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(1)

REACTION TYPES

(2)

TYPES OF REACTIONS

There are five types of chemical

reactions we will talk about for now:

1)

Combustion rxns

2)

Synthesis rxns

3)

Decomposition rxns

4)

Single Displacement rxns

5)

Double Displacement rxns

You need to be able to identify the type

of reaction and predict the product(s)

(3)

1. COMBUSTION REACTIONS

Combustion reactions occur when a

hydrocarbon (?) reacts with oxygen gas.

This is also called burning!!! You need

three (3) things

1)

A Fuel (hydrocarbon)

2) Oxygen (O

2

) to burn it with

3)

Something to ignite the rxn (spark)

(4)

COMBUSTION RXNS

In general:

C

x

H

y

+ O

2

CO

2

+ H

2

O

Products in combustion are CO

2

and

H

2

O. (although incomplete burning

(5)

2. SYNTHESIS RXNS

Synthesis reactions

occur when two

substances (generally

elements

)

combine and form a compound.

reactant + reactant

1 product

Basically:

A + B

AB

Example: 2H

2

+ O

2

2H

2

O

Example: C

+ O

2

CO

2

(6)

SYNTHESIS RXNS

Here is an example of a synthesis reaction

(7)

DIFFERENT TYPES

1) Metal + nonmetal  metal nonmetal (ide)

 Ex: Aluminum + Chlorine  Aluminum Chloride

2) Nonmetal + nonmetal  covalent compound  Ex: Carbon + Chlorine  Carbon Tetrachloride

3) Metal oxide + water  base (metal hydroxide)  Calcium oxide + water  Calcium hydroxide

4) Nonmetal oxide + water  acid (has H+ ion)

 Carbon dioxide + water  Carbonic acid

(8)

PREDICTING PRODUCTS

 Here are a few important things to remember when predicting products:

The compounds form must be neutral

ionic compounds (which means you’ll be

paying attention to their charges)

You do NOT carry subscripts from the

reactants to the products.

(9)

SYNTHESIS

 Two or more reactants combine to form…

ONE

PRODUCT!!

A + B

(10)

SYNTHESIS CONTINUED

Mg + O

2

MgO

Two reactants form one product

BUT WAIT!!

Don’t forget about everything you have already learned! Is your equation balanced??

(11)

LET’S GO BACK TO THAT

SYNTHESIS EXAMPLE

 Remember the reaction:

Mg + O

2

Helpful hint for later…why is oxygen O2 and not just O?

Click to find out why

Click to find out why

(12)

WHY O

2

??

 What are the other diatomic elements?

Oxygen is a diatomic molecule, which

means when oxygen is by itself it

must be O

2

. Remember that this

DOES NOT mean that oxygen is O

2

in

compounds, only by itself!

Go back Go back

H

2

I

2

Br

2

O

2

N

2

Cl

2

F

2

(13)

NOW TO PREDICT THE

PRODUCTS…

Remember A + B

AB so Mg + O

2

will make a compound with

magnesium and oxygen. What

does a compound with magnesium

and oxygen look like??

(14)

A COMPOUND WITH MAGNESIUM

AND OXYGEN…

Magnesium is a metal, oxygen is a nonmetal so

we must be forming an

IONIC

compound.

What’s the charge of Mg?

Mg

2+

What’s the charge of O?

(15)

2-SO WHAT’S THE COMPOUND?

Mg

2+

O

2-Pick…

MgO

2

Mg

2

O

2

(16)

NOPE!

+2 + 2(-2) DOES NOT EQUAL ZERO

MgO

2

Try again!

(17)

NOPE!

2(+2) + 2(-2) = 0

But remember ionic compounds need to be in the simplest form

Mg

2

O

2

Try again!

(18)

YES! VERY GOOD!

MgO is a neutral, correct ionic compound so

our formula is

Mg + O

2

MgO

Finally, balance the equation to satisfy the

law of conservation of mass…

(19)

3. DECOMPOSITION

forms two or more products

ONE REACTANT…

A + B

AB

(20)

DECOMPOSITION CONTINUED

The electrolysis of water is when water

decomposes into hydrogen and oxygen gas as shown below:

(21)

PREDICTING PRODUCTS AND

DECOMPOSITION

 What if we were not already given the products, how would we predict them?

H

2

O

??

Water is made of hydrogen and oxygen, so will my products just be H and O?

(22)

NO!

 Remember, H and O are both diatomic elements.

H

2

O

H

2

+ O

2

But wait….something

is still missing….

