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PS Unit 6

Total questions: 111

Worksheet time: 2hrs 39mins

Name
Class
Date
1.

The 3 types of chemical bonds are ________, ________, and ______. (Choose 3)

a)

ionic

b)

valence

c)

covalent

d)

metallic

e)

atomic

2.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
3.

A bond between two nonmetal atoms is a __________ bond.

a)

ionic

b)

nuclear

c)

metallic

d)

covalent

4.

Which of the following is NOT a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

5.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

6.
Covalent bonds are between...
a)
two or more nonmetals
b)
sodium and chlorine
c)
metals and metals
d)
metals and nonmetals
7.

Ionic bonds form between ---

a)

nonmetals.

b)

metals and nonmetals.

8.
What is the name for an ion with a negative charge?
a)
cation
b)
anion
c)
onion
d)
union
9.

Which compound has high melting point?

a)

Ionic

b)

Covalent

10.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

11.

Which of the following is NOT an ionic bond?

a)

NH3

b)

KCl

c)

K3N

d)

NaCl

12.

A bond between a metal atom and a nonmetal atom is a __________ bond.

a)

ionic

b)

atomic

c)

metallic

d)

covalent

13.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
14.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
15.

What happens when two oppositely charged ions are pushed together?

a)

they will repel (move apart)

b)

they will be attracted to each other (move together)

16.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
17.
What is the name for an ion with a positive charge?
a)
cation
b)
anion
c)
onion
d)
union
18.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

19.

For nonmetals, its easier to _____ electrons to have a full outer shell.

a)

gain

b)

lose

c)

share

20.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
21.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

22.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

23.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

24.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
25.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
26.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
27.

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

28.

Ionic bonds form between two ions that have...

a)

Positive Chargers

b)

negative charges

c)

Same Charges

d)

Opposite Charges

29.

How does calcium become a calcium ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

30.

How does oxygen become an oxide ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

31.

What is the ionic compound that is formed when you combine Li+ and N-3 ions? LiN3

a)

LiN

b)

LiN3

c)

Li3N2

d)

Li3N

32.

Electrons located on the outermost shell are called _________ electrons

a)

Hybrid

b)

Atomic

c)

Neutral

d)

Valence

33.

Which of the following would be the correct formula for a compound of Aluminum and Fluorine?

a)

AlF3

b)

Al2F3

c)

AlF2

d)

AlFI

34.

Which of these has five valence electrons?

a)

Nitrogen

b)

Oxygen

c)

Hydrogen

d)

Chlorine

35.

Which of the following will become a positively charged cation?

a)

An atom with 2 valence electrons

b)

An atom with 7 valence electrons

c)

An atom with 5 valence electrons

d)

An atom with 8 valence electrons

36.

Why are ions attracted to each other?

a)

Cations and Anions have opposite charges.

b)

Cations think Anions are cool.

c)

The fact that both are metals allows them to mix.

d)

The ions change their electrons again.

37.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
38.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
39.

What kind of Ion does Aluminum form?

a)

Al+3Al^{+3}  

b)

Al−3Al^{-3}  

c)

Al−1Al^{-1}  

d)

Al+2Al^{+2}  

40.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
41.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
42.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
43.
What is ionization energy?
a)
Energy required to remove an electron
b)
Energy needed to split an electron
c)
Energy required to add an electron
44.

Ionization energy __________ as you go across a period

a)

stays the same

b)

decreases

c)

increases

45.

Ionization energy __________ as you go down a group.

a)

stays the same

b)

decreases

c)

increases

46.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting point and it conducts electricity when molten or dissolved

c)

A high boiling point and it conducts electricity when solid

47.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
48.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

49.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

50.

Why do atoms share electrons?

a)

to increase their atomic number

b)

to become ions

c)

to obtain noble gas electron configuration

d)

to become less polar

51.

Which of the following can form diatomic molecules held by triple covalent bonds?

a)

N2

b)

O2

c)

F2

d)

C2

52.

Which of the following diatomic molecules can be formed with a double covalent bond?

a)

N2

b)

O2

c)

F2

d)

C2

53.

If two identical atoms bond covalently, the bond is:

a)

a coordinate covalent bond

b)

a dipole covalent bond

c)

a nonpolar covalent bond

d)

a polar covalent bond

54.

What does a molecular formula tell you?

a)

information about the molecule's structure

b)

the number and kind of atoms bonded in the molecule

c)

the whole-number ratio of atoms bonded in the molecule

d)

the number and kind of atoms bonded by electron transfer

55.

Which of the following covalent bonds is the most polar?

a)

H-N

b)

H-C

c)

H-H

d)

H-F

56.

If the atoms that share electrons have an unequal attraction for the electrons, the bond is called

a)

dipolar

b)

nonpolar

c)

ionic

d)

polar

57.

In covalent bonds electrons are:

a)

shared

b)

transferred

c)

mobile

58.

A neutral group of atoms held together by covalent bonds is a

a)

chemical formula

b)

molecular formula

c)

molecule

d)

polyatomic ion

59.

When one atom in a covalent bond attracts the shared electron more strongly, that compound is called __________________.

a)

polar

b)

nonpolar

60.

When both atoms in a covalent bond share the electron equally, it is called a ________________ compound.

a)

polar

b)

nonpolar

61.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
62.

