Types of Chemical Reactions - Wikispaces - SCH3UKING

SCH3U- R.H.KING ACADEMY CHEMICAL REACTIONS WORKSHEET Name: W2 B) SYNTHESIS A + B AB During a synthesis reaction, two or more...

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SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

Name:

Types of Chemical Reactions A) DECOMPOSTION AB  A + B During a decomposition reaction, one compound splits into two or more pieces. These smaller pieces can be elements or simpler compounds. Examples: magnesium chloride magnesium + chlorine calcium carbonate  calcium oxide + oxygen potassium chlorate  potassium chloride + oxygen iron(III) hydroxide  iron (III) oxide + water carbonic acid  carbon dioxide + water

2 H2O  2 H2 + O2 Na2CO3  Na2O + CO2 Ba(ClO3)2  BaCl2 + 3 O2 Cu(OH)2  CuO + H2O 2 H3PO4  P2O5 + 3 H2O

The following rules will help when determining the products of a decomposition reaction. 1. 2. 3. 4. 5.

All binary compounds will break down into their elements. All carbonates break down to the metal oxide and carbon dioxide gas. All chlorates break down to the metal chloride and oxygen gas. Metal hydroxides break down to the metal oxide and water. Oxy acids break down to the non-metal oxide (with the non-metal having the same valence) and water.

Practice Problems: Provide a completed word and full balanced chemical equation for each reaction. a) nickel (II) chloride 

g) Cs2CO3 

b) silver oxide 

h) Al(OH)3 

c) nitrous acid 

i) H2SO4 

d) iron (III) hydroxide 

j) RbClO3 

e) zinc carbonate 

k) LiCl 

f) carbonous acid 

l) Au(ClO3)3  W1

SCH3U- R.H.KING ACADEMY

B) SYNTHESIS

CHEMICAL REACTIONS WORKSHEET

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A + B  AB

During a synthesis reaction, two or more elements or simple compounds come together to form 1 compound. These are the reverse of a decomposition reaction. Examples: sodium + oxygen  sodium oxide lead (II) oxide + carbon dioxide  lead(II) carbonate iron (II) chloride + oxygen  iron (II) chlorate zinc oxide + water  zinc hydroxide silicon dioxide + water  silicic acid

Sn + F2  SnF2 K2O + CO2  K2CO3 BeCl2 + 3 O2  Be(ClO3)2 Na2O + H2O  2 NaOH SeO2 + H2O  H2SeO3

Since synthesis reactions are the reverse of decomposition reactions, reverse the rules from above to determine the products of a synthesis reaction. 1. 2. 3. 4. 5.

Two elements will react to form the binary compound. A metal oxide and carbon dioxide will react to form the metal carbonate. A metal chloride and oxygen will react to form the metal chlorate. A metal oxide and water will react to form a metal hydroxide. A non-metal oxide and water will react to form the oxy acid (with the non-metal having the same valence).

Practice Problems: Provide a completed word and full balanced chemical equation for each reaction. a) magnesium chloride + oxygen 

g) BeO + CO2 

b) cesium + iodine 

h) Al2O3 + H2O 

c) diphosphorus trioxide + water 

i) N2O3 + H2O 

d) potassium oxide + water 

j) NaCl + O2 

e) barium oxide + carbon dioxide 

k) Ga + Br2 

f) silver + sulfur 

l) Ca + P4  W2

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

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C) SINGLE DISPLACEMENT AX + Y  YX + A or AX + B  AB + X During a single displacement (also called single replacement) reaction one element replaces another element in a compound forming a new compound. There are 2 different possibilities. 1. One cation replaces another: AX + Y  YX + A, where both A and Y are cations (usually metals and hydrogen). For an element to displace another in a compound, it must be higher up in the activity series than the element in the compound. Examples: copper + silver nitrate  silver + copper (II) nitrate calcium + water  calcium hydroxide + hydrogen

Fe + Cu(NO3)2  Fe(NO3)2 + Cu Zn + HCl(aq)  ZnCl2 + H2

2. One anion replaces another: AX + B  AB + X, where both X and B are anions (usually nonmetals). For an element to displace another in a compound, it must be more reactive than the element in the compound. Examples: chlorine + sodium bromide  sodium chloride + bromine

