Determine the oxidation states of the elements in the compounds listed. none of the oxygen-containing compounds are peroxides or superoxide.
(a)h2so4
(b)ca(oh)2
(c)broh
(d)clno2
(e)ticl4
(f)nah

Explanation:

a)

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of S be x.

Oxidation state of S in = +6

b)

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of Ca be x.

Oxidation state of Ca in = +2

c) BrOH

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of Br be x.

Oxidation no. of Br in BrOH is +1

d)

oxidation state of Cl = -1

Oxidation state of O = -2

Let the oxidation no. of N be x.

Oxidation state of N in = +3

e)

oxidation state of Cl = -1

Let the oxidation no. of Ti be x.

Oxidation state of Ti in = +4

f) NaH

Na is more electropositive than H.

Therefore, oxidation state of Na = +1

Oxidation state of H = -1