WorksheetsCovalent Bonds
Total questions: 68
Worksheet time: 28mins
Name
Class
Date
1.
How well electricty flows through water is the definition for
a)
Conductivity
b)
Solubility
c)
Ionization
d)
Electrification
2.
Substances that are soluble in water and conduct electricity have these types of bonds
a)
Ionic
b)
Covalent
c)
Metallic
d)
Network Covalent
3.
Substances that might be soluble in water but don't conduct electricity have these types of bonds
a)
Covalent
b)
Ionic
c)
Metallic
d)
Network Covalent
4.
Substances that are not soluble in water but do conduct electricity have these types of bonds
a)
Metallic
b)
Covalent
c)
Ionic
d)
Network Covalent
5.
Substances that are not soluble in water and do not conduct electricity have these types of bonds
a)
Network Covalent
b)
Metallic
c)
Covalent
d)
Ionic
6.
A substance that dissolves in water is considered to be
a)
Soluble
b)
Insoluble
c)
Covalent
d)
Network Covalent
7.
Substances that conduct electricity have
a)
Metallic elements
b)
Many valence electrons
c)
High solubility
d)
Few electrons
8.
Which of the follow will conduct electricity?
a)
Sodium chloride
b)
Pure water
c)
Gasoline
d)
Plastic
9.
The "glue" that holds atoms together
a)
Electron bonds
b)
Protons
c)
Neutrons
d)
Atomic Nucleus
10.
Which of the following is NOT a type of chemical bond?
a)
Epoxy
b)
Ionic
c)
Metallic
d)
Covalent
11.
Which bond forms a "sea" of electrons?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Network Covalent
12.
Which chemical bond is between a positive and negative ion?
a)
Ionic
b)
Metallic
c)
Covalent
d)
network Covalent
13.
Which chemical bond forms between two altoms that are sharing electrons?
a)
Covalent
b)
Ionic
c)
Metallic
d)
Temporary
14.
Which type of bonds never dissolve in water
a)
Network Covalent & Metallic
b)
Network Covalent & Ionic
c)
Metallic & Ionic
d)
Covalent & Ionic
15.
Which of these substances will NOT dissolve in water?
a)
C6H6
b)
NaCl
c)
CuF2
d)
KI
16.
Which of these substances will dissolve in water?
a)
KI
b)
C7H16
c)
C8H17OH
d)
Oil
17.
A molecular formula will indicate the
a)
Number of atoms
b)
Connection between atoms
c)
Shape of the molecule
d)
Length of the moelcule
18.
A molecular formula will indicate the
a)
Types of atoms
b)
Connection between atoms
c)
Shape of the molecule
d)
Length of the moelcule
19.
The advantage of a structural formula is that it shows
a)
How the atoms are connected
b)
The shapte of the molecule
c)
the color of the moelcule
d)
The molecule in 3-D
20.
Molecules with the same structural formula but different structural formulas are called
a)
Isomers
b)
Isotopes
c)
Isoplanes
d)
Isotonic
21.
How many covalent bonds does hydrogen make?
a)
1
b)
2
c)
3
d)
4
22.
How many covalent bonds does oxygen make?
a)
2
b)
1
c)
3
d)
4
23.
How many covalent bonds does nitrogen make?
a)
3
b)
1
c)
2
d)
4
24.
How many covalent bonds does carbon make?
a)
4
b)
1
c)
2
d)
3
25.
How many covalent bonds does chlorine make?
a)
1
b)
2
c)
3
d)
4
26.
How many covalent bonds does sulfur make?
a)
2
b)
1
c)
3
d)
4
27.
How many covalent bonds does phosphorus make?
a)
3
b)
1
c)
2
d)
4
28.
How many covalent bonds does silicon make?
a)
4
b)
1
c)
2
d)
3
29.
The atoms involved in a covalent bond _________ a pair of valence electrons between themselves
a)
Share
b)
Trade
c)
Steal
d)
Buy
30.
Covalent bonds form between a/an
a)
Nonmetal & metal
b)
Metal and metal
c)
Nonmetal & nonmetal
d)
Ion & ion
31.
Each line in a structural formula represents
a)
An electron pair
b)
An electron
c)
A lone pair
d)
A lone ranger
32.
These two atoms have only 2 valence electrons
a)
H & He
b)
Li & Be
c)
F & Cl
d)
Na & Ne
33.
A Lewis dot structure shows the total number of ______ in a molecule
a)
Valence electrons
b)
Electrons
c)
Lone pairs
d)
Neutrons
34.
