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Ch.8 - Basic Concepts of Chemical Bonding
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.8 - Basic Concepts of Chemical BondingProblema 19d
Capitolo 8, Problema 19d

Predict the chemical formula of the ionic compound formed between the following pairs of elements: (d) Mg and N

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Identify the charges of the ions formed by each element: Magnesium (Mg) typically forms a cation with a charge of +2, while Nitrogen (N) typically forms an anion with a charge of -3.
Use the criss-cross method to balance the charges: The charge of the magnesium ion (+2) becomes the subscript of the nitrogen ion, and the charge of the nitrogen ion (-3) becomes the subscript of the magnesium ion.
Write the chemical formula by placing the subscripts obtained from the criss-cross method next to the respective elements: Mg_3N_2.
Ensure the subscripts are in the lowest whole number ratio: In this case, the subscripts 3 and 2 are already in the lowest ratio.
Verify the neutrality of the compound: The total positive charge from magnesium ions (3 x +2 = +6) balances the total negative charge from nitrogen ions (2 x -3 = -6), resulting in a neutral compound.

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Ionic Bonding

Ionic bonding occurs when atoms transfer electrons to achieve full outer electron shells, resulting in the formation of charged ions. Metals, like magnesium (Mg), tend to lose electrons and form cations, while nonmetals, like nitrogen (N), gain electrons to form anions. The electrostatic attraction between these oppositely charged ions creates a stable ionic compound.
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Chemical Bonds

Charge of Ions

The charge of ions is determined by the number of electrons lost or gained by an atom. Magnesium typically loses two electrons to form a Mg²⁺ ion, while nitrogen gains three electrons to form an N³⁻ ion. Understanding the charges of the ions is crucial for predicting the correct ratio of ions in the resulting ionic compound.
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Polyatomic Ion Charges

Empirical Formula

The empirical formula of an ionic compound represents the simplest whole-number ratio of the ions present. For magnesium and nitrogen, the charges of Mg²⁺ and N³⁻ must be balanced to determine the formula. The least common multiple of the charges (6) indicates that two magnesium ions and three nitrogen ions combine to form the compound, resulting in the empirical formula Mg3N2.
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Empirical vs Molecular Formula
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