Science 10
Unit 6 Worksheet
Unit 6 – Investigating chemical reactions (Ch. 9)
Chapter 9.3 – Types of Chemical Reactions
1.
List the six main types of chemical reactions.
C
C
C
C
C
C
2.
Synthesis
Decomposition
Single replacement
Double replacement
Neutralization
Combustion
Describe a synthesis reaction. Be sure to include an example in your description.
C Two or more reactants combine to produce a single product as in A + B ! AB.
C An example of this reaction is combining sodium with chlorine gas to form table salt,
where 2Na + Cl2 ! 2NaCl.
3.
When a synthesis reaction occurs between a metal and a non-metal,
ionic
formed. When a
synthesis reaction
occurs between two non-metals,
compounds are formed.
4.
Complete and balance the following synthesis reactions in the spaces below.
compounds are
covalent
a. Na + N2 !
C 6Na + N2 ! 2Na3 N
b. K + O2 !
C 4K + O2 ! 2K2 O
c. N2 + O2 !
C 2N2 + O2 ! 2N2 O
5.
A decomposition reaction is the
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reverse
of a synthesis reaction.
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6.
Describe a decomposition reaction. Be sure to include an example in your description.
C Decomposition reactions occur when a single reactant is broken down to produce
smaller compounds or separate elements. For example, AB !A + B
C An example of this reaction is breaking down table salt to form sodium and chlorine gas.
C 2NaCl ! 2Na + Cl2
7.
Complete and balance the following decomposition reactions in the spaces below:
a. AuBr3 !
C 2AuBr3 ! 2Au + 3Br2
b. CaF2 !
C CaF2 ! Ca + F2
c. N2O !
C 2N2 O ! 2N2 + O2
8.
Describe a single replacement reaction. Be sure to include an example in your description.
C Single replacement reactions occur when a reactive element and a compound react to
produce another element and another compound. For example, A + BC ! B + AC
(where A is a metal) or A + BC ! C + AB (where A is a non-metal).
C An example of this reaction is 2Al + 3CuCl2 ! 3Cu + 2AlCl3
9.
Complete and balance the following single replacement reactions in the spaces below:
a. Cl2 + CuBr2 !
C Cl2 + CuBr2 ! Br2 + CuCl2
b. Al(NO3)3 + Mg !
C 2Al(NO3 )3 + 3Mg
! 3Mg(NO3)2 + 2Al
c. PbF4 + Na !
C PbF4 + 4Na ! 4NaF + Pb
10. Describe a double replacement reaction. Be sure to include an example in your description.
C Double replacement reactions usually involve two ionic solutions that react to produce
two other ionic compounds. For example, AB + CD ! AD + CB
C An example of this reaction is: 3NaOH + FeCl3 ! 3NaCl + Fe (OH)3
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11. Complete and balance the following double replacement reactions in the spaces below:
a. KOH + CuBr2 !
C 2KOH + CuBr2 ! Cu(OH)2 + 2KBr
b. Al(NO3)3 + FeF3 !
C Al(NO3 )3 + FeF3 ! AlF3 + Fe(NO3 )3
c. CaS + K3PO4 !
C 3CaS + 2K3 PO4 ! 3K2S + Ca3(PO4)2
12. Describe a neutralization reaction. Be sure to include an example in your description.
C Neutralization reactions involve an acid reacting with a base to form a salt and
water. For example, HX + MOH !
MX + H2O.
C An example of this reaction is HCl + NaOH ! NaCl + H2O.
13. Complete and balance the following neutralization reactions in the spaces below:
a. HBr + Al(OH)3 !
C 3HBr + Al(OH)3 ! AlBr3 + 3H2 O
b. CH3COOH + NaOH !
C CH3 COOH + NaOH ! Na(CH3 COO) + H2 O
c. H3PO4 + Ca(OH)2 !
C 2H3 PO4 + 3Ca(OH)2 ! Ca3 (PO4 )2 + 6H2 O
14. Describe a combustion reaction. Be sure to include an example in your description.
C Combustion reactions involve the rapid reacting of a compound or element with oxygen
to form an oxide and to produce heat. Often the compound being reacted is a
hydrocarbon. For example, CxHy + O2 !
