Paramagnetism is directly related with presence of unpaired electron. As each unpaired electron has a magnetic moment associated with its spin angular momentum and orbital angular momentum. For the 3 d series, the contribution of orbital angular momentum is effectively quenched and hence is of considerably importance. Thus, the magnetic moment is determined by the number of unpaired electrons and is calculated by using the spin only formula, i.e. μ=√n(n+2) BM where hn= number of unpaired electrons. The paramagnetic metal ion among

Question

Paramagnetism is directly related with presence of unpaired electron. As each unpaired electron has a magnetic moment associated with its spin angular momentum and orbital angular momentum. For the 3 d series, the contribution of orbital angular momentum is effectively quenched and hence is of considerably importance. Thus, the magnetic moment is determined by the number of unpaired electrons and is calculated by using the spin only formula, i.e. μ=√n(n+2) BM where hn= number of unpaired electrons. The paramagnetic metal ion among (A) Ag + (B) Zn 2+ (C) Cu 2+ (D) Au +

Tardigrade Admin · Accepted Answer

Ag +, Zn 2+ and Au +have d10 configuration and therefore are paramagnetic in nature.

$A g^{+}$

$Z n^{2 +}$

$C u^{2 +}$

$A u^{+}$

$A g^{+}, Z n^{2 +}$ and $A u^{+}$ have $d^{10}$ configuration and therefore are paramagnetic in nature.

Ag+

Zn2+

Cu2+

Au+

Ag+,Zn2+ and Au+have d10 configuration and therefore are paramagnetic in nature.

$A g^{+}$

$Z n^{2 +}$

$C u^{2 +}$

$A u^{+}$

$A g^{+}, Z n^{2 +}$ and $A u^{+}$ have $d^{10}$ configuration and therefore are paramagnetic in nature.