What are the oxidation numbers of the elements in the nitrite ion
1 answer:
Answer : The oxidation number of nitrogen and oxygen in nitrite ion is, (+3) and (-2) 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 molecule is,
Let the oxidation state of 'N' be, 'x'
Therefore, the oxidation number of nitrogen and oxygen in nitrite ion is, (+3) and (-2) respectively.
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Answer :
(a) The charge and full ground-state electron configuration of the monatomic ion is, (+1) and
(b) The charge and full ground-state electron configuration of the monatomic ion is, (-3) and
(c) The charge and full ground-state electron configuration of the monatomic ion is, (-1) and
Explanation :
For the neutral atom, the number of protons and electrons are equal. But, they are unequal when the atoms present in the form of ions or the atom has some charges.
When an unequal number of electrons and protons then it leads to the formation of ionic species.
Ion : An ion is formed when an atom looses or gains electron.
When an atom looses electrons, it will form a positive ion known as cation.
When an atom gains electrons, it will form a negative ion known as anion.
(a) The given element is, Rb (Rubidium)
As we know that the rubidium element belongs to group 1 and the atomic number is, 37
The ground-state electron configuration of Rb is:
This element will easily loose 1 electron and form ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Rb ion is:
(b) The given element is, N (Nitrogen)
As we know that the nitrogen element belongs to group 15 and the atomic number is, 7
The ground-state electron configuration of N is:
This element will easily gain 3 electrons and form ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of N ion is:
(c) The given element is, Br (Bromine)
As we know that the bromine element belongs to group 17 and the atomic number is, 35
The ground-state electron configuration of Rb is:
This element will easily gain 1 electron and form ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Br ion is: