Halogens trends

• Group VII elements

  • MOST reactive non metal
• Halogens

  Group VII elements
• Halogens are Highly reactive.
• Smaller atoms gain electrons more easily
• Halogens form diatomic covalent molecules
• Characteristics of halogens

  • Low melting and boiling points
  • More soluble in non-polar solvents
  • Non-electrolytes
  • Exist as gases at room temp / liquids / solids
• Substances that accept electrons

  Oxidising agents
• Halogens readily accept electrons from substances they react with
• The ability of the halogens to attract electrons

  Decreases down the group (ease of ionisation)
• When halogens act as oxidising agents


  1. Coloured halogens are changed to colourless halide ions

  2. Halogen reacted with metals to form a 1- ion changing the name to (ide)
• The first ionization energy is the amount of energy required to remove one electron from an atom or molecule.
• Ionization energies increase across periods due to increasing nuclear charge, which attracts electrons more strongly.
• Ionization energies decrease down groups because there are more shells available for electrons to be removed.
• Electronegativity increases across periods due to increasing attraction between nucleus and valence shell electrons.
• $X2+$$2ky -->2kX +$$Y2$


  Displacement reaction (The switch) y and X switch

  
• Halide ion

  A negatively charged ion formed when a halogen gains an extra electron and changes its name to ide by replacing the "-ine" ending with "-ide."
• Halogens

  Elements in Group 7 of the periodic table, which includes fluorine, chlorine, bromine, iodine, and astatine.