TOPIC Carbon Compound _class

CHAPTER 2 : CARBON COMPOUND COMPOUND ORGANIC COMPOUND

INORGANIC COMPOUND

"all compound that contain carbon elements"

"all compound that not contain carbon elements"

"except: carbonate compound (CaCO3) : hydrogen carbonate (CaCHO3) : cyanide compound (HCN) : oxide carbon (CO2, CO)

-

" all including the 4 on the left" " example : Silica (Si)

HYDROCARBON compound that only contain Carbon (C) and hydrogen (H) only example : o Petroleum gas, Petrol

o o

Saturated compound - molecule that made of single bond ( - )

Unsaturated compound

Kerosene , Diesel Fuel oil

- molecule that made of double bond (=)

COMBUSTION OF HYDROCARBON PRODUCT - Hydrocarbon is a good source of fuel because it can form a reaction that can emit(membebaskan) a lot of heat when burn in the air [exothermic reaction] Hydrocarbon + Oxygen gasses → carbon dioxide + water

-

-

- Example : CH4 + O2 → CO2 + H2O [observation : CO2 gas will turn lime water into chalky] ALKANE

-

Alkanes are family of hydrocarbons.

- Alkanes has SINGLE covalent bond

General molecular formula for alkanes is CnH2n +2 IUPAC name for alkanes is end with -ane Number of Carbon

Name

Molecuar formula [CnH2n +2]

1

Methane

CH4

2

Ethane

C2 H6

3

Propane

C3 H8

4

Butane

5

Pentane

6

Hexane

Structural Formula Expended H ǀ H−C–H ǀ H H H ǀ ǀ H−C–C–H ǀ ǀ H H H H H ǀ ǀ ǀ H−C–C–C–H ǀ ǀ ǀ H H H

1

Condensed

CH4

CH3CH3

CH3CH2CH3

7

Heptane

8

Octane

9

Nonane

10

Decane

ALKENES

-

Alkenes has a DOUBLE covalent bond General molecular formula for alkenes is CnH2n IUPAC name for alkenes is end with -ene Number of Carbon

Name

2

Ethene

3

Propene

4

Butene

5

Pentene

6

Hexene

7

Heptene

8

Octene

9

Nonene

10

Decene

Molecuar formula [CnH2n]

Structural Formula Expended

Condensed

C2 H6

H−C=C–H ǀ ǀ H H

CH2CH2

C3 H8

H ǀ H−C=C–C–H ǀ ǀ ǀ H H H

CH2CHCH3

2

;p=PHYSICAL PROPERTIES

-

Alkanes and alkenes are bonded with a COVALENT BOND So both of the alkanes and alkenes have SAME physical properties.

Decane

Decene

Melting Point

Density

Solubility

Density increases as moved down the groupAll alkanes and alkenes less dense than water.

Ethene Propene Butane Pentene Hexene Heptene Octene Nonene

Boiling Point

Melting Point increases as moved down the groupBoiling Point of alkanes and alkenes is high.

Methane Ethane Propane Butane Pentane Hexane Heptane Octane Nonane

RMM

Relative Molecular Mass increases as moved down the group

ALKENES

Boiling Point increases as movedBoiling down the Point group of alkanes and alkenes is high.

PHYSICAL PROPERTIES ALKANES

All alkanes and alkenes dissolve in organic compound only but not dissolve in water

Electric Conductivity

All alkanes and alkenes cannot conduct electricity - Because there is no free moving ions

CHEMICAL PROPERTIES ALKANES Complete Combustion :[excess oxygen] - Alkanes that COMPLETELY burn in the air will produce carbon dioxide (CO2) , water (H2O) and release heat. The bigger the number of Carbon attached, more SOOT produced. 2C2H6 (g) +7O2 → 4CO2 + 2H2O (l) 2CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)

ALKENES Complete Combustion :[excess oxygen]

Incomplete Combustion : [limited oxygen] In incomplete combustion, more sooty flames are produce because more carbon and carbon monoxide produce.

Incomplete Combustion : [limited oxygen]

C2H4 (g) + O2 → CO2 + H2O (l) C3H6 (g) + O2 (g) → CO2 (g) + H2O (l)

CH4 (g) + O2 (g) → CO (g) + H2O CH4 (g) + O2 (g) → C (g) + H2O

3

C2H4 (g) + O2 (g) → CO (g) + H2O (l) C3H6 (g) + O2 (g) → C (g) + H2O (l)

Substitution Reaction : 1. Halogenations - When alkanes react with halogen (Group 17) and exposed in ultraviolet rays @ sunlight.

Substitution[penggantian] :

1.

Halogenations [penggantian H dengan kumpulan Halogen]

CH4 (g) + Cl2 (g) → CH3Cl + HCl

[chlorination] H H ǀ ǀ H–C=C–H + Ethane

Cl – Cl

→

Chlorine

H H ǀ ǀ H–C– C–H ǀ ǀ Cl Cl 1,2-dichloroethane

[Bromination] H H ǀ ǀ H – C = C – H + Br – Br Ethene

Bromine

→

H H ǀ ǀ H–C– C–H ǀ ǀ Br Br 1,2-dibromoethane

" If ethane is passed through bromine water or in tetrachloromethane, the brown colour of bromine is decolourised immediately”

4

2. Hydrogenation [penukaran double bond kpd single bond] H H ǀ ǀ H–C=C–H + Ethene 3.

H H Ni/Pt ǀ ǀ H–H → H–C– C–H 200OC ǀ ǀ H H Hydrogen Ethane

Hydration [addition of water to form alcohol]

H H ǀ ǀ H–C=C–H +

H3PO4

H – OH 300O, 60 atm

Ethene 4.

Water

With Hydrogen Halides

H H ǀ ǀ H–C=C–H + Ethene

5.

H – Cl

→

hydrogen Chloride

Ni/Pt KMnO4 200OC

Ethane

n

H H ǀ ǀ H–C– C–H ǀ ǀ H Cl chloroethane

With acidified potassium manganate (VII) solution

H H ǀ ǀ H–C=C–H +

-

H H ǀ ǀ H–C– C–H ǀ ǀ H OH Ethanol

potassium manganate (purple)

H H ǀ ǀ H–C– C–H ǀ ǀ OH OH ethan-1,2-diol

-

KMnO4 is an oxidising agent Purple color of potassium manganate turn colourless.

6.

Polymerisation

H H ǀ ǀ C=C ǀ ǀ H H

+

H H ǀ ǀ C=C ǀ ǀ H H

polymerisation

H ǀ C– ǀ H

H ǀ C– ǀ H

H H ǀ ǀ C–C ǀ ǀ H H n

ethene

5

ethene

polyethane

DIFFERENCES

6