3.4 D block Flashcards

1
Q

Define D block element

A

have their outer most electron in a full or partly full d orbital

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2
Q

Define transition metal

A

have atoms or ions with a partly filled d d orbital

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3
Q

properties of transition metals

A
  • variable ox state
  • form coloured compounds
  • can react to form complex ions
  • act as catalysts
    VCCC
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4
Q

Discuss variable oxidation state

A

transition metals have partly filled d orbitals which easily loose or gain electrons (because they require small amounts of energy) which results in more than 1 ox state.

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5
Q

What is a catalyst and what are the two types?

A
  • substance which speeds up the rate of a reaction without being used up providing an alternative route lowering the activation energy.
  • homogenous- same phase as reactants
  • heterogenous- diff phase as reactants
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6
Q

example of catalyst:
1) heterogenous

A

iron (Fe) in haber process N2 + 3H2 -> 2NH3

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7
Q

example of catalyst:
2) heterogenous

A

nickel in hydrogenation of alkenes to alkanes

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8
Q

example of catalyst:
3) heterogenous

A

MnO2 in decomposition of h2o2

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9
Q

example of catalyst:
4) homogenous

A

V2o5 vanadium oxide in contact process
2s202 + o2 -> 2so3

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10
Q

modes of catalyst: heterogenous

A

reactants adsorb onto to surface of a transition metal which allows and increase in collisions between reactants and the products deadsorp from the surface of the metal

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11
Q

modes of catalyst: homogenous

A

work by transition metals changing ox state and allowing reaction to proceed with a lower ea

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12
Q

How do catalysts work?

A

a) cuz tm have partly filled d orbitals they can accept/ release extra electrons e.g mno4- to mn2+
b) also cuz they have partly filled d orbitals they have spaces to act as docking stations for gas reactants to bind to and are held long enough for a reaction to happen and pop off as a new product.

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13
Q

Define complex ion

A

when a tm ion binds using co-ordinate bonds to one or more ligands

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14
Q

structure of complex ion

A

[ Cu(H20)6 ] 2+
ligand- brackets inside of square brackets
central tm ion- Cu

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15
Q

Define ligand

A

a molecule or ion with a lone pair of electrons that form co-ordinate bonds with a tm ion which has a partially filled d orbital.

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16
Q

Define co-ordination number

A

number of ligands that bond to a central tm ion

17
Q

How are coloured complexes formed?

A
  • partially filled d orbitals arrange so that 3 are at lower energy than the other two
  • there will be energy available for an electron to be promoted from lower to higher energy level but in doing so energy adsorbed from white light and remaining wavelengths reflect to give colour .
18
Q

colour changes with:

A

metal ion
ox state of ion
ligand bonded