First row d-block elements questions

Assignment: Question Topic 13.1 : First row d-block elements

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The first row d-block elements comprise of scandium (electron configuration [Ar]4s23d1) through to zinc (electron configuration[Ar]4s23d10). Explain why zinc is not considered to be a transition element.

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Explain why all first row transition elements show an oxidation state of +2 whereas only copper has compounds with common oxidation states of +1 and +2.

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Explain why carbon monoxide, CO, is a good ligand, whereas methane cannot function as a ligand.

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The following statement is from the ‘Applications and skills’ section of the syllabus: “Explain the ability of transition metals to form variable oxidation states by considering successive ionization energies.”

i.  Examine this statement by comparing the first six ionization energies of aluminium and vanadium.

 

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ii. Examine whether the statement is still valid for manganese which has the common oxidation states of +2, +3, +4, +6 and +7.

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Explain why copper(I) and scandium(III) complex ions are diamagnetic whereas many of the complex ions of most transition metals are paramagnetic.

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Give the formula of the complex ion formed between:

i.   iron(III) ions and six cyanide ions.

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ii.  copper(II) ions and four chloride ions.

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iii. cobalt(III) ions and three 1,2-ethanediamine bidentate ligands.

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iv. iron(III) and one thiocyanate ion and five water molecules.

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