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WorksheetsBonding Review
Total questions: 55
Worksheet time: 38mins
Name
Class
Date
1.
A cation is a ____ ion.
a)
negative
b)
positive
2.
A anion will be a ____ ion.
a)
negative
b)
positive
3.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
4.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
5.
Helium will ____ valence electrons when forming an ionic bond.
a)
lose 2
b)
gain 2
c)
both
d)
not form a bond
6.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
7.
What is the most common ion for Calcium?
a)
Ca+2
b)
Ca+
c)
Ca-2
d)
Ca-
8.
What is the most common ion for bromine?
a)
Br-
b)
Br+
c)
Br+2
d)
Br-2
9.
When atoms share more than one pair of electrons
a)
Single Bond
b)
Double Bond
c)
Triple Bond
d)
None of The Above
10.
What is an ionic bond?
a)
When two ions are held to each other by attraction of between the opposite charges
b)
When ions seperate by force
c)
None of the above
11.
What is the main rule when naming ionic compounds?
a)
The cation named first and anion named second
b)
A monatomic anion is named by taking the first part of an element’s name and adding -ide to the end
c)
A monatomic anion is named by taking the first part of an elements name and adding -ide to the end
d)
All
12.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
13.
Covalent bond forms between....
a)
Nonmetals
b)
Metals
c)
Nonmetal and a Metal
d)
Metal and a Nonmetal
14.
What is a single bond?
a)
When atoms share one pair of electrons
b)
When atoms share more than one pair of electrons
c)
When three-pairs of electrons are being shared
d)
When one pair of neutrons is being shared
15.
What is the chemical formula for dinitrogen trioxide?
a)
N2O3
b)
NO2
c)
N3O
d)
N2O4
16.
Cr3N
a)
chromium nitride
b)
chromium (I) nitride
c)
chromium (II) nitride
d)
chromium (III) nitride
17.
chromium (III) nitrate
a)
Cr3N2
b)
Cr2N
c)
Cr2NO3
d)
Cr(NO3)3
18.
calcium oxide
a)
Ca2O2
b)
Ca2O
c)
CaO
d)
CaO2
19.
barium phosphide
a)
Ba3(PO4)2
b)
BaP
c)
Ba3P2
d)
Ba2P3
20.
Ru2S
a)
Rubidium sulfate
b)
Rubidium sulfite
c)
Rubidium (II) sulfide
d)
Rubidium sulfide
21.
AgOH
a)
silver hydroxide
b)
silver (I) hydroxide
c)
silver hydrogen oxide
d)
silver hydride
22.
SeCl4
a)
selenium chloride
b)
monoselenium tetrachloride
c)
selenium tetrachloride
d)
monoselenium chloride
23.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
24.
carbon monoxide
a)
CO
b)
CO2
c)
C2O
d)
COH
25.
P2O5
a)
phosphorus oxide
b)
phosphorus (II) oxide
c)
diphosphorus pentoxide
d)
phosphorus pentoxide
26.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
27.
Which of the following would require a Roman Numeral in its name?
a)
Al2O3
b)
Na2S
c)
CuSO4
d)
Sr(ClO3)2
28.
What kind of bond does a diatomic nitrogen N2 molecule have? You should draw the Lewis structure to see!
a)
single covalent
b)
double covalent
c)
triple covalent
d)
ionic
29.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
30.
Ionic bonds are formed when one atom gives electrons to another atom.
a)
True
b)
False
31.
Ionic bonds can be formed between two nonmetals.
a)
True
b)
False
32.
AgNO2 is called...
a)
silver oxide
b)
silver nitrogen oxide
c)
silver nitrate
d)
silver nitrite
33.
The formula for magnesium cyanide is...
a)
Mg(CN)2
b)
MgCN2
c)
MgCN
d)
(Mg)2CN
34.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
35.
FeSO3
a)
iron (I) sulfate
b)
iron sulfite
c)
iron (III) sulfite
d)
iron (II) sulfite
36.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
37.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
38.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
39.
What is the correct Lewis Dot Structure for ammonia NH3
a)
b)
c)
d)
40.
Which is the correct molecular structure for carbon dioxide?
a)
b)
c)
d)
41.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
42.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
43.
Which of the following is an ionic compound?
a)
HCl
b)
H2O
c)
MgO
d)
CO2
44.
What type of bond is formed between Li and F?
a)
Covalent
b)
Ionic
c)
Metallic
d)
Carbon
45.
Which of the following is an Covalent compound?
a)
NaCl
b)
CaCl2
c)
KI
d)
CO
46.
NH3
a)
Covalent
b)
Ionic
c)
Metallic
47.
NO2
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
48.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
49.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
50.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
51.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
52.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
53.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
54.
usually soft
a)
ionic compounds
b)
covalent compounds
55.
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
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