The lines indicate ____________________.

a)

lone pairs

b)

bond pairs

63.

How many bond pairs are in a double covalent bond?

a)

0

b)

1

c)

2

d)

3

64.

Diatomic molecules are more stable together than alone.

a)

True

b)

False

65.

dichloride pentoxide

a)

Cl2O5

b)

ClO5

c)

Cl5O2

d)

Cl2O6

66.

What type of bond is pictured?

a)

Ionic bond

b)

Single Covalent Bond

c)

Double Covalent Bond

d)

Triple Covalent Bond

67.

Which bond type is more likely to be liquids or gases at room temperature?

a)

ionic bonds

b)

covalent bonds

c)

metallic bonds

68.

Name this compound

SeH3

a)

triselenium trihydride

b)

Selenium hydride

c)

Trihydrogen monoselenide

d)

Selenium trihydride

69.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
70.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
71.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
72.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
73.
What is a double bond?
a)
a bond between two atoms
b)
one pair of electrons shared between two atoms
c)
two pairs of electrons shared between two atoms
d)
James Bond's brother
74.

H2O has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

75.

The chemical name of P₄S₁₀ is:

a)

phosphorous sulfide

b)

phosphorus sulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

76.
 Li2O
a)
Dilithium oxideDilithium oxide
b)
Lithium oxide
c)
Lithium dioxide
77.
CsCl
a)
Monocesium monochloride
b)
Cesium monochloride
c)
Cesium Chloride
78.
MgS 
a)
Magnesium sulfide
b)
Monomagnesium monosulfide
c)
Magnesium monosulfide
79.
Na2S
a)

Disodium sulfide

Disodium sulfide

b)
Sodium sulfide
c)
Sodium monosulfide
80.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
81.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
82.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
83.
The chemical formula for an ionic compound of aluminum and chlorine is
a)
AlCl.
b)
ClAl.
c)
AlCl3.
d)
Al3Cl.
84.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
85.

Name the compound: N2O5.

a)

dinitrogen pentaoxide

b)

binitrogen pentaoxide

c)

nitrogen oxide

d)

pentanitrogen dioxide

86.

Name the compound: SO3

a)

sulfur trioxide

b)

sulfite ion

c)

sulfur oxide

d)

sodium trioxide

87.

Name the compound: CF4

a)

carbon tetrafluoride

b)

monocarbon tetrafluoride

c)

carbon fluoride

d)

chlorine tetrafluoride

88.

Name the compound: P4O8

a)

tetraphosphorus octoxide

b)

phosphorus oxide

c)

tetrapotassium octoxide

d)

potassium oxide

89.

Name the compound: SF6

a)

sulfur heptafluoride

b)

sulfur hexafluoride

c)

monosulfur hexafluoride

d)

monosulfur heptafluoride

90.

Write the formula: tetraarsenic decoxide

a)

As4O10

b)

As10O4

c)

As6O9

d)

AsO

91.

Write the formula: iodine heptafluoride

a)

IF7

b)

I2F14

c)

IHF7

d)

IF6

92.

Write the formula: nitrogen trichloride

a)

NCl3

b)

N1Cl3

c)

N1Cl5

d)

Cl3N

93.

Write the formula: carbon monoxide

a)

CO

b)

CO2

c)

OC

d)

C2O4

94.

Lithium nitride

a)

Li3N

b)

LiN

c)

Li3(NO3)2

d)

LiNO3

95.

Write the formula: beryllium oxide

a)

BO

b)

BeO

c)

BeO2

d)

BO2

96.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
97.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
98.
What is the formula for sodium nitrate?
a)
Na3NO
b)
NaNO
c)
Na3NO3
d)
NaNO3
99.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
100.
Identify Gallium Sulfate
a)
GaSO4
b)
Ga2(SO4)3
c)
Ga3(SO4)2
d)
Ga2SO4
101.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
102.
The oxidation number for Fe in Fe2O3:
a)
+2
b)
+3
c)
+1
d)
-2
103.
The oxidation number for copper in Cu2S:
a)
+1
b)
+2
c)
-1
d)
-2
104.
What oxidation number is Roman Numeral (IV)?
a)
5
b)
4
c)
1
d)
3
105.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
106.
The name for CrN:
a)
Chromium nitride
b)
Chromium (I) nitride
c)
Chromium (III) nitride
d)
Chromium nitride (III)
107.

Brass is an alloy made of

a)

copper and zinc

b)

copper and tin

c)

copper and nickel

d)

copper and aluminum

108.

Steel can become stainless when alloyed with _____.

a)

chromium and nickel

b)

copper and zinc

c)

tin and lead

d)

iron aand carbon

109.

Which of the following are alloys? (choose 3)

a)

Lead

b)

Bronze

c)

Brass

d)

Aluminium

e)

Stainless Steel

110.

The most common element added to iron to create steel alloy is ...

a)

tungsten

b)

vanadium

c)

chromium

d)

carbon

111.

Why do jewelers not create jewelry with pure gold, silver, or copper?

a)

It is a soft metal, so it will rub or scratch away over time.

b)

It will not be shiny.

c)

It is impossible to find a pure form of these metals.

d)

It is too hard to shape into a design.

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