Br2 + 2 KI  2 KBr + I2

Practice Problems: Provide a completed word and full balanced chemical equation for each reaction. a) aluminum + lead (II) nitrate 

g) Al + HCl 

b) chlorine + lithium iodide 

h) Zn + H2SO4 

c) iron + silver acetate 

i) Pb + AgNO3 

d) aluminum + copper (II) chloride 

j) Fe + CuSO4 

e) bromine + iron (III) chloride 

k) Li + H2O 

f) barium + water 

l) PbI4 + F2 

W3

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

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D) DOUBLE DISPLACEMENT AB + XY  AY + XB During a double displacement (also called a double replacement) reaction, the cations and anions of two different compounds switch places. Examples:

iron (II) acetate + sodium chloride  iron(II) chloride + sodium acetate

2 NaCl + H2SO4  Na2SO4 + 2 HCl AgNO3 + NaCl  AgCl + NaNO3 When an acid and base react, this is a special case of a double displacement reaction called a neutralization which forms a salt (ionic compound) and water. Examples:

potassium hydroxide + sulfuric acid  potassium sulfate + water 2 H3PO4 + 3 Ca(OH)2  Ca3(PO4)2 + 6 H2O

In some cases, a product will form in the double displacement reaction that will then decompose further. Whenever H2CO3, H2SO3 and NH4OH are formed in the reaction, they will decompose to CO2 and H2O, SO2 and H2O and NH3 and H2O respectively. Examples: calcium carbonate + hydrochloric acid  calcium chloride + carbon dioxide + water K2SO3 + 2 HNO3  2 KNO3 + SO2 + H2O NH4Cl + NaOH  NaCl + NH3 + H2O

Practice Problems: Provide a completed word and full balanced chemical equation for each reaction. a) calcium hydroxide + carbonic acid 

g) Na2CO3 + H2SO4 

b) potassium carbonate + barium chloride 

h) Al(OH)3 + HC2H3O2 

c) zinc phosphate + ammonium sulfide 

i)

Al2(SO4)3 + Ca3(PO4)2 

d) cobaltic hydroxide + nitric acid 

j)

Cr2(SO3)3 + H2SO4 

e) silver nitrate + potassium chloride 

k) AgC2H3O2 + K2CrO4 

f)

l)

ammonium chloride + magnesium hydroxide 

(NH4)2SO4 + KOH 

W4

SCH3U- R.H.KING ACADEMY E) COMBUSTION

CHEMICAL REACTIONS WORKSHEET CxHy + O2 (g)  CO2 (g) + H2O

(g)

or CxHy + O2 (g)  C (s) + CO

Name: (g)

+ CO2 (g) + H2O (g)

In a combustion reaction, a hydrocarbon (a compound made of carbon and hydrogen) reacts with oxygen gas. There are 2 types of combustion. 1. Complete Combustion: CxHy + O2 (g)  CO2 (g) + H2O (g) 2. Incomplete Combustion: CxHy + O2 (g)  C (s) + CO (g) + CO2 (g) + H2O (g) Examples: CH4 + O2 (g)  CO2 (g) + 2 H2O (g) C3H6 + 3 O2 (g)  C (s) + CO (g) + CO2 (g) + 3 H2O (g) In some cases the hydrocarbon may also contain nitrogen or sulfur, in which case NO2 or SO2 is also produced. Examples: C21H24N2O4 + 27 O2 (g)  21 CO2 (g) + 12 H2O (g) + 2 NO2 (g) 2 C2H5SH + 9 O2 (g)  4 CO2 (g) + 6 H2O (g) + 2 SO2 (g) Practice Problems: Complete a balanced chemical equation for each reaction. Assume complete combustion in each. a) C6H6 + O2 (g) 

b) C11H22O11 + O2 (g) 

c) C25H52 + O2 (g) 

d) C2H5OC2H5 + O2 (g) 

e) C4H9OH + O2 (g) 

f) C6H13SH + O2 (g) 

W5

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

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F) EXOTHERMIC AND ENDOTHERMIC Many reactions require or release heat and in addition to being classified as one of the types discussed above can also be classified as exothermic or endothermic. Exothermic reactions are those accompanied by a release of heat (energy) Example: 2 H2(g) + O2(g)  2 H2O(g) + Energy Endothermic reactions are those that require heat (energy) to be added for the reaction to occur. Example: CaCO3(s) + Energy  CaO

