The oxidation state and covalency of Al in [A | vedclass

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(A) To find the oxidation state of $Al$ in $[AlCl(H_2O)_5]^{2+}$,let the oxidation state be $x$. The charge on $Cl$ is $-1$ and $H_2O$ is a neutral li

Vedclass · Accepted Answer

$+3$ and $6$

Vedclass · Answer

(A) To find the oxidation state of $Al$ in $[AlCl(H_2O)_5]^{2+}$,let the oxidation state be $x$. The charge on $Cl$ is $-1$ and $H_2O$ is a neutral ligand $(0)$. $x + (-1) + 5(0) = +2$ $x - 1 = +2$ $x = +3$. The covalency is defined as the total number of coordinate bonds formed by the central metal atom with the ligands. Here,$Al$ is bonded to $5$ $H_2O$ molecules and $1$ $Cl^-$ ion. Total covalency = $5 + 1 = 6$. Therefore,the oxidation state is $+3$ and the covalency is $6$.

The oxidation state and covalency of $Al$ in $[AlCl(H_2O)_5]^{2+}$ respectively are

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