Question

Oxidation number of carbon in \(\mathrm{CHI}_{2} \mathrm{Cl}_{2}\) is (1) \(-4\) (2) \(+4\) (3) 3 (4) 0

Short answer

The oxidation number of carbon in \(\text{CHI}_2\text{Cl}_2\) is +2.

Step-by-step solution

Understand the problem

The objective is to determine the oxidation number of carbon in the compound \(\text{CHI}_2\text{Cl}_2\).

Recall oxidation number rules

The common oxidation numbers to consider are: - Hydrogen (H): +1 - Iodine (I): -1 - Chlorine (Cl): -1

Assign oxidation numbers to each atom

In \(\text{CHI}_2\text{Cl}_2\), assign the oxidation numbers: - Hydrogen (H): +1 - Iodine (I): -1 - Chlorine (Cl): -1

Set up the oxidation state equation

Use the fact that the sum of oxidation numbers in a neutral compound is zero: \( \text{C} + 2(\text{I}) + 2(\text{Cl}) + 2(\text{H}) = 0 \)

Substitute and solve the equation

Substitute the known oxidation numbers: \( \text{C} + 2(-1) + 2(-1) + 2(+1) = 0 \)Simplify to find the oxidation number of Carbon (C): \( \text{C} - 2 - 2 + 2 = 0 \)\( \text{C} - 2 = 0 \)\( \text{C} = +2 \)

Verify the result

Check that the sum of the oxidation numbers is zero: \( +2 \text{(Carbon)} + 2(-1) \text{(I)} + 2(+1) \text{(H)} - 2 = 0\)This confirms the solution.

Key concepts

Oxidation Number Rules

To solve problems involving oxidation states, understanding oxidation number rules is crucial. Each element in a compound has an oxidation number that helps determine how electrons are distributed among atoms. Here are some key rules to remember:

• Hydrogen usually has an oxidation number of +1.
• Oxygen usually has an oxidation number of -2.
• Halogens like chlorine and iodine often have oxidation numbers of -1.
• The sum of oxidation numbers in a neutral compound must be zero.

These rules help us systematically determine which atoms gain or lose electrons in a reaction, allowing us to solve oxidation state problems efficiently.

Chemical Compound Analysis

Analyzing a chemical compound involves breaking it down to understand its structure and behavior. For oxidation state calculations, follow these steps: First, identify each element and its common oxidation states based on the rules mentioned earlier. Then, consider the overall charge of the compound. Most compounds are neutral, so their oxidation numbers should sum to zero. For example, in \(\text{CHI}_{2}\text{Cl}_{2}\), we assign oxidation numbers to each element based on their common states:

• Hydrogen (H): +1
• Iodine (I): -1
• Chlorine (Cl): -1

We then use these values in the oxidation state equation to solve for the unknown oxidation number, ensuring the sum is zero.

Neutral Compound

A neutral compound means that it has no overall charge. Each molecule's total oxidation numbers must add up to zero. This is essential for calculating unknown oxidation states. Let's consider \- \(\text{CHI}_{2}\text{Cl}_{2}\). The sum of oxidation numbers in this neutral compound \ is zero. Using the known oxidation numbers of H, I, and Cl, we set up the equation:
\{\text{C} + 2(\text{I}) + 2(\text{Cl}) + 2(\text{H}) = 0}\. Replace the oxidation numbers to get:
\(\text{C} + 2(-1) + 2(-1) + 2(+1) = 0\)\.
Simplify to find the oxidation number of Carbon (C):
\(\text{C} - 2 - 2 + 2 = 0\)
\(\text{C} - 2 = 0\)
\(\text{C} = +2\). This calculation confirms that the oxidation state of carbon in \(\text{CHI}_{2}\text{Cl}_{2}\) is +2, ensuring that the compound remains neutral.