Chem 11.2

Front 1

What are the five types of chemical reactions?

Back 1

Combination, Decomposition, Single-Replacement, Double-Replacement and Combustion

Front 2

What are the keys to predicting the products of the five general types of reactions?

Back 2

Combination leads to a single compound; Decomposition leads to a combo in reverse; Single replacement creates a different element and a new compound; Doube-replacement creates two new compounds and combustion usually produces CO2 and H2O

Front 3

Classify and Balance

C3H6 + O2 --> CO2 + H20

Back 3

Combustion

2C3H6 + 9O2 --> 6CO2 + 6H2O

Front 4

Classify and Balance

Al(OH)3 --> Al2O3 and H2O

Back 4

Decomposition

2Al(OH)3 --> Al2O3 and 3H2O

Front 5

Classify and Balance

Li + O2 --> Li2O

Back 5

Combination

4Li + O2 --> 2Li2O

Front 6

Classify and Balance

Zn + AgNO3 --> Ag + Zn(NO3)2

Back 6

Single Replacement

Zn + 2AgNO3 --> 2Ag + Zn(NO3)2

Front 7

Which of the five general types of reaction would most likely occur, given each set of reactants? What are the probable products?

An aqueous solution of two ionic compounds

Back 7

Double Replacement Reaction

It would produce two new compounds driven by a precipitate, a gaseous product, or water

Front 8

Which of the five general types of reaction would most likely occur, given each set of reactants? What are the probable products?

a single compound

Back 8

Decomposition.

Two elements or an element and a compound

Front 9

Which of the five general types of reaction would most likely occur, given each set of reactants? What are the probable products?

Two elements

Back 9

Combination

a single compound

Front 10

Which of the five general types of reaction would most likely occur, given each set of reactants? What are the probable products?

oxygen and a compound of carbon and hydrogen

Back 10

Combustion

CO2 and H2O

Front 11

Complete and Balance

CaI2 + Hg(NO3)2 --> (HgI2 precipitates)

Back 11

Double Replacement

CaI2 + Hg(NO3)2 --> HgI2 + Ca(NO3)2

Front 12

Al + Cl2 --> ?????

Back 12

Al + Cl2 --> AlCl3

Combination

Front 13

Ag + HCL --????

Back 13

Ag + HCL --> H + AgCl

Single replacement

Front 14

C2H2 + O2 --????

Back 14

C2H2 + 3O2 --> 2CO2 + 2H2O

Combustion

Front 15

MgCl --> ????

Back 15

Decomposition

MgCl --> Mg + Cl

Front 16

What are the three types of products that result from a double-replacement reaction?

Back 16

precipitate, a gaseous product and Water.

Front 17

Write the equation

Cu(s) + S (s) --> two reactions are possible

Back 17

For copper (II):
Cu(s) + S(s) --> CuS (s) (balanced)
For copper (I):
2Cu(s) + S (s) --> Cu2S(s)

Front 18

Complete and Balance

Be + O2 -->

Back 18

2Be + O2 --> 2BeO

Front 19

Write and Balance the formation of magnesium nitride (Mg3N2) from its elements.

Back 19

3Mg + N2 --> Mg3N2

Front 20

Complete and balance this decomp

HI -->

Back 20

2HI --> H2 + I2

Front 21

Write the formula for the binary compound that decomposes to the products H2 and Br2

Back 21

HBr

Front 22

Complete the equations for these single replacement reactions in teh aqueous solution. Balance each equation. Write "no reactoin" if a reaction does not occur.
Fe(s) + Pb(NO3)2(aq) -->

Back 22

Fe(s) + Pb(NO3)2(aq) --> Fe(NO3)2(aq) + Pb(s)

Front 23

Complete the equations for these single replacement reactions in teh aqueous solution. Balance each equation. Write "no reactoin" if a reaction does not occur.
Cl2(aq) + NaI(aq) -->

Back 23

Cl2(aq) + 2Nal(aq) --> 2NaCl(aq) +I2(aq)

Front 24

Complete the equations for these single replacement reactions in teh aqueous solution. Balance each equation. Write "no reactoin" if a reaction does not occur.
Ca(s) + H2O(l) -->

Back 24

Ca(s) + 2H2O(l) -->Ca(OH)a(aq) + H2(g)

Front 25

Write the products of these double replacement reactions. Then balance each equation.
NaOH(aq) + Fe(NO3)3(aq) --> (iron (III) hydrooxide is a preciptiate

Back 25

3NaOH(aq) + Fe(NO3)3(aq) --> Fe(OH)3(s) +3NaNO3(aq)

Front 26

Write the products of these double replacement reactions. Then balance each equation.
Ba(NO3)2(aq) + H3PO4(aq)-->
(Barium phosphate is a precipitate.)

