Bonding

Question 1

Describe the bonding in metallic bonding
(define, structure, conductivity etc)

Answer 1

• electrostatic attraction between positive metal ions and delocalised electrons
• giant metallic lattice
• conductive as delocalised e- free to move
• malleable, ductile, as layers of ions can slide over eachother

Question 2

Describe the bonding in ionic bonding
(define, structure, conductivity etc)

Answer 2

• electrostatic attraction between oppositely charged ions
• giant ionic lattice
• when solid not conductive, molten conductive

Question 3

Describe the bonding in covalent (simple) bonding
(define, structure, conductivity etc)

Answer 3

• shared pair of e-
• IMF forces
• not conductive no delocalised e-

Question 4

Describe the bonding in covalent (macromolecular) bonding
(define, structure, conductivity etc)

Answer 4

• covalent bonds
• not conductive, except graphite/graphene which has delocalised e-

Question 5

describe cooridinate bonding

Answer 5

• A coordinate bond is a covalent bond where both electrons in the shared pair have come from
  the same atom
• represented by an arrow

Question 6

Define electronegativity

Answer 6

• The ability of an atom to attract electron density in a covalent bond

Question 7

Non-polar covalent bonds exist between:

Answer 7

• Atoms with the same electronegativity
• Examples: H-H, C-H, Br-Br

Question 8

Polar covalent bonds exist between:

Answer 8

• Atoms with the different electronegativities
• Examples: C-F, C=O, N-H

Question 9

Strength of Induced Dipole-Dipole Intermolecular Attractions are affected by

Answer 9

• Number of electrons in molecule. More electrons = stronger induced dipole-dipole attractions
• Shape of molecule. Straight-chain alkanes have more surface contact between their molecules than branched chain alkanes. Therefore, straight-chain alkanes have stronger induced dipole-dipole intermolecular attractions`

Question 10

Explain how Induced Dipole-Dipole Intermolecular Attractions Occur

Answer 10

• Random movement of electrons in one molecule results in an
• Uneven distribution of electrons, which creates a
• Temporary dipole in one molecule.
• Induces an dipole in a neighbouring molecule
• Dipoles attract

Question 11

This question is about pentan-2-ol and pent-1-ene.
(a) The boiling point of pentan-2-ol is 119 °C
The boiling point of pent-1-ene is 30 °C
Explain why pentan-2-ol has a higher boiling point than pent-1-ene.