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Chemistry A-Level > Topic 15- Transition metals > Flashcards

Topic 15- Transition metals Flashcards

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1
Q

What colour is produced when copper ions react with HCL?

A

Yellow solution

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2
Q

What is meant by the coordination number?

A

number of dative bonds in a complex

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3
Q

What colour precipitate is Iron(II) Hydroxide?

A

Green precipitate

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4
Q

What is the colour of solution of Hexaquacobalt(II)

A

Pink solution

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5
Q

Colour of tetraaminediaquacopper(II)

A

Dark Blue solution

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6
Q

What colour precipitate is Iron(III) hydroxide

A

Brown precipitate

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7
Q

Colour of V2+

A

purple

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8
Q

Colour of V3+

A

green

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9
Q

Colour of VO 2+

A

blue

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10
Q

What is meant by a Ligand?

A

a species which uses lone pair of electrons to form a dative bond with a metal ion

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11
Q

3 steps of Catalytic converters

A

-adsorption of CO and NO molecules onto the surface of the catalyst
-weakening of bonds and chemical reaction
-desorption of CO2 and N2 product molecules from the surface of the catalyst

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12
Q

Properties of transition metals

A

Have variable oxidation states
Good catalysts
Form coloured ions in solutions

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13
Q

Why do transition metals have variable oxidation states?

A

The outer electrons sit in the 4s and 3d sub shells which are very close in energy levels

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14
Q

Why is Scandium not a transition metal?

A

Forms Sc3+ ion only has one stable ion
Has an empty d-subshell

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15
Q

Why is zinc not a transition metal?

A

The Zn2+ ion forms a full d-subshell

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16
Q

Examples of bidentate ligands

A

Ethanedioate (C2O4 2-)
Ethane-1,2-diamine (NH2CH2CH2NH2)

17
Q

Examples of multi dentate ligands

A

EDTA4- can form 6 bonds (coordination number of 6)

18
Q

Haemoglobin shape

A

Octahedral

19
Q

What can haemoglobin carry and replace the ligand with

A

Can replace H2O with O2 to form oxyhaemoglobin
Can also bond to carbon monoxide- harder to replace ligand because has a very strong bond

20
Q

Square planar examples

A

Cis-Platin and Trans-platin (90 degrees)

21
Q

When does the d-orbital split

A

When ligands begin to attach to the central metal ion

22
Q

Why do colours show

A

When white light is absorbed from electrons in the ground state they become excited and move further up to their excited state. Drop back down to ground level releasing visible light on electromagnetic spectrum

23
Q

What is colour dependent on?

A

The central metal ion
The type of ligand
The shape of the ligand

24
Q

What do redox potentials tell us about transition metals?

A

Tells us how easy a complex is reduced

25
Q

What is meant if a transition metal has a larger Ecell value?

A

It is unstable

26
Q

Why are zinc ions colourless?

A

They have a full d-subshell and therefore electrons cannot be promoted

27
Q

Equation for reaction between amphoteric chromium hydroxide with base (OH-)

A

Cr(H2O)3(OH)3 + 3OH- –> [Cr(OH)6]3+ +3H2O

28
Q

Equation for reaction between amphoteric chromium hydroxide and acid (H+)

A

Cr(H2O)3(OH)3 + 3H+ –> [Cr(H2O)6]3+ +3H2O

29
Q

Reaction between iodine and thiosulfate ions

A

2S2O3(2-) + I2 –> 2I- + S4O6(2-)

30
Q

what colour is the [Co(Η2Ο)6]2+ ion

A

pink solution

31
Q

what colour is the [CoCl4]2− ion

A

blue in solution

32
Q

How V2O5 acts as a catalyst in the contact process

A

V 2 O 5 is used as a catalyst to reduce the higher temperature requirements and it increases the rate of reaction as well

33
Q

colour of Cr2O7 2- (dichromate)

A

orange

34
Q

colour of CrO4 2- (chromate)

A

yellow

35
Q

colour of Cr3+

A

green

36
Q

colour of Cr2+

A

blue

37
Q

equilibrium reaction between chromate(VI) and dichromate(VI)

A

Cr2O7 2- + OH- <–> CrO4 2- + H+

38
Q

Addition of acid to reaction between dichromate and chromate equilibrium

A

Will shift to the left, produce more dichromate

39
Q

Addition of alkali to reaction between dichromate and chromate equilibrium

A

Will shift yo the right, produce more chromate ions

Chemistry A-Level (16 decks)

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