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# Oxidation number of carbon in $C{{H}_{2}}C{{l}_{2}}$\begin{align} & A)\text{ 0} \\ & B)\text{ +1} \\ & C)\text{ +2} \\ & D)\text{ +4} \\ \end{align}

Last updated date: 12th Jul 2024
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Hint: Oxidation state is termed as Oxidation number which describes the degree of oxidation. Oxidation state of an atom is the hypothetical charge that it would have when all the bonds are treated as purely ionic.

The IUPAC name of $C{{H}_{2}}C{{l}_{2}}$ is dichloromethane, often abbreviated as DCM. Carbon in $C{{H}_{2}}C{{l}_{2}}$ is $sp3$ hybridized leading to a Tetrahedral geometry of molecule as shown below-

Let oxidation state of carbon in $C{{H}_{2}}C{{l}_{2}}$ be $x$
Oxidation state of $H$ in $C{{H}_{2}}C{{l}_{2}}$ is $+1$
Oxidation state of $Cl$ in $C{{H}_{2}}C{{l}_{2}}$ is $-1$
Since, there is no net charge on the DCM molecule, the sum of the oxidation state of all the atoms constituting it will be zero.
Sum of oxidation state = zero
\begin{align} & \text{ }C+2(H)+2(Cl)=0 \\ & \Rightarrow x+2(+1)+2(-1)=0 \\ & \Rightarrow \text{}x+2-2=0 \\ & \Rightarrow \text{}x=0 \\ \end{align}
The oxidation state of carbon in $C{{H}_{2}}C{{l}_{2}}$ is Zero. Hence the option A is correct.

Note: Sum of oxidation state of a constituting atom of a molecule or compound is equal to the net charge present on that molecule. Hydrogen shows two oxidation states $(+1,-1)$. It shows normally $+1$ oxidation state when attached to Carbon, Oxygen, halogen etc. When attached to metals it shows $-1$ oxidation state because metals are electropositive.