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Worksheets

Chemistry Mid Term

Total questions: 150

Worksheet time: 16hrs 29mins

Name
Class
Date
1.

The Big Bang Theory suggests that our universe formed as the result of a huge explosion that sent all existing matter flying outward from a single point. The Big Bang Theory is supported by which of these observations?

a)

All matter in the universe is composed of the same atoms.

b)

All galaxies appear to be moving away from all other galaxies.

c)

All stars in the universe are approximately the same age.

d)

The universe is relatively the same temperature in all locations.

2.

The Big Bang Theory suggests that our universe originated hot long ago?

a)

10 - 20 billion years ago

b)

10 - 20 million years ago

c)

10 - 20 thousand years ago

d)

10 - 20 centuries ago

3.

Cosmic Microwave Background Radiation (CMBR) is the term used to describe the residual microwave radiation observed everywhere in the universe that seems to have no single source. The observation of CMBR is used as evidence of The Big Bang Theory because it is believed to be -

a)

The result of collisions between neighboring galaxies.

b)

Particles of dust that have absorbed radioactivity.

c)

Radiation left over from the rapid expansion of matter.

d)

Light energy emitted from the source of The Big Bang.

4.

The lightest noble gas, containing two protons

a)

Hydrogen

b)

Helium

c)

Molecules

5.

A reaction in which two light nuclei combine to produce a nucleus of heavier mass, resulting in the release of a large amount of energy.

a)

Nuclear Bomb

b)

Nuclear Fusion

c)

Nuclear Fission

6.

Most scientists believe the Big Bang Theory explains which of the following questions?

a)

How our planets and moons formed

b)

How our universe began

c)

How the sun turns hydrogen into helium

d)

How fast light travels through space

7.
What does the Big Bang theory suggest?
a)
The universe was just there
b)
The Milky Way is the only solar system
c)
The universe is continually expanding
d)
The universe is collapsing in toward a single point
8.
What were the original two elements in our universe?
a)
Lithium and Carbon
b)
Hydrogen and Neon
c)
Helium and Chlorine
d)
Hydrogen and Helium
9.

As galaxies move away from our galaxy

a shift on the electromagnetic spectrum is noticed. This phenomena is

called _____________.

a)

redshift

b)

blueshift

10.
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
11.
What is the mass number defined as?
a)

average mass of all isotopes

b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
12.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

13.

How many neutrons does C-14 contain? (tap to enlarge the image)

a)

6

b)

7

c)

14

d)

8

14.

How many neutrons does an atom of the isotope Neon-22 have? (tap to enlarge the image)

a)

12

b)

10

c)

22

d)

20

15.

How many electrons are in an neutral atom with an atomic number of 50?

a)

5

b)

48

c)

50

d)

119

16.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
17.

The average atomic mass of an element is the ___.

a)

average of the mass number and the atomic number for the element

b)

average of the masses of the isotopes of the element

c)

total mass of the isotopes of the element

d)

number of protons + number of neutrons

18.

A neutral atom of chlorine-35 can be described as the following EXCEPT

a)

contains 17 protons

b)

contains 35 electrons

c)

contains 18 neutrons

d)

has a mass of 35 amu

19.

An element with 11 protons, 11 electrons, and 12 neutrons is identified as

a)

sodium - 11

b)

magnesium - 12

c)

sodium - 23

d)

magnesium - 34

20.

The gold foil experiment performed in Rutherford's lab __________.

a)

confirmed the plum-pudding model of the atom

b)

Led to the discovery of the atomic nucleus

c)

determine the charge on an electron

d)

utilized the deflection of beta particles by gold foil

21.

Match the following

a)
1.

atomic number of 8

b)
2.

atomic number of 10

c)
3.

atomic number of 3

22.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

23.

What is the atomic number of Nickel? (enlarge the periodic table)

a)

110

b)

28

c)

46

d)

78

24.

