EXPECTATIONS

1. C1

2. EXPECTATIONS • Don’t talk when the teacher is talking • Respect others in the classroom • Ask questions if you are unsure • Complete all homework on time

3. Atoms and Elements Starter Draw what the particles in a solid, liquid and gas look like Understand the structure of atoms ALL – state what is meant by an atom MOST – Describe how elements are formed SOME – Explain where most of the mass in an atom is KEYWORDS: atom, element, periodic table

4. LO: understand the structure of atoms What is an atom? An atom is the smallest amount of a substance that you can possibly have In Y7 and Y8, you might have called atoms ‘particles’. However, the proper term for them is atoms

5. LO: understand the structure of atoms Elements A substance that is made of just one type of atom is called an element. There are over 100 different elements that have already been discovered and more are still being discovered now.

6. LO: understand the structure of atoms The Periodic Table The periodic table shows all the elements that have been discovered so far

7. LO: understand the structure of atoms Task Stick your periodic table into your books. Highlight the section that are metals, non-metals and metalloids

8. LO: understand the structure of atoms Spot-the-element! You will be given the name of an element. You must find the element on your periodic table and show where it is on the periodic table on the board before the person that you are up against…

9. LO: understand the structure of atoms Spot-the-element!

10. LO: understand the structure of atoms Representing elements • An element is represented using a symbol. This symbol is either one or two letters. The first letter is ALWAYS A CAPITAL.e.g. • Sodium = Na (not na) • Oxygen = O (not o) • Fluorine = F (not f) • Potassium = K • Iron = Fe • Mercury = Hg • Magnesium = Mg

11. LO: understand the structure of atoms Task • Work out what element symbols have been used to construct the words below. For each word, write down the word and the elements that been used to make it. • ClOSe • LiP • NiP • FUN • NeAr • PHONe • ScONe • WAr

12. LO: understand the structure of atoms Ernest Rutherford For a long time, scientists believed that there was nothing smaller than atom. It took a scientist called Ernest Rutherford to prove that atoms were, in fact, made of smaller particles themselves.

13. LO: understand the structure of atoms The structure of an atom • Rutherford shown that an atom is made up of three smaller particles: • Protons • Neutrons • Electrons

14. LO: understand the structure of atoms The structure of an atom Protons and neutrons are in the centre of the atom called the nucleus. The electrons orbit around the nucleus.

15. LO: understand the structure of atoms The structure of an atom In each atom, the number of protons will ALWAYS be the same as the number of electrons. This makes sure that the overall charge is zero.

16. LO: understand the structure of atoms The structure of an atom http://www.youtube.com/watch?v=hhbqIJZ8wCM

17. KNOWLEDGE CHECK C Start Timer State the three particles that make up an atom 10 Minutes 10 8 B What is the charge on each of the particles that make up an atom? 6 4 Explain why the number of protons and electrons is always the same for an atom A 2 0

18. The Periodic Table Understand how to interpret the periodic table ALL – state the definition of mass and atomic number MOST – Calculate the number of protons and electrons in an atom SOME – Draw electron sub-shell diagrams KEYWORDS: atom, element, periodic table

19. LO: understand how to interpret the periodic table The periodic table Closer inspection of the periodic table shows us that each element has two numbers next to it. What do these numbers represent?

20. LO: understand how to interpret the periodic table Atomic and Mass number Atomic number: This is the number of protons inside the nucleus of an atom Mass number: This is the number of protons + neutrons in the nucleus of an atom Which is which?

21. LO: understand how to interpret the periodic table Atomic and Mass number Atomic number: This is the number of protons inside the nucleus of an atom Mass number: This is the number of protons + neutrons in the nucleus of an atom

22. LO: understand how to interpret the periodic table Atomic and Mass number The Atomic number is ALWAYS the smaller number next to the element. The mass number is always the bigger number.

23. LO: understand how to interpret the periodic table Example 1 Calculate the following quantities for the element below Atomic number Mass number Number of protons Number of electrons Number of neutrons

24. LO: understand how to interpret the periodic table Example 2 Calculate the following quantities for the element below Atomic number Mass number Number of protons

25. LO: understand how to interpret the periodic table Example 3 Calculate the following quantities for the element below Atomic number Mass number Number of neutrons

26. LO: understand how to interpret the periodic table Task Use your periodic table to find the following quantities for: nitrogen, oxygen, iron, platinum, gold, lead, mercury, potassium, calcium, phosphorus, argon, xenon Atomic number Mass number Number of protons Number of electrons Number of neutrons

27. LO: understand how to interpret the periodic table True or false? Copy the true sentences and change the false sentences to make them true: Atoms are the smallest unit of matter Atoms are made up of three fundamental particle: protons, neutrons and smurfs Protons are positively charged, neutrons are negatively charged and electrons are neutral The number of protons and electrons in a neutral atom is the same The atomic number is the number of protons in the nucleus of an atom

28. LO: understand how to interpret the periodic table Electron shells Consider Calcium. Calcium has an atomic number of 20. How many electrons does it have? All of calcium’s 20 electrons can NOTfit in one orbit. Therefore, there must be multipleorbits for electrons to occupy

29. LO: understand how to interpret the periodic table Shell break down Atoms have 4 shells where electrons can live Shell 1 – 2 electrons Shell 2 – 8 electrons Shell 3 – 8 electrons Shell 4 – Whatever is left!

