3.2.5 Transition metals (A-level only) Flashcards

1
Q

Where do the d block elements sit on the periodic table?

A

In the middle of the periodic table

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2
Q

What is a transition metal

A

A d-block element that can form at least one stable ion with a partially filled d-subshell

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3
Q

What are two metals that are not transition metals?

A

Zinc and Scandium

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4
Q

Why is scandium not a transition metal? [2]:

A
  • Scandium only forms 1 stable ion of Sc³⁺

- It has an EMPTY d-subshell

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5
Q

Why is zinc not a transition metal? [2]:

A
  • It only forms one stable ion of Zn²⁺

- It has a FULL d-subshell

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6
Q

Properties of transition metals [4]:

A
  • Variable oxidation states
  • Partially full d-subshell
  • Coloured ions in solution
  • Good catalysts
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7
Q

Why do transition metals have variable oxidation states?

[2]:

A
  • electrons sit in 4s and 3d energy levels which are very close
  • so electrons are gained and lost using a similar amount of energy
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8
Q

What does Iron(II) look like as an aqueous ion?

A

Green solution

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9
Q

What does Copper(II) look like as an aqueous ion?

A

Blue solution

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10
Q

What does Iron(III) look like as an aqueous ion?

A

Purple solution but may look brown/yellow cus of [Fe(H₂O)₅(OH)]²⁺₍ₐᵩ₎

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11
Q

What is an example of a transition metal being a good catalyst? [2]:

A
  • Iron in the Haber process

- Nickel or Platinum in hydrogenation

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12
Q

What does Aluminium(III) look like as an aqueous ion?

A

Colourless solution

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13
Q

What does Iron(II) look like due to the action of NaOH?

A

green precipitate that goes brown on standing in air

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14
Q

What does Copper(II) look like due to the action of NaOH?

A

Blue precipitate

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15
Q

What does Iron(III) look like due to the action of NaOH?

A

Brown precipitate / may look orangey brown

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16
Q

What does Aluminium(III) look like due to the action of NaOH?

A

White Precipitate

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17
Q

What does Iron(II) look like due to the action an excess of NaOH(aq)?

A

No further change

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18
Q

What does Copper(II) look like due to the action an excess of NaOH(aq)?

A

No further change

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19
Q

What does Iron(III) look like due to the action an excess of NaOH(aq)?

A

No further change

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20
Q

What does Aluminium(III) look like due to the action an excess of NaOH(aq)?

A

Colourless solution

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21
Q

What does Iron(II) look like due to the action of NH3(aq)?

A

green ppt goes brown

on standing in air

22
Q

What does Copper(II) look like due to the action of NH3(aq)?

23
Q

What does Iron(III) look like due to the action of NH3(aq)?

A

No further change

24
Q

What does Aluminium(III) look like due to the action of NH3(aq)?

A

No further change

25
What does Iron(II) look like due to the action an excess of Na2CO3(aq)?
green ppt
26
What does Copper(II) look like due to the action an excess of Na2CO3(aq)?
blue-green ppt
27
What does Iron(IlI) look like due to the action an excess of Na2CO3(aq)? [3]:
- brown ppt - (ppt may look orange-brown) - and CO2 gas evolved
28
What does Aluminium(IlI) look like due to the action an excess of Na2CO3(aq)? [2]:
- white ppt | - CO2 gas evolved
29
Transition metal ions use...
vaccant, hybridised 4s, 4p, 4d orbitals to accept ligand coordinate bonds
30
Ligand [definition]:
A species with a lone pair
31
Coordinate bonds [explanation]:
Lone pair on ligand accepted by vacant orbitals
32
How many lone pairs do transition metal ions accept? [2]:
- 4 lone pairs/ ligands | - 6 lone pairs/ ligands
33
Monodentate =
1 lone pair per ligand so can only form one coordinate bond
34
Examples of monodentate ligands [4]:
- Water - NH3 - Cl- - CN-
35
Bidentate =
2 LPs per ligand so form 2 coordinate bonds
36
Example of bidentate logo =
H₂NCH₂CH₂NH₂
37
Multidentate =
Multiple lone pairs that can be used to make ligands/ multiple coordinate bonds per ligand
38
Example of multidentate ligand =
EDTA⁴⁻
39
What are the shapes of complex ions [4]:
- Octahedral - Tetrahedral - Square planar - Linear
40
Octahedral complex ions [3]:
- 6 coordinate bonds - 90° bond angle - Most common shape
41
What is the coordination number of an octahedral ion?
6
42
How do you work out the coordination number?
Count the no. of coordinate bonds
43
Tetrahedral complex ions [3]:
- 4 coordinate bonds - 109.5° bond angle - Seen when ligands are large and charged
44
Square planar complex ion [2]:
- 4 coordinate bonds | - 90° bond angle
45
What is the coordinate number for a tetrahedral ion?
4
46
What is an example of a square planar complex ion?
CISPLATIN
47
What is the coordination number of a square planar ion?
4
48
Linear complex ions [2]:
- 2 coordinate bonds | - 180° bond angle
49
What is the coordination number for a linear complex ion?
2
50
What is an example of a linear complex ion?
Tollen's reagent