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http://mrged.flexinet.com.au. Types of Chemical Change. You already know about,. 1.The two main types of chemical bonding. 2. Writing chemical formulas (formulae). This week we will find out about;. 1.Synthesis Reactions. 2. Decomposition reactions. 3. Single replacement reactions.

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slide1

http://mrged.flexinet.com.au

Types of Chemical Change

slide2

You already know about,

1.The two main

types of chemical bonding

2. Writing chemical formulas

(formulae)

slide3

This week we will find out about;

1.Synthesis Reactions

2. Decomposition reactions

3. Single replacement reactions

4. Double replacement reactions

slide6

Ionic Bonding

This type of bonding

will occur when a metal reacts with a non -metal

It always involves a complete transfer of electrons

  • It always produces IONS (charged particles)
slide7

1 Na reacts with 1 Cl

Formula = NaCl

View animation at

http://mrged.flexinet.com.au

slide8

Covalent Bonding

This type of bonding

will occur when a non- metal reacts with a non -metal

Here both atoms will share electrons

  • It always produces molecules (particles with no charge)
slide10

Rules leading to correct formula

1. Positive ions (cations) can join to negative ions (anions)

2. Positive ions usually form the first part of the name (99% cases)

3. If the formula is correct there is no overall charge

Please copy into your exercise books

4. If you have more than one polyatomic ion it is placed inside brackets

slide11

Positive ions

(Cations)

Negative ions

(Anions)

+ 1

- 1

fluoride F

sodium Na

chloride Cl

potassium K

bromide Br

hydroxide OH

hydrogen H

Essential training ions

nitrate NO3

lithium Li

silver Ag

hydrogencarbonate HCO3

ammonium NH4

- 2

carbonate CO3

magnesium Mg

+2

oxide O

calcium Ca

sulphide S

barium Ba

zinc Zn

sulphate SO4

iron(11) Fe

sulphite SO3

copper Cu

chromate CrO4

+3

- 3

nitride N

aluminium Al

chromium Cr

phosphate PO4

iron(111) Fe

slide12

sodium fluoride

Chemical Formulae 1.

IONS

CHARGES

NUMBERS

Na

F

FORMULA

slide13

magnesium fluoride

Chemical Formulae 2.

CHARGES

IONS

NUMBERS

Mg

F

FORMULA

slide14

Chemical Formulae 3.

silver hydroxide

CHARGES

IONS

NUMBERS

Ag

OH

FORMULA

slide15

calcium nitrate

Chemical Formulae 4.

CHARGES

IONS

NUMBERS

Ca

NO3

FORMULA

slide16

ammonium carbonate

Chemical Formulae 5.

CHARGES

IONS

NUMBERS

NH4

CO3

FORMULA

slide17

aluminium bromide

Chemical Formulae 6.

CHARGES

IONS

NUMBERS

Al

Br

FORMULA

slide18

chromium sulphide

Chemical Formulae 7.

CHARGES

IONS

NUMBERS

Cr

S

FORMULA

slide19

Chemical Formulae 8.

BLANK ITEM

CHARGES

IONS

NUMBERS

FORMULA

slide20

Try these:

1. lithium sulphite

2. barium hydroxide

3. copper carbonate

4. hydrogen sulphide

5. magnesium nitride

6. ammonium bromide

7. aluminium oxide.

slide21

In chemistry there are millions of chemical reactions.

But most reactions can be classified as

one of four types of reactions:

Synthesis: A + B -> AB

Decomposition: AB -> A + B

Single Replacement: A + BC -> AC + B

Double Replacement: AB + CD -> AD + CB

slide22

Synthesis (Composition)

C

O

O

O

O

C

In a synthesis reaction

(also known as a composition reaction),

two substances combine to form a larger substance.

+

slide23

Here are 3 synthesis reactions:

Hydrogen + oxygen yields water

2H2 + O2 -> 2H2O

Magnesium + nitrogen yields magnesium nitride

3Mg + N2 -> Mg3N2

Iron + sulphur yields iron(II) sulphide

Fe + S -> FeS

slide24

Decomposition

In a decomposition reaction, a larger substance

breaks apart and forms two or more simpler substances.

slide25

The first thing you may notice about a decomposition reaction

is that it is the complete opposite of a synthesis reaction.

In fact many synthesis reactions

can be reversed into a decomposition reaction.

When you burn hydrogen gas,

the hydrogen combines with oxygen to produce water.

2H2 + O2 -> 2H2O

With an electrical current, water can be

decomposed into hydrogen and oxygen gas.

2H2O -> 2H2 + O2

slide27

Some examples of decomposition

Heat copper carbonate and it will decompose

(Refer to flash animation .swf)

CuCO3 -> CuO + CO2

(Most carbonates decompose producing the oxide and carbon dioxide)

Heat lead(11) hydroxide and it will decompose

Pb(OH)2 -> PbO + H2O

slide28

PrecipitaReact.MOV

FormWater.MOV

FORMALUMBRO.MOV

THERMITE.MOV

NitrogTriiodide.MOV

REDUCTIONCUO.MOV

6x Quicktime mov files

slide29

TRY THESE:

1. Watch all 12 mov files (available on SET drive)

2. Classify each as either, synthesis, decompostion, single of double replacement reactions

3. Write a correct chemical equation for each!

Some may require some research

slide30

Single Replacement

In a single replacement reaction,

a more active element replaces

a less active element in a compound.

more reactive

less reactive

slide31

Single Replacement

Here Mg is more reactive than Pb

slide32

Single Replacement

If fluorine gas is bubbled through a solution of

potassium chloride, the fluorine will replace the chlorine.

This reaction can be represented as follows;

2KCl + F --> 2KF + Cl

No surprise! fluorine is more reactive than chlorine

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