Column A
1.
The oxidation number of H in HClO4 is _______.
:
The oxidation number of H in HClO4 is _______.
2.
The oxidation number of Cl in HClO4 is _______.
:
The oxidation number of Cl in HClO4 is _______.
3.
The oxidation number of O in HClO4 is _______.
:
The oxidation number of O in HClO4 is _______.
Column B
a.+2
b.-2
c.+1
d.-8
e.+7
Column A: Oxidation Numbers
1. The oxidation number of H in HClO4 is _c_.
The oxidation number of hydrogen (H) is usually +1 in its compounds, except when it is bonded to metals in binary metal hydrides where its oxidation state is -1.
2. The oxidation number of Cl in HClO4 is _e_.
To find the oxidation number of chlorine (Cl) in HClO4 (perchloric acid), one can use the rule that the sum of oxidation numbers in a neutral compound must be zero. Knowing that oxygen (O) usually has an oxidation number of -2, we can calculate:
Let the oxidation number of Cl be x.
x + 1*(+1) + 4*(-2) = 0
x + 1 - 8 = 0
x - 7 = 0
x = +7
3. The oxidation number of O in HClO4 is _b_.
The oxidation number of oxygen (O) is generally -2 in compounds, except in peroxides or when bonded to fluorine.
So, the answers are:
1. c. +1
2. e. +7
3. b. -2