types of reactions including reaction prediction

Types of Reactions

Including reaction prediction

Generals about writing Equations

Generals about writing Equations

Reactants on the left and products on the right

Symbols - see text for symbols that are included in equations.Ex: g for gas, l for liquid, s for solidDownward arrow for precipitate, aq for aqueous

Catalyst goes above the arrow KI

Ex H2O2(aq) ---> H2O(l) + O2(g)

Diatomic Molecules - BrINClHOFElemental state - Br2I2N2Cl2H2O2F2

Reactants on the left and products on the right

Symbols - see text for symbols that are included in equations.Ex: g for gas, l for liquid, s for solidDownward arrow for precipitate, aq for aqueous

Catalyst goes above the arrow KI

Ex H2O2(aq) ---> H2O(l) + O2(g)

Diatomic Molecules - BrINClHOFElemental state - Br2I2N2Cl2H2O2F2

1. Synthesis (Combination)1. Synthesis (Combination)

Two or more substances react to form a single substance

R + S --> RSEx) SO3(g) + H2O(l) --> H2SO4(aq) Usually gives off energy when forming

bondsExample: Write the balanced equation for:

magnesium ribbon reacting with oxygenMg(s) + O2(g) ---> MgO(s)

2 Mg(s) + O2(g) --> 2MgO(s)

Two or more substances react to form a single substance

R + S --> RSEx) SO3(g) + H2O(l) --> H2SO4(aq) Usually gives off energy when forming

bondsExample: Write the balanced equation for:

magnesium ribbon reacting with oxygenMg(s) + O2(g) ---> MgO(s)

2 Mg(s) + O2(g) --> 2MgO(s)

1. Synthesis (Combination)1. Synthesis (Combination)

Your turn. Write balanced equations for the following:Aluminum (s) reacts with oxygen (g)Hydrogen (g) reacts with oxygen (g)

Answers:4 Al(s) + 3 O2 ---> 2 Al2O3(s)

2 H2(g) + O2(g) ---> 2 H2O(l)

Your turn. Write balanced equations for the following:Aluminum (s) reacts with oxygen (g)Hydrogen (g) reacts with oxygen (g)

Answers:4 Al(s) + 3 O2 ---> 2 Al2O3(s)

2 H2(g) + O2(g) ---> 2 H2O(l)

2. Decomposition2. Decomposition

A single compound is broken down into simpler products

RS --> R + SEx) BCl3 --> B + Cl2Requires energy to break chemical bonds

(heat, light, electricity)Example - Write the balanced equation for

mercury (II) oxide decomposing;HgO --> Hg + O2

2HgO --> 2Hg + O2

A single compound is broken down into simpler products

RS --> R + SEx) BCl3 --> B + Cl2Requires energy to break chemical bonds

(heat, light, electricity)Example - Write the balanced equation for

mercury (II) oxide decomposing;HgO --> Hg + O2

2HgO --> 2Hg + O2

2. Decomposition2. Decomposition

Your turn. Write balanced equations for the following:

The decomposition of waterThe decomposition of lead (IV) oxideAnswers

2 H2O(l) --> 2 H2(g) + O2(g)

PbO2(s) --> Pb(s) + O2(g)


The decomposition of waterThe decomposition of lead (IV) oxideAnswers

2 H2O(l) --> 2 H2(g) + O2(g)

PbO2(s) --> Pb(s) + O2(g)

3. Single Replacement Reactions

3. Single Replacement Reactions

An element replaces an element of a compound

T + RS --> TS + REx) Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)

A metal may replace a metal or a nonmetal may replace a nonmetal

Activity Series - list of metal in order of decreasing activity

Nonmetals reactivity decreases as you go down the periodic table

This is limited to the halogens -group 7A

An element replaces an element of a compound

T + RS --> TS + REx) Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)

