“C1.1 Fundamentals of Chemistry”

1. “C1.1 Fundamentals of Chemistry” Ks4 Science Mr Powell 2013

2. P Definitions Match Up TASK: Logically compare these word to match the terms O O H H H H C N O O N O

3. P Knowing your terms... A • Think about the task you have just completed. Here are six groups of atoms to look at. Can you put a word(s) to describe the groups chemically from what you previously learned; • A) • B) • C) • D) • E) • F) B Elements or atoms Mixture of elements or atoms Compound Mixture of compounds Compound Mixture of elements C D F E

4. Periodic Table...

5. What do you know? • In your book write down all you know about these items..... • Gold • Group 1 Metals • Group 7 Non-metals • Structure of an Atom

6. C11.1 Atoms, Elements and Compounds (page 24)

7. The Periodic Table (Video First 15 mins) Student – “Self Assessed” • What is she panning for? (Gold) • Why is gold special? (It does not corrode) • What is the periodic table (a roadmap of all the elements) • Peter Atkins talks about the shiny ones on the left, what do we call these (metals) • What do we call the other side of the table (non-metals) • What is mercury used for? (thermometers / dental fillings) • What state is mercury in at room temperature (liquid) • Name a property of most metals (silvery grey/conduct electricity) • What do the transition metals show in the table (a history of the use of metals bronze, age, titanium) • How does the periodic table show similar elements? (in vertical groups) • Name a metal similar to lithium? (sodium, potassium etc..) • What properties of gold are useful in making the jewellery? (melts at a low temperature, is non-reactive.) • Why is carbon very useful? (it can form long chains such as DNA) • What are some metals are found as ores, how are they extracted (smelting – heating) • What happens with group 1 metals when they meet water (they react violently) • Why are the more reactive at the bottom of the group? (the outer electrons are shielded) • What can group 7 elements be used for? (chemical weapons – Cl reacts with water to form bleach) Score /17 ?????

8. I'm Sorry I Haven't got a Clue • Form into a small group of 3-4 people. One person is the “quizmaster” for a “round” Contestants have 30 seconds to talk about a topic without... • Hesitation • Repetition • Stalling • Talking rubbish off topic • Telling lies! • Other contestants can challenge and take the floor, the winner is the person who finishes the 30s and gets 2 points but you also get a 1 point for each correct challenge. • Talk about these topics.... • Gold • Group 1 Metals • Group 7 Non-metals • Structure of an Atom • Extension: others ideas from the worksheet!

9. Atomic Model – RECAP! We used to think that atoms weren't made up of smaller pieces. The word "atom" actually comes from a Greek word which means "can't be split up". Now we know that all atoms are actually made of the same 3 tiny particles; protons, electrons and neutrons. The protons are positive and the electrons are negative. Neutrons are neutral. Protons and neutrons are much heavier than electrons and they are found in the middle of the atom called the nucleus. The electrons are in orbit around the outside.

10. Quick Test.... Student – “Self Assessed” • Which particles are found in the nucleus of an atom? • Which particles orbit the nucleus? • Which atomic particle has a charge of +1? • Which atomic particle has no charge? • Which atomic particle has a charge of −1? • Two of the particles each have a mass of one atomic mass unit. The other has almost no mass. Which one has almost no mass? • protons and neutrons • electrons • proton • neutron • electron • electron

11. C1.1 Book Answers... Student – “Self Assessed” In text questions... about 100 Because you can combine them together in millions of different ways. Because an element may have different names in different languages. metals – barium (Ba), vanadium (V), mercury (Hg) non-metals – phosphorus (P), krypton (Kr) (Harder) Summary Questions 1 atoms, molecule, compounds, bonds 2 In a mixture, the different substances are not joined to each other by chemical bonds, but in a compound the atoms are held together tightly by chemical bonds – this makes them difficult to separate. (Harder)

12. S Atomic Model Recap Charge Neutral Electrons Protons Protons Nucleus Atomic Proton Nucleons Nucleus Mass Atomic Mass Write a-l in your book and write in the correct order for the words. A*-B – don’t use the word bank (9/12) C-D - Use the word bank to help you (6/12) Word BANK Nucleus, Mass, Protons, Charge, Proton ,Nucleons, Atomic, Atomic Mass, Protons, Nucleus, Neutral, Electrons

13. C11.2 Atomic Structure (page 26)

14. Modelling.... TASK: Can you create your own particle model for atoms, mixtures & compounds. Work as a team of 2 or 3. Draw some diagrams, then make some examples (S/H) Explain/ Discuss its strengths and weaknesses? (H) Extra Help... page 26

15. Ions.... TASK: Using the model you have made for an Atom can you now use it to show the following. Atoms have a small central nucleus, of protons and neutrons, surrounded by electrons. (L) The relative electrical charges are +1/-1/0 for proton, electron and neutron (S) Atoms have no overall electrical charge. (S) All atoms of a particular element have the same number of protons (Atomic Number). (L) The total mass (atomic mass) of an atom is the sum of the number of protons and neutrons. (S/H) Discuss your ideas in a small group then write down your findings on your sheet and share with others in your group and “Peer Assess”...

