Predict the chemical formula for the ionic compound formed by (d) NH4+ and SO42-

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Identify the ions involved: ammonium ion \( \text{NH}_4^+ \) and sulfate ion \( \text{SO}_4^{2-} \).

Determine the charges on each ion: \( \text{NH}_4^+ \) has a charge of +1 and \( \text{SO}_4^{2-} \) has a charge of -2.

To form a neutral compound, balance the total positive and negative charges by adjusting the number of each ion.

Since the sulfate ion has a charge of -2, you will need two ammonium ions to balance the charge, resulting in a neutral compound.

Write the chemical formula by combining the ions in the correct ratio: \( (\text{NH}_4)_2\text{SO}_4 \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed when cations (positively charged ions) and anions (negatively charged ions) bond together through electrostatic forces. The overall charge of the compound must be neutral, meaning the total positive charge from cations must balance the total negative charge from anions.

Polyatomic Ions

Polyatomic ions are ions that consist of two or more atoms bonded together, which carry a net charge. In this case, NH4+ (ammonium) and SO42- (sulfate) are both polyatomic ions, and understanding their charges is crucial for determining the correct ratio in the resulting ionic compound.

Chemical Formula Representation

The chemical formula of an ionic compound reflects the ratio of the constituent ions that results in a neutral charge. For NH4+ and SO42-, the formula is determined by balancing the charges, leading to the formula (NH4)2SO4, which indicates two ammonium ions for every sulfate ion to achieve charge neutrality.

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