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WorksheetsMid Unit 2 Review
Total questions: 40
Worksheet time: 32mins
Name
Class
Date
1.
How many electrons would a molecule of H2O have?
a)
10
b)
6
c)
8
d)
16
2.
How many electrons would a molecule of CO2 have?
a)
10
b)
14
c)
22
d)
16
3.
Because it is already in the most stable form with a full valence shell, which element will not form bonds?
a)
Mercury
b)
Carbon
c)
Hydrogen
d)
Krypton
4.
How many valence electrons does Aluminum have to lose in order to have an octet?
a)
1
b)
2
c)
3
d)
5
5.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons
c)
The transfer of electrons
d)
None Of the above
6.
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
7.
What type of bond would form between calcium and sulfur?
a)
Ionic
b)
Metallic
c)
Covalent
d)
No bond would form.
8.
Atoms gain or lose electrons because they ...
a)
are too full.
b)
want to lose weight.
c)
want a full outer shell.
d)
can
9.
How do you find the number of valence electrons in an atom?
a)
use the atomic mass
b)
use the atomic number
c)
Use the periods
d)
Use the groups
10.
Covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
11.
Carbon dioxide
a)
C2O2
b)
C20
c)
CO
d)
CO2
12.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
13.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
14.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
15.
What types of elements are covalent bond made of?
a)
Metals and Nonmetals
b)
Metals
c)
Two metals and one metal
d)
Nonmetals
16.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
17.
What is Ionic bonding?
a)
The mixture between two metals
b)
The combination of two nonmetals
c)
The combination of a metal and a nonmetal
18.
What usually forms a positive ion.
a)
Metals
b)
Nonmetals
19.
What usually forms a negative ion.
a)
Nonmetals
b)
Metals
20.
AlBr3
a)
aluminum bromide
b)
aluminum tribromide
c)
aluminum bromine
d)
monoaluminum tribromide
21.
sodium nitride
a)
NaNO3
b)
NaN
c)
NaN3
d)
Na3N
22.
calcium iodide
a)
CaI
b)
Ca2I
c)
CaI2
d)
Ca2I3
23.
magnesium sulfide
a)
MgS
b)
Mg2S
c)
Mg2S2
d)
MgS2
24.
calcium iodide
a)
CaI
b)
Ca2I
c)
CaI2
d)
Ca2I3
25.
Name the compound Na2O
a)
Sodium Oxide
b)
Sodium Dioxide
c)
Sodium Oxygen
d)
Natride Oxide
26.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
27.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
28.
The name of N₂O is
a)
nitrogen oxide
b)
nitrogen (II) oxide
c)
dinitrogen monooxide
d)
dinitrogen monoxide
29.
Balance this equation.
_SnO2 +_H2-->_Sn +_H2O
_SnO2 +_H2-->_Sn +_H2O
a)
1,1,2,1
b)
1,2,1,1
c)
1,2,1,2
d)
1,2,2,1
30.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
31.
Balance this equation-
_SeCl6+_O2>_SeO2+_Cl2
_SeCl6+_O2>_SeO2+_Cl2
a)
1,2,1,2
b)
1,1,1,3
c)
1,2,1,1
d)
2,1,1,1
32.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction.
33.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
34.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
35.
Balance this equation-
__P4 + __O2 --> __P2O3
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
36.
HI --> H2 + I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
37.
Zn + H2S --> ZnS + H2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
38.
FeS + HCl --> H2S + FeCl2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
39.
Mg + HCl --> MgCl2 + H2
a)
combustion
b)
synthesis
c)
decomposition
d)
single replacement
40.
Pb(NO3)2 + KI --> KNO3 + PbI2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
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