Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair. Ion K⁺ NH₄⁺ Mg²⁺ Fe³⁺ Cl^- KCl OH^- CO₃^2- PO₄^3-
Complete the first row of the table.
Complete the second row of the table.
Complete the third row of the table.
Complete the fourth row of the table.

검증된 단계별 안내

Identify the cation and anion in the fourth row: Fe^{3+} and PO_4^{3-}.

Determine the charges of the cation and anion: Fe^{3+} has a charge of +3 and PO_4^{3-} has a charge of -3.

To form a neutral ionic compound, the total positive charge must balance the total negative charge.

Since the charges are already balanced (3+ and 3-), one Fe^{3+} ion will pair with one PO_4^{3-} ion.

Write the formula for the ionic compound by placing the cation first followed by the anion: FePO_4.

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주요 개념

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Ionic Compounds

Ionic compounds are formed through the electrostatic attraction between cations (positively charged ions) and anions (negatively charged ions). The overall charge of the compound must be neutral, meaning the total positive charge from the cations must balance the total negative charge from the anions. This principle is essential for determining the correct formula of the compound.

Charge Balance

To write the formula for an ionic compound, it is crucial to ensure that the charges of the cations and anions balance each other. For example, if a cation has a charge of +2, it will require two anions with a charge of -1 to achieve neutrality. This concept helps in determining the subscripts in the chemical formula.

Common Ions and Their Charges

Familiarity with common cations and anions, along with their respective charges, is vital for constructing ionic formulas. For instance, K+ (potassium) has a +1 charge, while Cl- (chloride) has a -1 charge. Knowing these charges allows for the correct pairing of ions to form stable ionic compounds.