Explain the following observations giving an appropriate reason for each.
(i) The enthalpies of atomization of transition elements are quite high.
(ii) There occurs much more frequent metal-metal bonding in compounds of heavy transition metals (i.e. $3^{r d}$ series).
(iii) $M n^{2 +}$ much more resistant than $F e^{2 +}$ towards oxidation.

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Solution

I) Transition metals have high effective nuclear charge and more number of valence electrons. Therefore, they form strong metallic bonds as a result the enthalpy of atomization is very high.
II) The presence of valence electrons and unpaired d-orbital electron helps heavy transition metals to form metallic bonds.
III) Due to stability of $M n^{2 +}$ because it has half filled ( $3 d^{5}$ ) d-orbital. Hence, it does not oxidized. But $F e^{2 +}$ has $3 d^{6}$ configuration and it can lose one electron to get stable $d^{5}$ configuration. Therefore, it can easily oxidized.

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Similar questions

M n^{2 +}

F e^{2 +}

Explain giving reasons:

(i) Transition metals and many of their compounds show paramagnetic

behaviour.

(ii) The enthalpies of atomisation of the transition metals are high.

(iii) The transition metals generally form coloured compounds.

(iv) Transition metals and their many compounds act as good catalyst.

K_{2} M n O_{4}

M n O_{2}

{N a}_{2} {C r}_{2} O_{7}

{N a}_{2} C r O_{4}

{M n}^{2 +}

{F e}^{2 +}

+ 3

Z n

3 d

Explain giving reasons :
Transition metals and many of their compounds show paramagnetic behaviour.

The enthalpies of atomisation of the transition metals are high.

The transition metals generally form coloured compounds.

Transition metals and their many compounds act as good catalyst.

(d^{4}), C r^{2 +}

M n^{3 +}

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