Exploring Matter & Chemical Reactions: Atom Structures, Periodic Table, and Bonding

1. Year 10 Matter, matters. Chemical reactions.

2. SLO’s • Explain that all matter is made up of atoms in different arrangements. • Describe the properties of solids, liquids and gases. • Define an element. • List the names and symbols of the 1st 20 elements in the correct order. • Draw a simple model of an atom, showing the location of protons, neutrons and electrons. • Use atomic and mass numbers to work out the numbers of protons, neutrons and electrons in an atom. • Define an ion. • Describe where groups such as metals, non-metals, noble gases, etc. are found on the Periodic Table. • Work out the ion an element will form from its electron arrangement. • Define a compound. • Given a table of ions, write formulae for simple ionic compounds. • Describe what occurs during a chemical reaction. • Write chemical equations for simple reactions and balance them. • Use physical and chemical properties to discriminate between compounds and mixtures. • Give appropriate safety measures for the storage and use household chemicals. • Link the use of different packaging materials to their physical and chemical properties.

3. Rātū te whitu Hui-tanguru. • Welcome back! • Learning outcomes for the topic. • Key words. • What is matter? • Review states of matter. • Hmwk; KW 15

4. Matter? • Matter is simply what the universe is made of; atoms, subatomic particles, dark matter (and goodness knows what else). • This year will focus on atoms and their subatomic particles.

6. Matter has 3 states. • Matter comes in 3 main states; solid, liquid and gas. • From last year you will remember, the state depends on how close together the atoms are and how much kinetic energy they have. • Solid; close together, low kE. • Liquid; further apart, some kE. • Gas; really far apart, lots of kE. • Song

7. Solid Liquid Gas Fixed shape Fixed volume Particle held together tightly Low Ek No shape Fixed volume Slight compression Particle held together weakly Moderate Ek No fixed shape No fixed volume Large compression Particle’s not held together High Ek

8. Matter can change states. Re

9. Rāapa te waru Hui-tanguru. • QQ; KW 1  5 • Periodic table patterns. • Atomic structure and the 2,8,8 rule. • Shell diagrams. • Hmwk; KW 6  10, Ex 14.08

10. Elements. • An element is an atom with a set number of protons. They are found on the periodic table of the elements.

11. Key Alkali metals Transition metals Noble gases Alkali Earth metals Non-metals

12. Columns; similar properties The table tells you…lots! • Tim & Moby Rows; proton number increases

14. Atoms; the smallest unit of matter.

15. What is an atom made of?

16. Rāmere te tekau Hui-tanguru. • KW 15 • Mark home work Ex 14.08 • Review atoms. • Mass & Number. • Electron shell diagrams (2,8,8 rule). • Hmwk; KW 610 & Ex 14.10

17. Using the mass and number. • The atomic mass and atomic number of an element tells you what they look like. Atomic mass= Number of protons + neutrons Atomic number = Number of proton Number of electrons

18. How many neutrons? • Atomic mass-atomic number= number of neutrons • Li; 7-3=4 neutrons.

19. Complete the table

20. Electron shells. • When filling electron shells you must follow the 2,8,8 rule. • 2 in the first shell, 8 in the second and 8 in the third. • This will be important when we get to ions too. • Complete the worksheet to fill in shells.

21. So… • Li has 3 protons, 3 electrons and 4 neutrons. (7-3=4) • Now we need to draw it.

22. 5 9 7 1 Xp Xn 3 4 10 8 2 6

23. Rāhinā te tekau ma toru Hui-tanguru • Key words 610. • Mark home work Ex 14.10 • Finish electron shell diagrams (2,8,8 rule). • Covalent bonding. • Ionic bonding. Hmwk; KW 610 & Ex 14.09

25. Patterns in the electron table. • What patterns emerge from the electron table? • Why would this be? • Is there a relationship between the number of electrons in the outer shell, and how reactive an atom is?

26. Covalent bonding. • When two atoms come near each other, sometimes they ‘stick’ together to make a molecule. One way they can stick together is by covalent bonding.

