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Chapter 18 PS Review (2013 Book)

Total questions: 142

Worksheet time: 2hrs 58mins

Name
Class
Date
1.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
2.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
3.
Ionic bonds exist between a metal with a non-metal.
a)
True
b)
False
4.
Magnesium (Mg) and Oxygen (O) form an ________ bond.
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nothing
5.

What usually forms the negative ion?

a)

nonmetals

b)

metal

c)

none

6.

A covalent bond forms when atoms ___________ electrons.

a)

gain

b)

share

c)

increase

d)

transfer

7.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
8.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
9.

______ molecules are found in nature as pairs of two atoms of the same type covalently bonded together.

a)

Diatomic

b)

Monatomic

c)

Polyatomic

d)

Network

10.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
11.

Which of the following elements LOSES 1 electron in order to attain a a full outer energy shell?

a)

potassium

b)

calcium

c)

hydrogen

d)

fluorine

12.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

13.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

14.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

15.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

16.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

17.

Can be a solid, liquid, or gas at room temperature

a)

Ionic compounds

b)

Covalent compounds

18.

What kind of bond does this show?

a)

Ionic

b)

Covalent

19.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

20.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

21.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
22.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
23.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
24.
Which is the charge that results when oxygen becomes an ion?
a)
+3
b)
+2
c)
-2
d)
-3
25.
LiF
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
26.
MgBr2
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
27.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

28.

What type of bond is depicted in the image?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

29.

What kind of bond is depicted in the picture?

a)

Ionic Bond

b)

Polar Covalent Bond

c)

Covalent Bond

d)

Nonpolar Covalent Bond

30.

Which element is MORE possessive of its electrons?

a)

O

b)

Be

31.

A plastic rod is rubbed with a piece of wool. During the process the plastic rod acquires a positive charge and the wool

a)

acquires an equal positive charge

b)

acquires an equal negative charge

c)

acquires a smaller positive charge

d)

acquires a smaller negative charge

e)

remains neutral

32.

A positively charged sphere is brought near end A of the uncharged metal bar shown below. Ends A and B of the metal bar will be charged:

a)

positive, negative

b)

negative, positive

c)

positive, positive

d)

negative, negative

e)

neutral, neutral

33.

When you have a bond between Br-Br, what is the polarity?

a)

Polar

b)

Nonpolar

c)

Ionic

34.

When you have an attraction between H-Cl, what is the polarity?

a)

Nonpolar

b)

Polar

c)

Ionic

35.

When you have an attraction between Li-O, what is the polarity?

a)

Nonpolar

b)

Polar

c)

Ionic

36.

When you have a bond between Si-O, what is the polarity?

a)

Nonpolar

b)

Polar

c)

Ionic

37.

When you have a bond between F-F, what is the polarity?

a)

Nonpolar

b)

Polar

c)

Ionic

38.

Water (H2O) is a polar molecule. This means that:

a)

It has a positive electric charge on both sides of the molecule

b)

It has a positive electric charge on one side and a negative charge on the opposite side

c)

The electrical charges are evenly distributed across the molecule

d)

It has no charge

39.

Which of the following is the correct molecular structure for water, H2O?

a)
b)
c)
d)
40.

How many hydrogen atoms are in a water molecule?

a)

5

b)

1

c)

2

d)

0

41.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
42.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

43.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
44.
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
45.

Atoms form compounds when the compound is more ______________ than the separate atoms. Noble gases are more _________than other elements because they have a complete outer energy level.

a)

reactive

b)

stable

c)

explosive

d)

toxic

46.

The sum of the charges in the ions of the compound is ___________.

a)

positive

b)

negative

c)

zero

d)

±1

47.

What do the vertical columns on the periodic table tell us?

a)

The number of orbitals

b)

The number of valence electrons (electrons on the outer most shell)

48.

What are the vertical columns on the periodic table called?

a)

groups

b)

periods

c)

nonmetals

d)

metals

e)

metalloids

49.

What are the horizontal rows on the periodic table called?

a)

periods

b)

groups

c)

metals

d)

nonmetals

e)

metalloids

50.

What do the horizontal rows on the periodic table tell us?

a)

The number of shells occupied by electrons

b)

The number of valence electrons (the electrons on the outer most shell)

51.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

52.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
53.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

54.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

55.

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

56.
Metals tend to 
a)
gain electrons
b)
lose electrons
57.
Nonmetals 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.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
60.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
61.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
62.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
63.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
64.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
65.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
66.

When two or more different elements are chemically combined.

a)

Mixture

b)

Element

c)

Solution

d)

Compound

67.

A chemical bond where electrons are taken/stolen

a)

Ionic Bond

b)

James Bond

c)

Covalent Bond

d)

Polar Bond

68.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
69.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
70.

Name the following compound: CaCl2

a)

calcium dichloride

b)

calcium chloride

c)

calcium (II) chloride

d)

carbon chloride

e)

None of these.

