Respuesta :
Answer : The oxidation states of chlorine in these three ions [tex]ClO^-[/tex], [tex]ClO_3^-[/tex] and [tex]Cl^-[/tex] is, (+1), (+5) and (-1) respectively.
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.
The given ion is, [tex]ClO^-[/tex]
Let the oxidation state of 'Cl' be, 'x'
[tex]x+(-2)=-1\\\\x-2=-1\\\\x=-1+2\\\\x=+1[/tex]
The oxidation number of chlorine in [tex]ClO^-[/tex] is, (+1)
The given ion is, [tex]ClO_3^-[/tex]
Let the oxidation state of 'Cl' be, 'x'
[tex]x+3(-2)=-1\\\\x-6=-1\\\\x=-1+6\\\\x=+5[/tex]
The oxidation number of chlorine in [tex]ClO_3^-[/tex] is, (+5)
The given ion is, [tex]Cl^-[/tex]
Let the oxidation state of 'Cl' be, 'x'
[tex]x=-1[/tex]
The oxidation number of chlorine in [tex]Cl^-[/tex] is, (-1)
