1. Chemistry

2. This is how the atom is made up Number of protons (in nucleus) Number of neutrons (in nucleus) Number of electrons (going around outside nucleus) Atomic Structure

3. This is the way the electrons are arranged in SHELLS 2 in first shell 8 in second shell 8 in third shell Remainder in fourth shell E.g. Calcium, Ca, is 2, 8, 8, 2. Electron Configuration

4. This is made up of Groups (vertical) and Rows (horizontal) Rows are which electron shell is being filled Groups are how many electrons are in the valance shell. Periodic table

5. Periodic Table

6. Ions have gained or lost electrons to get a FULL OUTER SHELL. They have a charge: A positive charge for each electron lost A negative charge for each electron gained Ions

7. This is where a positive ion is attracted to a negative ion, and they combine. The positive charges are balanced by the negative charges. Use the “swap and drop” method to write polyatomic ions. Polyatomic Ions

8. These are atoms which have gained or lost NEUTRONS An atom that has gained a neutron will gain mass An atom that has lost a neutron will lose mass Tell by the MASS NUMBER Isotopes

9. Atomic and Mass Numbers MASS NUMBER – this is the number of Protons + Neutrons ATOMIC NUMBER – this is the number of Protons

10. A reaction equation says the products and the reactants Reactants are the 2 things that you start with Products are the things that you end with Reactant 1 + Reactant 2 Product 1 + Product 2 Reaction equations

11. We write the reactants and products as words: E.g. Magnesium + oxygen Magnesium Oxide Word equations

12. Use the chemical symbols as the products and reactants. We balance these by adding numbers in front of the products and reactants so that there are the same number of atoms on both sides of the arrow. E.g. C 2 H 6 + 3 ½ O 2 2 CO 2 + 3 H 2 O Balanced chemical equations

13. There are 4 ways to change the rate of reaction 1.Temperature 2.Surface Area 3.Concentration 4.Catalyst Rates of Reaction (speed of the reaction)

14. There is a pH scale going from: 1 (acidic) to 7 (neutral) to 14 (basic) Universal indicator shows pH with a colour: red (acidic) to green(neutral) to blue/purple (basic) Acid – Base Reactions

15. Acids and bases react together and give/receive IONS Acids always give HYDROGEN Bases give (usually) Hydroxide or Carbonate. Acid – Base Reactions

16. This is an acid base reaction where the acid neutralises the base – and vice versa. Leaving pH around 7 Not all acid base reactions are neutralisation reactions. Neutralisation Reaction