period 7

• Colours and states?


  F2- pale yellow gas- Cl2- pale green gas, Br- brown liquid and I2- grey solid
• b.p and EN?


  b.p increases down the group VDW increase. EN decreases down the group- more shielding so harder to attract electrons.
• Displacement?


  displaces the one below it. Cl- Br (orange solution) & I. Br- I (brown solid).
• chlorine?


  kill bacteria- stop algae growth. Cl toxic when inhaled, liquid chlorine can cause severe burns.
• Chlorine + H2o?


  Cl2 + H20 --> ClO- + Cl- + 2H+
• reducing power?


  reducing power increases down- reducing agent it gets oxidised to the larger the atomic radius the easier to lose an electron.
• hallide + sulphuric -> hydrogen hallide? chlorine?

  Nacl + h2so4 --> NaHso4 + HCl
• Hbr + Bromine?


  2HBr + H2so4 --> So2 + 2H2o + Br2 ( Br stronger reducing agent so reduces sulphuric acid to so2 ) of state of S: +6 --> +4
• HI + suphuric acid?

  6HI + h2so4 --> 3I2 + 2h2s+ 2h2o Iodine strongest reducing agent. Sulphur oxidation: +6 -->+2 I: -6--> 0
• iodine to idodie- half equation?

  2I- --> I2 + 2e
• sulphuric acid to sufur?

  H2o4 + 6h+ 6I- --> S2 + 3I2 + 4H2O
• chlorine + H20?

  Cl2 + H2o --> ClO + HClO
• displacement half equation?

  Cl2 + 2Br- --> 2Cl- + br2