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Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

Define a transition metal

A

Stable ions with partially filled d orbitals

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2
Q

What are the characteristics of transition metals?

A

They have no electrons in the 3d orbitals

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3
Q

Why are zinc and scandium not transition metals?

A

4s

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4
Q

Define ligands

A

They have many stable oxidation states

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5
Q

Define complex

A

Donates a lone pair of electrons to the central atom

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6
Q

What is a co-ordination number?

A

A central atom or ion surrounded with ligands

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7
Q

What is a monodentate ligand?

A

Number if co-ordinate bonds to the central atom/ion

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8
Q

State three examples of monodentate ligands

A
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9
Q

What are the similarities between NH3 and H2O?

A

Small ligands- H2O, NH3, OH-, CN-
Larger ligands- Cl-

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10
Q

Describe the change in co-ordination number and charge when H2O replaces NH3

A

No change

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11
Q

Why may a ligand substitution be incomplete?

A

Change in the co-ordination number

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12
Q

Give an example of a ligand larger than NH3 and H2O

A

Oxygen forms a co-ordinate bond to iron (II) in Haemoglobin, this enables oxygen to be transported in the blood

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13
Q

What changes when you replace H2O with Cl- ?

A

It replaces the oxygen co-ordinately bonded to Fe(II) in haemoglobin

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14
Q

Define bidentate ligand

A

Octahedral complexes that display cis-trans isomerism

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15
Q

State two examples of bidentate ligands

A

Electrons get excited by heat and radiation so some of the wavelengths of visible light are absorbed and the remaining are transmitted or reflected.

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16
Q

Define multidentate ligand

A

The d orbital electrons move from the ground state to an excited state when light is absorbed.

17
Q

Give an example of a multidentate ligand

A
18
Q

What is heam and example of?

A

Change in oxidation state.
Change in Co-ordination number
Change in ligand.

19
Q

What is one role of O2 in the blood?

A

Use of radiation to determine the structure/identity of a molecule.

20
Q

Define entropy

A

Measure of disorder that determines what reactions are feasible.

21
Q

State the chelate effect.

A

A large increase in disroder/entropy when a bidentate ligand subs out a mondentate ligand.

22
Q

What makes a reaction feasible?

A

When the products are less than the reactants therefore the reaction is more stable and entropically favourable.
This is an exothermic reaction.

23
Q

Explain what kind of reaction is never feasible.

A

When the reactants are greater than the products, there’s an increase of energy in the system (endothermic) but a decrease in disorder but these two can not occur at once, therefore it’s not feasible.

24
Q

State the role of a catalyst.

A

Speed up rate of chemical reactions- lowering the activation energy by providing an alternate pathway for molecules to travel though

25
Q

What is a heterogenous catalyst?

A

A catalyst that is in a different phase from the reactants and the reaction occurs at active sites on the surface.

26
Q

Give examples of two heterogeneous catalysts and what processes they are used in.

A

Fe in the Haber process
V2O5 in the Contact process.

27
Q

What causes reduced efficiency in heterogeneous catalysts?

A

They can become poisoned by impurities that block active sites

28
Q

Define a homogenous catalyst.

A

A catalyst that is in the same phase as the reactants.

29
Q

State the equation of the catalyst used in the Contact process

A
30
Q

State the equation of the catalyst used in the Haber process

A
31
Q

What is amphoteric character?

A

When a metal hydroxide dissolves in both acids and bases.

32
Q

How does V2O5 act as a catalyst in the contact process?

(Use equations)

A
33
Q

How do Fe ^2+ ions catalyse the reaction between I- and S2O8^2- ?

(Use equations)

A
34
Q

How do Mn^2+ ions autocatalyse the reaction between C2O4^2- and MnO4- ?

(Use equations)

A

Chemistry (34 decks)

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