Transition Metals Flashcards

1
Q

Define Transition Metal

A

Metal atom with partially filled d subshell

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2
Q

What transition metals do we cover?
What is an exception that isn’t a transition metal?

A

Top row Sc-Zn
Zn exception 3d10 subshell for atoms & ions

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3
Q

How do transition metals form complexes?

A

Forms coordinate bond with ligand from e-s from ligand for dative bond

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4
Q

Define a Ligand

A

Particle with lone pair that forms a co-ordinate bond with metals

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5
Q

Define a Complex

A

Metal ion + ligand with a co-ordinate bond

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6
Q

Define co-ordination number

A

Number of co-ordinate bonds in a complex

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7
Q

Define a Lewis Base

A

Lone pair donor

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8
Q

Define a Lewis Acid

A

Lone pair acceptor

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9
Q

What shapes do 4 co-ordinate bonds make?

A

Tetrahedral mostly but sometimes square planar

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9
Q

What shape do 6 co-ordinate bonds make?

A

Octahedral

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10
Q

What shape do 2 co-ordinate bonds make

A

Linear

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11
Q

What type of ligand forms 2 co-ordinate bonds?

A

Bidentate ligands

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12
Q

How do transition metals form coloured ions?

A

They absorb different wavelengths of light

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13
Q

What does the colour of the transition metal ion depend on?

A
  1. The metal ion
  2. The Type of ligand attached
  3. The co-ordination number
  4. The oxidation state of the transition metal
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14
Q

What happens to transition metal d orbitals when ligands bond?

A

When ligands bond 5 d orbitals don’t have same energy
e- excited from lower d orbitals to higher d orbitals

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15
Q

How do coloured ions form?

A

Different energy of d orbitals is in the UV/Visible region -> d-d

16
Q

Outline the Planck equation with units

A

E diff between 2 d-d orbitals (J) = Planck’s constant (6.63x10-34 Jhz-1) X frequency (hz)
E diff = hf