Group 17 (Halogens)

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  • Created by: OxSarah
  • Created on: 01-05-15 12:50
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  • Group 17 (Halogens)
    • Fluorine (F)
    • Chlorine (Cl)
    • Bromine (Br)
    • Iodine (I)
    • Astatine (At)
    • Non-metals
      • Outer principal quantum shell : 7 electrons
        • E.C : ns2-np5
      • Their colours get darker going down the group
  • Outer principal quantum shell : 7 electrons
    • E.C : ns2-np5
  • Diatomic (made up of two atoms) molecules at room temperature
    • Single covalent bond between the two atoms in each molecule
      • Simple molecular structure
        • Weak Van der Waals' forces between molecules
          • Melting and Boiling points increase as you go down the group
            • Increase in the atomic size
              • More electrons
                • The larger the molecules the stronger the Van Der Waals' forces between them
                  • Volatility (the ease with which elements evaporate) decreases as you go down the group
              • Reactivity (most reactive non-metals) decreases
                • The atomic radius increases
                  • Low attraction between the nucleus and the outer electrons
                    • an electron is less easily gained
                • Electronegativity decreases
                  • less electron 'pulling'
                • Reactions with
                  • Metals
                    • One electron is gained and the atom becomes an ion with a 1- charge
                      • Halide ion
                        • A halogen ion bearing a negative charge
                        • presents in all ionic halide salts
                  • Non-metals
                    • A halogen atom shares a pair of electrons with the other non-metal atom in a covalent bond
                      • Halide
                        • Binary compound of which one part is
                          • Halogen atom
                          • Element less electronegative than the halogen
                • Can also be judged by looking at DISPLACEMENT REACTIONS
                  • may take place when a reactive element comes into contact with the compound of a less reactive element
                    • the less reactive element is removed from the compound
                      • and replaced by the more reactive element
                    • No reaction if the element which is meant to be displaced results more reactive
                  • A more reactive halogen can displace a less reactive halogen from a halide solution of the less reactive halogen
              • Ionisation energy decreases
                • More electrons=more energy levels
    • Group 17 (Halogens)
      • Fluorine (F)
      • Chlorine (Cl)
      • Bromine (Br)
      • Iodine (I)
      • Astatine (At)
      • Non-metals
        • Their colours get darker going down the group

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