A metal may replace a metal or a nonmetal may replace a nonmetal

Activity Series - list of metal in order of decreasing activity

Nonmetals reactivity decreases as you go down the periodic table

This is limited to the halogens -group 7A

3. Single replacement reactions3. Single replacement reactions

Ex) Write the balanced equation when aluminum reacts with sulfuric acid

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

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

Ex) Write the balanced equation when aluminum reacts with sulfuric acid

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

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

3. Single replacement reactions3. Single replacement reactions


When chlorine reacts with potassium iodide

When copper (assume Cu2+) is added to Iron (II) Sulfate

Answers Cl2(g) + 2 KI(aq) --> 2 KCl(aq) + I2Cu + FeSO4 --> no reaction (no rxn)


When chlorine reacts with potassium iodide

When copper (assume Cu2+) is added to Iron (II) Sulfate

Answers Cl2(g) + 2 KI(aq) --> 2 KCl(aq) + I2Cu + FeSO4 --> no reaction (no rxn)

4. Double Replacement4. Double Replacement

Exchange of positive ions between two compounds. Just swap the positive ions and write the new formula.

R+S- + T+U- --> R+U- + T+S-

Ex) FeS(s) + 2HCl(aq) --> H2S(g) + FeCl2(aq)

Ex) Write the balanced equation for barium chloride added to potassium carbonate

BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + KCl(aq)

BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2 KCl(aq)

Exchange of positive ions between two compounds. Just swap the positive ions and write the new formula.

R+S- + T+U- --> R+U- + T+S-

Ex) FeS(s) + 2HCl(aq) --> H2S(g) + FeCl2(aq)

Ex) Write the balanced equation for barium chloride added to potassium carbonate

BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + KCl(aq)

BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2 KCl(aq)

4. Double Replacement4. Double Replacement

Your turn. Write balanced equations for the following.

Iron (III) Sulfide reacting with hydrochloric acid

AnswerFe2S3(s)+ 6 HCl(aq) --> 2 FeCl3(aq) + 3

H2S(g)

Your turn. Write balanced equations for the following.

Iron (III) Sulfide reacting with hydrochloric acid

AnswerFe2S3(s)+ 6 HCl(aq) --> 2 FeCl3(aq) + 3

H2S(g)

5. Combustion Reactions5. Combustion Reactions

Oxygen reacts with another substance, often producing heat and light

Often involve hydrocarbons Compounds of hydrogen and carbon

Combustion of hydrocarbons produces a lot of energy, therefore, hydrocarbons are used as fuels.

Examples: methane, propane, butane, octane

Oxygen reacts with another substance, often producing heat and light

Often involve hydrocarbons Compounds of hydrogen and carbon

Combustion of hydrocarbons produces a lot of energy, therefore, hydrocarbons are used as fuels.

Examples: methane, propane, butane, octane


Two types of combustion1. Complete combustionCxHy + O2(g) --> CO2(g) + H2O(g) +

energy2. Incomplete combustionTwo more products: CO and C CxHy + O2(g) --> CO2(g) + H2O(g) + CO(g) + C(s) +

energy

Two types of combustion1. Complete combustionCxHy + O2(g) --> CO2(g) + H2O(g) +

energy2. Incomplete combustionTwo more products: CO and C CxHy + O2(g) --> CO2(g) + H2O(g) + CO(g) + C(s) +

energy


Ex) Write a balanced equation for the complete combustion of C3H8.

C3H8(g) + O2(g) --> CO2(g) + H2O(g) + energy C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4H2O(g) + energy

Your turn: Write a balanced equation for the complete combustion of C8H18.

Answer2 C3H18(l) + 25 O2(g) --> 16 CO2(g) + 18 H2O(g) +

energy

Ex) Write a balanced equation for the complete combustion of C3H8.

C3H8(g) + O2(g) --> CO2(g) + H2O(g) + energy C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4H2O(g) + energy

Your turn: Write a balanced equation for the complete combustion of C8H18.

Answer2 C3H18(l) + 25 O2(g) --> 16 CO2(g) + 18 H2O(g) +

energy

QuickTime™ and aYUV420 codec decompressor

are needed to see this picture.

types of reactions including reaction prediction

Documents