But wait….something

is still missing….

(23)

BALANCE!

 Don’t forget to balance your equation after you make your products! Your final answer should look like this:

(24)

YOU TRY ONE…

What is the correct reaction for the

decomposition of sodium chloride, NaCl?

NaCl Na + Cl NaCl Na + Cl

2NaCl 2Na + Cl2

2NaCl 2Na + Cl2

2NaCl Na2 + Cl2

2NaCl Na2 + Cl2

(25)

NOPE!

 Don’t forget that chlorine is a diatomic element, so it must be Cl2

NaCl Na + Cl NaCl Na + Cl

Try again!

(26)

NOPE!

 Although this reaction is correctly balanced, sodium is NOT a diatomic element

2NaCl Na2 + Cl2

2NaCl Na2 + Cl2

Try again!

(27)

YES! VERY GOOD!

 This is a correct reaction for the decomposition of sodium chloride.

2NaCl 2Na + Cl2

2NaCl 2Na + Cl2

(28)

TYPE 1- DECOMPOSITION

Metal Chlorate- when heated, the

compound will decompose into a metal

chloride and oxygen gas.

2

KCl

O

3

2

KCl

+ 3

O

2

Ni(Cl

O

3

)

2

NiCl

2

+ 3

O

2

(29)

TYPE 2- DECOMPOSITION

Metal Carbonate- when heated the

compound decomposes into a metal oxide

and carbon dioxide.

Ca

CO

3

Ca

O + CO

2

Fe

2

(CO

3

)

3

Fe

2

O

3

+ 3CO

2

(30)

TYPE 3- DECOMPOSITION

Some metal hydroxides- When heated the

compound will decompose into a metal

oxide and water

 Group 1 will not decompose

Mg

(

O

H)

2

MgO + H

2

O

Cu

(

O

H)

2

CuO + H

2

O

(31)

TYPE 4- DECOMPOSITION

Some acids- When heated will break down

into a nonmetal oxide and water.

H

2

CO

3

CO

2

+ H2O

H2SO4

SO3 + H2O

(32)

TYPE 5- DECOMPOSITION

 If the compound is made up of only 2

elements, then they will decompose into their individual elements.

NaCl

Na + Cl

2

H

2

O

H

2

+ O

2

(33)

4. SINGLE DISPLACEMENT

Single displacement: occurs when one

element or compound replaces another

element or compound.

For most reactions:

AB + C

AC + B (If A is a metal)

AB + C

BC + A (if A is a nonmetal)

Use activity series chart to see if rxn occurs!

(34)

TYPE 1

Replacement of a metal in a

compound by a more reactive metal.

Ca

+

Zn

(NO

3

)

2

Ca

(NO

3

)

2

+

Zn

Pb + Na

2

SO

4

No reaction

1/6/21 34

(35)

TYPE 2

Replacement of a hydrogen in an

acid by a more active metal.

H

2

SO

4

+ 2Na

Na

2

SO

4

+ H

2

1/6/21 35

(36)

TYPE 3

Replacement of one hydrogen in water by

an active metal

Active metals are in group 1 or 2

One product of a metal hydroxide

Ca + 2H

2

O

Ca(OH)

2

+ H

2

(37)

TYPE 4

Replacement of a halogen by a halogen

2NaI + F

2

2NaF + I

2

(38)

5. DOUBLE DISPLACEMENT

Occur when a metal replaces a metal in a

compound and a nonmetal replaces a

nonmetal in a compound

AB + CD

AD + CB

(switch the last names)

Check solubility!

(39)

TYPE 1

Two aqueous solutions mix to form a

precipitate.

AgNO

3

+ NaCl

AgCl + NaNO

3

 (silver chloride is a insoluble/precipitate)

(40)

TYPE 2

Similar to type 1, but a gas is

released instead of a precipitate

forming

H

2

SO

4

+ 2NaCl

2HCl + Na

2

SO

4

 (hydrogen chloride is a gas)

(41)

TYPE 3

 An acid reacts with a base to form water and a salt

HCl + NaOH

H

2

O + NaCl

 NaOH = base

 When you mix an acid with a base, they will neutralize

(42)

TYPE 4

Two aqueous solutions produce two

aqueous solutions and therefore react

again in the reverse direction.

Ca(NO

3

)

2

+ 2NH

4

Cl

CaCl

2

+ 2NH

4

NO

3

Both products are soluble, so this is an

equilibrium reaction.

When this happens, use a 2

nd

arrow to

point backwards.

References

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