1. REVIEW OF THE ATOM term 4

2. ATOMIC STRUCTURE + electron orbit proton neutron

3. Definitions (refer to handout) Atom – small particles that make up everything around us (matter). Element – If a substance is made up of only one type of atom. Eg. Zinc, Oxygen, Copper. Compound – a substance that contains two or more different elements that are chemically combined. Eg. Copper Sulphate, Water. Mixture – a substance that contains two or more different substances that are not chemically combined. Proton – a positive charged object held within the nucleus of an atom. Neutron – an uncharged object held within the nucleus of an atom. Electron – a negatively charged object that is free to move around the nucleus.

4. Atomic Number – the number of protons in an atom. Mass Number – the number of protons and neutrons in an atom. Atomic Number – the average Mass Number of all the different isotopes of an element. Isotope – when two atoms have the same number of protons but a different number of neutrons (therefore a different mass number). Ion – an element or a compound, which takes on a charge due a variation between the number of protons and electrons, it possesses. Ionic Charge – the charge of an atom. Eg. Oxygen contains 8 protons and 10 electrons, therefore 8 positive charges and 10 negative charges, i.e. 2- charge. Definitions (refer to handout)

5. Question: Complete the following table ElementSymbolAtomic #Mass #ProtonsNeutron s Hydrogen 2 12 Fe 79

6. Answers: Complete the following table ElementSymbolAtomic #Mass #ProtonsNeutron s HydrogenH1110 HeliumHe2422 CarbonC61266 IronFe26562630 GoldAu7919779118

7. How do you find the Charge of an ion? If it is a Group A Element - 1A = 1+, 2A = 2+, 3A = 3+, 4A = ??, 5A = 3-, 6A = 2-, 7A = 1-, 8A = 0. (See Periodic Table)

8. Question: Complete the following table SymbolAtomic #ProtonsElectronsCharge H0 Na1110 F 2018

9. Answers: Complete the following table SymbolAtomic #ProtonsElectronsCharge H1101+ Na11 101+ F9910 Ca20 182+

10. Finding Chemical Formula’s When ions bond together, they donate or receive electrons so that the new substance will have no net charge! To do this the number of positive charges is equal to the number of negative charges, therefore cancelling each other out. Eg. Sodium + Chloride, Na + + Cl -  NaCl.

11. When balancing chemical formulas… 1. write the charge of each ion, 2. cross multiply, 3. simplify the ratio (if need be). Eg. Magnesium sulphide = Mg 2+ + S 2- = Mg 2 S 2 = Mg 1 S 1 = MgS

12. Question: Find the formula for the following compounds 1. Lithium bromide 2. Calcium flouride 3. Potassium oxide 4. Hydrogen sulphide 1. Li + + Br -  LiBr 2. Ca 2+ + F -  CaF 2 3. K + + O 2-  K 2 O 4. H + + S 2-  H 2 S

13. Ions Ions - are atoms or groups of atoms that have a positive or negative charge. Ions are formed when an atom gains or loses and electron. Cations - are ions, which have a positive charge (due to losing electrons) Anions - are ions, which have a negative charge (due to gaining electrons) Polyatomic ions - are groups of atoms that have a charge and act as a unit. Eg. SO 4 2- contains 1 Sulphur and 4 Oxygen atoms and carries a 2- charge. Diatomic elements - are two atoms of the same element bonded together. Eg. H 2, I 2, Br 2, Cl 2, O 2, N 2, Hg 2,

14. Questions: Determine the charge of each of the elements listed and identify if they are anions or cations 1. Zinc 2. Sulphur 3. Sodium 4. Potassium 5. Neon 6. Manganese (II) 7. Magnesium 8. Chlorine 9. Aluminium 10. Iron (III) 1. 2+, cation 2. 2-, anion 3. 1+, cation 4. 1+, cation 5. 0, neutral 6. 2+, cation 7. 2+, cation 8. 1-, anion 9. 3+, cation 10. 3+, cation

15. Questions 1. Fill in the table ChlorateSulphatePhosphateSulfite ClO 3 - Hydrogen Copper(II) Cu 2+ Cu(ClO 3 ) 2 magnesium Barium

16. Lesson Summary Several Definitions ( Atom, Element, Compound, Mixture, Proton, Neutron, Electron, Atomic Number, Mass Number, Atomic Number, Isotope, Ion, Ionic Charge, Cations, Anions, Polyatomic ions, Diatomic elements) Writing chemical formulas

17. Lesson 1 Homework Questions Name of CompoundIons InvolvedFormula Lead(II) nitratePb 2+, NO 3 - Pb (NO 3 ) 2 Zinc carbonate Barium chloride Potassium sulphate Silver oxide Sodium carbonate Copper(II) nitrate