Section A

Question 1

HSAB - Hard Soft Acid Base Theory

Answer 1

Hard acids prefer to bind to hard bases

Soft acids prefer to bind with soft bases

Question 2

Factors that affect Hardness

Answer 2

Hard Acids - H+
Small + High Charge

Soft Acids - Cu+
Large + Small or neutral charge

Hard Base - F- , OH-
High Electronegativity

Soft Base - CN- ,I-
Low electronegativity

Question 3

No. of e- at the central atom

Answer 3

No. of Valence e- at central Atom +

1 e- for each single Bond -

Overall charge on the compound

Question 4

Finding the number of electron pairs

Answer 4

                     2

Question 5

VSEPR

Total No. of e-

Answer 5

No. of Valence e- +

1 e- per single Bond -

Overall charge

Question 6

VSEPR

No. of e- Pairs

Answer 6

                     2

Question 7

Layout for VSEPR

Answer 7

Compound

Val e- =
Bonds =
Charge =

Total e- =
No e- pairs =

Describe the bond angle and how many pairs you have.

Name of the shape of molecule

Question 8

Name the Shape of molecules

Answer 8

Linear

Trigonal Planar **Careful of orientation ** think of example = ClF 3
(lp and bp)

T- Shaped ##

Tetrahedral

Trigonal Bipyramidal

Octahedral

Seahorse shape* ask if we need this*

Square Based Pyramid *

Triangle Based Pyramid *

Square Planar *

Question 9

Name the Shape of molecules

Answer 9

Linear

Trigonal Planar **Careful of orientation ** think of example = ClF 3
(lp and bp)

T- Shaped ##

Tetrahedral

Pyramidal

Trigonal Bipyramidal

Octahedral

Seahorse shape* ask if we need this*

Square Based Pyramid *

Triangle Based Pyramid *

Square Planar *

Question 10

d - orbitals

Answer 10

Draw

Question 11

Table P15

n - principle quantum number
l - orbital angular quantum number
ml - magnetic quantum number
n^2 - number of orbitals

Answer 11

Scan

Question 12

Rule - 1

Aufbau Principle

Answer 12

Electrons are placed in the lowest available orbital first in sequence

Question 13

Rule - 2

Pauli Exclusion Principle

Answer 13

No two electrons can have the same set of four quantum numbers meaning only two electrons can occupy an orbital with opposite spins

n, l, ml and ms

Question 14

Rule - 3
####extra practice ###
Hunds first Rule

Answer 14

Degenerate orbitals are filled singly for as long as possible with parallel spins

Orbitals of the same energy = Looks exactly the same

They have the same “ms” Value for as long as possible

Question 15

Rule - 3
####extra practice ###
Hunds first Rule

Answer 15

Degenerate orbitals are filled singly for as long as possible with parallel spins

Orbitals of the same energy = Looks exactly the same

They have the same “ms” Value for as long as possible

Question 16

Extra Hunds first rule

Explaation

Answer 16

1. Spin pairing energy
   It takes energy to put 2 electrons into the same orbital
2. Spin exchange energy
   is energy gained when two or more electrons can exchange positions with no change in electron configuration.

100kJ/mol

Spin exchange favours Filled anf half filled shells as you get the maximum possible spin exchanges.

Question 17

Extra Hunds first rule

Explaation

Answer 17

1. Spin pairing energy
   It takes energy to put 2 electrons into the same orbital
2. Spin exchange energy
   is energy gained when two or more electrons can exchange positions with no change in electron configuration.

100kJ/mol

Spin exchange favours Filled anf half filled shells as you get the maximum possible spin exchanges.

Question 18

Electronegativity

Trend and how to work out

Answer 18

Top right = Biggest
Bottom left = Smallest

E > 1.7 (Ionic)
E

Question 19

Electronegativity

def

Answer 19

The ability of an atom to attract a pair of shared electrons in a covalent bond.