Definitions

Question 1

Electromagnetic spectrum

Answer 1

Different types of radiation arranged in order of wavelength

Question 2

Quanta

Answer 2

Fixed amounts of energy

Question 3

Principle quantum number

Answer 3

(n) - indicates the main energy level for an electron & is related to the size of the orbital

Question 4

Angular momentum quantum number

Answer 4

(l) - determines the shape of the sub shell (values from 0 to n-1)

Question 5

Magnetic quantum number

Answer 5

(ml) - determines the orientation of the orbital (values between -l and +l)

Question 6

Spin magnetic quantum number

Answer 6

(ms) - determines the direction of spin (either 1/2 or -1/2)

Question 7

Aufbau principle

Answer 7

electrons fill orbitals in order of increasing energy

Question 8

Hund’s rule

Answer 8

when degenerate orbitals are available, electrons fill singly, keeping their spins parallel before spin pairing

Question 9

Pauli exclusion principle

Answer 9

no two electrons in an atom can have the same set of 4 quantum numbers, so no orbital can hold more than 2 electrons (the 2 must have opposite spins)

Question 10

s block

Answer 10

group 1 & 2 and helium

Question 11

p block

Answer 11

group 3-8

Question 12

d block

Answer 12

transition metals

Question 13

f block

Answer 13

lanthanides & actinides

Question 14

Special stability

Answer 14

associated with half-filled and full subshells

Question 15

VSEPR

Answer 15

valence shell electron pair repulsion theory, used to predict the shapes of molecules and polyatomic ions

Question 16

linear arrangement

Answer 16

2 electron pairs

Question 17

trigonal planar

Answer 17

3 electron pairs

Question 18

tetrahedral

Answer 18

4 electron pairs

Question 19

trigonal bipyramidal

Answer 19

5 electron pairs

Question 20

octahedral

Answer 20

6 electron pairs

Question 21

Electron pair repulsion order

Answer 21

non-bonding pair/ non-bonding pair/ > non-bonding pair/ bonding pair > bonding pair/ bonding pair

Question 22

Oxidation

Answer 22

an increase in oxidation number

Question 23

Reduction

Answer 23

a decrease in oxidation number

Question 24

How to determine if an oxidation or reduction has occurred

Answer 24

changes in oxidation number of transition metal ions

Question 25

Oxidising agents

Answer 25

compounds containing metals in high oxidation states

Question 26

reducing agents

Answer 26

compounds containing metals in low oxidation states

Question 27

Ligands

Answer 27

negative ions/ molecules with non-bonding pairs of electrons they donate to the central metal atom/ion to form dative covalent bonds

Question 28

How can ligands be classified

Answer 28

monodentate, bidentate, up to hexadentate

Question 29

Coordination number

Answer 29

the total number of bonds from the ligand to the central transition metal

Question 30

Strong field ligands

Answer 30

ligands that cause a large difference in energy between subsets of d orbitals

Question 31

Weak field ligands

Answer 31

ligands that cause a small difference in energy between subsets of d orbitals

Question 32

When is a chemical reaction in equilibrium

Answer 32

when the composition of the reactants & products remains constant indefinitely

Question 33

Equilibrium constant (K)

Answer 33

characterises the equilibrium composition of the reaction micture

Question 34

orbitals in increasing energy

Answer 34

1s 2s 2p 3s 3p 4s 3d 4p 5s

Question 35

Ionisation energy

Answer 35

the energy required to remove one mole of electrons from one mole of gaseous atoms

Question 36

Oxygen oxidation number

Answer 36

-2

Question 37

Hydrogens oxidation number

Answer 37

+1

Question 38

Fluorines oxidation number

Answer 38

-1

Question 39

Dative bond

Answer 39

When a transition metal bonds with the lone pair of a molecule

Question 40

How a coordination number is determined

Answer 40

How many bonds the metal atom can form with the ligand