What results did Rutherford observe in his Gold-Foil experiment?

a)

He observed that all alpha particles did go through a gold-foil in straight lines

b)

He observed that most alpha particles did not go through a gold-foil and stopped on one side of the gold foil.

c)

He observed that a small number of alpha particles bounced off the gold-foil at very large angles

d)

He observed that all alpha particles slightly deflected from the straight line when going through a gold-foil

25.
Barium-122 has a half-life of 2 minutes. A fresh sample weighing 80 g was obtained. If it takes 10 minutes to set up an experiment using barium-122, how much barium-122 will be left when the experiment begins?
a)
0.25g
b)
2.5g
c)
25g
d)
80g
26.
How many quantum numbers are needed to describe the energy state of an electron in an atom?
a)
1
b)
2
c)
3
d)
4
27.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
28.
How many quantum numbers are needed to describe the energy state of an electron in an atom?
a)
1
b)
2
c)
3
d)
4
29.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
30.
An electron fro which n=4 has more ____ than an electron for which n=2.
a)
spin
b)
particle nature
c)
energy
d)
wave natrue
31.
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called 
a)
d orbitals.
b)
p orbitals.
c)
f orbitals.
d)
s orbitals
32.
The total number of orbitals that can exist at the second main energy level is
a)
2
b)
3
c)
4
d)
8
33.
What is the electron configuration for nitrogen?
a)
1s2 2s2 2p3
b)
1s2 2s3 2p2
c)
1s2 2s3 2p1
d)
1s2 2s2 2p2 3s1
34.
The distance traveled between two successive peaks of a waves is the
a)
speed
b)
frequency
c)
wavelength
d)
energy
35.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
36.
According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus
a)
in specific, allowed orbits.
b)
in one fixed orbit at all times.
c)
at any of an infinite number of distances, depending on its energy.
d)
counterclockwise.
37.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

38.

If n = 3, what is the maximum number of electrons that can fit in this shell?

a)

2

b)

8

c)

18

d)

32

39.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

40.

What is the difference in a 1s orbital and a 2s orbital?

a)

The shape of the orbital

b)

The size of the orbital

c)

The number of electrons it can hold

d)

None of the above

41.

Which quantum number represents the shape of the orbital?

a)

principal quantum number

b)

azimuthal (angular momentum) quantum number

c)

magnetic quantum number

d)

spin quantum number

42.

Which of the following values does NOT represent a valid electron?

a)

n=(2), l=(1), ml=(1), ms=(+1/2)

b)

n=(4), l=(2), ml=(-1), ms=(-1/2)

c)

n=(2), l=(0), ml=(0), m=(-1/2)

d)

n=(4), l=(2), ml=(-3), ms=(+1/2)

43.

Which quantum number represents the orientation of the orbital?

a)

principal quantum number

b)

azimuthal (angular momentum) quantum number

c)

magnetic quantum number

d)

spin quantum number

44.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

45.

Heisenberg's Uncertainty Principle states that it is impossible to know both the ___________ and the __________ of a particle at the same time.

a)

velocity, position

b)

velocity, energy

c)

position, energy

d)

velocity, speed

46.

State the number of significant figures in the following measurement: 216 m

a)

1

b)

2

c)

3

d)

0

47.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
48.

Match the following

a)

three

1.

tri-

b)

four

2.

tetra-

c)

six

3.

hexa-

d)

seven

4.

hepta-

e)

eight

5.

octa-

49.

Match the following

a)

one

1.

mono-

b)

two

2.

di-

c)

five

3.

penta-

d)

nine

4.

nona-

e)

ten

5.

deca-

50.
Name the following compound: 
N2O4
a)
dinitrogren tetraoxide
b)
tetranitrogen dioxide
c)
nitrogen oxide
d)
dinitrogen tetraoxygen
51.
Name the following compound: 
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
52.
Name the following compound: 
CCl4
a)
monocarbon quadchloride
b)
carbon tetrachloride
c)
carbon chloride
d)
monocarbon quadchloide
53.
Name the following compound:
NF3
a)
nitrogen triflouride
b)
mononitrogen triflouride
c)
nitrogen flouride
d)
tetranitroflouide
54.
Name the following compound:
H2O
a)
hydrogen oxide
b)
dihydrogen oxide
c)
trihydroxide
d)
dihydrogen monoxide
55.
Write the formula for:
dinitrogen tetroxide
a)
N2O4
b)
NO2
c)
NO
d)
N4O8
56.
Write the formula for:
dinitrogen pentoxide
a)
NO
b)
N2O5
c)
2NO5
d)
O5N
57.
Write the formula for:
chlorine trifluoride
a)
ClF3
b)
ClF
c)
Cl3F
d)
3ClF
58.
Write the formula for:
trilithium mononitride
a)
Li2N1
b)
Li3N3
c)
LiN3
d)
Li3N
59.
Write the formula for:
trilithium mononitride
a)
Li2N1
b)
Li3N3
c)
LiN3
d)
Li3N
60.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
61.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
62.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
63.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
64.
The chemical bond formed when two atoms share electrons  is called a(an) IONIC bond. 
a)
True
b)
False
65.
Covalent bonds usually form when a nonmetal combines with a(an) METAL.
a)
True
b)
False
66.
A(n) ION is a neutral group of atoms joined by covalent bonds.
a)
True
b)
False
67.
If a molecule contains polar bonds, the molecule MAY OR MAY NOT be polar overall. 
a)
True 
b)
False
68.
In a(an) POLAR bond, one atom pulls on the shared electrons more than the other atom. 
a)
True
b)
False
69.
The forces between molecules are much STRONGER than the forces between ions. 
a)
True
b)
False
70.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
71.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
72.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
73.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
74.

