Determine the oxidation number of each carbon indicated by an arrow.
(b)

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Identify the carbon atom indicated by the arrow. This carbon is bonded to two chlorine atoms and two other carbon atoms.

Recall that the oxidation number of carbon is determined by assigning electrons in bonds to the more electronegative atom. Chlorine is more electronegative than carbon, so each C-Cl bond will assign the bonding electrons to chlorine.

Assign oxidation numbers: Each C-Cl bond contributes +1 to the oxidation number of carbon because the electrons are assigned to chlorine.

Consider the C-C bonds: In a C-C bond, the electrons are shared equally, so they do not contribute to the oxidation number of carbon.

Sum the contributions: Add the contributions from the C-Cl bonds to determine the oxidation number of the carbon atom indicated by the arrow.

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Oxidation Number

The oxidation number, or oxidation state, is a theoretical charge assigned to an atom in a molecule, reflecting its degree of oxidation. It helps in understanding electron transfer in redox reactions. For carbon, common oxidation states range from -4 in methane (CH4) to +4 in carbon dioxide (CO2), depending on the number of bonds to more electronegative atoms.

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Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. In determining oxidation numbers, the relative electronegativities of atoms are crucial; more electronegative atoms (like oxygen) will pull electron density away from carbon, increasing its oxidation state. Understanding electronegativity helps in assigning accurate oxidation numbers.

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Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They are essential for visualizing how atoms are connected and for determining the oxidation states of individual atoms, including carbon. By analyzing a Lewis structure, one can deduce the formal charges and oxidation numbers of the atoms involved.

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