Question

Which of the following arrangements does not represent the correct order of the property stated against it?

• A. $V ^{2+} < Cr^{2+} < Mn^{2+} < Fe^{2+}$: paramagnetic behaviour
• B. $Ni^{2+} < Co^{2+} < Fe^{2+} < Mn^{2+}$ : ionic size
• C. $Co^{3+} < Fe^{3+} < Cr^{3+} < Sc^{3+}$ : stability in aqueous solution
• D. $Sc < Ti < Cr < Mn$ . number of oxidation states

Answer 1

Answer: (A)

$V ^{2+} < Cr^{2+} < Mn^{2+} < Fe^{2+}$: paramagnetic behaviour

Answer 2

The correct answer is Option A) $V ^{2+} < Cr^{2+} < Mn^{2+} < Fe^{2+}$: paramagnetic behaviour

V$^{2+}$ = 3 unpaired electrons
Cr$^{2+}$ = 4 unpaired electrons
Mn$^{2+}$ = 5 unpaired electrons
Fe$^{2+}$ = 4 unpaired electrons
Hence, the order of paramagnetic behaviour should be
$\, \, \, \, \, \, \, \, V^{2+} < Cr ^{2+} = Fe^{2+} < Mn^{2 +}$
Ionic size decreases from left to right in the same period
Paramagnetic property is dependent on the number of unpaired electrons. As the unpaired electrons increase in number, the paramagnetic property also increases.

Discover More From Chapter:D and F Block Elements