomes a

a)

negatively charged cation.

b)

negatively charged anion.

c)

positively charged cation.

d)

positively charged anion.

203.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

204.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

205.

The charge for oxygen is:

a)

1-

b)

2-

c)

1+

d)

2+

206.

The correct formula for copper (II) nitride is:

a)

CuNCuN  

b)

CuN2CuN_2  

c)

Cu3N2Cu_3N_2  

d)

Cu2N3Cu_2N_3  

207.

What is the formula for copper(II) phosphide?

a)

Cu2P3

b)

Cu3P2

c)

Cu3(PO4)2

d)

Cu2P

208.
The roman numeral in a compound name indicates ___________________.
a)
the number of metal ions
b)
the charge of the metal ion
c)
nothing
d)
the number of total ions
209.
What is the correct chemical name for the ionic compound: Fe3N2
a)
Iron nitride
b)
Iron (III) nitride
c)
Iron (II) nitride
d)
TriIron dinitride
210.
What is the correct chemical name for the ionic compound: CuS
a)
copper sulfide
b)
copper (I) sulfide
c)
copper (II) sulfide
d)
copper monosulfide
211.
Define a liquid
a)
no shape, no volume
b)
Definite shape, definite volume
c)
Found in stars
d)
Definite volume, no shape
212.
What term describes a solid changing to a gas?
a)
Deposition
b)
Sublimation
c)
Evaporation
d)
Freezing
213.
What term describes a liquid changing to a solid?
a)
Deposition
b)
Sublimation
c)
Evaporation
d)
Freezing
214.
Define a liquid.
a)
Indefinite shape, indefinite volume
b)
Definite shape, definite volume
c)
Found in stars
d)
Definite volume, indefinite shape
215.
When a gas changes directly to a solid, the process is known as what?
a)
Sublimation
b)
Condensation
c)
Deposition
d)
Evaporation
216.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
217.

A compound consists of two or more ____________.

a)

Molecules

b)

Atoms

c)

Elements

d)

Pieces of matter

218.

Evaporation is the change in state of a

a)

gas to a liquid

b)

gas to a solid

c)

solid to a liquid

d)

liquid to a gas

219.

In which state are the distances between the particles greatest?

a)

Both gas and liquid

b)

Liquid

c)

Gas

d)

Solid

220.
What term describes a solid changing to a gas?
a)
Deposition
b)
Sublimation
c)
Evaporation
d)
Freezing
221.

what state of matter is this

a)

liquid

b)

plasma

c)

solid

d)

gas

222.
Which of the following occurs when a liquid becomes a gas?
a)
the particles slow down
b)
the particles beak away from one another
c)
the particles move closer together
223.
The speed of the molecules determines the _____.
a)
volume
b)
density
c)
pressure
d)
temperature
224.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
225.
Identify the state of matter by looking at the particles in the image.
a)
solid 
b)
liquid
c)
gas
226.

State of matter with a definite shape and definite volume.

a)

solid

b)

liquid

c)

gas

227.

State of matter with a definite volume, but no definite shape.

a)

solid

b)

liquid

c)

gas

228.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma!!!

229.
What state of matter is this?
a)
solid
b)
liquid
c)
gas
230.
What does this picture represent? 
a)
solid
b)
liquid 
c)
gas
d)
plasma
231.

Particles are not so closely spaced and slide past each other.

a)

solid

b)

liquid

c)

gas

232.

Particles are closely spaced.

a)

solid

b)

liquid

c)

gas

233.

What are the states of matter?

a)

Liquid, water, fizz

b)

Solid, liquid, gas, plasma

c)

Rain, sleet, snow

d)

Solid and gas

234.

What state of matter does this picture show?

(a)  

235.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
236.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
237.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
238.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
239.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
240.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
241.
What is the left part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
242.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

243.

What is the number before a chemical formula called?

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

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

244.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
245.

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

246.

What is the general reaction scheme for a decomposition reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

CxHy+O2 −> CO2+H2OC_xH_y+O_2\ ->\ CO_2+H_2O

247.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

248.

compound ---> element + element

a)

synthesis

b)

decomposition

c)

combustion

d)

single replacement

249.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

250.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
251.
a substance that is formed as the result of a chemical reaction
a)
Product 
b)
Reactant
c)
Starters
d)
Enders
252.
the starting materials in a chemical reaction
a)
Products
b)
Reactants
c)
Starters
d)
Enders
253.
What are Chemical Reactions?
a)
It's when you mix substances.
b)
a process in which atoms rearrange to form new substances
c)
When something bubbles.
d)
letter and numbers showing the types and number of atoms
254.

Which of the following is a common sign that a chemical change has occurred?

a)

A chemical has turned a different color, bubbled, and/or changed temperature.

b)

A chemical has changed to a different state of matter, such as a liquid to a solid.

c)

A chemical has changed size.

d)

A chemical has become a different shape.

255.
The Law of Conservation of Matter states that the total mass of the reactants should be 
a)
More than the mass of the products
b)
Equal to the mass of the products
c)
Ignored during the reaction
d)
Less than the mass of the products
256.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
257.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

polar covalent bonding

c)

London dispersion forces

d)

dipole-dipole interaction

258.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

259.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
260.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

261.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

262.

Which is NOT an intramolecular force?

a)

Polar Covalent Bond

b)

Nonpolar Covalent Bond

c)

London Dispersion Force

d)

Ionic Bond

263.

Which has the strongest forces between particles (usually)?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

264.

Which of the following types of bonding results in materials which are malleable and ductile?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

265.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

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