Bonding

Question 1

Shape and bond angle of atom with 2 BP and 0 LP

Answer 1

Linear
180°

Question 2

Shape and bond angle of atom with 3 BP and 0 LP

Answer 2

Trigonal planar
120°

Question 3

Shape and bond angle of atom with 2 BP and 1 LP

Answer 3

Bent (V-shape)
118°

Question 4

Shape and bond angle of atom with 4 BP and 0 LP

Answer 4

Tetrahedral
109.5°

Question 5

Shape and bond angle of atom with 3 BP and 1 LP

Answer 5

Trigonal pyramidal
107°

Question 6

Shape and bond angle of atom with 2 BP and 2 LP

Answer 6

Bent (V-shape)
104.5°

Question 7

Shape and bond angle of atom with 5 BP and 0 LP

Answer 7

Trigonal bipyramidal
90° and 120°

Question 8

Shape and bond angle of atom with 4 BP and 1 LP

Answer 8

Trigonal pyramidal or see-saw
89° and 119°

Question 9

Shape and bond angle of atom with 3 BP and 2 LP

Answer 9

Trigonal planar or T-shape
120° or 89°

Question 10

Shape and bond angle of atom with 6 BP and 0 LP

Answer 10

Octahedral
90°

Question 11

Shape and bond angle of atom with 5 BP and 1 LP

Answer 11

Square pyramid
89°

Question 12

Shape and bond angle of atom with 4 BP and 2 LP

Answer 12

Square planar
90°

Question 13

Ionic bonding

Answer 13

electrostatic attraction between oppositely charged ions in a lattice

Question 14

Formulas of the following compound ions

sulfate, hydroxide, nitrate, carbonate and ammonium

Question 15

Define dative covalent bond

Answer 15

covalent bond formed by one atom donating its lone pair of electrons to another atom

Question 16

Metallic bonding

Answer 16

attraction between delocalised electrons and positive ions arranged in a lattice

Question 17

4 types of crystal structure

Answer 17

ionic
metallic
macromolecular (giant covalent)
molecular

Question 18

Why do pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible

Answer 18

To minimise repulsion

Question 19

Lone pair–lone pair repulsion is _____ than lone pair–bond pair repulsion, which is _____ than bond pair–bond pair repulsion

Answer 19

Greater
Greater

Question 20

Define electronegativity

Answer 20

power of an atom to attract the pair of electrons in a covalent bond

Question 21

Ionic crystal structure properties, using sodium chloride as an example

Answer 21

-strong electrostatic forces of attraction between oppositely charged ions in a giant lattice
-high melting point
-can conduct electricity when molten or aqueous, as not in lattice
-brittle, as like charges repel when layers of alternating charges are distorted
-breaks lattice into fragments

Question 22

Metallic crystal structure properties, using aluminium as an example

Answer 22

-strong electrostatic forces of attraction between positive nucleus and sea of delocalised electrons in a giant lattice
-hence high melting point
-malleable as layers can slide over each other
-good conductors as sea of delocalised electrons can carry a flow of charge

Question 23

Simple molecular crystal structure properties, using iodine as an example

Answer 23

-covalently bonded
-held together by weak Van der Waals between molecules
-low melting and boiling points
-poor conductors as no charged particles

Question 24

Macromolecular crystal structure properties, using diamond and graphite as examples

Answer 24

-rigid due to strength of giant lattice
-very high melting point as each atom has multiple covalent bonds
-sometimes has flat sheets which has delocalised electrons, hence can conduct electricity