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Ch.2 - Atoms, Molecules, and Ions
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.2 - Atoms, Molecules, and IonsProblema 62e
Capitolo 2, Problema 62e

Predict the chemical formulas of the compounds formed by the following pairs of ions: (e) Ti4+ and O2-.

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Identify the charges of the ions: Ti^{4+} has a charge of +4 and O^{2-} has a charge of -2.
Determine the ratio of ions needed to balance the charges. Since Ti^{4+} has a +4 charge and O^{2-} has a -2 charge, you need two O^{2-} ions to balance one Ti^{4+} ion.
Write the chemical formula by placing the cation first followed by the anion. Use subscripts to indicate the number of each ion needed to balance the charges.
The chemical formula is written as TiO_{x}, where x is the number of O^{2-} ions needed to balance the charge of one Ti^{4+} ion.
Since two O^{2-} ions are needed to balance one Ti^{4+} ion, the chemical formula is TiO_{2}.

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Ionic Compounds

Ionic compounds are formed when positively charged ions (cations) and negatively charged ions (anions) combine. The overall charge of the compound must be neutral, meaning the total positive charge must balance the total negative charge. Understanding how to combine these ions based on their charges is essential for predicting the correct chemical formula.
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Ionic Compounds Naming

Charge Balance

Charge balance is a fundamental principle in chemistry that dictates how ions combine to form neutral compounds. For example, if a cation has a charge of +4 (like Ti4+) and an anion has a charge of -2 (like O2-), the ratio of ions must be adjusted so that the total positive charge equals the total negative charge, leading to the correct stoichiometry in the formula.
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Formal Charge

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the elements in a compound. When predicting the formula for the compound formed by Ti4+ and O2-, one must determine the lowest ratio of titanium to oxygen that results in a neutral compound, which is crucial for accurately expressing the compound's composition.
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Empirical vs Molecular Formula
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