An atom of carbon has _______ unpaired electrons
a)
4
b)
3
c)
2
d)
1
35.
An atom of hydrogen has _______ unpaired electrons
a)
1
b)
4
c)
3
d)
2
36.
An atom of nitrogen has _______ unpaired electrons
a)
3
b)
4
c)
1
d)
2
37.
An atom of oxygen has _______ unpaired electrons
a)
2
b)
4
c)
1
d)
3
38.
The pairs of electrons between atoms are called
a)
Bonded pairs
b)
Lone pairs
c)
Isomers
d)
Locked pairs
39.
A pair of electrons in a molecule that are not shared bewteen atoms
a)
Lone pair
b)
Bonded pair
c)
Restricted pair
d)
Unshared pair
40.
Iodine (I) has _______ valence electrons
a)
5
b)
6
c)
7
d)
8
41.
Nitrogen (N) has _______ valence electrons
a)
5
b)
6
c)
7
d)
8
42.
Sulfur (S) has _____ valence electrons
a)
5
b)
6
c)
7
d)
8
43.
Bromine has _______ valence electrons
a)
5
b)
6
c)
7
d)
8
44.
Hydrogen has _____ valence electrons
a)
1
b)
2
c)
3
d)
4
45.
Carbon has _____ valence electrons
a)
4
b)
5
c)
6
d)
7
46.
The tendencey of many elements to bond until 8 valence electron surrounds an atoms is called the
a)
Octet Rule
b)
HONC 1234 Rule
c)
Bonding Rule
d)
Golden Rule
47.
In a Lewis dot structure a double bond is represented by _____ electrons
a)
4
b)
2
c)
6
d)
8
48.
In a Lewis dot structure all elements want to be surrounded by 8 electrons except
a)
Hydrogen
b)
Sulfur
c)
Chlorine
d)
Fluorine
49.
Which of the following molecules are connected with a triple bond?
a)
H2
b)
O2
c)
N2
d)
Cl2
50.
Which one of these non-metal elements will combin with 3 hydrogen atoms to satisfy the octet rule?
a)
Nitrogen
b)
Carbon
c)
Oxygen
d)
Sulfur
51.
Which of these molecules, based on bonding rules, is likely to exist in nature?
a)
PH3
b)
CH2
c)
SH3
d)
NH2
52.
Structural features that groups of molecules have in common are called
a)
Functional groups
b)
Isomers
c)
Bonding groups
d)
Lone pairs
53.
The process by which matter is changed so that new substances are formed is called a
a)
Chemical reaction
b)
Catalyst
c)
Physical reaction
d)
Combination reaction
54.
How many lone pairs are in ammonia (NH3)?
a)
1
b)
0
c)
2
d)
3
55.
How many lone pairs are in water (H2O)?
a)
2
b)
1
c)
0
d)
3
56.
How many lone pairs are in methane (CH4)?
a)
0
b)
1
c)
2
d)
3
57.
How many electron domains are around the carbon atom in CO2?
a)
2
b)
0
c)
1
d)
3
58.
How many electron domains are around the oxygen atom in H2O?
a)
4
b)
1
c)
2
d)
3
59.
How many electron domains are around the nitrogen atom in NH3?
a)
4
b)
1
c)
2
d)
3
60.
How many electron domains are in this molecule? HCN
a)
3
b)
1
c)
2
d)
4
61.
How many electron domains are in this molecule? CO2
a)
6
b)
5
c)
7
d)
8
62.
How many electron domains are in this molecule? CH2O
a)
5
b)
4
c)
6
d)
8
63.
An anion likes to ____ electrons and has a ____ charge
a)
gain, positive
b)
gain, negative
c)
lose, positive
d)
gain, positive
64.
A cation likes to ____ electrons and has a ____ charge
a)
gain, positive
b)
gain, negative
c)
lose, positive
d)
gain, positive
65.
The space occupied by electron pairs in a molecule is called the
a)
Ionization zone
b)
Electron space
c)
Electron domain
d)
Bonding area
66.
Electron domains consist of _____ pairs of electrons
a)
Bonded
b)
Lone
c)
No
d)
Both bonded and lone
67.
The tendency for electron pairs to be as far apart as possible is called
a)
Bond-Pair theory
b)
Electron domain theory
c)
the HONC 1234 rule
d)
Mutual repulsion
68.
Which one of the following does NOT apply to a catalyst
a)
Is changed by the reaction
b)
Speeds up a reaction
c)
Is not consumed by the reaction
d)
Might be required to start the reaction
100 %