71.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
72.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
73.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
74.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
75.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
76.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
77.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
78.
The chemical formula of dinitrogen textroxide is
a)
Ni₂O₄
b)
NiO
c)
N₂O₄
d)
NiO₂
79.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
80.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
81.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
82.
Which following is a molecular compound?
a)
SO2
b)
K2O
c)
CaO
d)
BeO
83.

Classify the following molecule.

a)

polar

b)

nonpolar

84.

Classify the following molecule.

a)

polar

b)

nonpolar

85.

Classify the following molecule.

a)

polar

b)

nonpolar

86.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

87.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

88.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

89.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

90.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

91.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

92.

Classify the following molecule.

a)

polar

b)

nonpolar

93.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

94.
HCl
a)
Polar 
b)
Nonpolar 
95.
F2
a)
Polar 
b)
Nonpolar 
96.
H2O
a)
Polar 
b)
Nonpolar 
97.
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.
98.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
99.

The two (2) factors that determine if a molecule is Polar or Non-polar:

a)

The atoms's ionization energy

b)

the type of atoms in the molecule

c)

The atom's oxidation number

d)

the shape of the molecule

100.

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

a)

Polar

b)

nonpolar

c)

Ionic

101.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

102.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

103.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

104.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
105.
a)

Metallic Bonding

b)

Covalent Bonding

c)

Ionic Bonding

d)

Electromagnetic Bonding

106.

Match the following

a)

Force that holds the atoms of a substance together

1.

chemical bond

b)

substance made of the combined atoms of two or more elements

2.

compound

c)

tells what elements a compound contains and the exact number of atoms of those elements

3.

chemical formula

d)

represents the number of units of each substance

4.

coefficient

e)

represents the number of atoms of a particular element

5.

subscript

107.

Match the following

a)

positively or negatively charged atom; gain or lose electrons

1.

ion

b)

force that brings opposite charged ions together

2.

Ionic bond

c)

neutral compound that consists of positive and negative ions

3.

ionic compound

d)

how many electrons the atoms needs to gain or lose to reach a full outer energy level.

4.

oxidation number

e)

force that brings nonmetal atoms together to share electrons

5.

covalent bonds

108.

Match the following

a)

a substance made of molecules

1.

molecular compound

b)

the neutral group of atoms held together by sharing electrons and a covalent bond

2.

molecule

c)

positively or negatively charged group of elelments

3.

polyatomic ions

109.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

110.

When an atom gains an electron it becomes

a)

negatively charged

b)

positively charged

c)

neurtal

111.

Ionic bonds happen when valence electrons are

a)

shared

b)

too heavy

c)

transferred

112.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

113.

Which type of bond occurs between non metals?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

114.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

115.

How many total atoms are in C6H1206

a)

3

b)

6

c)

12

d)

24

116.

What type of bond forms CaF2

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all answers are correct

117.

In order for a chemical reaction to occur,

a)

there must be an explosion or fire

b)

bubbling or gas must be produced

c)

a new substance must be formed

d)

the substance must turn color

118.

After a chemical reaction occurs, atoms are not created nor destroyed,

a)

just rearranged into a new substance

b)

just changed into different elements

c)

just turned into unstable elements

119.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

120.
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.
121.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

122.

Ionic Bonding is the _________ of electron/s between atoms.

a)

sharing

b)

transfer

c)

loose

d)

gain

123.

a type of covalent bond that shares two pairs of electron

a)

single bond

b)

double bond

c)

triple bond

124.

This refers to the tendency of atoms to prefer to have eight electrons in the valence shell

a)

Octet rule

b)

Valence electron

c)

Electronegativity

d)

Lewis symbol

125.

Electron that is located on the outermost shell

a)

proton

b)

neutron

c)

electron

d)

valence electron

126.

A bond between metal and non metal is called

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

127.

Predict the bond that form between Be and F

a)

Covalent

b)

Ionic

128.

If an atom loses two electrons what charge will it have?

a)

-1

b)

-2

c)

+1

d)

+2

129.

Which particle is responsible for bonding?

a)

Electrons

b)

Protons

c)

Nucleus

d)

Neutrons

130.

Which element is most likely to form 2 bonds?

a)

Carbon

b)

Fluorine

c)

Nitrogen

d)

Sulfur

131.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

132.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
133.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
134.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

135.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
136.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
137.

An atom with a different number of electrons than it should have (more or less) is called an ---

a)

isotope

b)

valence electron

c)

ion

d)

octet

138.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
139.

What is the charge of the cation in Mg(OH)2Mg\left(OH\right)_2

(a)  

140.

What is the charge of the cation in iron III nitride?

(a)  

141.

What is the charge of the cation in beryllium oxide?

(a)  

142.

What is the charge on the anion in lithium nitride?

(a)  

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