Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and P b. Ba and S c. Sr and Se d. Rb and I

Verified step by step guidance

1. Step 1: Identify the valence electrons for each element.
2. Step 2: Determine the charge each element will have when it forms an ion.
3. Step 3: Use the charges to determine the ratio of ions needed to balance the overall charge to zero.
4. Step 4: Write the chemical formula using the determined ratio of ions.
5. Step 5: Verify the formula by ensuring the total positive and negative charges cancel out.

Key Concepts

Lewis Symbols

Lewis symbols represent the valence electrons of an atom as dots around the element's symbol. This visual representation helps in understanding how atoms bond with each other by either sharing or transferring electrons. For example, the Lewis symbol for sodium (Na) shows one dot, indicating its single valence electron, which is crucial for predicting its bonding behavior.

Ionic and Covalent Bonds

Ionic bonds form when one atom donates electrons to another, resulting in charged ions that attract each other. In contrast, covalent bonds involve the sharing of electrons between atoms. Understanding the type of bond that forms between elements, such as metals with nonmetals typically forming ionic bonds, is essential for predicting the chemical formula of the resulting compound.

Chemical Formula Representation

A chemical formula indicates the types and numbers of atoms in a compound. It is derived from the charges of the ions formed during bonding, ensuring that the overall charge of the compound is neutral. For instance, when strontium (Sr) and phosphorus (P) bond, the resulting formula reflects the balance of their respective charges, leading to the correct stoichiometry in the compound.