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AH Chemistry > 1.4 Transition Metals > Flashcards

1.4 Transition Metals Flashcards

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1
Q

Transition metal

A

Metals with incomplete d sub shell in at least one of their ions (except Zn 2+)

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2
Q

Metals with incomplete d sub shell in at least one of their ions (except Zn 2+)

A

Transition metal

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3
Q

Properties of transition metals

A

Have atoms or ions with incomplete d sub shell (except Zn2+)

Can form complexes

Have variable oxidation states (numbers)

Show catalytic ability

Form coloured ions

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4
Q

When ions are formed from transition metals, what do they lose and from where

A

Electrons from the 4s orbitals

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5
Q

How to find oxidation number steps

A
  1. Write out molecule name
  2. Identify transition metal
  3. Add +1 if positive -1 if negative or 0 if no charge
  4. Multiply the number of atoms by the valency (+ if metal, - if non metal) for atoms that aren’t the transition metal
  5. Add the numbers together

6, the oxidation number is when the sun of numbers given + oxidation number = 0

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6
Q

Increase in oxidation number

A

Oxidation

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7
Q

Oxidation

A

Increase in oxidation number

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8
Q

Have atoms or ions with incomplete d sub shell (except Zn2+)

Can form complexes

Have variable oxidation states (numbers)

Show catalytic ability

Form coloured ions

A

Properties of transition metals

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8
Q

Decrease in oxidation number

A

Reduction

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9
Q

Reduction

A

Decrease in oxidation number

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10
Q

Oxidation number over +3

A

Oxidising agent

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11
Q

Oxidation number of oxidising agents

A

Over 3+

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12
Q

What does a complex consist of

A

A central metal ion surrounded by ligands

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13
Q

A central metal ion surrounded by ligands

A

A complex

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14
Q

Are ligands electron acceptors or donors

A

Donors

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15
Q

What bonds do ligands form

A

Dative covalent bonds

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16
Q

What are common ligands

A

Negative ions

Molecules with non bonding electrons

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17
Q

Negative ions

Molecules with non bonding electrons

A

Different forms of ligands

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18
Q

What can ligands be classified as

A

Monodente

Bidente

Quandridente

Hexadente

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19
Q

Monodente

Bidente

Quandridente

Hexadente

A

Classification of ligands

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20
Q

Monodente ligand

A

Donates one electron pair to a metal ion

(One dative covalent bond)

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21
Q

Donates one electron pair to a metal ion

(One dative covalent bond)

A

Monodente ligand

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22
Q

Bidente ligand

A

Donates 2 pairs of electrons to a metal ion

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23
Q

Donates 2 pairs of electrons to a metal ion

A

Bidente ligand

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24
Q

Donates 4 pairs of electrons to a metal ion

A

Quadridente ligand

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25
Q

Quadridente ligand

A

Donates 4 pairs of electrons to a metal ion

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26
Q

Hexadente ligand

A

Donates 6 pairs of electrons to a metal ion

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27
Q

Donates 6 pairs of electrons to a metal ion

A

Hexadente

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28
Q

Co ordination number

A

The total number of bonds from the ligands to the central metal ion

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29
Q

The total number of bonds from the ligands to the central metal ion

A

Co ordination number

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30
Q

Chromium name in a complex

A

Chromate

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31
Q

magnanese name in a complex

A

Manganate

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32
Q

iron name in a complex

A

Ferrate

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33
Q

cobalt name in a complex

A

Colbaltate

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34
Q

mickel name in a complex

A

Nickelate

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35
Q

copper name in a complex

A

Cupprate

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36
Q

tin name in a complex

A

Stannate

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37
Q

lead name in a complex

A

Plumbate

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38
Q

Plumbate

A

lead name in a complex

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39
Q

Stannate

A

Tin name in complex

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40
Q

Cupprate

A

copper name in a complex

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41
Q

Ferrate

A

Iron name in a complex

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42
Q

Chloride name in a complex

A

Chlorido

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43
Q

Oxide name in a complex

A

Oxido

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44
Q

cyanide name in a complex

A

Cyanido

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45
Q

oxalate name in a complex

A

Oxalato

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46
Q

iodine name in a complex

A

Iodido

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47
Q

Hydroxide name in a complex

A

Hydroxido

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48
Q

Ammonia name in a complex

A

Ammine

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49
Q

Water name in a complex

A

Aqua

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50
Q

Carbon monoxide name in a complex

A

Carbonyl

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51
Q

Flouride name in a complex

A

Fluorido

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52
Q

How do you order the ligands in a complex

A

Alphabetically

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53
Q

Naming complexes with no charge steps

A

Name the positive ion

Name the number of bonds

Name the ligand (bracketed)

