Question

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

Answer 1

Step-by-step explanation:

a)
`H_2SO_4`

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of S be x.

`2*1+ x+2* -4 =0`

`2 +x-8 = 0\\x=+6`

Oxidation state of S in
`H_2SO_4` = +6

b)
`Ca(OH)_2`

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of Ca be x.

`x+2*-2+2*+1 =0\\x=4 -2\\x=+2`

Oxidation state of Ca in
`Ca(OH)_2` = +2

c) BrOH

oxidation state of H = +1

Oxidation state of O = -2

Let the oxidation no. of Br be x.

`x+1*-2+1*+1 =+1`

Oxidation no. of Br in BrOH is +1

d)
`ClNO_2`

oxidation state of Cl = -1

Oxidation state of O = -2

Let the oxidation no. of N be x.

`-1+x+2*-2\\x = 4+1 =+5`

Oxidation state of N in
`ClNO_2` = +3

e)
`TiCl_4`

oxidation state of Cl = -1

Let the oxidation no. of Ti be x.

`x+4* -1 = 0\\x=+4`

Oxidation state of Ti in
`TiCl_4` = +4

f) NaH

Na is more electropositive than H.

Therefore, oxidation state of Na = +1

Oxidation state of H = -1