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Halogens

Halogens. In this presentation you will:. explore the chemical properties of the halogens. Next >. Introduction. Elements in group 17 of the periodic table are known as the halogens. The halogens are all non-metallic elements in the p block of the periodic table.

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Halogens

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  1. Halogens In this presentation you will: • explore the chemical properties of the halogens Next >

  2. Introduction Elements in group 17 of the periodic table are known as the halogens. The halogens are all non-metallic elements in the p block of the periodic table. All halogens require 1 electron to complete their outer p subshell. All the halogens are very reactive. Next >

  3. Introduction Container of fluorine gas, F2 Container of chlorine gas, Cl2 Container of iodine crystals, I2 Container of bromine liquid, Br2 Halogens all exist as diatomic molecules: F2, Cl2, Br2, I2 and At2. Fluorine and chlorine are gases, bromine is a liquid, and iodine and astatine (radioactive) are solids at standard temperature and pressure. Next >

  4. Reactivity of the Halogens Since all halogens have 5, out of a possible 6, electrons in their outer p shell, they will readily accept an extra electron to achieve a full subshell. 2s22p5 Halogens are not found naturally in the environment, due to their high reactivity. 3s23p5 They are found as ions and compounds. Next >

  5. Reactivity of the Halogens The name halogen was given to the group by Berzelius. It refers to the ability of the group to form a salt when it reacts with a metal. The reactivity decreases when moving down the group. Next >

  6. Question 1 Container of fluorine gas, F2 Container of chlorine gas, Cl2 Container of iodine crystals Container of bromine liquid, Br2 Which is the most reactive halogen? A) Fluorine B) Chlorine C) Bromine D) Iodine Next >

  7. Question 1 Container of fluorine gas, F2 Container of chlorine gas, Cl2 Container of iodine crystals Container of bromine liquid, Br2 Which is the most reactive halogen? A) Fluorine B) Chlorine C) Bromine D) Iodine Next >

  8. Reactions of the Halogens The halogens are all oxidizing agents. An oxidizing agent is an electron acceptor. Next >

  9. Reactions of the Halogens Reactions with Metals Halogens react easily with metals, particularly alkali and alkaline earth metals. 2Na(s) + F2(g) → 2NaF(s) Alkali metal + halogen → salt Mg(s) + Cl2(g) → MgCl2(s) Alkaline + halogen → salt Earth metal Fluorine, chlorine, bromine, and iodine, will even react with gold and platinum, that are normally considered as being very unreactive. 2Au(s)+3F2(g)→2AuF3(s) 2Au(s) + I2(g) → 2AuI(s) Pt(s) + 2Cl2(g) → PtCl4(s) Pt(s) + 2Br2(g) → PtBr4(s) These reactions will only happen at high temperatures. Next >

  10. Reactions of the Halogens Reactions with Non-metals Fluorine is very reactive. It will even react with glass in the presence of moisture. When it does react, it bonds so strongly that the resulting chemical is very inert. For example, teflon (the non-stick coating) is carbon bonded to fluorine. Next >

  11. Reactions of the Halogens Reactions with Non-metals Some of the reactions with non-metals can be complex. For example, chlorine can react with oxygen to form Cl2O7 (dichlorine heptoxide). Next >

  12. Reactions of the Halogens Reactions between Halogens Halogens can react with themselves. Example: 2KI(aq)+Cl2(aq)→2KCl(aq)+I2(aq) For example, iodine can react with chlorine to form iodine monochloride. Example: I2(s) + Cl2(g) → 2ICl(s) Next >

  13. Reactions of the Halogens Displacement of Halide Ions If aqueous solutions of the halogens are added to another halide salt in aqueous solution, then a displacement can occur. Chlorine can displace bromine and iodine. Bromine displaced by chlorine Iodine displaced by either chlorine or bromine Bromine can displace iodine. Iodine can displace neither bromine nor chlorine. Next >

  14. Question 2 Which equation correctly describes the reaction between sodium and chlorine that produces common salt? A) Na(s) +Cl(g) → NaCl(s) B) 2Na(s) +Cl2(g) → 2NaCl(s) C) 3Na(s) +Cl3(g) → 3NaCl(s) D) 4Na(s) +Cl4(g) → 4NaCl(s) Next >

  15. Question 2 Which equation correctly describes the reaction between sodium and chlorine that produces common salt? A) Na(s) +Cl(g) → NaCl(s) B) 2Na(s) +Cl2(g) → 2NaCl(s) C) 3Na(s) +Cl3(g) → 3NaCl(s) D) 4Na(s) +Cl4(g) → 4NaCl(s) Next >

  16. Uses of the Halogens Fluorine is used for non-stick surfaces and fluoride toothpastes. Chlorine compounds are used as disinfectants such as in swimming pools, and chlorine is a major constituent of bleach (sodium hyperchlorate). Most chlorine is used in plastics production – polyvinyl chloride (pvc). Next >

  17. Uses of the Halogens Bromine and iodine salts are light sensitive, so are much used in the production of photographic films and for X-ray pictures. Next >

  18. Summary In this presentation you have seen: • the chemical properties of the halogens End >

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