What bond is formed between a metal and a nonmetal?

a)

Covalent bond

b)

Ionic bond

c)

Hydrogen bond

d)

Metallic bond

75.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
76.

Which would be the only situation where valence electrons would be shared evenly?

a)

metals and nonmetals

b)

different nonmetals

c)

nonmetals of the same element

d)

metalloids of the same element

77.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

78.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
79.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

P2O6

80.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
81.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
82.

The octet rule means that all valence shells want to have the number......

a)

1

b)

9

c)

8

d)

16

83.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
84.
Which of the following is the correct LD Diagram for Hydrogen Cyanide? HCN?
a)
A
b)
B
c)
C
d)
D
85.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

86.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

87.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

88.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

89.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
90.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
91.
NO
a)
Mononitrogen monoxide
b)
nitrogen oxide
c)
nitrogen monoxide
d)
nitrate monoxide
92.

A farmer is looking to use ammonium phosphate as a fertilizer for his crops. Which of the following represents the chemical formula for ammonium phosphate?

a)

(NH4)3PO4

b)

NPO4

c)

NH4PO4

d)

NH4(PO4)3

93.

In a chemistry lab, you are tasked with creating a compound consisting of zinc and fluoride. Which of the following formulas represents zinc fluoride correctly?

a)

ZnF2

b)

ZnF

c)

Zn2F

d)

Zn2F4

94.

A chemist is working on a project that involves the use of aluminum sulfite. Which of the following represents the correct chemical formula for aluminum sulfite?

a)

Al2(SO3)3

b)

Al2(SO4)3

c)

AlSO3

d)

Al3(SO3)2

95.

A chemist is working on a project that involves the synthesis of silver phosphide. Which of the following chemical formulas represents silver phosphide?

a)

Ag3P

b)

Ag3PO4

c)

Ag3PO3

d)

AgP

96.

In an industrial setting, a worker needs to identify the chemical compound labeled as Ca(CN)2 in the storage area. What is the correct identification?

a)

Calcium Cyanide

b)

Calcium Dicyanide

c)

Calcium Dicarbon Dinitrogen

d)

Calcium Thiocyanate

97.

In a chemistry lab, a student is tasked with identifying the compound Sr(OH)2. What is its common name?

a)

Strontium Hydroxide

b)

Strontium Hydride

c)

Strontium Dihydroxide

d)

Strontium Dioxygen Dihydride

98.

A chemist is working on a project that involves the use of iron(II) carbonate. What is the correct formula for iron(II) carbonate?

a)

Fe2CO3

b)

FeCO3

c)

Fe2CO2

d)

FeCO4

99.

In a chemistry lab, you're given a compound labeled NaBr. What is the name of this compound?

a)

Bromide sodide

b)

Sodium bromide

c)

Sodium bromate

d)

Sodium bromite

100.

A chemist is analyzing a white powder in the lab and determines its chemical formula to be NH4F. What is the name of this compound?

a)

Ammonia fluoride

b)

Ammonium fluorite

c)

Ammonia fluorate

d)

Ammonium fluoride

101.

While studying geology, you come across a mineral sample in a limestone cave. The guide tells you it's composed of CaCO3. What is the name of this compound?

a)

Calcium carbon oxide

b)

Calcium(II) carbonate

c)

Calcium carbonate

d)

Carbonate(I) calcide

102.