CO2 + H2 O.
C An example of this reaction is CH4 + O 2 ! CO 2 + 2H2O
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15. Complete and balance the following combustion reactions in the spaces below:
a. C3H8 + O2 !
C C3 H8 + 5O2
! 3CO2 + 4H2 O
b. C3H6 + O2 !
C 2C3H6 + 9O2
! 6CO2 + 6H2 O
c. C6H12O6 + O2 !
C C6 H12 O6 + 6O2 ! 6CO2 + 6H2O
16. Classify each of the following reactions as synthesis, decomposition, single replacement, double
replacement, neutralization or combustion.
a. 2HCl ! H2 + Cl2
Decompostion
b. 2C2H2 + 5O2 ! 4CO2 + 2H2O
Combustion
c. H2SO4 + Ca(OH)2 ! CaSO4 + 2H2O
Neutralization
d. SrCl2 + 2NaNO3 ! Sr(NO3)2 + 2NaCl
Double replacement
e. 3Cl2 + 2FeBr3 ! 2FeCl3 + 3Br2
Single replacement
f. 2Cr + 3F2 ! 2CrF3
Synthesis
17. Complete the following reactions and classify them as synthesis, decomposition, single replacement,
double replacement, neutralization or combustion.
a. NaCl !
C NaCl ! 2Na + Cl2
Decomposition
b. CaI2 + Na2CO3 !
C CaI2 + Na2 CO3 ! CaCO3 + 2NaI
Double replacement
c. H2SO3 + Mg(OH)2 !
C H2 SO3 + Mg(OH)2 ! MgSO3 + 2H2 O
Neutralization
d. N2 + 3I2 !
C N2 + 3I2 ! 2NI3
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Synthesis
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e. C2H4 + O2 !
C C2 H4 + 3O2 ! 2CO2 + 2H2 O
Combustion
f. Mg + O2 !
C 2Mg + O2 ! 2MgO
Synthesis
g. Cl2 + CsI !
C Cl2 + 2CsI ! 2CsCl + I2
Single replacement
h. Be + Fe(NO3)2 !
C Be + Fe(NO3 )2 ! Be(NO3 )2 + Fe
Single replacement
i. AlBr3 + Cu2SO4 !
C 2 AlBr3 + 3Cu2 SO4 ! Al2(SO4)3 + 6CuBr
Double replacement
j. HCl + Al(OH)3 !
C 3HCl + Al(OH)3 ! AlCl3 + 3H2 O
Neutralization
Chapter 9.4 – Rates of Chemical Reactions
rate of reaction
1.
The
describes how quickly or slowly reactants turn into products.
2.
Temperature ,
surface area ,
the four main factors that affect reaction rates.
3.
Describe the kinetic molecular theory and the collision theory.
concentration
, and
catalysts
are
C The kinetic molecular theory suggests that matter is made up of tiny particles in
constant, random motion. Solid particles move the least, liquid particles move more,
and gas particles move the most.
C The collision theory states that in order for moving particles to react, they must
first collide. The collision must be an effective collision in which there is enough
energy for the particles that collide to react with each other.
solute
4.
Concentration refers to how much
5.
The greater the concentration, the greater the chance that
6.
Surface area
7.
Increasing
is dissolved in a solution.
collisions
among particles will occur.
is the measure of how much area of an object is exposed.
the surface area results in more collisions among particles.
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particles
of the reactants to move more
and more energy.
8.
Increasing the temperature of a reaction causes the
quickly , which leads to more
collisions
9.
A
catalyst
is a substance that speeds up the rate of a chemical reaction without being used
up in the reaction itself.
10. Catalysts make it possible for reactions to occur with less
otherwise need without the catalyst present.
energy
than reactions would
Vocabulary to Know
Write a concise definition of each of these terms found in this chapter.
Catalyst –
Chemical reaction –
Collision Theory –
Combustion reaction –
Decomposition reaction –
Double replacement reaction –
Kinetic Molecule Theory –
Neutralization reaction –
Reaction rate –
Single replacement reaction –
Synthesis reaction –
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