How to Draw Lewis Structures (IONIC) with 4 Examples (CaO, AlF3, Mn3N2, Fe2O3)?

Drawing Lewis structures for ionic compounds is like playing a game of matching pairs, but instead of cards, you're matching atoms to make stable ions.

Imagine you have some friends who really love to share toys. If someone has too many toys and someone else has too few, they’ll trade until everyone feels balanced. That’s what happens in ionic compounds: atoms give or take electrons so they can be happy.

Let’s see how it works with four examples:

You start by figuring out which atom gives electrons (the metal) and which takes them (the non-metal). Metals usually want to lose electrons, like a kid giving up their toys. Non-metals usually want to gain electrons, like a kid getting more toys.

For example:

• CaO: Calcium (Ca) gives 2 electrons to Oxygen (O), making Ca²⁺ and O²⁻.
• AlF3: Aluminum (Al) gives 3 electrons to Fluorine (F), making Al³⁺ and F⁻.
• Mn3N2: Manganese (Mn) gives 2 electrons each to Nitrogen (N), becoming Mn³⁺ and N³⁻.
• Fe2O3: Iron (Fe) gives 3 electrons each to Oxygen (O), becoming Fe³⁺ and O²⁻.

It's all about balance, like sharing toys so everyone is happy!