(s)

+ CO2 (g)

MAKING CONNECTIONS: 1. Use the textbook and Internet to summarize the following concepts and their applications in everyday life: a) Catalysts and Catalytic converters (P.201-202) b) Neutralization Reactions (P. 176 & P. 205-211) c) Extraction of Metals and Metallurgical Processes (P. 212, 217) d) Corrosion, Alloys and Corrosion Protection (P. 379)

2. Complete the following Textbook questions. P. P. P. P. P.

155 169 177 188 197

# # # # #

4, 6, 7; 5, 7, 9; 8; 71; 6, 8;

P. P. P. P.

204 # 201 # 217 # 221 #

5, 9; 3; 6; 6;

REVIEW - CHEMICAL REACTIONS P. 244- 253- read over all the questions, attempt as many as possible (write solutions to questions you find challenging).

W6

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

Name:

Types of Chemical Reactions 1. For each reaction below, indicate its type and then balance. a)

_____

H2

+

_____

O2



_____

H2O

Type: ________________________________________ b)

_____

H2O2



_____

O2

+

_____

H2

Al2(SO4)3

+

_____

H2

Hg

+

_____

O2

KCl

+

_____

Br2

PbCl2

+

_____

NaNO3

NaNO2

+

_____

O2

Ba3(AsO4)2

+

_____

H2O

Type: ________________________________________ c)

_____

Al

+

_____

H2SO4



_____

Type: ________________________________________ d)

_____

CO

+

_____

O2



_____

CO2

Type: ________________________________________ e)

_____

HgO



_____

Type: ________________________________________ f)

_____

KBr

+

_____

Cl2



_____

Type: ________________________________________ h)

_____

Cr2O3

+

_____

H2O



_____

Cr(OH)3

Type: ________________________________________ i)

_____

Pb(NO3)2

+

_____

NaCl



_____

Type: ________________________________________ j)

_____

NaNO3



_____

Type: ________________________________________ k)

_____

Ba(OH)2

+

_____

H3AsO4



_____

Type: ________________________________________ l)

_____

C5H12O

+

_____

O2



_____

CO2

+

_____

H2O

Type: ________________________________________ m)

_____

As2O5

+

_____

H2O



_____

H3AsO4 W7

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

Name:

2. Complete the following word equations by determining the products of the reaction, then write a balanced chemical equation and indicate the type of reaction. a) strontium bromide + fluorine 

b) magnesium + iron (III) oxide 

c) silver nitrate + zinc chloride 

d) nickel (III) carbonate 

e) tricarbon hexahydride + oxygen gas 

f) barium + water 

g) tin (II) hydroxide + phosphoric acid 

h) calcium chloride + oxygen 

i)

tetraphosphorus decaoxide + water 

j) lithium bicarbonate + hydrosulfuric acid 

k) acetic acid + nickel 

W8

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

Name:

Mixed Practice -State the type, predict the products, and balance the following reactions:

1.

BaCl2

+

H2SO4



2.

C6H12

+

O2



3.

Zn

+

CuSO4



4.

Cr2(SO3)3

+

HNO3



5.

Cs

+

Br2



6.

FeCO3



7.

NaClO3



8.

HCl(aq)

9.

Bi2O3



10.

Na2O



11.

CaCl2(aq)

+

Na3PO4(aq)



12.

Na2SO3

+

H3PO4



+

AgNO3(aq)



W9

SCH3U- R.H.KING ACADEMY

CHEMICAL REACTIONS WORKSHEET

13.

AlCl3

14.

C2H4

+

O2



15.

Pb(NO3)2(aq)

+

BaCl2(aq)



16.

Zn

+

AgNO3



17.

Al

+

P4



18.

H2SO4(aq)

+

NaOH(aq)



19.

NaI

+

MgS



20.

Cl2

+

NaBr



21.

C6H12O6

+

O2



22.

KOH(aq)

+

CuSO4(aq)



24.

Na2CO3

+

H2SO4



25.

(NH4)2S

+

Cd3(PO4)2



26.

(NH4)2S

+

Co(OH)3



Name:



W10