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Answer :
Final answer:
Nitrogen typically has a -3 charge in an ionic compound due to gaining 3 electrons to fill its outer shell and become stable.
Explanation:
The expected charge for a nitrogen atom in an ionic compound is typically -3. In the atomic structure of nitrogen, there are 5 electrons in its outermost shell. For an atom to be stable, it requires a full outer shell, which is often 8 electons. Thus, nitrogen will gain 3 electrons to fill its outer shell, developing a -3 charge. When nitrogen does this, it forms an anion (a negatively charged ion), specifically referred to as a nitride ion (N3-). This negative charge is typical in ionic compounds containing nitrogen.
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The expected charge for nitrogen in an ionic compound is typically -3.
Nitrogen is a nonmetal in Group 15 of the periodic table, and it has five valence electrons. To achieve a full valence shell (eight electrons), nitrogen tends to gain three electrons through ionic bonding. This results in a net charge of -3 for nitrogen in ionic compounds.
For example, in the ionic compound ammonium chloride (NH₄Cl), the nitrogen atom carries a -3 charge. The ammonium ion (NH₄+) is a polyatomic cation, where the nitrogen atom donates one of its valence electrons to form a covalent bond with four hydrogen atoms.
The three additional electrons gained by nitrogen give it an overall charge of -3, balancing the +3 charge of the four hydrogen atoms, resulting in a neutral compound. This -3 charge for nitrogen is commonly observed in various ionic compounds containing nitrate or amide ions.
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