Find the oxidation number of carbon in the following...

$$
\begin{aligned}
&\text { Find the oxidation number of carbon in the following compounds : }\\
&\left(11,_{3}()\right), \mathrm{CH}_{2} \mathrm{O}, \mathrm{HCOOH}, \mathrm{C}_{2} \mathrm{H}_{2}
\end{aligned}
$$

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Key Concepts

Oxidation Number

The oxidation number is a numerical value assigned to an atom in a molecule or ion to indicate its degree of oxidation, based on hypothetical charges if the bonds were ionic. This concept is essential in understanding electron transfer in redox reactions and is used to track how electrons are distributed in compounds.

Rules for Assigning Oxidation States

These are the guidelines used to calculate the oxidation number of each atom in a molecule. They include principles such as assigning a state of zero to pure elements, ensuring that the sum of oxidation numbers in a neutral molecule equals zero (and equals the net charge in ions), and applying common oxidation states (like hydrogen usually being +1 and oxygen usually being -2).

Electronegativity and Electron Distribution

This concept involves considering the tendency of an atom to attract electrons in a bond. When assigning oxidation numbers, electrons in bonds are hypothetically allocated to the more electronegative element. This approach helps determine the oxidation state of atoms, especially when bonds exist between atoms that have different electronegativities.

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