16. C1.2 Book Answers... Student – “Self Assessed” In text questions... protons, neutrons, electrons 8 electrons silicon They increase by 8 between each element. Summary Questions 1 neutrons, electrons, negative, atomic 2 Because protons and electrons have the same amount of charge but with opposite signs, the charge on a proton is exactly cancelled out by the charge on an electron. 3 a 7 protons, 7 electrons and 7 neutrons. (Harder) b 17 protons, 17 electrons and 18 neutrons. (Harder)

17. Homework – Revision! http://www.sporcle.com/games/g/elements

18. C11.3 The Arrangement of Electrons in Atoms (page 28)

19. Blind Date Do they Match – fill your sheet in? Chlorine, Cl 17, Group 7, with 7 outer electrons, makes PVC, corrosive, used in swimming pools, bleaches roses! Sodium, Na 11, Group 1, Alkali Metals, 1 electron in outer shell, reacts in water, releases hydrogen. Oxygen, O 8, Gives life! Group 6, 6 electrons in the outer shell, oxidises (burns) other elements. Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form MgO. Fluorine F 9, Group 7 missing 1 electron, reacts well with everyone, lights a cig on contact! Aluminium, Al 13, makes pans, Group 3, metal, reacts with bromine strongly. Lithium Li 3, Soft metal, shiny, very reactive, Group 1, kept in oil. Neon, Ne 10, Group 8, 8 electrons in outer shell, non-reactive, hangs about in ones!

20. Electronic Config…

21. Electronic Config…

22. C1.3 Book Answers... Student – “Self Assessed” In text questions... a Arranged around the nucleus in shells. b The energy level closest to the nucleus. c 2 d 2,8,6 (Harder) Summary Questions 1 nucleus, shells, energy, group, electrons 3 They both have full outer shells or energy levels of electrons/very stable arrangements of electrons.

23. Quick Check.... Student – “Self Assessed” A) For the following elements can you write down the electronic configuration.... For example.. Calcium is...... 2,8,8,2 Mg Al S Si K B) Can you draw the electronic configuration for Si and K (Harder) Answers Mg 2,8,2 Al 2,8,3 S 2,8,6 Si – 2,8,4 K – 2,8,8,1

24. Sodium, Na 11, Group 1, Alkali Metals, 1 electron in outer shell, reacts in water, releases hydrogen. Sodium, Na 11, Group 1, Alkali Metals, 1 electron in outer shell, reacts in water, releases hydrogen. Chlorine, Cl 17, Group 7, with 7 outer electrons, makes PVC, corrosive, used in swimming pools, bleaches roses! Chlorine, Cl 17, Group 7, with 7 outer electrons, makes PVC, corrosive, used in swimming pools, bleaches roses! Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form MgO. Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form MgO. Oxygen, O 8, Gives life! Group 8, 6 electrons in the outer shell, oxidises (burns) other elements. Oxygen, O 8, Gives life! Group 8, 6 electrons in the outer shell, oxidises (burns) other elements. Aluminium, Al 13, makes pans, Group 3, metal, reacts with bromine strongly. Aluminium, Al 13, makes pans, Group 3, metal, reacts with bromine strongly. Fluorine F 9, Group 7 missing 1 electron, reacts well with everyone, lights a cig on contact! Fluorine F 9, Group 7 missing 1 electron, reacts well with everyone, lights a cig on contact! Lithium Li 3, Soft metal, shiny, very reactive, Group 1, kept in oil. Lithium Li 3, Soft metal, shiny, very reactive, Group 1, kept in oil. Neon, Ne 10, Group 8, 8 electrons in outer shell, non-reactive, hangs about in ones! Neon, Ne 10, Group 8, 8 electrons in outer shell, non-reactive, hangs about in ones!

26. Reactions Review... • Atoms of which three elements are drawn above? • Write out the electronic configuration for all three? • What do they all have in common?

