Oxidation states of which oxides of halogens are not the same? A. ClO…

The correct answer is option 2. B and E only.

To determine which oxides of halogens have different oxidation states for the halogen, we need to calculate the oxidation state of the halogen in each of the given oxides:

A. \(ClO_2\) (Chlorine dioxide):

Oxygen has an oxidation state of -2.

Let the oxidation state of chlorine be \( x \).

The sum of oxidation states in the compound must equal zero: \( x + 2(-2) = 0 \).

Solving for \( x \): \( x - 4 = 0 \) ⇒ \( x = +4 \).

B. \(Cl_2O_3\) (Chlorine trioxide):

Oxygen has an oxidation state of -2.

Let the oxidation state of chlorine be \( x \).

The sum of oxidation states in the compound must equal zero: \( 2x + 3(-2) = 0 \).

Solving for \( x \): \( 2x - 6 = 0 \) ⇒ \( x = +3 \).

C. \(BrO_2\) (Bromine dioxide):

Oxygen has an oxidation state of -2.

Let the oxidation state of bromine be \( x \).

The sum of oxidation states in the compound must equal zero: \( x + 2(-2) = 0 \).

Solving for \( x \): \( x - 4 = 0 \) ⇒ \( x = +4 \).

D. \(I_2O_4\) (Iodine tetroxide):

Oxygen has an oxidation state of -2.

Let the oxidation state of iodine be \( x \).

The sum of oxidation states in the compound must equal zero: \( 2x + 4(-2) = 0 \).

Solving for \( x \): \( 2x - 8 = 0 \) ⇒ \( x = +4 \).

E. \(I_2O_5\) (Iodine pentoxide):

Oxygen has an oxidation state of -2.

Let the oxidation state of iodine be \( x \).

The sum of oxidation states in the compound must equal zero: \( 2x + 5(-2) = 0 \).

Solving for \( x \): \( 2x - 10 = 0 \) ⇒ \( x = +5 \).

From the calculations:

\(ClO_2\): +4

\(Cl_2O_3\): +3

\(BrO_2\): +4

\(I_2O_4\): +4

\(I_2O_5\): +5

The oxidation states are different in \(Cl_2O_3\) (Chlorine trioxide) and \(I_2O_5\) (Iodine pentoxide).

Thus, the correct answer is 2. B and E only.