DOES NO-3 VIOLATES OCTET RULE ?
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To determine whether NO3 violates the octet rule, we need to examine the Lewis structure of the molecule. The octet rule states that atoms in molecules tend to form stable electron configurations by acquiring eight electrons in their valence shell, which can be achieved by sharing, gaining, or losing electrons.
When we draw the Lewis structure of NO3, we find that nitrogen (N) is the central atom bonded to three oxygen (O) atoms. Each oxygen atom forms a double bond with the nitrogen, resulting in a total of three bonds. Additionally, nitrogen has a lone pair of electrons. The Lewis structure is as follows:
O
╱ ╲
O O
\ /
N
By counting the valence electrons, we find that each oxygen atom contributes six electrons (because they are in Group 16 on the periodic table) and nitrogen contributes five electrons (as it is in Group 15). The total number of valence electrons in NO3 is 24 (6 for each oxygen and 5 for nitrogen).
Now, let's distribute the electrons to satisfy the octet rule. Each oxygen atom has six valence electrons, already accounted for by the double bond, leaving no extra electrons.
For the nitrogen atom, it has an octet when it has eight valence electrons, so it requires three more electrons to fulfill the octet rule. Since it has a lone pair, it is already fulfilling this requirement.
Thus, we can conclude that NO3 does not violate the octet rule.