27. C11.4 Forming Bonds (page 30) – “Stealing” or “Sharing” OR?

28. Covalent Bonding – “Sharing” Look through the examples of covalent or “shared” bonded molecules from non-metals In your book draw out several examples to show how the electrons are configured before bonding and after bonding when electrons are shared.... More Examples... Chlorine Cl2 Ammonia NH3 Hydrogen H2 Hydrogen Chloride HCl Water H2O Oxygen O2 http://www.animatedscience.co.uk/ks4-covalent-bonding

30. Ionic Bonding “Stealing”

31. Ionic Bonding “Stealing” - Metals and non metals 1st Shell: 2 electrons 2nd Shell: 8 electrons 3rd Shell: 8 electrons Each shell has a maximum number of electrons that it can hold. In noble gases the shells are completely full rather than partially full…this is why they are so unreactive. During bonding other atoms try to attain the “full electron shell” structure of the noble gases.

32. Ionic Bonding “Stealing” Sodium atom Chlorine atom Sketch the atoms above and then consider… Both atoms would be more stable if they had full outer shells, what would be the simplest way for each atom to gain a full outer shell?

33. Ionic Bonding “Stealing” Sodium atom Chlorine atom Copy these ions Chloride ion Sodium ion -1 +1 Sodium ion Chlorine ion

34. Atoms have an equal number of protons and neutrons, so the charges cancel out. However after sodium has given an electron to chlorine, the electrons and protons in both atoms no longer balance: Sodium Chlorine 10 electrons 10- 18 electrons 18- 11 protons 11+ 17 protons 17+ 1+ 1- The atoms are now ions and are charged Na+ and Cl- Ionic Bonding... + - Na+ [2,8]+ Cl- [2,8,8]-

35. Draw diagrams to show the ions that would be formed when the following atoms are involved in ionic bonding. For each one state whether electrons have been lost or gained and show the charge on the ion. Aluminium (Al), Fluorine (F), Potassium (K), Oxygen (O) Ionic Bonding “Stealing” Learning Check.... Apply this skill to draw out these molecules using the square brackets KF AlF3 (Harder) Al2O3 (Harder) + Na+ [2,8]+

36. C1.4 Book Answers... Student – “Self Assessed” In text questions... a K+ b covalent bonds Summary Questions 1 positive, lose, gain, negative, attract, ionic, covalent, share 2 a Sodium fluoride b Na+ and F- cNaF

37. Progress Check... Write down the two key things we have learned about today, giving an example of each by... Diagram (Low Demand) Written Explanation (Standard Demand) Both linked in detail (High Demand) OR?

38. C11.5 Chemical Equations (page 32) • 2Na + Cl2 → 2NaCl

39. Balancing Equations.... Can you check the products and reactants and balance these equations... H2 + Br2 → HBr Na + Cl2 → NaCl CH4 + O2 → CO2 + H2O P + Cl2 → PCI3 CaCO3 → CO2 + CaO Fe + H2O → H2 + Fe3O4 (High Demand) • H2 + Br2 → 2HBr • 2Na + Cl2 → 2NaCl • CH4 + 2O2 → CO2 + 2H2O • 2P + 3Cl2 → 2PCl3 • CaCO3 → CO2 + CaO (already balanced) • 3Fe + 4H2O → 4H2 + Fe3O4

40. C1.5 Book Answers... Student – “Self Assessed” In text questions... a A lighted splint burns with a squeaky ‘pop’. b Reactant: calcium carbonate. Products: calcium oxide and carbon dioxide. c H2 + Cl2 → 2HCl Summary Questions 1 As no new atoms can be created or destroyed in a chemical reaction, the number and type of atoms in the reactants must equal the number and type of atoms in the products. 2 a 4.4 g b magnesium carbonate → magnesium oxide + carbon dioxide 3 a 2Ca + O2 → 2CaO b 4Al + 3O2 → 2Al2 O3 c 2Na + 2H2 O → 2NaOH + H2

41. Progress Check... Using an example of a reaction you have looked at today and page 33 in the book. “making an equation balance” Write a method of steps that you would employ to balance any other reaction you might be given Then swap with another person and test it out to see if it worked on all of these six. Check each reaction in turn, each one correct to the method gets 1 mark. • H2 + Br2 → 2HBr • 2Na + Cl2 → 2NaCl • CH4 + 2O2 → CO2 + 2H2O • 2P + 3Cl2 → 2PCl3 • CaCO3 → CO2 + CaO (already balanced) • 3Fe + 4H2O → 4H2 + Fe3O4 ? 6

42. Balancing Equations Extra Help.... Balancing Equations Extra Help.... Can you check the products and reactants and balance these equations... H2 + Br2 → HBr Na + Cl2 → NaCl CH4 + O2 → Can you check the products and reactants and balance these equations... H2 + Br2 → HBr Na + Cl2 → NaCl CH4 + O2 →