27. In covalent bonding, the atoms are unstable because their outer rings of electrons aren't filled up. By sharing electrons with other atoms, these atoms can fill up their outer rings and become stable. In water, for instance, the oxygen atom needs two more electrons to be stable, and the hydrogen atoms each need one.

28. Now that the atoms have become stable, it's pretty hard to knock them back into being unstable again, so covalent bonds are strong and molecules that form with covalent (sharing) bonds are strong molecules. • Let us make a model!

29. Model making 2; the ice cube

30. Which atoms might make a covalent bond? • Which atoms have gaps in their outer shell? • Which atoms do not? • Do they bond in different ratios? • Why might this be?

31. Ions. • An ion is an atom which has gained or lost electrons during a chemical reaction. • Gains = negative ion. • Loses = positive ion. • The atom will gain or lose depending on how many electrons are in the outer shell.

32. Ions II • Outer shell = 1, 2, 3 electrons = LOSE • Metals do this. • Outer shell = 5, 6, 7 electrons = GAIN • Non-metals do this. • Outer shell = 4 = SHARE • Carbon does this.

33. Now what? • The atomic symbol has a charge written above it. • Li +, Be2+, Al3+. • N3-, O2-, F-. • Look at the periodic table…see any patterns?

34. Rātū te tekau ma whā Hui-tanguru. • KW 6 10 • Mark homework Ex14.12 • Review ions table. • Ions love to bond. • Making ionic bonds. • Hmwk; KW set 2 15

37. Ions love to bond! • Opposites attract in ionic chemistry. • Li+ wants to bond with a negative ion. • When Li+ bonds with Cl- they form LiCl; an ionic compound. • The rule with ionic bonding is; When you see ions, you must STOP, SWAP& DROP!

38. The rules. • Same charge; combine symbols to make the compound formula. • H+ + Cl- HCl • Mg2+ + O2- MgO

39. Different charges; swap and drop the numbers and lose the charge. • H+ + O2- H20 • Fe3+ + S2- Fe2S3

40. Different charges with polyatomic ions; use brackets when there is more than 1 polyatomic ion. • Pb2+ + PO43+ Pb3(PO4)2 • Al3+ + NO3- Al(NO3)3 You must keep polyatomic ions together with brackets.

41. Ionic equations. • Na+ + Cl- • Fe 2+ + O2-  • Al3+ + PO43-  • K+ + S2-  • Fe3+ + I-  • Fe2+ + PO43-  • NH4+ + SO42- 

42. Rāapa te tekau ma rima Hui-tanguru • KW set 2; 15 • More ionic compounds. • Naming ionic compounds. • Hmwk KW 610& Ex 14.12

43. Try these! • K+ + O2- • Pb2++ I-  • Al3+ + S2-  • Fe 3+ + OH-  • Na+ + CO32-  • NH4+ + CO32- 

44. Making ionic compounds. • Complete the table. e e e e e e e

45. Ion names ide • Chloride, nitride, sulphide, oxide • “ide” rather be alone • Nitrate, Sulphate, Carbonate • Oxygen “ate” an atom.

46. CuBr2 KBrO3 ZnI2 NaIO3 CaCO3 Naming ionic compounds. • ZnS • CuSO4 • MgO- • Mg3N2 • Zn(NO3)2 • NaCl

47. CuBr2- copper bromide KBrO3- potassium bromate ZnI2- zinc iodide NaIO3- sodium iodate CaCO3- calcium carbonate ZnS- zinc sulphide CuSO4- copper sulphate MgO- magnesium oxide Mg3N2- magnesium nitride Zn(NO3)2- zinc nitrate NaCl- sodium chloride Naming ionic compounds.

48. Rāmere te tekau ma whitu Hui-tanguru • KW 610 • Ex 14.12 • Chemical reactions. • Hmwk KW610

49. What is a chemical reaction? • How do we know a chemical reaction has occurred? • What is happening inside the reaction? • Can we change it back after the reaction?

50. Experiments. • First watch the demo experiments. • Then carry out the 8 experiments on your info sheet. • We will continue into next lesson, so don’t rush. • Complete the questions that go with each experiment before you move on to the next station.