Which one of the following is the correct order of oxidation number of Iodine (I) in I2, HI, HIO4 and ICI?

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Q: 52 (NDA-II/2008)

Which one of the following is the correct order of oxidation number of Iodine (I) in I2, HI, HIO4 and ICI?

question_subject: 

Science

question_exam: 

NDA-II

stats: 

0,4,5,5,4,0,0

keywords: 

{'oxidation number': [0, 0, 1, 2], 'correct order': [0, 0, 2, 0], 'iodine': [2, 1, 1, 1], 'i2': [0, 0, 1, 0], 'ici': [0, 0, 1, 0], 'hio4': [0, 0, 1, 0], 'hi04': [0, 0, 1, 0]}

Option 1: HI04 < HI < ICI < I2

Option 2: HI < I2 < ICI < HI04

Option 3: I2

Option 4: ICI < HI04 < HI < I2

The question asks for the correct order of the oxidation number of iodine (I) in the given compounds: I2, HI, HIO4, and ICI.

To determine the oxidation number of iodine, we need to consider the electronegativity difference between iodine and the other elements in the compounds.

In I2, iodine is in its elemental form, so the oxidation number is zero.

In HI, hydrogen has an oxidation number of +1, so the oxidation number of iodine is -1.

In HIO4, oxygen has an oxidation number of -2 and hydrogen has an oxidation number of +1. Since the overall charge of the molecule is zero, the oxidation number of iodine must be +7 to balance the charges.

In ICI, chlorine has an oxidation number of -1. Since the overall charge of the molecule is zero, the oxidation number of iodine must be +1 to balance the charges.

Based on these oxidation

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