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171. Write down the number of 3d electrons in each of the following ions : Ti²⁺, V²⁺, Cr³⁺, Mn²⁺, Fe²⁺, Fe³⁺, Co²⁺, Ni²⁺ and Cu²⁺. Indicate how would you expect the five 3d orbitals to be occupied for these hydrated ions (octahedral)

Ions	Number of 3d electron	Filling of d- orbital
Ti²⁺	3d²	$t_{2 g}^{2}$
V²⁺	3d³	$t_{2 g}^{3}$
Cr³⁺	3d⁵	$t_{2 g}^{3}$
Mn²⁺	d⁵	$t_{2 g}^{3} e_{g}^{2}$
Fe²⁺	3d⁶	$t_{2 g}^{4} e_{g}^{2}$
Fe³⁺	3d⁵	$t_{2 g}^{3} e_{g}^{2}$
Co²⁺	3d⁷	$t_{2 g}^{5} e_{g}^{2}$
Ni²⁺	3d⁸	$t_{2 g}^{6} e_{g}^{2}$
Cu²⁺	3d⁹	$t_{2 g}^{6} e_{g}^{2}$

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172.

Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.

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173.

Mention the direct consequence of the following factors on the chemical behaviour of the transition elements.
(i) They have in completely filled d-orbitals in the ground state or in one of the oxidised states of their atoms.
(ii) They contribute more valence electrons per atom in the formation of metallic bonds?

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174. Why do the d-block elements exhibit a large number of oxidation states than the f-block elements?

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175. How do the transition elements form interstitial compounds? State an industrial advantage of such occurrence.

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176. Of the ions Co²⁺, Sc³⁺ and Cr³⁺ which one will give coloured aqueous solutions and will have each of them respond to a magnetic field and why? [Atomic numbers, Co = 27, Sc = 21, Cr = 24]

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