Fuels and heats of reaction

- Intramolecular bonding =

bonding that occurs within a molecule.

- Intramolecular bonding 3 types:

1. Non-polar covalent bonding

2. Polar covalent bonding

3. Ionic bonding

Non-polar covalent =

The equal sharing of electrons in a bond.

Non-polar covalent = The equal sharing of electrons in a bond.

Because ?

electrons are constantly moving in bonds and they are being shared equally, this results in temporary dipoles being formed.

Polar covalent: = ?

The unequal sharing of electrons in a bond.

Polar covalent: = The unequal sharing of electrons in a bond.

i.e. ?

The pair of electrons is closer to one atom in a bond at any one time. This results in the formation of permanent dipoles.

Dipole =

a partial charge

Ionic bonding =

The force of attraction between two oppositely charged ions.

To determine if a molecule is one of the three

(1. Non-polar covalent bonding

2. Polar covalent bonding

3. Ionic bonding),

we use the ?

electronegativity values.

non polar covalent electronegativity values

<0.4

Polar covalent electronegativity values

0.4 - 1.7

Ionic electronegativity values

>1.7

using electronegativity values

- This has a ?

big affect on solubility.

using electronegativity values

- Water is ? so only ? can ? in it.

polar

polar substances

dissolve

using electronegativity values

- Like substances can only dissolve in

like substances.

- Intermolecular bonding =

bonding that occurs between molecules.

3 types of intermolecular forces

1. Van Der Waals forces (weakest)

2. Dipole - dipole bonding

3. Hydrogen bonding (strongest)

What is the weakest intermolecular force?

Van der Waals

What is the strongest intermolecular force?

hydrogen bonding

Intermolecular forces between molecules are determined by ?

the intramolecular bonding.

- Van Der Waals: forces can only occur ?.

between temporary dipoles

- Dipole-dipole: bonding requires ?

permanent dipoles to form.

- Hydrogen bonding: requires

hydrogen to bond to one of the three (N, O, F)

It can only ever be intermolecular bonding between ?,

positive and negative dipoles

Opposite charges attract

like charges repel

- Intermolecular bonding determines

how strong particular organic molecules are.

- Strength is determined by the ?

boiling point.

- oxidation and reduction agents these ? agents are capable of ?

redox

converting more organic molecule to another.

- The best reduction agent is ?

H2 with a nickel catalyst.

- The best oxidation agent is either ? or ?

acidified potassium permanganate (MnO₄-/H+)

sodium dichromate (Cr₂O₇-).

Organic chemistry=

the study of compounds of carbon

Hydrocarbon=

a compound that contains only carbon hydrogen

Three classes of hydrocarbons=

alkanes alkenes alkynes

the three classes differ because of the presence of

single double or triple bonds

The alkanes:

? compounds due to them only containing ?

saturated

carbon-carbon single bonds

The alkanes:

endings all contain ?

ane

The alkanes:

the first ten alkanes each differ by

one CH₂

Methane

CH₄

ethane

C₂H₆

propane

C₃H₈

Butane

C₄H₁₀

pentane

C₅H₁₂

hexane

C₆H₁₄

Heptane

C₇H₁₆

Octane

C₈H₁₈

Nonane

C₉H₂₀

Decane

C₁₀H₂₂

Alkanes all have ? but there is a ? for every additional ?

similar properties

slight change

CH₂ unit

alkanes feature ? forces

vander waals

ALKANES:

the larger the molecule ?

the greater the strength

ALKANES:

the larger the molecule the greater the strength

this increasing strength between bonds is why alkanes go from ? to ? with ?

gases

liquids

increasing molecule size

Homologous series -

A series of compounds of similar chemical properties that show gradations in physical properties and have a general formula for its members with each member differing from the previous member by a CH₂ unit

IUPAC

International Union of pure and applied chemistry

IUPAC provide the rules for

the naming of organic compounds

ethane C2H6 equals

C-C

and

6 H's

Alkyl groups 3 types

methyl - CH₃

Ethyl - C₂H₅

Propyl - C₃H₂

Alkyl groups are

side chains "substituents"

Nomenclature rules 1.

number the longest continuous chain of carbons

ensure that the alkyl groups have the lowest number possible

Nomenclature rules 2.

write down the name of the chain

Nomenclature rules 3.

now include the positions and names of the alkyl groups

di

2 alkyl groups

cyclohexane shape

diamond

Structural isomers

compounds with the same molecular formula but different structural formulas

isomers

the molecular formulas are the same but their structured formulas are different

isomer of C4H10

butane and 2-methylpropane

carbon always has

four bonds

hydrogen always has

one bond

The alkenes:

? compound due to containing ?

Unsaturated

at least one double bond

The alkenes:

Ending –

ene

The alkenes:

because there is a ? bond between ? there is no such thing as a ? for example ? cannot exist

double

carbon atoms

single carbon alkene molecule

methene

The alkenes:

have a ? bond

double

The alkenes:

each carbon atom still has ?

4 bonds

The alkenes:

ethene C2H4 used as ?

solvents,ripens fruits, plant growth regulator

The alkenes:

there only has to be ? present for it to be classed as an alkene

one carbon - carbon double bond

The alkenes:

banana bags have tiny holes to allow ?

ethene gas in and out

The alkenes:

more ? than alkanes due to ?

reactive

high electron density among double bonds

The alkenes:

boiling points increase with size due to ?

follow a similar trend for boiling points as ?

vander waals forces

alkanes

Naming of Alkenes

Same procedure as naming alkanes

But you have to include the ?

double bond

Naming of Alkenes

1.?

Double bond = ?

no. carbon atoms

lowest no.