2. Many issues in society involve science and technology.

4. A physical change occurs when the fundamental entities remain unchanged at a molecular level. e.g. change in phase, shape, or dissolving A chemical change involves some kind of change in the chemical bonds. At least one new substance is formed. A nuclear change involves changes in the nucleus, resulting in new elements.

6. The Kinetic Molecular Theory The smallest particles of a substance are in constant random motion. If a collision between different entities occurs with enough energy and in the right orientation, a chemical reaction will occur.

8. A Balanced Chemical Equation The number of each kind of atom is the same on each side of the arrow (mass is conserved).

9. Read pgs. 44 – 45 pg. 45 Section 2.1 Questions #’s 1 – 3 Read pgs. 46 – 49 pg. 50 Section 2.2 Questions #’s 1 – 10

11. A mole is the unit of chemical amount of substance.

12. Balance this equation KI (aq) + Cl 2(g)  KCl (aq) + I 2(s) 2 KI (aq) + Cl 2(g)  2 KCl (aq) + I 2(s)

13. Balance this equation NH 3(g) + O 2(g)  N 2(g) + H 2 O (l) 4 NH 3(g) + 3 O 2(g)  2 N 2(g) + 6 H 2 O (l)

14. Balance this equation KClO 3(aq) → KCl (aq) + O 2(g) 2 KClO 3(aq) → 2 KCl (aq) + 3 O 2(g)

15. Al (s) + H 2 SO 4(aq) → Al 2 (SO 4 ) 3(aq) + H 2(g) 2 Al (s) + 3 H 2 SO 4(aq) → Al 2 (SO 4 ) 3(aq) + 3 H 2(g) Balance this equation

16. Hg(OH) 2(s) + H 3 PO 4(aq)  Hg 3 (PO 4 ) 2(s) + H 2 O (l) 3 Hg(OH) 2(s) + 2 H 3 PO 4(aq)  Hg 3 (PO 4 ) 2(s) + 6 H 2 O (l) Balance this equation

17. CuO (s) + NH 3(g)  Cu (s) + H 2 O (l) + N 2(g) 3 CuO (s) + 2 NH 3(g)  3 Cu (s) + 3 H 2 O (l) + N 2(g) Balance this equation

18. NH 3(g) + O 2(g)  N 2 O 4(g) + H 2 O (g) 4 NH 3(g) + 7 O 2(g)  2 N 2 O 4(g) + 6 H 2 O (g) Balance this equation

19. chlorine + magnesium iodide  magnesium chloride + iodine Cl 2(g) + MgI 2(aq)  MgCl 2(aq) + I 2(s) Balance this equation

20. sodium chloride + sulfuric acid  hydrochloric acid + sodium sulfate 2 NaCl (aq) + H 2 SO 4(aq)  2 HCl (aq) + Na 2 SO 4(aq) Balance this equation

21. potassium nitrate decomposes into potassium nitrite and oxygen 2 KNO 3(aq)  2 KNO 2(aq) + O 2(g) Balance this equation

22. bismuth (III) nitrate + calcium iodide  bismuth (III) iodide + calcium nitrate 2 Bi(NO 3 ) 3(aq) + 3 CaI 2(aq)  2 BiI 3(aq) + 3 Ca(NO 3 ) 2(aq) Balance this equation

23. i ron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide Fe 2 O 3(s) + 3 CO (g)  2 Fe (s) + 3 CO 2(g) Balance this equation

24. Read pgs. 51 – 53 pgs. 53 – 54 Section 2.3 Questions #’s 1 – 6

25. The molar mass, M, of a substance is the mass of one mole of a substance. m = mass (g) n = number of moles (mol) M = molar mass (g/mol)

26. Molar masses are always to two decimal places!

28. Mass-Amount Conversions Examples 1) Calcium carbonate helps to neutralize acidic soil under spruce trees. Convert a mass of 1500 g of calcium carbonate to a chemical amount. 14.99 mol 2) Sodium sulfate is mined from lakes and deposits along the Alberta-Saskatchewan border. Convert a reacting amount of 3.46 mmol of sodium sulfate into mass in grams. 0.491 g

29. Read pgs. 55 – 57 pg. 57 Section 2.4 Questions #’s 1 – 7

31. elements → compound Formation Reactions magnesium + oxygen → magnesium oxide

32. compound → elements Simple Decomposition Reactions water → hydrogen + oxygen

33. Combustion Reactions substance + oxygen → most common oxides SubstanceOxide carbon hydrogen sulfur nitrogen a metal oxide with the most common ion charge butane + oxygen → carbon dioxide + water

36. element + compound → compound + element Single Replacement Reactions copper + silver nitrate → silver + copper (II) nitrate

37. compound + compound → compound + compound Double Replacement Reactions calcium chloride + sodium carbonate → calcium carbonate + sodium chloride acid + base → water + ionic compound (a salt) Neutralization

38. Read pgs. 58 – 59 pgs. 59 – 60 Section 2.5 Questions #’s 1 – 6 Read pgs. 61 – 63 pg. 64 Section 2.6 Questions #’s 1 – 5