• Halogens react with metals by accepting an electron from the metal atom to become an ion with 1- charge

Eg.? ?Ca (s) + Cl2?(g) → CaCl2?(s)??consisting of?Ca2+?and?2Cl-?ions

• Halogens are therefore?oxidising agents:
  • Halogens?oxidise?the metal by removing an electron from the metal (the oxidation number of the metal increases)
  • Halogens become?reduced?as they gain an extra electron from the metal atom (the oxidation number of the halogen decreases)

   

• The?oxidising power?of the halogens?decreases?going?down the group?(the halogens get less reactive)
• This can be explained by looking at their electronegativities:

The electronegativity of the halogens decreases going down the group

• The?electronegativity?of an atom refers to how strongly it attracts electrons towards itself in a covalent bond
• The decrease in electronegativity is linked to the size of the halogens
• Going down the group, the atomic radii of the elements increase which means that the outer shells get further away from the nucleus
• An ‘incoming’ electron will therefore experience more?shielding?from the attraction of the positive nuclear charge
• The halogens’ ability to accept an electron (their?oxidising power) therefore decreases going down the group

With increasing atomic size of the halogens (going down the group) their electronegativity, and therefore oxidising power, decreases

• The reactivity of halogens is also shown by their?displacement?reactions?with other halide ions in solutions
• A?more?reactive?halogen can displace a?less reactive?halogen from a halide solution of the less reactive halogen
  • Eg. The addition of chlorine water to a solution of bromine water:

   

Cl2?(aq) + 2NaBr (aq) → 2NaCl (aq) + Br2?(aq)

• • The chlorine has displaced the bromine from solution as it is more reactive which can be summarised in the following ionic equation:

Cl2?(aq) + 2Br-?(aq) → 2Cl-?(aq) + Br2?(aq)

• Halogens react with hydrogen gas to form?hydrogen halides
• Due to the decrease in reactivity of the halogens going down the group, the reactions between halogen and hydrogen gas become less vigorous
• The table below shows a summary of the reaction between the halogen and hydrogen gas

Reaction between Halogen & Hydrogen Gas

• Thermal stability?refers to how well a substance can resist breaking down when heated
  • A substance that is thermally stable will break down only at high temperatures

   

• The hydrogen halides formed from the reaction of halogen and hydrogen gas decrease in?thermal?stability?going down the group
• The decrease in thermal stability can be explained by looking at the bond energies of the hydrogen-halogen bond
  • Going down the group, the atomic radius of the halogens increases
  • The overlap of its outer shell with a hydrogen atom therefore gives a longer bond length
  • The longer the bond, the weaker it is, and the less energy required to break it

   

• As the bonds get weaker, the hydrogen halogens become less stable to heat going down the group

The thermal stability of the hydrogen halide decreases going down the group as their bonds become weaker due to the increased atomic radius of the halogens

• Halide ions can also act as?reducing agents?and donate electrons to another atom
• The halide ions themselves get?oxidised?and lose electrons
• The?reducing power?of the halide ions?increases?going down the group
• This trend can be explained by looking at the ionic radii of the halide ions

The diagram shows that going down the group the ionic radii of the halide ions increases

• Going down the group, the halide ions become?larger
• The outermost electrons get further away from the nucleus
• The outermost electrons also experience more?shielding?by inner electrons
• As a result of this, the outermost electrons are held?less?tightly?to the positively charged nucleus
• Therefore, the halide ions lose electrons more easily going down the group and their?reducing power?increases

The reducing power of the halide ions increases going down the group