Name the cation followed by its oxidation number

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54
Q

If the ion is negative, what do you do when naming the complex

A

Add the word “ate” on the end

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55
Q

If the ion is positive, what do you do when naming the complex

A

Leave the metal as it is

56
Q

Why are transition metals often coloured

A

Because they absorb light in certain parts of the visible spectrum

And the colour seen is the complementary one

57
Q

What are 5d orbitals when the transition metal is non bonded

A

All degenerate

57
Q

What does degenerate mean

A

Of equal energy

58
Q

What happens when ligands approach a molecule with lone pair

A

The lone pair repels the d orbitals

The d sub shell is split into 2 distinct sets of orbitals with a difference in energy between them.

59
Q

When does a lone pair repel the d orbitals

The d sub shell is split into 2 distinct sets of orbitals with a difference in energy between them.

A

When ligands approach the 5d orbitals

59
Q

What does the size of the energy gap vary with

A

The transition metal ion

Oxidation state (number)

Type of ligands

59
Q

Size of energy gap aka

A

Crystal field strength

60
Q

Crystal field strength aka

A

Size of the energy gap

61
Q

What happens when light enters in the visible region of the spectrum

A

Electrons raised from a lower energy level to a higher energy level

62
Q

What means that electron will be raised from a lower to higher energy level

A

Entry of light on the visible region of the spectrum

63
Q

What determines the colour produced by the compound or complex

A

The size of the split

64
Q

What does the size of the split determine

A

The colour produced by the compound or complex

65
Q

The _____ the energy of light absorbed, the shorter the wavelength

A

Greater

66
Q

The greater the ________, the shorter the wavelength

A

Energy of light absorbed

67
Q

The greater the energy of light absorbed, the ______ the wavelength

A

Shorter

68
Q

The greater the energy of light absorbed, the shorter the _________

A

Wavelength

69
Q

As splitting increases, the light absorbed moves away from …..

A

Red

70
Q

If a sample absorbs a light, it will emit what colour

A

A colour opposite on the colour wheel

71
Q

What determines the concentration of transition metals in solution

A

The absorbante of visible or UV light

72
Q

The _______, the greater the absorbance of light

A

Higher the concentration of ions

73
Q

The higher the concentration of ions, _______

A

the greater the absorbance of light

74
Q

What is used to study the effects of d to d transitions

A

A UV / Vis spectrometer

75
Q

What can be used to study the effects of d to d transitions

A

A UV / Vis spectrometer

76
Q

What does a UV / vis spectrometer do

A

Measures the intensity of radiation transmitted through the sample and compares this with the intensity of incident radiation

77
Q

Measures the intensity of radiation transmitted through the sample and compares this with the intensity of incident radiation

A

Uv / vis spectrometer

78
Q

What colour is a compound that absorbs energy in the UV part of ur EM spectrum

A

Colourless

79
Q

What compounds are colourless

A

Those that absorb in the UV part of the EM spectrum

80
Q

What is used for colourless compounds

A

A ultraviolet spectrometer

81
Q

What is a UV spectrometer used on

A

Colourless compounds

82
Q

Transition metals and their compounds at important as what

A

Catalysts

83
Q

What are important catalysts

A

Transition metals

84
Q

What are transition metals and their compounds important in as catalysts

A

Industrial and biological reactions

85
Q

Haber process metal

A

Fe

86
Q

Enzymes metal

A

Zn

87
Q

Ostwald metal

A

Pt

88
Q

Hydrogenation metal

A

Ni

89
Q

Catalysts

A

Speed up the rate of reaction by providing an alternative pathway of lower activation energy

90
Q

Speed up the rate of reaction by providing an alternative pathway of lower activation energy

A

Catalysts

91
Q

Homogenous catalysts

A

In the same state as the reactants

92
Q

In the same state as the reactants

A

Homogenous catalysts

93
Q

Heterogeneous catalysts

A

In a different state as the reactants

94
Q

In a different state as the reactants

A

Heterogeneous catalysts

95
Q

What catalysts are used in most industrial processes

A

Heterogeneous catalysts

96
Q

How many bonds can transition metals form

A

A variable number of bonds

97
Q

How can transitional metals form a variable number of bonds

A

As they have unoccupied or partially occupied d orbitals

98
Q

Transition metals and reactants

A

Reactant molecules are absorbed onto the active sites and are weakened and held in a more favourable conformation for the reaction

