Unit 1-Transition Metals Flashcards

1
Q

Why are transition metals known as d block elements?

A

The d block transition metals are metals with an incomplete d subshell in at least one of their ions.

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2
Q

Explain why Copper and Chromium appear not to follow the aufbau principle (orbitals are filled in order of increasing energy).

A

Chromium [Ar] 3d5 4s1

Copper [Ar] 3d10 4s1

Half-filled or fully filled d orbitals have a special stability. However, whenever transition metals form ions electrons are lost first from the outermost subshell the 4s.

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3
Q

What is the electron configuration of Co2+ ?

A

1s22s22p63s23p63d7

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4
Q

Explain why Scandium 3+ and Zinc 2+ ions are often considered not to be transition metals.

A

Scandium only forms 3+ ions and Zinc only forms 2+ ions. Neither of these result in an incomplete d subshell, therefore do not fit the definition of a transition metal.

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5
Q

Consider the electronic configurations of the Fe2+ and Fe3+ ions in terms of orbital box notation. Explain why Fe(III) compounds are more stable than Fe(II) compounds.

A

Fe3+ ions would have a half-filled d subshell which is stable.

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6
Q

What are the oxidation states of sulfur in H2S, S8 (elementary sulphur), SO2 and SO42-

A

H2S, S8 (elementary sulphur), SO2, SO3, and H2SO4

-2, 0, +4 and +6.

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7
Q

Define oxidation and reduction in terms of oxidation number

A

OXIDATION can be defined as an increase in oxidation number, while REDUCTION can be defined as a decrease in oxidation number.

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8
Q

What is a transition metal complex?

A

A complex consists of a central metal ion surrounded by ligands

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9
Q

What is a ligand and how does it bond to a TM?

A

Ligands are electron donors which may be negative ions or molecules with non-bonding pairs of electrons.

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10
Q

What is meant by a dative bond?

What is co-ordination number?

A

a covalent bond (a shared pair of electrons) in which both electrons come from the same atom.

and

the number of bonds attached to the TM

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11
Q

How many pairs of electrons do each of the following types of ligands donate?

i) monodentate
ii) bidentate
iii) polydentate

A

i) one
ii) two
iii) more than one

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12
Q

one nickel(II) ion will form six bonds with one ‘molecule’ of EDTA

i) What type of ligand is EDTA
ii) what is the coordination number of nickel?

A

i) polydentate or hexadentate
ii) 6

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13
Q

i) Name this complex
ii) What its coordiation number of the transition metal ion
iii) What is the oxidation state of the metal ion

[Co(OH2)6]Cl2

A

i) Hexaaquacobalt(II)
ii) 6
iii) +2

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14
Q

Na[CrF4]

i) Name the complex in the square brackets
ii) What its coordiation number of the transition metal ion
iii) What is the oxidation state of the metal ion

A

i) tetrafluorochromate(III)
ii) 4
iii) +3

We need 1 Na+ to balance charge on complex.

If we have 4 F- then this means that the chromate

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15
Q

i) Name this complex
ii) What its coordiation number of the transition metal ion
iii) What is the oxidation state of the metal ion

[Co(H2O)6]Cl2

A

i) Hexaaquacobalt(II) chloride
ii) 6
iii) +2

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16
Q

What name is given to AOs which have the same energy?

A

Degenerate

17
Q

What happens to the 5 degenerate d AOs when a ligang(s) approach a TM ion?

A

They split:

_ _

_ _ _

18
Q

Describe how TM complexes are coloured

A

Light is absorbed and electrons are promoted to a d orbital of higher energy

The complimentary colour is observed which is in the visible or UV regions

19
Q

Different ligands can cause different splitting between the d AOs.

What is the relationship between E and wavelength?

A

As E increases, wavelength decreases.

20
Q

A use of TMs is

A

Catalysts

21
Q

What is a:

  • heterogeneous catalyst
  • homogeneous catalyst
A

a catalyst in the different physical state to the reactants

a catalyst in the same physical state to the reactants

22
Q

How does a catalyst work?

A

reactants are adsorbed onto the active site of the catalyst forming an activated complex (because the TM has an unfilled d AO) which lowers the activation energy