1. They have low meting and boiling points. The atoms within each molecule are held together by strong covalent bonds, but the forces between the molecules ( Van der Waals forces) are very weak. THE HALOGENS WHY?

2. Physical Properties of HALOGENS How does the colour change down the group? How does the state change down the group? What does that imply about the melting and boiling point down the group? Make a guess how At would look like (the colour, state and melting point)?

3. Physical Properties of HALOGENS ElementMelting Point ( o C) Boiling Point ( o C) ColourState at room temp Flourine-220-189ColourlessGas Chlorine-101-35Yellow- greenish Gas Bromine-759Reddish- brown Liquid Iodine114184Purpleish- black Solid Astatine300337Blacksolid

4. Halogens in Hexane & Water When halogens undergo a physical change of moving from a water solvent to a hexane solvent, they change color. Halogens are nonpolar, so they are not very soluble in water (which is polar) Halogens are very soluble in hexane (which is nonpolar) When X 2 (aq) is mixed (shook!!) with hexane, the X 2 moves out of the water solvent and into the hexane solvent if possible (and also changes color)

5. Ns 2 np 5 Ionic or covalent bond with oxidation state –1 or +1 (F shows –1 only) Except F, all other halogens can expand their octet byusing the low-lying, vacant d-orbitals to form bonding. Their oxidation states range from –1 to +7. Bonding and Oxidation State   ns np nd (+3 states)  HClO 2, ClO 2 -   ns np nd (0, +1, -1 states) Cl 2, Cl -, OCl 2

6. Cl 2 (g) + NaOH(aq)  NaOCl(aq) + NaCl(aq) Oxidation Cl in NaCl Oxidation Cl in NaOCl Chlorines Disproportionation in Water The disproportion reaction produces the strong acid HCl(aq) and weak hypochlorous acid HOCl(aq): Cl 2 (aq) + H 2 O(l)  HCl(aq) + HOCl(aq) Oxidation Cl in HCl Oxidation Cl in HOCl What would you expect to happen if this reaction were monitored using a pH meter and explain why this is? Disproportionation +1 +1

7. Be able to apply knowledge of hydrogen bonding to HF properties Be able to explain the precipitation reactions of silver halides Be familiar with the use of silver halides in photography Objectives: Group 7 Halogens Part II

8. Bonding in HF

9. Why is the HF Boiling point so high? Flourine is the smallest of all group 7 elements in the periodic table. It is the most charge dense of the halogens because it is the smallest in size with the least electron shells. Flourine is highly electronegative Flourine can only take the -1 oxidation state because it has no near-by d-orbitals to promote extra electrons to. Hydrogen bonding is a stronger intermolecular force than permanent dipole attractions or Van der Waals forces. Hydrogen bonding only occurs between a hydrogen atom and an electronegative atom e.g. F, N or O Strong hydrogen bonding causes strong forces between molecules raising their boiling point. A A B B C C D D E E F F G G

10. Acidity of HF Explanation of weak acid strength of HF: HF has the greatest bond dissociation energy and exceptionally small electron affinity. It has the least exothermic  H (dissociation enthalpy) Due to formation of strong hydrogen bond HF has the smallest decrease of dissociation.

11. Halogen Reactivity Electronegativity: Electron Affinity: When halogens react with another substance, they become negative ions, as they are gaining an extra electron. These compounds are HALIDES. Once it has reacted – instead of ending with ‘–ine’, they end with ‘-ide’. HalogenHalidereaction fluoride (F - ) chloride (Cl - ) bromide (Br - ) iodide (I - ) (F) (Cl) (Br) (I) ElementEN value F4.0 Cl3.0 Br2.8 I2.5 Generally high electron affinity. All are exothermic. X(g) + e -  X - (aq) ElementEA kJ/mol F-348 Cl-364 Br-342 I-285

12. A test for Halide Ions…. AddAg + (aq)Silver Nitrate Ag + (aq) + Cl - (aq)  AgCl(s), white precipitate Ag + (aq) + Br - (aq)  AgBr(s), pale yellow precipitate Ag + (aq) + I - (aq)  AgI(s), yellow precipitate As a further test try the precipitates solubility in ammonia. When working with concentrated ammonia take your test tube to the fume hood. Use the concentrated NH 3 in the fume hood and dispose of the test tube contents in the fume hood sink!!!

13. Expected Results: Halides + Ag + (aq)

14. Electron ejected from chlorine (Oxidation): Ag+ + Cl- + light energy → Ag+ + Cl + 1 electron Electron captured by silver (Reduction): Ag+ + 1 electron → Ag (metal) When silver metal is produced as a result of the electron capture, it forms a dark image on film. Ag+ has been reduced to Ag (metal), and Cl- has been oxidised. Silver Chloride and Photos

15. 1.-1, +1, +3, +5, +7 2.Electron affinity decreases as you go down the group 3.Br 2(l) + H 2 O (l)  HBr(aq) + H0Br(aq) 4.Cl 2(g) + 2Br -(aq)  2Cl - (aq) + Br 2(aq) 5.Disproportionation 6.There is much more hydrogen bonding in HF than in the other hydrogen halides 7.HCl 8.The H-X bond energy 9.HI – Most readily donates electrons most displaced 10.F 2 - oxidisingagent accepts - electrons Test Answers