Ionic bonding

• Ionic bonding is a type of chemical bonding where electrons are completely transferred from one atom (typically a metal) to another atom (typically a non-metal). This transfer creates ions with opposite electrical charges that are attracted to each other.

  Key points:

  • Involves complete electron transfer
  • Occurs between metals and non-metals
  • Results in positively and negatively charged ions

  Example: When sodium (Na) and chlorine (Cl) react, sodium transfers an electron to chlorine, forming Na⁺ and Cl⁻ ions.
• Electron transfer is the core mechanism of ionic bonding. It happens because atoms want to achieve a stable electron configuration, typically matching the electron arrangement of noble gases.

  Key principles:

  • Metals tend to lose electrons
  • Non-metals tend to gain electrons
  • The goal is to reach a full outer shell (8 electrons)

  Example: Sodium (Na) has 1 electron in its outer shell. It wants to lose this electron to become like neon, creating a stable Na⁺ ion.
• Potassium (K) is a metal located on the left side of the periodic table. Metals typically lose electrons to achieve a stable configuration.

  
  

  
  

  Fluorine (F) is a non-metal located on the right side of the periodic table. Non-metals typically gain electrons to complete their outer shell.

  
  

  So in an ionic bond, fluorine is more likely to gain electrons, while potassium is more likely to lose electrons.
• Sodium (a metal) and chlorine (a non-metal) would be most likely to form an ionic compound.

  The key characteristics are:

  • Ionic compounds form between a metal and a non-metal
  • The metal will donate electrons to the non-metal
  • This creates positively and negatively charged ions that are attracted to each other

  Sodium and chlorine fit this pattern perfectly, as sodium can donate an electron to chlorine, forming the stable ionic compound sodium chloride (NaCl).
• Ionic lattices are the three-dimensional arrangement of ions in an ionic compound.

  Key points:

  • Ions are arranged in a repeating, geometric pattern
  • Each ion is surrounded by multiple opposite-charged ions
  • Creates a strong, rigid structure
  • Extends in all directions like a 3D crystal grid

  Example: In sodium chloride (NaCl), each sodium ion is surrounded by six chloride ions, and each chloride ion is surrounded by six sodium ions, creating a cube-like structure.
• The ions in an ionic lattice are held firmly in their fixed positions due to the strong electrostatic attractions between the oppositely charged ions.

  
  

  The positive metal ions are attracted to the negative non-metal ions, creating a rigid, crystalline structure.

  
  

  This electrostatic force is what gives ionic compounds their characteristic properties, like high melting/boiling points and brittleness.
• When ionic compounds like sodium chloride (NaCl) are dissolved in water, the ions (Na⁺ and Cl⁻) become free to move around independently.

  
  

  This allows them to carry an electrical charge, making the solution conductive.

  
  

  The high mobility of the separated ions is what gives ionic compounds the ability to conduct electricity when dissolved or melted.
• Ionic compounds form crystalline structures, due to the arrangement of ions in a regular, repeating pattern

  
  

  They have high melting and boiling points, because of the strong ionic bonds that require significant energy to be broken

  
  

  Ionic compounds can conduct electricity when melted or dissolved in water as the ions are free to move.
• Ions form when an atom loses or gains electrons to gain a stable electronic configuration.

  
  

  Metals form positive ions by losing electrons, while non-metals form negative ions by gaining electrons
• The transfer of electrons during ionic bonding leads to a more stable electron configuration for both ions

  
  

  Stable electron configurations are often achieved when an atom has a full outermost energy level

  
  

  This stability explains why elements tend to form ions in the first place, contributing to the formation of ionic compounds.
• ELECTROSTATIC ATTRACTION:

  The force experienced by oppositely charged particles. It holds the particles strongly together