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Ionic, Covalent, and Metallic Bonding

Total questions: 103

Worksheet time: 2hrs 38mins

Name
Class
Date
1.
Metals tend to 
a)
gain electrons
b)
lose electrons
2.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
3.
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
4.

Identify the following compound as ionic or covalent: MgO

a)

ionic

b)

covalent

5.

Identify the following compound as ionic or covalent: CF4

a)

ionic

b)

covalent

6.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

7.

Identify the following compound as ionic or covalent: CO

a)

ionic

b)

covalent

8.

When naming covalent compounds...

a)

You need roman numerals and no prefixes

b)

You do not need roman numerals or prefixes

c)

You need roman numerals and prefixes

d)

You do not need roman numerals but you do need prefixes

9.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
10.
H+ and S2- create...
a)
H2S
b)
HS2
c)
H2S2
d)
HS
11.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
12.
Li+ and P3- create...
a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
13.

Pb4+ and O2- create...

a)

Pb2O

b)

PbO2

c)

Pb2O2

d)

PbO

14.

Rb+ and P3- create...

a)

Rb3P

b)

RbP3

c)

RbP

d)

Rb2P

15.

Ca2+ and F- create...

a)

Ca2F2

b)

Ca3F

c)

CaF2

d)

Ca2F

16.
Which is the Roman Numeral for +3?
a)
I
b)
II
c)
III
d)
+III
17.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

18.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

19.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

20.

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

21.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

22.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

23.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

24.

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

25.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

26.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

27.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

28.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
29.
What is the formula for sodium nitrate?
a)
Na3NO
b)
NaNO
c)
Na3NO3
d)
NaNO3
30.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
31.
What is the formula for iron(II) carbonate?
a)
Fe2CO3
b)
FeCO3
c)
Fe2CO2
d)
FeCO4
32.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
33.
Find the formula zinc sulfate
a)
ZnSO3
b)
ZnSO4
c)
ZnS
d)
Zn(SO4)2
34.
What is the formula for copper (II) hydroxide?
a)
CuOH
b)
Cu(OH)2
c)
Cu2OH
d)
Cu2O
35.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
36.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
37.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
38.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
39.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
40.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
41.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
42.
The chemical formula of dinitrogen textroxide is
a)
Ni₂O₄
b)
NiO
c)
N₂O₄
d)
NiO₂
43.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
44.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
45.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
46.

Which of the following is NOT covalently bonded?

a)

K2S

b)

H2O

c)

I2

d)

CO2

47.

Name the following compound:

CO2

a)

monocarbon dioxide

b)

carbon oxide

c)

carbon dioxide

d)

oxygen carbonide

48.

Name the compound: NO

a)

Mononitrogen monoxide

b)

nitrogen oxide

c)

nitrogen monoxide

d)

mononitrogen oxide

49.

Name the compound: SO3

a)

Monosulfur trioxide

b)

Sulfate trioxide

c)

Sulfur trioxide

d)

Monosulfate oxide

50.

Which pair of atoms is most likely to form a covalent molecule?

a)

Hydrogen and lithium

b)

Phosphorus and sulfur

c)

Helium and neon

d)

Zinc and Boron

51.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
52.
Ionic compounds can conduct electricity as a solid
a)
true
b)
false
53.
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
54.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

55.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
56.
which types of elements become cations?
a)
nonmetals
b)
all metals
c)
only transition metals
d)
some metals and some metalloids
57.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

58.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

59.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
60.

Why do atoms form bonds?

a)

to attain a noble gas configuration

b)

to increase their mass

c)

to increase their atomic number

d)

to attain an alkali metal configuration

61.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
62.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
63.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
64.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
65.
When dissolved in water, the solution does NOT conduct electricity.
a)
ionic compounds
b)
covalent compounds
66.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
67.
usually soft
a)
ionic compounds
b)
covalent compounds
68.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

69.

A single covalent bond is made up of _____ electrons.

a)

one

b)

two

c)

three

d)

four

70.
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.
71.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
72.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
73.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
74.

How are compounds with metallic bonds similar to ionic compounds?

a)

Both tend to have double and triple bonds.

b)

Both tend to have low boiling point

c)

Both tend to have poor conductivity.

d)

Both tend to have high melting points.

75.
Which type of bonding allows for the conduction of electricity in the solid state?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
76.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
77.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
78.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
79.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
80.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
81.
Diatomic molecules are __________ found in nature as their single element: I, O, N, H, Br, Cl, or H.
a)
often
b)
never
c)
sometimes
d)
always
82.
N2, Cl2, and O2 are all 
a)
diatomic molecules.
b)
ionic bonds.
c)
of equal mass.
d)
solids.
83.
N2, Cl2, and O2 are all 
a)
gases.
b)
solids.
c)
in the same family.
d)
safe to breathe.
84.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
85.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
86.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
87.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
88.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
89.
What is the correct order of the states of matter?
a)
Solid, Liquid, Gas
b)
Gas, Liquid, Solid
c)
Liquid, Gas, Solid
d)
Solid, Gas, Liquid
90.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma!!!

91.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

92.

What state of matter?

a)

Solid

b)

Liquid

c)

Gas

93.

Electrons that are free to move in metals

a)

sea of electrons

b)

oxidation number

c)

chemical bond

d)

salts

94.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

95.

Why do metals conduct heat and electricity

a)

They are shiny

b)

The electrons are held tightly within the lattice

c)

The electrons are in a sea and able to move

d)

The electrons are shared between two metal ions

96.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
97.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
98.

Which type of bond creates a "sea" of electrons between atoms?

a)

Ionic Bonds

b)

Covalent Bonds

c)

Metallic Bonds

d)

James Bonds

99.

What type of bond?

a)

Ionic

b)

Covalent

c)

Metallic

d)

None

100.
Name this formula: 
K3N
a)
Potassium (III) Nitride
b)
Potassium Nitride
c)
Potassium (I) Nitride
d)
Nitrogen Potaside
101.

What type of bond?

a)

Ionic

b)

Covalent

c)

Metallic

d)

None

102.

What type of bond?

a)

Ionic

b)

Covalent

c)

Metallic

d)

None

103.

What type of bond?

a)

Ionic

b)

Covalent

c)

Metallic

d)

None

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