Back 26

3Ba(NO3)2(aq) + 2H3PO4(aq) --> Ba3(PO4)2(s) + 6HNO3(aq)

Front 27

Write a balanced equation

KOH(aq) + H3PO4(aq) -->

Back 27

3KOH(aq) + H3PO4(aq) --> K3(PO4)(aq) + 3H2O(l)

Front 28

Write a balanced equation

H2SO4(aq) + Al(OH)3(aq) -->

Back 28

3H2SO4(aq) + 2Al (OH)3(aq) --> Al2(SO4)3(aq) + 6H2O (l)

Front 29

Write a balanced equation for the complete combustion

formic acid (HCOOH)

Back 29

2HCOOH + O2 --> 2CO2 +2H2O

Front 30

Write a balanced equation for the complete combustion

heptane (C7H16)

Back 30

C7H16 + 11O2 --> 7CO2 + 8H2O

Front 31

Write a balance equation for the combustion of glucose (C6H12O6)

Back 31

C6H12O6 +6O2 -->6CO2 + 6H2O

Front 32

Write a balanced chemical reaction for the following combo reaction

Mg + O2 -->

Back 32

2Mg + O2 --> 2MgO

Front 33

Write a balanced chemical reaction for the following combo reaction

P + O2 --> diphosphorus pentoxide

Back 33

4P + 5O2 --> 2P2O5

Front 34

Write a balanced chemical reaction for the following combo reaction

Ca + S -->

Back 34

Ca + S --> CaS

Front 35

Write a balanced chemical equation for each decomposition reaction

Ag2O(s) --heat-->

Back 35

2Ag2O --heat-> 4Ag + O2

Front 36

Write a balanced chemical equation for each decomposition reaction

ammonium nitrate --heat--> dinitrogen monooxide + water

Back 36

NH4NO3 --heat--> N2O + 2H2O

Front 37

Use the activity series of metals to write a balanced chemical equation for each single replacement reaction.

Au(s) + KNO3(aq) -->

Back 37

Ask Pippen since gold is not in the reactivity table. Does this mean it is not very reactive?

Front 38

Use the activity series of metals to write a balanced chemical equation for each single replacement reaction.

Zn(s) + AgNO3(aq) -->

Back 38

Zn(s) + 2AgNO3(aq) --> 2Ag + Zn(NO3)2

Front 39

Use the activity series of metals to write a balanced chemical equation for each single replacement reaction.

Al(s) + H2SO4 (aq) -->

Back 39

2Al(s) + 3H2SO4 (aq) --> 3H2 + Al2(SO4)3

Al does replace H in this acid (sufuric) as indicated in the activity series of Metals

Front 40

Write a balanced equation for the double replacement reaction

H2C2O(aq) + KOH(aq) -->

Back 40

H2C2O4(aq) + KOH(aq) --> K2C2O4(aq) + 2H2O(l)

Front 41

Write a balanced equation for the double replacement reaction

CdBr(aq) + Na2S(aq) --> Cadmium sulfide is a precipitate

Back 41

CdBr2(aq) + NaS(aq) --> CdS(s) + 2NaBr(aq)

Front 42

What substance is common to all combustion reactions?

Back 42

Oxygen

Front 43

What the common products in combustion reactions?

Back 43

Carbon dioxide and Water

Front 44

Write a balance equation for the completed combustion of this compound

butene (C4H6)

Back 44

C4H8 + 6O2 --> 4CO2 + 4H2O

Front 45

Write a balance equation for the completed combustion of this compound

acetone (C3H6O)

Back 45

C3H6O + 4O2 --> 3CO2 + 3H2O

Front 46

Balance the equation and identify the type

Hf + N2 --> Hf3N4

Back 46

3Hf + 2N2 --> Hf3N4

Combination

Front 47

Balance the equation and identify the type


Mg + H2SO4 --> MgSO4 + H2

Back 47

Mg + H2SO4 --> MgSO4 + H2

Single Replacement

Front 48

Balance the equation and identify the type

C2H6 + O2 --> CO2 + H2O

Back 48

2C2H6 + 7O2 --> 4CO2 + 6H2O

Combustion

Front 49

Balance the equation and identify the type

Pb(NO3)2 + Nal --> PbI2 + NaNO3

Back 49

Pb(NO3)2 + 2Nal --> PbI2 + 2NaNO3

Double replacement

Front 50

Balance the equation and identify the type

Fe + O2 --> Fe3O4

Back 50

3Fe + 2O2 --> Fe3O4

Combination