3 rd Year Revision. (from second year: Conservation of Mass Acids, Alkalis and Indicators)

Transcription

1 3 rd Year Revision (from second year: Conservation of Mass Acids, Alkalis and Indicators)

2 To revise: Elements, compounds, mixtures. Periodic table names (eg groups, periods, transition metals, alkali metals, noble gases, halogens, alkali earth metals). Mass and Atomic Numbers. Building a nucleus rules (numbers of p and n). Building an atom rules. (numbers of p,n, and e). Electron arrangement (picture) and configuration( 2,8,8,2). Flame tests, (Lithium, Sodium, Potassium, Calcium, Copper, Barium). Counting Atoms. Balancing Equations. Naming Compounds (check your own examples)

3 Elements, compounds, mixtures. Give an example of each Periodic table names. Group Period Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble Gases Label each on the table

4 Mass and Atomic Numbers. Add the mass and atomic numbers for: Ca C F

5 Building a nucleus rules (numbers of p and n). How many protons and neutrons in: 41 Ca 14 C 18 F

6 Building an atom rules. (numbers of p,n, and e). Electron arrangement and configuration( 2,8,8,2). Draw the nucleus & electron arrangement for 17 O. Label the inner shell Label the outer shell Write the electron configuration

7 Flame tests Name the colours for: Lithium Sodium Potassium Calcium Copper Barium

8 Counting Atoms. Name and count the atoms in: NaCl MgCl 2 Li 2 CO 3 Be(OH) 2 H 2 SO 4 C 2 H 5 OH

9 Balancing Equations. Balance these (remember only add BIG numbers) H 2 + O 2 H 2 O NaOH + HCl NaCl + H 2 O H2 + N2 NH 3 Cr + O 2 Cr 2 O 3 NaClO 3 NaCl + O 2 C 3 H 8 + O 2 CO 2 + H 2 O

10 1. use the symbol for a reversible reaction I can 2. write a balanced word and symbol equation for heating hydrated copper sulfate. 3. explain what the. means 4. explain the heat energy changes when heating and rehydrating copper sulfate. 5. explain how anhydrous copper sulfate can be used to test for water. 6. write a balanced equation for thermal decomposition of ammonium chloride. 7. explain how we know that thermal decomposition of ammonium chloride is reversible. 8. use the names ammonium chloride, ammonia, and hydrogen chloride correctly, with correct state symbols. 9. explain how hydrogen chloride and hydrochloric acid are different. 10. use state symbols on symbol equations. 11. describe the changes observed when heating copper carbonate. 12. name the gas produced when copper carbonate thermally decomposes. 13. write a symbol and word equation, with state symbols, for the above reaction. 14. describe the test for and properties of the gas formed. 15. use correct terms to describe liquids (opaque, translucent, transparent, coloured, colourless) 16. if a liquid is opaque, use the term precipitate (eg white precipitate). 17. use a reactivity series to compare metals. 18. describe patterns from group 1 and 2 in the reactivity series. 19. describe displacement reactions as a fight over the salt ion. (eg the sulfate) 20. give an example of a displacement reaction that will happen. 21. give an example of a displacement reaction that will not happen. 22. use the reactivity series to predict which mixtures of metal salt solutions with metals will react and which will not. 23. explain why the blue colour reduces when copper sulphate solution reacts with magnesium. 24. write out enough displacement reactions to get them right every time. 25. use the term native to describe metals 26. describe the test for hydrogen gas (Squeaky pop with a LIT splint (not from this unit)

11 I can 1. Describe how to do a flame test, the colours you might see and the conclusions. 2. Describe how to sulfate test, the steps, the observations and conclusions. 3. Describe how to halide test, the steps, the observations and conclusions. 4. Use, a combination of flame-, sulfate- and halide- tests to conclude an exact name for a substance. 5. Describe how the solubility of different salts is tested, and which salts might be soluble. 6. Give the general equation of a neutralisation reaction. 7. Give examples of neutralisation word equations. 8. Describe how to use neutralisation to prepare a pure dry sample of Sodium Chloride. 9. Describe how to react copper oxide and sulfuric acid to prepare a pure dry sample of copper sulfate. 10. Draw graphs accurately (title, axis labels, axis units, line of best fit rules) 11. Describe patterns from graphs (correlation, proportion, gradient, intercept) 12. Give the symbol formulae for Nitric Acid, Hydrochloric acid and Sulfuric Acid.

12 Isotopes, Ions and Ionic Bonding What are isotopes? What are ions? How do atoms form ions? How do you draw ions? What happens if oppositely charged ions move close together? How do you draw two ions bonded together?