Assign oxidation numbers to each element in the following compounds. (c) COCl

Verified step by step guidance

1. Identify the oxidation number of oxygen (O) in most compounds, which is typically -2.
2. Recognize that chlorine (Cl) usually has an oxidation number of -1 in compounds.
3. Let the oxidation number of carbon (C) be x.
4. Set up the equation based on the compound COCl: x + (-2) + (-1) = 0, because the sum of oxidation numbers in a neutral compound is zero.
5. Solve the equation for x to find the oxidation number of carbon (C).

Key Concepts

Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical compounds. They indicate the degree of oxidation of an atom in a molecule, helping to identify how many electrons an atom has gained, lost, or shared. The rules for assigning oxidation numbers include that the oxidation number of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as: hydrogen is usually +1, oxygen is typically -2, and the sum of oxidation numbers in a neutral compound must equal zero. In compounds with multiple elements, the more electronegative element usually has a negative oxidation number. Understanding these rules is essential for accurately determining oxidation states in complex molecules.

Chemical Structure of COCl

The chemical structure of COCl involves a carbon atom bonded to an oxygen atom and a chlorine atom. In this compound, carbon typically has a +2 oxidation state, oxygen is -2, and chlorine is usually -1. Analyzing the structure helps in applying the rules of oxidation numbers effectively, ensuring that the total charge balances according to the compound's neutrality.