The Basics
* Ionic bonds occur between a metal and a nonmetal. Metals tend to lose electrons, while nonmetals tend to gain electrons.
* Electrons are transferred, not shared. This is a key difference between ionic and covalent bonds.
The Process
1. Metal loses an electron: The metal atom, with its loosely held electrons, loses one or more electrons. This creates a positively charged ion (called a cation).
2. Nonmetal gains an electron: The nonmetal atom, with a strong desire to complete its outer electron shell, gains the electron(s) lost by the metal. This creates a negatively charged ion (called an anion).
3. Electrostatic attraction: The oppositely charged ions are now attracted to each other due to electrostatic forces. This attraction is what holds the ions together in the ionic compound.
Example: Sodium Chloride (NaCl)
* Sodium (Na), a metal, loses one electron to become a sodium ion (Na+).
* Chlorine (Cl), a nonmetal, gains the electron to become a chloride ion (Cl-).
* The oppositely charged ions (Na+ and Cl-) attract each other, forming an ionic bond and creating the compound sodium chloride (NaCl).
Key Points
* The transfer of electrons is what defines ionic bonding.
* The resulting ions have full outer electron shells, making them more stable.
* The strong electrostatic attraction between the ions leads to a compound with a high melting point and high boiling point.
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