Inorganic Chemistry

Question 1

Electromagnetic spectrum: order

Answer 1

RMIVUXG

Question 2

Electromagnetic radiation in order of wavelength

Answer 2

GXUVIMR

Question 3

Electromagnetic spectrum: names

Answer 3

Radio, Microwave, Infrared, UV, X-Ray, Gamma

Question 4

Finding energy using wavelength

Answer 4

Energy is in kj. So wavelength (nm) is x10 to power of -9. Answer x10 to power of -3 (milli to 1)

Question 5

how are lines on a spectrum formed?

Answer 5

An electron is promoted to a higher energy level. When the excited electron drops back to a lower level, energy is given off to a corresponding wavelength. DO NOT MENTION ABSORBING LIGHT.

Question 6

absorption spectroscopy

Answer 6

electromagnetic radiation is directed at an atomised sample. radiation is absorbed as electrons are promoted to higher energy levels

Question 7

emission spectroscopy

Answer 7

high temperatures are used to excite electrons, making them drop to lower energy levels, emitting a photon as they do so

Question 8

atomic spectroscopy: conc. of an element

Answer 8

concentration of an element is related to the intensity of light emitted or absorbed

Question 9

number of electrons found in an orbital

Answer 9

max of 2

Question 10

n

Answer 10

principal quantum number, main energy level for an electron

Question 11

shapes of orbitals

Answer 11

s, p, d, f

Question 12

l

Answer 12

angular momentum quantum number. shape of subshell (s, p, d)

Question 13

ml

Answer 13

orientation of the orbital. -l to +l values

Question 14

ms

Answer 14

direction of spin. +1/2 of -1/2

Question 15

the aufbau principle

Answer 15

electrons fill orbitals in order of increasing energy

Question 16

hund’s rule

Answer 16

electrons fill degenerate orbitals singly and with parallel spins before pairing occurs

Question 17

the pauli exclusion principle

Answer 17

no two electrons in one atom have the same set of four quantum numbers. therefore, no orbital can hold more than two electrons and those electrons must have parallel spins

Question 18

division of periodic table into s, p, d, f

Answer 18

corresponds to the outer electronic configurations of the elements within these blocks

Question 19

special stability

Answer 19

associated with half-filled and full subshells

Question 20

stability and ionisation energy

Answer 20

the more stable the electronic configuration, the higher the ionisation energy

Question 21

VSEPR

Answer 21

valence shell electron pair repulsion theory: used to predict the shapes of molecules and polyatomic ions. electron pairs are negatively charged so repel each other, therefore they are arranged to minimise repulsion and maximise separation

Question 22

electron pair repulsion strength

Answer 22

decrease in order of: non-bonding pair/ non-bonding pair> non-bonding pair/ bonding pair> bonding pair/ bonding pair

Question 23

transition metal

Answer 23

metals with an incomplete d subshell in at least one of their ions

Question 24

copper and chromium

Answer 24

have a complete d subshell due to the special stability associated with having the d subshell being half-filled or completely filled

Question 25

transition metals becoming ions

Answer 25

the 4s electrons are lost before the 3d electrons

Question 26

oxidation state

Answer 26

is the oxidation number

Question 27

oxidation number

Answer 27

the sum of all the oxidation numbers of all the atoms in a neutral compound must add up to zero. the sum of all the oxidation numbers of all the atoms in a polyatomic ion must be equal to the charge on the ion

Question 28

oxidation

Answer 28

increase in oxidation number

Question 29

reduction

Answer 29

decrease in oxidation number

Question 30

oxidising agents

Answer 30

compounds containing metals in high oxidation states

Question 31

reducing agents

Answer 31

compounds with metals in low oxidation states

Question 32

ligands

Answer 32

negative ions or molecules with non-bonding pairs of electrons that they donate to the central metal atom or ion, forming dative covalent bonds

Question 33

ligand classification

Answer 33

monodentate up to hexadentate

Question 34

coordination number

Answer 34

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

Question 35

complex of a transition metal

Answer 35

d orbitals no longer degenerate

Question 36

splitting of d orbitals

Answer 36

splitting to higher and lower energies occurs when the electrons present in approaching ligands cause the electrons in the orbitals lying along the axes to be repelled

Question 37

strong field ligands

Answer 37

create a large difference in energy between subsets of d orbitals

Question 38

weak field ligands

Answer 38

create a small energy difference between subsets of d orbitals

Question 39

colours of transition metals

Answer 39

explained in terms of d-d transitions. light is absorbed when electrons in a lower energy d orbital are promoted to a d orbital of higher energy

Question 40

heterogeneous catalysis

Answer 40

presence of unpaired d electrons or unfilled d orbitals allows activated complexes to form as reactive molecules are adsorbed, providing a reaction pathway with a lower activation energy. therefore, transition metals are often catalysts

Question 41

homogeneous catalysis

Answer 41

changing oxidation states with the formation of intermediate complexes

Question 42

Ionic bonds

Answer 42

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

Question 43

Minimising electron repulsion

Answer 43

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

Question 44

Bonding pairs

Answer 44

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

Question 45

Octahedral

Answer 45

6 pairs. 90

Question 46

Trigonal bipyramidal

Answer 46

5 pairs. Down 90, across 120

Question 47

Tetrahedral

Answer 47

4 pairs. 109.5

Question 48

Trigonal planar

Answer 48

3 pairs. 120

Question 49

Linear

Answer 49

2 electron pairs. 180

Question 50

Number of electron pairs, formula

Answer 50

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

Question 51

Resonance structure

Answer 51

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

Question 52

Dative covalent bond

Answer 52

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

Question 53

Orbital boxes

Answer 53

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

Question 54

Oxidation number

Answer 54

How many electrons have been lost

Question 55

Coordination compound

Answer 55

Cation/ anion can’t exist on their own so must have charges balanced. The complex ion will bond with oppositely charged ions to form a complex