A chemist is labeling containers for a new laboratory setup and comes across a bottle containing KF. What should the label read?

a)

Potassium fluoride

b)

Potassium fluorite

c)

Fluorine potasside 

d)

Potassium fluorate

103.

A chemist is working on a solution that requires magnesium hydroxide. Which of the following represents the correct chemical formula they should use?

a)

MgOH₂

b)

Mg(OH)₂

c)

Mg(OH)

d)

MgH₂

104.

During the manufacturing of airbags, sodium azide (NaN3) is used. What is the charge on the nitrogen in this compound?

a)

1+

b)

1-

c)

3+

d)

3-

e)

None of these.

105.

Imagine you are working in a laboratory and analyzing the composition of minerals. You come across a sample labeled as iron (II) oxide. What is the charge on the iron in this compound?

a)

2+

b)

2-

c)

1+

d)

1-

e)

None of these.

106.

In a chemistry lab, you come across a compound labeled
Na2S. What is the NAME of this compound?

a)

sodium (II) sulfide

b)

sodium sulfide

c)

disodium sulfide

d)

sodium sulfur

107.

In the process of manufacturing semiconductors, a technician needs to know the correct formula for calcium arsenide. Which of the following is it?

a)

Ca3As2

b)

CaAs2

c)

Ca3As

d)

Ca3Ar2

108.

In a chemistry lab, a student is asked to identify the compound K3PO4. What is its name?

a)

Tripotassium Phosphate

b)

Tripotassium Phosphite

c)

Potassium phosphide

d)

Potassium phosphate

109.

In a chemistry lab, a student is tasked with identifying the compound Al(NO3)3. What is its name?

a)

Aluminum trinitrate

b)

Monoaluminum nitrate

c)

Aluminum (III) nitrate

d)

Aluminum Nitrate

110.

A chemist is analyzing a sample and needs to identify the compound present. The compound's formula is given as Cr(NO2)3. What is the name of this ionic compound?

a)

chromium nitrite

b)

chromium nitride

c)

chromium III nitride

d)

chromium III nitrite

111.

A chemist is preparing a solution and needs to use magnesium hydroxide. Which of the following is the correct formula for magnesium hydroxide?

a)

MgOH

b)

Mg2OH

c)

Mg(OH)2

d)

Mg2OH2

112.

A chemist is working on a project that involves the bonding of copper (II) and phosphate. What would be the resulting chemical formula of their combination?

a)

Cu2(PO4)3

b)

CuPO4

c)

Cu3(PO4)2

d)

Cu3PO4

113.

A chemist is working on a project that involves the synthesis of copper(I) sulfate. What is the correct formula for copper(I) sulfate that the chemist should use?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

114.

A chemist is working on a project that involves the use of iron(II) carbonate. What is the correct formula for iron(II) carbonate that the chemist should use?

a)

Fe2CO3

b)

FeCO3

c)

Fe2CO2

d)

FeCO4

115.

A geologist finds a mineral and determines its chemical composition to be Ca2CO3. What is the name of this mineral?

a)

Calcium carbon oxide

b)

Calcium (II) carbonate

c)

Calcium carbonate

d)

Carbonate (I) calcide

116.

A chemist is analyzing a sample in the lab and discovers its chemical formula is FeSO4. What is the name of this compound?

a)

Iron (I) Sulfate

b)

Iron (II) Sulfate

c)

Iron Sulfate

d)

Iron Sulfide

117.

A geologist discovers a mineral and determines its chemical formula to be PbS2. What is the correct name of this mineral?

a)

lead sulfide

b)

lead sulfur

c)

lead(II) sulfide

d)

lead(IV) sulfide

118.

Imagine you're observing a chemical reaction in a laboratory where Lithium and Fluorine are combining. What does the red arrow indicate in the diagram showing this reaction?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

119.

Which of the following is NOT a step in forming an ionic bond in the process of salt (NaCl) formation?

a)

One atom shares its electrons with another one

b)

Opposite charged ions form due to the transfer of electrons

c)

Sodium (Na) gives an electron to Chlorine (Cl)

d)

Oppositely charged ions attract, forming NaCl

120.

