• As a general rule,?metals?are on the?left?of the Periodic Table and?non-metals?are on the?right-hand?side
• Ionic?bonds?involve the?transfer?of electrons from a?metallic?element to a?non-metallic?element
• Transferring electrons usually leaves the metal and the non-metal with a?full?outer?shell
• Metals?lose?electrons from their valence shell forming positively charged?cations
• Non-metal atoms?gain?electrons forming negatively charged?anions
• Once the atoms become ions, their electronic configurations are the same as a noble gas.
  • A sodium ion (Na⁺) has the same electronic configuration as neon: [2,8]
  • A chloride ion (Cl^-) also has the same electronic configuration as argon: [2,8,8]

Forming cations by the removal of electrons from metals

Forming anions by the addition of electrons to nonmetals

• Cations?and?anions?are oppositely charged and therefore attracted to each other
• Electrostatic?attractions?are formed between the oppositely charged ions to form?ionic?compounds
• This form of attraction is very?strong?and requires a lot of energy to overcome
  • This causes high melting points in ionic compounds

Cations and anions bond together using strong electrostatic forces, which require a lot of energy to overcome