1. Unit 3 – The Periodic Table Review Game

2. State two properties of transition metals

3. High mp/bp, high density, coloured compounds, hard

4. Write a balanced chemical equation for the reaction of potassium with oxygen

5. 4 K + O2 → 2K2O

6. For the following reaction in aqueous reaction, write the equation and write down one observation that you would see a) the reaction of silver ions with iodide ions b) the reaction of potassium with water

7. Ag+ + I- → AgI yellow ppt (2 marks) 2 K + 2 H2O → H2 + 2 KOH bubbles, flame/fire (2 marks)

8. List two ways that metals differ from nonmetals

9. Metals Nonmetals good conductors non-conductors shiny (when polished) dull malleable brittle form positive ions form negative ions

10. Explain why neon is an unreactive monatomic gas

11. Neon has full valence energy level (with 8 electrons) so it has no need to form covalent bonds with other atoms (also it would take A LOT of energy for this to happen)

12. Write an ionic equation if chlorine water is added to a solution of sodium astatide. Assume that astatine is insoluble in water.

13. Cl2(aq) + 2 At-(aq) → 2 Cl-(aq) + At2 (s)

14. Explain why bromine displaces iodine from a solution of potassium iodide

15. Chlorine is a stronger oxidizing agent (that is, it can gain electrons more readily) than iodine. So, it can remove electrons from the iodide ion which results in the formation of chloride ions and iodine

16. State and explain which atom is larger: Na or Al

17. Na has a larger radius because even though both Al and Na have their valence electrons in the same energy level, it has a lower nuclear charge (11 protons in its nucleus vs 13 protons for Al). As a result, the attraction of the electrons is less so the electrons are not pulled as close to the nucleus (and the size of the atom is larger)