Imagine you have a metal atom in a piece of jewelry that forms a cation with a charge of 2+. How would you describe the formation of that ion in this context?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

121.

Imagine you're working in a chemistry lab and you've just created an anion with a charge of 3-. How would you describe the formation of this ion in your lab notebook?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 3 electrons

d)

lost 3 electrons

122.

Imagine you're a scientist observing alkali metals in a lab. When these metals form an ion, what charge do they typically have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

123.

Imagine you are a scientist working in a lab and you're examining the properties of elements. When you observe the alkaline earth metals on the periodic table, what charge do they typically have when they form an ion?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

124.

Imagine you are a scientist analyzing the chemical properties of elements. When you examine the halogens in the periodic table, what charge do they typically have upon forming an ion?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

125.

In a chemistry lab, a student is asked to determine the ion that Nitrogen, N, will most likely form. Which ion will Nitrogen form?

a)

N

b)

N-3

c)

N-5

d)

N+5

126.

When manufacturing aluminum cookware, which ion forms the cation in the aluminum oxide layer that enhances its corrosion resistance?

a)

[ Al ] +3

b)

Al

c)

[ O ] -2

d)

O

127.

When a chemist is noting down the ionic charge of sodium in a chemical equation, it is always written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

128.

When writing the chemical formula for water, H2O, the number of hydrogen atoms is represented as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

129.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

130.

In the formation of table salt (NaCl), the type of bond between sodium (Na) and chlorine (Cl) is...

a)

Metal and Non-metal

b)

Non-metal and Non-metal

c)

Metal and Metal

131.

Imagine a party where atoms are guests. These guests mingle and react with each other to achieve a perfect balance, aiming to hold ____ electrons in their outermost energy level or shell, as per the Octet Rule.

a)

2

b)

4

c)

6

d)

8

e)

10

132.

Imagine you're an architect designing a building. In this scenario, what would be the best definition of valence electrons?

a)

The outermost electron NOT involved in chemical reactions

b)

The innermost electrons involved in chemical reactions

c)

The outermost electrons involved in chemical reactions.

d)

The innermost electrons NOT involved in chemical reactions

133.

Imagine you are a chemist trying to create a new salt by combining different ions. Which of the following pairs would NOT result in the formation of an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

134.

Imagine you're working in a high-tech laboratory and you're tasked with creating a battery using lithium, which is in group 1 of the periodic table. Considering its position, which ion would lithium most likely form to achieve stability?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

135.

In the formation of table salt (NaCl), what determines how the sodium (Na) and chlorine (Cl) atoms will bond together?

a)

Number of protons in Na and Cl

b)

Mass of the Na and Cl atoms

c)

Number of total electrons in Na and Cl

d)

Number of valence electrons in Na and Cl

136.

If a balloon's charge becomes 2+ what does that say about it?

a)

It is stealing 2 electrons

b)

It is losing 2 electrons

c)

It is in period 2

d)

It has an atomic # of 2

137.

In a saltwater solution, a sodium ion (Na+) is a ____ ion.

a)

negative

b)

positive

138.

In a salt solution, the chloride ion (Cl-) will be a ____ ion.

a)

negative

b)

positive

139.

In a science fiction movie, a space rock that has gained or lost electrons is called ...

a)

a winner

b)

an isotope

c)

an ion

d)

a loser

140.

When a balloon is rubbed against hair, the balloon that gains electrons becomes...

a)

negatively charged

b)

positively charged

c)

remain neutrally charged

d)

21

141.

In the process of salt formation, the attraction between sodium (Na) and chlorine (Cl) to form sodium chloride (NaCl) is an example of a(n) _______________.

a)

ionic bond

b)

polyatomic ion

142.
What is the charge on a noble gas & why?
a)
0; they don't exchange electrons
b)
+1; they give away an electron
c)
-1; they gain an electron
d)
1; they form only single bonds
143.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
144.
Ionic bonds form because
a)
Two ions of the same charge are attracted to each other
b)
Two ions of different charges are attracted to each other
c)
Two atoms share their electrons
d)
Two or more atoms share protons
145.
An ionic bond may or may not include a metal.
a)
True
b)
False
146.
An ionic bond involves two elements...
a)
Transferring electrons
b)
Sharing electrons
147.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

148.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
149.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
150.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly

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