Question

What is the oxidation state of Chlorine in \( Cl_2O_7 \)?

• A. \(+1\)
• B. \(+3\)
• C. \(+5\)
• D. \(+7\)

Hint:

To find oxidation states quickly:
• Oxygen generally has oxidation state \( -2 \).
• Multiply oxidation states by the number of atoms.
• The total for a neutral molecule must equal \(0\).

Answer 1

The Correct Option is D

Step 1: Understanding the Question:
The objective is to determine the oxidation number of Chlorine in the compound Dichlorine Heptoxide (\( Cl_2O_7 \)).
Step 2: Key Formula or Approach:
1. The sum of the oxidation states of all atoms in a neutral molecule is zero.
2. Generally, the oxidation state of Oxygen is \(-2\) (except in peroxides or with Fluorine).
Step 3: Detailed Explanation:
Let the oxidation state of Chlorine be \( x \).
In \( Cl_2O_7 \), we have 2 Chlorine atoms and 7 Oxygen atoms.
The equation for the total charge is:
\[ 2(x) + 7(-2) = 0 \]
\[ 2x - 14 = 0 \]
\[ 2x = 14 \]
\[ x = \frac{14}{2} \]
\[ x = +7 \]
Step 4: Final Answer:
The oxidation state of Chlorine in \( Cl_2O_7 \) is \( +7 \).