They form an intermediate complex before forming the product

99
Q

What does transition metals having varying oxidation states enable them to do

A

They can act as homogenous catalysts

100
Q

What means that transition metals can be homogenous catalysts

A

Varying oxidation numbers

101
Q

Transition metals at the end of a reaction it catalysed

A

Returns to its original oxidation state

102
Q

oxidation number of an uncombined element

A

0

103
Q

oxidation number of monatomic ions

A

same as the charge on the ion

104
Q

oxygen oxidation number

A

-2

105
Q

hydrogen oxidation number

A

usually +1

in metal hydrides, -1

106
Q

metallic hydrides

A

one or more metal ions

and

one or more hydrogen ions

107
Q

sum of all oxidation numbers of all atoms in a molecule or neutral compound

A

0

108
Q

the sum of all the oxidation numbers of all the atoms in a polyatomic ion

A

the charge on the ion

109
Q

ct

A
110
Q

transition metal complex

A

central transition metal ion

many organic molecules attached to the transition metal centre by dative bonds (ligands)

111
Q

central transition metal ion

many organic molecules attached to the transition metal centre by dative bonds (ligands)

A

transition metal complex

112
Q

what allows neutral compounds to be ligands, like water and ammonia

A

they have lone pairs available to donate to form dative bonds

113
Q

dentate meaning

A

teeth

number of attachment points onto metal ion

number of dative bonds formed with central transition metal ion

114
Q

how to construct formula of TM complexes with ligands

A
  1. state TM
  2. state ligand in round brackets and denote how many there are outside of the bracket
  3. put that formula in square brackets
  4. add charge outside square brackets

calculate charge:

charge of TM ion + charge of ligands

115
Q

rules for writing complexes

A

symbol of the metal is written first

this is follow by the symbols of the ligands

ligands are written in alphabetical order according to which atom of the ligand binds.

eg, water is written as OH2

formula of complex ion is enclosed in square brackets with charge outside

116
Q

rules for naming complex ions

A

ligands are named in alphabetical order

ligands are followed by the name of the metal and its oxidation state

if there is more than one of a ligand, the name of the ligand is preceded by the prefix for the no., eg di, tri, tetra

if the ligand is a negative ion ending in -ide, the ligands name charges to end in ‘o’. chloride -> chlorido

ammonia=ammine
water=aqua

if the complex is a negative ion, the name of the complex ends in -ate

copper=cupprate
ion=ferrate

if the complex is a salt, the name of the positive ion precedes the name of thr negative ion

117
Q

charge on water

A

nothing

118
Q

is the positive or negative written first in a complex ion

A

positive

119
Q

charge on cyanide ion

A

1-

120
Q

when can a transition metal be colourless

A

d orbtials are completely full as there is no where for the electrons to be promoted to

or completely empty as there is no electrons to promote

121
Q

d orbtials are completely full as there is no where for the electrons to be promoted to

or completely empty as there is no electrons to promote

A

transition metal is colourless

122
Q

what can change the gap in energy between d orbitals

A

ligands

123
Q

strong field ligands create a _________

A

large split in d orbitals

124
Q

_______ create a large split in d orbitals

A

strong field ligands

125
Q

why are TMs good catalysts

A

the empty d orbitals are thought to provide sites where you can form activated complexes

126
Q

what does the empty d orbitals are thought to provide sites where you can form activated complexes mean for TMs

A

good catalysts

127
Q

VSEPR

A

valence
shell
electron
pair
repulsion

128
Q

electron pairs ____ eachother

A

repel

129
Q

How are different colours formed

A

Ligands split the degenerate d orbitals into orbitals of different energies

The difference in energy corresponds to light in three visible religion of the spectrum

130
Q

How do ligands cause different colours

A

They cause differing degrees of splitting

131
Q

Why peaks are at shorter wavelengths for one ligand

A

Ligand results in greater ligand field splitting

This means that more energy is needed to promote the electron

Therefore the wavelength absorbed is less

132
Q

Colour of ion with complete d shell

A

Colourless

133
Q

Colour of ion with complete d shell

A

Colourless

134
Q

how do heterogeneous catalysts work

A

absorption into active sites

AH Chemistry (8 decks)

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