30. LO: understand how to interpret the periodic table Example 1 Draw the electron arrangement for sodium

31. LO: understand how to interpret the periodic table Example 2 Draw the electron arrangement for oxygen

32. LO: understand how to interpret the periodic table Example 3 Draw the electron arrangement for potassium. It has an atomic number of 12

33. LO: understand how to interpret the periodic table Example 4 Draw the electron arrangement for hydrogen. It has an atomic number of 1

34. LO: understand how to interpret the periodic table Task Complete the worksheet on drawing electron arrangements for atoms. Make sure you use crosses to represent the electrons and you remember how many electrons can go in each shell Stick the sheet in when you are done

35. LO: understand how to interpret the periodic table Mini-plenary Create a mind-map about everything that you have learnt about atoms, elements and the periodic table so far

36. LO: understand how to interpret the periodic table Electrons and Groups • Find the following elements on your periodic table and note what group these elements are in: • Sodium • Potassium • Argon • Neon • Magnesium • Aluminium • Sulpher • Now go to the sheet that you have filled in with electron arrangements. What do you notice about the groups and the number of electrons in the final shell?

37. LO: understand how to interpret the periodic table Electrons and Groups The number of electrons in the outer shell of an element is the same as the group that it is in. e.g. Group 1 elements ALL have 1 electron in their outer shell, Group 7 all have 7 in their outer shell etc. The elements in group 8 are called Noble gases. They have 8 electrons in their outer shell (except for helium, which has two) and are very unreactive.

38. LO: understand how to interpret the periodic table Task Complete the exam questions on atoms and elements

39. Chemical reactions To understand why chemical reactions occur ALL – State some everyday chemical reactions MOST – Construct word equations for chemical reactions SOME – Construct chemical equations for reactions Starter Think of as many chemical reactions that occur in everyday life KEYWORDS: combustion, products, Refine, harvest, electrolysis

40. Chemical Reactions

41. LO: understand why chemical reactions occur Chemical reactions When chemical reactions occur, the atoms join together to form compounds. This involves either giving/taking electrons, or sharing electrons.

42. LO: understand why chemical reactions occur Practical: Reacting magnesium Task: To react magnesium with oxygen Method: Take a small piece of magnesium Hold it with a pair of tongs Light the magnesium using the Bunsen burner Make sure you don’t look directly at the magnesium when it is alight

43. LO: understand why chemical reactions occur Chemical reactions We can represent chemical reactions using word and chemical reactions. For example, for the reaction that you have just done, we have the following equation:

44. LO: understand why chemical reactions occur Reacting with oxygen • When something reacts with oxygen, it always form an oxide. e.g. • Magnesium  Magnesium oxide • Sodium  Sodium oxide • Calcium  Calcium oxide • Potassium  Potassium oxide

45. LO: understand why chemical reactions occur Task • (i) Construct the word equations for the reactions of the following elements with oxygen • (ii) Construct the chemical equations for the reactions of the following elements with oxygen • (iii) Balance the chemical equations that you have made • Aluminium • Potassium • Sodium • Calcium • Beryllium • Iron • Lithium

46. LO: understand why chemical reactions occur Why do chemical reactions happen? When elements react together, they do so for a reason. They are trying to achieve a FULL OUTER ELECTRON SHELL. Consider the reaction that we have just done:

47. LO: understand why chemical reactions occur What happens once a compound is formed? What will the electron arrangements of the magnesium and oxygen be once they have reacted?

48. LO: understand why chemical reactions occur Ions When a metal and a non-metal react together, they will each form an ion. An ion is a charged particle. BOTH IONS NOW HAVE FULL OUTER SHELLS!

49. LO: understand why chemical reactions occur Task • Draw the electron arrangements for the following ions: • Cl- (Chloride ion) • Al3+ (Aluminium ion) • Fl- (Fluoride ion) • K+ (Potassium ion) • Li+ (Lithium ion) • Note that the metals always LOSE ELECTRONS and form +ve ions and non-metals always GAIN ELECTRONS and become –ve ions.

50. LO: understand why chemical reactions occur The Noble Gases The group 8 elements are also known as ‘Noble Gases’. These elements are very unreactive. Why do you think this is? They are unreactive as they already have a full outer shell. Therefore, they don’t need to try to gain/lose any electrons through reacting to get a full outer shell.