1. 04/24/2016 The Periodic Table Properties of the groups: Each group is like a family – they have similarities such as how they react and their appearance and state at room temperature.

2. These are in the centre of the periodic table 04/24/2016 Transition Metals

3. Common properties The transition metals have the following properties in common: -They form coloured compounds -They are good conductors of heat and electricity -They can be hammered or bent into shape easily -They are less reactive than alkali metals such as sodium -They have high melting points - but mercury is a liquid at room temperature -They are usually hard and tough -They have high densities 04/24/2016 Transition Metals

4. 04/24/2016 Metallic structure Structure- Positive ions in a sea of delocalised electrons

5. 04/24/2016 Malleability- they can be hammered into shape because rows of atoms can slide over each other. Transition Metals

6. 04/24/2016 Good conductors of electricity- Electrons are free to flow through metal and so transfer charge. Transition Metals

7. 7 The diagram shows the structure of a metal. Use the diagram to describe the structure of a metal and to explain why metals are malleable and conduct electricity. (6) Answer must include description of : Structure Malleability Conductivity 04/24/2016

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9. 04/24/16 Group 1 – The alkali metals Li Na K Rb Cs Fr Watch video of these metals reacting with water (from Sky One’s Brainiac)

10. 10 For example: Group 1 in the periodic table contains (1) A transition metals B noble gases C halogens D alkali metals 04/24/2016

11. 11 Melting and Boiling point Alkali metals have low melting and boiling points Hardness The alkali metals are very soft. Lithium is the hardest alkali metal and they become softer as you go down the group. Density The alkali metals have low densities compared to most other metals (they feel lighter). 04/24/2016 11

12. 12 lithium + water → lithium hydroxide + hydrogen 2Li(s) + 2H 2 O(l) → 2LiOH(aq) + H 2 (g) Reactions of alkali metals All alkali metals react vigorously with cold water. In each reaction, hydrogen gas is given off and the metal hydroxide is produced. The speed and violence of the reaction increases as you go down the group. This shows that the reactivity of the alkali metals increases as you go down group 1. 04/24/2016 potassium + water → potassium hydroxide + hydrogen 2K(s) + 2H 2 O(l) → 2KOH(aq) + H 2 (g)

13. (d) Potassium reacts with water. In a class demonstration, a teacher drops a piece of potassium on to water. (i) The teacher ties back her hair and wears a laboratory coat and goggles. Suggest another safety precaution that the teacher should take. (1)............................................................................. (ii) The word equation for this reaction is given below. Two of the state symbols have been given. Write the other two state symbols in the spaces provided. (2) potassium(s) + water (l) → potassium hydroxide(.........) + hydrogen(.........) (iii) Describe what you see when potassium is added to water. (2)............................................................................. (iv) Balance the equation for the reaction between potassium and water by putting numbers in the spaces provided. (2)......... K + 2H 2 O →......... KOH + H 2 (Total for Question is 11 marks) 04/24/2016 Now test your knowledge on Alkali Metals

14. 04/24/2016 Group 7 – The halogens F Cl Br I At

15. 04/24/2016 The Halogens - Chlorine Each molecule has a strong force holding the atoms together, but the forces between molecules are very weak so chlorine is a gas at room temperature and is pale yellow.

16. 04/24/2016 The Halogens - Bromine The forces between molecules are slightly stronger so bromine is a liquid at room temperature. It is reddish-brown in colour.

17. 04/24/2016 The Halogens - Iodine Iodine is a solid at room temperature but with gentle heating it will melt. The atoms will remain in pairs. In solid form iodine is grey like metal but gaseous iodine is purple.

18. 04/24/2016 The halogens – some reactions 1) Halogen + metal: Na + Cl - Na Cl + Halogen + metal metal halide sodium + chlorine → sodium chloride2Na(s) + Cl2(g) → 2NaCl(s)

19. 19 04/24/2016 19 2) Halogen + hydrogen: H Cl + H Halogen + hydrogen a hydrogen halide This can be dissolved in water to form an acid

20. 04/24/2016 Trends in Group 7 Colour The halogens become darker as you go down the group. Fluorine is very pale yellow, chlorine is yellow-green, and bromine is red-brown. Iodine crystals are shiny purple - but easily turn into a dark purple vapour when they are warmed up.

21. 21 1. Describe the appearance of bromine at room temperature and pressure. 2. Balance the equation for the reaction between sodium and chlorine to produce sodium chloride by putting numbers in the spaces provided.(2).................. Na + Cl2 →.................. NaCl 3. The table shows the appearance of bromine and iodine at room temperature. Complete the table to show the appearance of chlorine at room temperature. (2) 4. Chlorine reacts with hydrogen to form hydrogen chloride.Write the word equation for this reaction. (2)..................... +....................... →................................... 04/24/2016 Exam examples 21

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23. Displacement reactions To put it simply, a MORE reactive halogen will displace a LESS reactive halogen from a solution of its salt. F Cl Br I Decreasing reactivity Potassium chloride KCl (aq) Potassium bromide KBr (aq) Potassium iodide KI (aq) Chlorine Cl 2 Bromine Br 2 Iodine I 2

24. 04/24/201604/24/16 Group 0 – The Noble gases He Ne Ar Kr Xe Rn Common properties The noble gases have the following properties in common: They are non-metals They are very unreactive gases They are colourless They exist as single atoms (they are monatomic)

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27. 27 (b) Helium and argon are noble gases. (i) Choose the correct word from this box to complete the sentence below. (1) Argon can be used to put out fires because it is....................................................... (ii) Choose the correct phrase from this box to complete the sentence below. (1) Helium is used in airships because it....................................................... 04/24/2016

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