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).

Question

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). (A) [Co(H2O)6]2+] (B) [Cr(H2O)6]2+] (C) [Mn(H2O)6]2+] (D) [Fe(H2O)6]2+]

Tardigrade Admin · Accepted Answer

∴ Since Co2+ has lowest no. of unpaired electrons hence lowest paramagnetic behaviour is shown by [Co(H2O)6]2+

Q. The d-electron configurations of $C r^{2 +}, M n^{2 +}, F e^{2 +}$ and $C o^{2 +}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit the lowest paramagnetic behaviour?
(Atomic no. $C r = 24, M n = 25, F e = 26, C o = 27$ ).

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

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

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

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

$∴$ Since $C o^{2 +}$ has lowest no. of unpaired electrons hence lowest paramagnetic behaviour is shown by $[C o (H_{2} O)_{6}]^{2 +}$

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).

[Co(H2​O)6​]2+]

[Cr(H2​O)6​]2+]

[Mn(H2​O)6​]2+]

[Fe(H2​O)6​]2+]