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WorksheetsChemical Reactions Review
Total questions: 25
Worksheet time: 13mins
Name
Class
Date
1.
What type of chemical reaction is the following: 3Mg + N2 →Mg3N2?
a)
Synthesis
b)
Combustion
c)
Double Replacement
d)
Decomposition
2.
What is the representative formula for Double Replacement?
a)
A + B → AB
b)
AB + CD → AD + CB
c)
AB → A + B
d)
AB + C → AC + B
3.
Which of the following reactions is balanced?
a)
H2 + O2 → H2O
b)
PCl5 + 4 H2O → H3PO4 + 5 HCl
c)
Xe + F2 → XeF6
d)
3Xe + F2 → XeF6
4.
Which of these is rule 1 of the solubility rules?
a)
salts containing group I elements are soluble
b)
Nitrate ions are soluble
c)
Silver salts are generally insoulble
5.
What is the law of conservation of mass?
a)
Matter can be destroyed but not created.
b)
Mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations.
c)
matter can be created but not destroyed.
d)
Destroyed and forms carbon monoxide.
6.
What type of equation is this?
a)
Synthesis
b)
Single - Replacement
c)
Double - Replacement
d)
Combustion
7.
Which of the following do NOT increase the reaction rate?
a)
Increase Temperature
b)
Presence of a Catalyst
c)
Decrease Surface Area
d)
Increase Concentration
8.
How can you balance equations?
a)
Change the subscripts
b)
Change the superscripts
c)
Use coeffiecents
9.
What do net ionic equations consist of? (best answer)
a)
Only spectator ions.
b)
show only those chemical species participating in a chemical reaction.
c)
Only polyatomics.
d)
the balanced version of the equation.
10.
Which of the following reactions would NOT realistically occur due to solubility?
a)
CdSO4(aq)+K2S(aq)→CdS(s)+K2SO4(aq)CdSO4(aq)+K2S(aq)→CdS(s)+K2SO4(aq)
b)
NH4NO3 (aq) + NaCl (aq)→ NH4Cl (aq) + NaNO3 (aq)
c)
PbCl2(s) →Pb(aq) + 2 Cl(a q)
11.
What types of elements are in a covalent bond?
a)
Metal and a nonmetal
b)
Metal and a metal
c)
Nonmetal and a nonmetal
12.
Which rule should you use first if two are applicable? (for solubility rules)
a)
The rule that comes first
b)
The rule you feel is most important
c)
The one that comes second
d)
Hope they both say the same solubility
13.
The products of the equation occur on the _______ side of the equation.
a)
left
b)
right
c)
both
d)
depends
14.
The reactants of the equation occur on the ________ side of the equation.
a)
right
b)
left
c)
both
d)
depends
15.
The mass of the reactants is ______ to the mass of the products.
a)
less
b)
more
c)
equal
d)
depends on elements
16.
The reaction rate can be increased by which of the following:
a)
decrease collisions
b)
Increase temperature
c)
increase activation energy
d)
decrease concentration
17.
Which of the following describes exothermic reactions?
a)
heat is given out.
b)
heat is taken in.
c)
heat is not taken in or given out.
18.
True or false when the activation energy decreases the reaction rate increases.
a)
True
b)
False
19.
What is a total ionic equation?
a)
A chemical equation that shows all the ions in a reaction.
b)
A chemical equation that shows all the spectator ions in the equation.
c)
Is the same thing as a net ionic equation.
20.
What can solubility do?
a)
Help predict the formation of a precipitate.
b)
Help predict the state of matter the Ions are in.
c)
Tell what type of reaction is occurring.
21.
Which ion is insoluble?
a)
NH4
b)
CaCO3
c)
LiOH
d)
Ba(OH)2
22.
What must happen in order for a reaction to occur? (best answer)
a)
Collisions must occur with the correct amount of energy.
b)
Collisions that occur at the correct angle.
c)
All the above.
23.
Which group of elements is entirely soluble in a reaction?
a)
Alkaline Earth Metals
b)
Alkali metals
c)
Noble gases
d)
Halogens
24.
True or false the cation always comes last in the reaction.
a)
true
b)
false
25.
true or false endothermic reactions have a higher activation energy.
a)
true
b)
false
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