Respuesta :
Answer :
(1) The oxidation number of P is, (+3)
The oxidation number of H is, (+1)
The oxidation number of O is, (-2)
(2) The oxidation number of Al is, (+3)
The oxidation number of O is, (-2)
(3) The oxidation number of I is, (+7)
The oxidation number of H is, (+1)
The oxidation number of O is, (-2)
Explanation :
Oxidation number : It represent the number of electrons lost or gained by the atoms of an element in a compound.
Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.
When the atoms are present in their elemental state then the oxidation number will be zero.
Rules for Oxidation Numbers :
The oxidation number of a free element is always zero.
The oxidation number of a monatomic ion equals the charge of the ion.
The oxidation number of Hydrogen (H) is +1, but it is -1 in when combined with less electronegative elements.
The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in peroxides.
The oxidation number of a Group 1 element in a compound is +1.
The oxidation number of a Group 2 element in a compound is +2.
The oxidation number of a Group 17 element in a binary compound is -1.
The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.
(1) The given compound is, [tex]HPO_3^{2-}[/tex]
Let the oxidation state of 'P' be, 'x'
[tex](+1)+x+3(-2)=-2\\\\x=+3[/tex]
The oxidation number of P is, (+3)
The oxidation number of H is, (+1)
The oxidation number of O is, (-2)
(2) The given compound is, [tex]Al_2O_3[/tex]
Let the oxidation state of 'Al' be, 'x'
[tex]2x+3(-2)=0\\\\x=+3[/tex]
The oxidation number of Al is, (+3)
The oxidation number of O is, (-2)
(3) The given compound is, [tex]HIO_4[/tex]
Let the oxidation state of 'I' be, 'x'
[tex](+1)+x+4(-2)=0\\\\x=+7[/tex]
The oxidation number of I is, (+7)
The oxidation number of H is, (+1)
The oxidation number of O is, (-2)
