1.3

Question 1

Orbital boxes

Answer 1

1s, 2s, 2p, 3s, 3p, 4s, 3d. 4s comes before 3d if it is an ion or transition metal

Question 2

Dative covalent bond

Answer 2

When one atom provides both of the electrons that form the covalent bond

Question 3

Resonance structure

Answer 3

More stable than normal structure. A double and single bond will flip around e.g. ozone

Question 4

VSEPR

Answer 4

Valence Shell Electron Pair Repulsion Theory. Outer electrons repel each other

Question 5

Strength of electron repulsions

Answer 5

(Decreasing in strength): non-bonding/non-bonding; non-bonding/bonding; bonding/bonding. This can cause distortions in the shapes of molecules

Question 6

Number of electron pairs, formula

Answer 6

Number of outer electrons on central atom + number of bonded atoms — charge. DIVIDE ALL THIS BY 2

Question 7

Linear

Answer 7

2 electron pairs. 180

Question 8

Trigonal planar

Answer 8

3 pairs. 120

Question 9

Tetrahedral

Answer 9

4 pairs. 109.5

Question 10

Trigonal bipyramidal

Answer 10

5 pairs. Down 90, across 120

Question 11

Octahedral

Answer 11

6 pairs. 90

Question 12

Bonding pairs

Answer 12

Shape is dependent on number of bonded electrons, so answer to formula may not always be right

Question 13

Minimising electron repulsion

Answer 13

Lone pairs of electrons are always positioned equatorially to minimise repulsion. The shape of the molecule is also supposed to minimise this

Question 14

Ionic bonds

Answer 14

Will form when atoms can rearrange their electrons to produce an arrangement of lower energy. Ionic lattices are more stable