2. 12 3 6 9 11 10 8 7 1 2 4 5 10 s 1 min 20 s 30 s 40 s 50 s 10 s 2 min 20 s 30 s 40 s 50 s 10 s 3 min 20 s 30 s 40 s 50 s 10 s 4 min 20 s 30 s 40 s 50 s 10 s 5 min 20 s 30 s 40 s 50 s 10 s 6 min 20 s 30 s 40 s 50 s 10 s 7 min 20 s 30 s 40 s 50 s 10 s 8 min 20 s 30 s 40 s 50 s 10 s 9 min 20 s 30 s 40 s 50 s 10 s 10 min 20 s 30 s 40 s 50 s Settler: Why is helium used in air balloons? C2 independent study task. Challenge: What happens to noble gases when you pass electricity through them?

3. C2.1 – Mendeleev and the periodic table C2.2 – Ionic compounds C2.3 – Covalent compounds C2.4 – Groups in the periodic table C2.5 – Rates of reaction Choose your own tasks Answer all the questions and then get a lead learner near you to check your answers with red pen. Choose your own tasks Answer all the questions and then get a lead learner near you to check your answers with red pen. C2.6 – quantitative chemistry

4. C2.1 – Mendeleev and the periodic table 1) What was special about Mendeleev’s periodic table. 2) What is the relationship between proton number and electron number 3) How is neutron number calculated? 4) Describe the structure of an atom 5) What is formed when an atom loses or gains an electron? 6) What does group number tell us about an atom? 7) What does period number tell us about an atom? 8) What is an isotope? 9) 25% of chlorine is Cl-37 and 75% is Cl- 35. What is the relative atomic mass (Ar)

5. C2.2 – Ionic bonding 1) Describe what ionic bonding is. 2) Draw an ionic lattice 3) Draw the ionic bonding in sodium chloride 4) Draw and explain the ionic bonding in sodium oxide. 5) List the flame tests results for K +, Na + Cu 2+ and Cu 2+ 6) Describe the test for Cl – ions. 7) Describe the test for sulfate ions. 9) Describe the barium meal test 8)Describe the test for carbonate ions.

6. C2.3 – Covalent bonding 1) What is covalent bonding? 2) Draw the covalent bonding in hydrogen chloride 3) Draw the covalent bonding in carbon dioxide 4) Compare the properties of ionic compounds to covalent compounds 5) Give the uses of diamond and link them to its properties 6) Give the uses of graphite and link them to its properties 7) Compare the properties of simple covalent compounds to giant covalent compounds 9) Why do giant covalent substances have high melting and boiling points? 8) What does the term ‘delocalised electrons ‘ mean?

7. C2.4 – Groups of the periodic table 1)Describe the reactions of Li and K with water. Give balanced symbol equations 1)Describe the reactions of Li and K with water. Give balanced symbol equations 2) Explain the reactivity in group 1 3)Explain the reactivity in group 7 What is displacement? 3)Explain the reactivity in group 7 What is displacement? 4) Explain what would happen when chlorine is added to potassium iodide. Add balanced symbol equations. 4) Explain what would happen when chlorine is added to potassium iodide. Add balanced symbol equations. 5) Describe the properties and uses of transition metals 6) Draw metallic bonding. 7) Why are noble gases inert? 9) Describe what happens to atomic radius and nuclear attraction as we go down each group 8) Give the uses of helium and argon and link them to their properties.

8. C2.5 – Rates of reaction 1) Explain how an increase in temperature affects rate of reaction? 2) Explain how an increase in concentration affects rate of reaction? 3) Explain how use of a catalyst affects rate of reaction? 4) Explain how surface area affects rate of reaction? 5) Describe what an exothermic reaction is with 2 examples. 6) Describe what an endothermic reaction is with 2 examples. 7) Draw an energy level diagram for an exothermic reaction 8) Draw an energy level diagram for an exothermic reaction 9) If the number of reactants is doubled in a chemical reaction, what will happen to the amount of products?

9. C2.6 – Quantitative chemistry 1)How are number of moles calculated? How many moles are there in 238g of potassium? 1)How are number of moles calculated? How many moles are there in 238g of potassium? 2) What is the relative formula mass of Mg(OH) 2 3) What is the % of Cl in CaCl 2 4) 1.35g of aluminium was heated in oxygen until there was no further gain in weight. The white oxide ash formed weighed 2.55g. Deduce the empirical formula of aluminium oxide. 5) Na 2 S(aq) + AgNO 3 (aq) → Ag 2 S(s) + NaNO 3 (aq) How many grams of Ag 2 S can be produced from 7.88 grams of AgNO 3 and excess Na 2 S? 6) What is theoretical yield? 7) Describe what makes a chemical reaction ‘good’. 8) Describe why percentage yield is never 100%? 9) The theoretical yield of a reaction is 9.5g but the actual yield was 4.7g. What is the % yield?

10. Review Did going through this type of task help you? How? Did going through this type of task help you? How?