Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Advanced Higher Chemistry > U1-3 - Transition Metals > Flashcards

U1-3 - Transition Metals Flashcards

1
Q

Which two transition metals are exceptions to the Aufbau principle?

A

Chromium, [Ar] 4s1 3d5

Copper, [Ar] 4s1 3d10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why do chromium and copper adopt 3d5 and 3d10 configurations?

A

Special stability associated with half-filled and full 3d subshell.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Which electrons are lost first when transition metals form ions?

A

4s electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why is valency 2 common in transition metals?

A

Loss of two 4s electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Oxidation state/number

A

Valency equivalent. Can include charge.

E.g. II, +2, 2 all the same.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Oxidation state of oxygen

A

–2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Oxidation state of halogens

A

–1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Oxidation state of group 1 metals

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How can you predict if an oxidation state is stable?

A

If its electronic configuration is stable, the oxidation state is also stable.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Oxidation can be defined as an ___________ in oxidation number.

A

increase

(e.g. +2 to +3)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Reduction can be considered as a ___________ in oxidation number.

A

decrease

(e.g. +2 to 0)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Compounds with metals in _______ oxidation states tend to be oxidising agents.

A

high

(e.g. +5)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Compounds with metals in high oxidation states tend to be __________ agents.

A

oxidising

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Compounds with metals in _____ oxidation states tend to be reducing agents.

A

low

(e.g. +2)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Compounds with metals in low oxidation states tend to be __________ agents.

A

reducing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Ligand

A

A negative ion or molecule with non-bonding
e− pairs that they donate to the central metal atom or ion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What type of bonds are formed between ligands and metals?

A

Dative (covalent)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Denticity

A

No. of e− pairs a ligand can donate to the central metal ion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Monodentate ligands donate _________.

A

1 e− pair​

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

List as many monodentate ligands as you can.

A

H2O, NH3, CN−, halide ions, nitrite (NO2−), OH−.

(In general, charge of 1− or has 1 atom with non-bonding pairs.)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Bidentate ligands donate _________.

A

2 e− pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Name two bidentate ligands.

A

oxalate and ethylenediamine (en)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Coordination number

A

The number of dative bonds formed between the ligands and the central metal ion.

24
Q

Higher coordination number = _______ stable complex.

A

more

25
Q

The number of dative bonds formed between the ligands and the central metal ion.

A

Coordination number

26
Q

If the coordination number is 6, the complex shape is ______.

A

octahedral

27
Q

Normally a Cl branch is called ‘chloro’.

What changes when naming Cl in a transition metal complex?

A

Ending is ‘ido’ = chlorido

Apply this to most negative ions, e.g. hydroxido, cyanido.

28
Q

Name of NH3 ligand in a TM complex

A

ammine

29
Q

Name of H2O ligand in a TM complex

A

aqua

30
Q

Why is water written as OH2 in complex formulae?

A

O is the atom bonded to metal so must be written first.

31
Q

In a complex name, does OH2 or Cl go first?

A

aqua, OH2 (alphabetical order)

32
Q

In a formula, does OH2 or NH3 go first?

A

NH3 (alphabetical order)

33
Q

Positive complex ion names end in ________.

A

the name of the metal, unchanged

(e.g. hexaamminecopper(II))

34
Q

Negative complex ion names end in ______.

A

-ate

(e.g. hexacyanidocobaltate(II))

35
Q

Negative complex ion containing iron will end in ____.

A

ferrate

36
Q

Negative complex ion containing copper will end in ____.

A

cuprate

37
Q

What is missing from this name?

hexacyanidoferrate

A

Oxidation state of iron

38
Q

In a free transition metal ion the d orbitals are ________.

A

degenerate

39
Q

Why are d orbitals split in TM complexes?

A

The e− present in approaching ligands cause the e− in the orbitals pointing at ligands to be repelled.

This repulsion increases the energies of these orbitals.

40
Q

What is delta (∆)?

A

Crystal field splitting energy

(energy gap between split d orbitals)

41
Q

How are split d orbitals filled?

A

Lower ones filled in first. After d6, the higher ones are filled.

42
Q

Electrons can be promoted from __________ energy d orbitals by absorbing light. This is called a d→d transition.

A

lower to higher

43
Q

Electrons can be promoted from lower to higher energy d orbitals by _________________. This is called a d→d transition.

A

absorbing light

44
Q

Electrons can be promoted from lower to higher energy d orbitals by absorbing light. This is called a _________________.

A

d→d transition

45
Q

What is the spectrochemical series?

A

List of ligands in order of their ability to split d orbitals.

46
Q

State a general principle to how the ligands are ordered.

A

Ligands containing N split the d orbitals the most.

Ligands containing O are in the middle.

Halides split the d orbitals the least.

47
Q

If a complex is colourless, it absorbs _________.

A

UV light

48
Q

Suggest two reasons a complex could be colourless (in terms of electrons/orbitals).

A

No d → d transitions possible (e.g. d10)

Crystal field splitting energy is large (wavelength absorbed in UV and not visible spectrum)

49
Q

The complex colour is ___________ to the colour absorbed (opposite on colour wheel).

A

complementary

50
Q

The complex colour is complementary to the colour absorbed (___________ on colour wheel).

A

opposite

51
Q

Homogenous catalyst

A

Catalyst in the same state as the reactants

52
Q

Heterogenous catalyst

A

Catalyst in a different state to the reactants

53
Q

Transition metals and their complexes can act as catalysts due to their ______________ and variable oxidation states.

A

incomplete d orbitals

54
Q

Transition metals and their complexes can act as catalysts due to their incomplete d orbitals and _______________.

A

variable oxidation states

55
Q

Catalyst in the same state as the reactants

A

Homogenous catalyst

56
Q

Catalyst in a different state to the reactants

A

Heterogenous catalyst

Advanced Higher Chemistry (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions