Which of the following arrangments does not represent the correct order of the property stated against it?
(1) $V^{2 +} < C r^{2 +} < M n^{2} < F e^{2 +}$ : paramagnetic behaviour
(2) $N i^{2 +} < C o^{2 +} < F e^{2 +} < M n^{2 +}$ : ionic size
(3) $C o^{3 +} < F e^{3 +} < C r^{3 +} < S c^{3 +}$ : stability in aqueous solution
(4) $S c < T i < C r < M n$ : number of oxidation states

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Solution

a) Paramagnetic behavoiur :
$V^{2 +} ({3 d}^{3}) \to n = 3$
${C r}^{2 +} ({3 d}^{4}) \to n = 4$
${M n}^{2 +} ({3 d}^{5}) \to n = 5$
${F e}^{2 +} ({3 d}^{0}) \to n = 4$
$\Rightarrow {M n}^{2 +} > {F e}^{2 +} > {C r}^{2 +} > V^{2 +}$
b) ${N i}^{2 +} < {C O}^{2 +} < {F e}^{2 +} < {M n}^{2 +}$ : ionic size
For same O.S, the ionic radii generally decreases with increase in nuclear charge and nuclear charge increases as we move across period.
c) ${C O}^{3 +} < {F e}^{3 +} < {C r}^{3 +} < {S C}^{3 +}$ : stability in aq. solutions the lowest the electrode potential, the more stable is the transition metal in aq. solution. The value becomes less $- v e$ across the series.
d) $S c < T i < C r < M n$ : number of oxidation states.

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Q. Consider the ions

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Which of the following arrangments does not represent the correct order of the property stated against it?(1) V2+<Cr2+<Mn2<Fe2+ : paramagnetic behaviour (2) Ni2+<Co2+<Fe2+<Mn2+ : ionic size (3) Co3+<Fe3+<Cr3+<Sc3+ : stability in aqueous solution(4) Sc<Ti<Cr<Mn : number of oxidation states