Question 1

In which pair of species are the oxidation numbers of the d-block elements the same?

  A  

[Cr(NH3)4Cl2]+ and [Mn(H2O)6]2+


  B  

CrO42- and TiCl3

  C  

Cr2O3 and [Fe(CN)6]3-

  D  

Cr2O72- and MnO4-

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Question 2

The electronic configuration of the atoms of an element is 1s22s22p63s23p63d54s1.

What is the maximum oxidation number shown in compounds of this element?

  A  

+1

  B  

+5

  C  

+6

  D  

+7

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Question 3

Which of the following species will not act as a ligand in the formation of a complex ion?

  A  

CH3NH2

  B  

CN-

  C  

NH3

  D  

NH4+

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Question 4

Iodide ions are oxidised by peroxodisulfate ions in aqueous solution:

2I- + S2O82- ➔ I2 + 2SO42-

This reaction is catalysed by Fe3+ ions. This catalysis is effective because

  A  

Fe3+ is readily reduced to Fe2+ which is then oxidised to Fe3+

  B  

Fe3+ has many electrons in its outermost subshells

  C  

Fe3+ has many active sites on which the reaction can occur

  D  

Fe3+ will oxidise peroxodisulfate ions to sulfate ions

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Question 5

Which has the greatest number of unpaired electrons in each of its atoms?

  A  

vanadium

  B  

chromium

  C  

manganese

  D  

iron

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Question 6

Which of these complex ions could exist as stereoisomers?

  A  

[Co(NH3)6]3+


  B  

[Co(NH3)5(H2O)]3+


  C  

[Co(NH3)5(Cl)]2+


  D  

[Co(NH3)4(Cl)2]+

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Question 7

Chromium is classified as a transition element because

  A  

it is in the d block of the periodic table

  B  

it forms stable ions in which it has different oxidation numbers

  C  

it has incompletely filled d orbitals

  D  

it forms stable ions which have incompletely filled d orbitals

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Question 8

Copper(II) sulfate solution is blue. This is because

  A  

excited electrons emit light in the blue region of the spectrum as they drop back to the ground state

  B  

excited electrons emit light in the red region of the spectrum as they drop back to the ground state

  C  

electrons absorb light in the red region of the spectrum and the residual  frequencies are observed

  D  

electrons absorb light in the blue region of the spectrum and the residual  frequencies are observed

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Question 9

Platinum forms a complex with the formula Pt(NH3)2Cl2 and chromium forms a complex ion with the formula CrCl4-.

Considering the bonding between the central atom and the ligands in these complexes,

  A  

the bonding in both complexes is dative covalent

  B  

the bonding in both complexes is ionic

  C  

the bonding in Pt(NH3)2Cl2 is dative covalent and in CrCl4- is ionic

  D  

the bonding in Pt(NH3)2Cl2 is ionic and in CrCl4- is dative covalent

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Question 10

The transition metal complex Pt(NH3)2Cl2 exists as two geometric isomers. This is because the complex

  A  

is square-planar

  B  

is tetrahedral

  C  

contains a double bond

  D  

is octahedral

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Question 11

The reaction below can be catalysed by either Fe2+ ions or Fe3+ ions.

S2O8-(aq) + 2I-(aq) ➔ 2SO42-(aq) + I2(aq)

This is because

  A  

both reactants can react with Fe2+ ions

  B  

both reactants can react with Fe3+ ions

  C  

S2O82- ions can be oxidised by Fe3+ ions and I- ions can be reduced by Fe2+ ions

  D  

S2O82- ions can be reduced by Fe2+ ions and I- ions can be oxidised by Fe3+ ions

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Question 12

What is the number of stereoisomers that Ni(H2NCH2CH2NH2)2Cl2 can form?

  A  

2

  B  

3

  C  

4

  D  

6

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Question 13

Which is not a correct statement?

  A  

transition metals form coloured ions and complexes

  B  

transition metals display variable oxidation states

  C  

a ligand accepts a pair of electrons from a transition metal

  D  

a complex is a central metal atom or ion surrounded by

ligands

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Question 14

A solution absorbs light with wavelengths corresponding to red, yellow and green light.

Which ion is most likely to be in the solution?

  A  

Cr2O72-(aq)

  B  

Fe2+(aq)

  C  

Fe3+(aq)

  D  

Cu2+(aq)

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