Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F

Verified step by step guidance

1. Identify the valence electrons for each element using the periodic table.
2. Use Lewis symbols to represent the valence electrons for each element.
3. Determine how many electrons each element needs to gain or lose to achieve a full outer shell (octet rule).
4. Pair the elements such that the total number of electrons lost by the metal equals the total number of electrons gained by the non-metal.
5. Write the chemical formula by balancing the charges to ensure the compound is neutral.

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 calcium (Ca) shows two dots, indicating its two valence electrons, which are crucial for forming ionic or covalent bonds.

Ionic Bonding

Ionic bonding occurs when one atom donates electrons to another, resulting in the formation of charged ions. This typically happens between metals, which lose electrons, and nonmetals, which gain electrons. For instance, in the case of calcium (Ca) and nitrogen (N), calcium loses two electrons to form Ca²⁺, while nitrogen gains three electrons to form N³⁻, leading to the compound Ca₃N₂.

Covalent Bonding

Covalent bonding involves the sharing of electron pairs between atoms, usually between nonmetals. This type of bond is characterized by the formation of molecules where the shared electrons allow each atom to achieve a stable electron configuration. For example, when magnesium (Mg) bonds with iodine (I), they share electrons to form MgI₂, illustrating the concept of covalent bonding in molecular compounds.