Organic Chemistry

Question 1

Homologous series

Answer 1

families of organic compounds with the same functional group and same general formula.

Question 2

Order of priority

Answer 2

Carboxylic acids>aldehydes>ketones>alcohols>alkenes>halogenoalkanes

Question 3

Catalytic cracking

Answer 3

The breaking down of alkanes or larger molecules in order to produce smaller molecules to be used in different industries

Question 4

Free radical

Answer 4

an atom or group of atoms with an unpaired electron

Question 5

Nucleophile

Answer 5

A nucleophile is a species attracted to a region of positive charge and is an electron pair donor.

Question 6

Electrophile

Answer 6

An electrophile is a species attracted to a region of negative charge and is an electron pair acceptor

Question 7

Electrophilic addition

Answer 7

A type of reaction where an electrophilic species combines with another compound to form a product without losing any atoms present in the reactants.

Question 8

Free radical substitution

Answer 8

A type of reaction when hydrogen atoms on an alkane are substituted by a halogen atom

Question 9

Nucleophilic substitution

Answer 9

A type of reaction when a nucleophile replaces a halogen atom

Question 10

Primary

Answer 10

When a halogen or a foreign molecule is bonded to a carbon with 2 hydrogen atoms

Question 11

Secondary

Answer 11

When a halogen or a foreign molecule is bonded to a carbon with 1 hydrogen atom

Question 12

Tertiary

Answer 12

When a halogen or a foreign molecule is bonded to a cation with no hydrogen bonded to it

Question 13

Sigma bonds (Two eyes overlapping)

Answer 13

A type of covalent bond result from end to end overlapping of atomic orbitals. The electron density in a σ bond is symmetrical about a line joining the nuclei of the atoms forming the bond. The pair of electrons is found between the nuclei of the two atoms. The electrostatic attraction between the electrons and nuclei bonds the atoms to each other

Question 14

Pi bonds (Dumbbell)

Answer 14

A type of covalent bond resulting from the sideways overlap of adjacent p orbitals. The two lobes that make up the π bond lie above and below the plane of the σ bond. This maximizes overlap of the p orbitals. A single π bond is drawn as two electron clouds, one arising from each lobe of the p orbitals. The two clouds of electrons in a π bond represent one bond containing two electrons