Organic Chemistry

Question 1

What is a 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

What is 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

Define first ionisation energy

Answer 4

the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+.

Question 5

Factors that effect first ionisation energy

Answer 5

Atomic radius-the half distance from the nucleus to the outermost electron
Nuclear charge- the number of protons in the nucleus which attract the outer electrons more
Shielding- the inner electron shells repel the outer electron shells. The more the inner shells increase the weaker the attraction between the nucleus and the furthermost electron decreases

Question 6

What are orbitals?

Answer 6

regions of space that electrons are likely to occupy and inhabit. They have the notations s,p,d,f.

Question 7

What is the periodicity for ionic radii in metals?

Answer 7

The size of the ions are smaller than the atom in the beginning as they lose valence electrons but they don’t lose entire shells. The nuclear charge becomes stronger and pulls in the electrons

Question 8

What is the periodicity for ionic radii in non metals?

Answer 8

The size of the ions are bigger than the atom in the beginning as they gain more electrons in an attempt to gain a noble gas configuration. New shells are not formed but unpaired electrons in orbitals are now being filled. The repulsion effect is increased between shells increasing the overall atomic radius

Question 9

What is the order of method of mass spectrometry?

Answer 9

1.Vaporisation
2.Ionisation
3.Acceleration
4.Deflection
5.Detection

Question 10

Define Relative Atomic Mass

Answer 10

The average mass of an atom of an element compared to 1/12 of the mass of a carbon-12 isotope

Question 11

Define Relative Isotopic Mass

Answer 11

the mass of one atom of an isotope relative to 1/12th of the mass of an atom of the isotope carbon-12

Question 12

Lone pairs

Answer 12

a pair of valence electrons that are not shared with another atom in a covalent bond

Question 13

Dative covalent bond

Answer 13

a covalent bond between 2 atoms where one of the atoms provides both electrons that form the bond

Question 14

Order of the pairs that cause the biggest bond angle reduction

Answer 14

Lone pair-lone pair>lone pair-bonding pair>bonding pair- bonding pair

Question 15

What is the electron pair repulsion theory?

Answer 15

The shape of a molecule is determined by the number of electron pairs (only valance shell) surrounding the central atom. This is because the pairs of electrons repel all the other electron pairs. The electron pairs more away from each other to achieve the maximum separation and minimum separation

Question 16

Electronegativity

Answer 16

the ability of an atom to attract the bonding electrons towards oneself in a covalent bond

Question 17

Explain the periodicity of electronegativity across periods

Answer 17

The electronegativity increases across periods due the shielding affect being constant and the overall nuclear charge of the nucleus attracting in the electron pair

Question 18

Explain the periodicity of electronegativity down a group

Answer 18

The electronegativity decreases down a group as the number of electron shells increases which increases repulsion between orbitals. This increases the atomic radius and weakening the attraction between the nucleus and outermost electron and making it easier for the other electron to attract the bonding pair

Question 19

Describe metallic bonding

Answer 19

this type of bonding is between metals where a sea of delocalised electrons flows within its structure and holds the lattice of metal cations from repelling each other as they have the same charge. this allows them to be very good conductors of electricity

Question 20

What does metallic bond strength depend on?

Answer 20

The number of outer electrons donated to the cloud and the size of the metal ion

Question 21

Explain the periodicity for boiling point in metals across periods?

Answer 21

The boiling point increases due to the number of electrons being donated by each metal cation to the electron cloud increasing. The increasing size of the metal ions is constant so the electron cloud becomes more effective in holding the metal cations together and stop them from repelling each other due to their same charge