Question

The average oxidation number of bromine in Br₃O₈ is

• A. \(\frac{16}{3}\)
• B. \(\frac{4}{3}\)
• C. \(\frac{3}{4}\)
• D. \(\frac{5}{2}\)
• E. \(\frac{8}{3}\)

Answer 1

The Correct Option is A

To find the average oxidation number of bromine in Br\(_3\)O\(_8\), we can assume that oxygen has an oxidation number of \(-2\) (since oxygen is typically \(-2\) in compounds). Let the oxidation number of bromine be \( x \). The compound is Br\(_3\)O\(_8\), so:
There are 3 bromine atoms, each with oxidation number \( x \).
There are 8 oxygen atoms, each with oxidation number \(-2\). The sum of oxidation numbers in the compound must be zero because the compound is neutral. Therefore, we can write the equation: \[ 3x + 8(-2) = 0 \] Simplifying: \[ 3x - 16 = 0 \quad \Rightarrow \quad 3x = 16 \quad \Rightarrow \quad x = \frac{16}{3} \]

The correct option is (A) : \(\frac{16}{3}\)

Answer 2

To find the average oxidation number of bromine in Br₃O₈, let the oxidation number of each bromine atom be x.

There are 3 bromine (Br) atoms, so total contribution = 3x
There are 8 oxygen (O) atoms, and each oxygen has an oxidation number of -2, so total contribution = 8 × (-2) = -16

The compound is neutral, so the sum of oxidation numbers is 0:
3x - 16 = 0
3x = 16
x = \(\frac{16}{3}\) 

Therefore, the average oxidation number of bromine in Br₃O₈ is \(\frac{16}{3}\).