Questions: MISSED THIS? Read Section 10.3. You can click on the Review link to access the section in your eText. Use the Lewis model to determine the formula for the compound that forms from each pair of atoms. Sr and S Express your answer as a chemical formula.

MISSED THIS? Read Section 10.3. You can click on the Review link to access the section in your eText.

Use the Lewis model to determine the formula for the compound that forms from each pair of atoms.

Sr and S
Express your answer as a chemical formula.

Transcript text: MISSED THIS? Read Section 10.3. You can click on the Review link to access the section in your eText. Use the Lewis model to determine the formula for the compound that forms from each pair of atoms. Sr and S Express your answer as a chemical formula.

Solution

Solution Steps

Step 1: Determine the Valence Electrons for Each Element

Strontium (Sr) is in Group 2 of the periodic table, which means it has 2 valence electrons. Sulfur (S) is in Group 16, which means it has 6 valence electrons.

Step 2: Determine the Ionic Charges

Strontium tends to lose its 2 valence electrons to achieve a stable electron configuration, forming a \( \text{Sr}^{2+} \) ion. Sulfur tends to gain 2 electrons to complete its valence shell, forming a \( \text{S}^{2-} \) ion.

Step 3: Determine the Ratio of Atoms in the Compound

To form a neutral compound, the total positive charge must balance the total negative charge. Since both the \( \text{Sr}^{2+} \) and \( \text{S}^{2-} \) ions have charges of magnitude 2, they will combine in a 1:1 ratio.