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Q.

The d-electron configurations of Cr²⁺, Mn²⁺, Fe²⁺ and Co²⁺ are d⁴, d⁵, d⁶ and d⁷ respectively. Which one of the following will exhibit the lowest paramagnetic behaviour?
$(Atomic no. Cr = 24, Mn = 25, Fe = 26, Co = 27).$

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a

${[Cr {(H_{2} O)}_{6}]}^{2 +}$

b

${[Co {(H_{2} O)}_{6}]}^{2 +}$

c

${[Mn {(H_{2} O)}_{6}]}^{2 +}$

d

${[Fe {(H_{2} O)}_{6}]}^{2 +}$

answer is A.

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$∴$ Since Co²⁺ has lowest number of unpaired electrons hence lowest paramagnetic behaviour is shown by ${[Co {(H_{2} O)}_{6}]}^{2 +}$

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The d-electron configurations of Cr2+, Mn2+, Fe2+ and Co2+ are d4, d5, d6 and d7 respectively. Which one of the following will exhibit the lowest paramagnetic behaviour? (Atomic no. Cr=24,Mn=25,Fe=26,Co=27 ).