1. What are the two equations used to calculate rates? Rate of reaction = amount of reactant used Time And Rate of reaction = C2 REVISION – Section C2.4.1 – Rates of Reaction In terms of particles how does increasing temperature effect the rate of reaction? Chemical reactions can only happen when what type of collisions occur between particles? _______________________ How does a catalyst effect the rate of reaction? In terms of particles how does increasing the surface area effect the rate of reaction? In terms of particles how does increasing the pressure effect the rate of reaction? In terms of particles how does increasing the concentration effect the rate of reaction? Rate Graphs: Draw a line to show what the curve would look like if the temperature of the acid was increased. How much CO2 was produced in 1.5 mins? After how long did the reaction finish?

2. Which elements are mostly used to make catalysts? What are the problems with using these elements? C2 REVISION – Section C2.4.1 – Rates of Reaction and Energy Nano particles are very small and have a large surface area – volume ratio this makes them good catalysts. Are catalysts used up in chemical reactions? Are catalysts specific to reactions? Example of a catalyst: Platinum catalysts are often used in cars as catalytic converters. They are expensive and they escape over time meaning they need to be replaced. New catalysts are being developed. Give two reasons why scientists may want to use other substances for the reaction instead of platinum? C2 REVISION – Section C2.5.1- Exothermic and Endothermic Reaction What can happen to energy during chemical reactions? What is the difference between an endothermic and exothermic reaction? Give an example of a reversible reaction: If the reaction was endothermic in a forwards direction what type of reaction would it be in the reverse direction?

3. Draw a DIAGRAM to represent the bonding in Magnesium Oxide C2 REVISION – Section C2.1.1 – Structure and Bonding Explain why metals have high melting points, are malleable and can conduct electricity. (consider their structure and bonding). What is a covalent bond? How does Fluorine form a fluoride ion? Explain why water has a low melting and boiling point. (you should include details of the bonding). Give some examples of uses of fullerenes. Which atom are fullerenes made from. Describe its structure. Draw a diagram to represent the bonding in Ammonia (NH 3 ) Explain why ionic compounds are able to conduct electricity when molten or in solution. Below are diagrams of some macromolecules. Use your knowledge of bonding to explain: Why diamond is hard and used as cutting tools. Why all three structures have high melting points. Why graphite is used in the leads of pencils and as electrodes in electrolysis.

4. Draw a DIAGRAM to show the structures of thermosetting and thermo softening polymers. C2 REVISION – Section C2.1.1 – Structure and Bonding Explain what properties of nano particles make them suitable for uses as catalysts, coatings etc? How large are nanostructures? What is an alloy? Draw a diagram and explain why alloys have different properties to pure metals. Define the term ‘shape memory alloy’ What effects the properties of polymers? Polymers: What does LD and HD polymers stand for? Tennis balls normally have to be replaced because air slowly escapes effecting the ‘bounce’. Scientists have used new naonparticles to coat the tennis balls. Using your knowledge of nano particles explain why the new tennis balls are better for the environment.

5. What is the general equations for: Acid + Alkali  Salt + Water C2 REVISION – Section C2.5.1 – Ions in Solutions In terms of particles how does increasing temperature effect the rate of reaction? What ions are found in acids? What ions are in alkalis? What is the half equation for the neutralisation of an acid and alkali? Name some common acids and alkalis and their symbol formulae. Describe how and why some metals are electroplated. Explain why Hydrogen would come off at the negative electrode (cathode) in the electrolysis of Potassium Iodide solution. Describe the method for the formation of a salt from a base, acid reaction. Consider the method and the equipment you would use. Draw an example of the following electrolysis cells: 1.Molten Lead Bromide. 1.Half equation at (+ anode) 2.Half equation at (- cathode) 1.Aqueous Sodium Chloride (Brine) 1.Half equation at (+ anode) 2.Half equation at (- cathode)

6. C2 REVISION – Section C2.5.1 – Ions in Solutions Name some common acids and alkalis and their symbol formulae. Draw an diagram to show how aluminium oxide is electrolysed. Write the half equations for the half equation at the positive (anode) electrode and the negative electrode (cathode). State why cryolite is added to aluminium oxide.

7. A mole is the chemical name for 6.02x10 23 atoms of a substance. 1 mole of any atom has the same mass in g as its mass number e.g. 1 mole of Carbon = 12g Draw the triangle used to calculate moles. C2 REVISION – Section C2.3.1 Calculations Write the formula for calculating the percentage of an element in a compound. Calculate the Mr and Ar for the following: H 2 CO 2 K Al 2 O 3 Calculate the percentage of Aluminium in Aluminium Oxide (Al 2 O 3 ) A student produced some sodium chloride using 2 different methods. 1.2Na + Cl 2  2NaCl 2.2Na + 2HCl  2 NaCl + H 2 Calculate the atom economy of these reactions for the formation of NaCl. A Hydrocarbon is made up of 72g of C and 2g of Hydrogen. What is the empirical formula of this compound? Unknown Amount of substance (Theoretical yield) Calculate the mass of CO 2 produced from 30g of Methane (CH 4 ) burned in Oxygen. CH 4 + 2O 2  CO 2 + 2H 2 O In reality only 70g was produced. What is the percentage yield. Why is it unlikely that a 100% yield can be produced?