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. Homework: Read pgs. 44 – 45 pg. 45 Section 2.1 Questions #’s 1 – 3

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

12. KI(aq) + Cl2(g)  KCl(aq) + I2(s)
Balance this equation
KI(aq) + Cl2(g)  KCl(aq) + I2(s)
2 KI(aq) + Cl2(g)  2 KCl(aq) + I2(s)

13. NH3(g) + O2(g)  N2(g) + H2O(l)
Balance this equation
NH3(g) + O2(g)  N2(g) + H2O(l)
4 NH3(g) + 3 O2(g)  2 N2(g) + 6 H2O(l)

14. KClO3(aq) → KCl(aq) + O2(g) 2 KClO3(aq) → 2 KCl(aq) + 3 O2(g)
Balance this equation
KClO3(aq) → KCl(aq) + O2(g)
2 KClO3(aq) → 2 KCl(aq) + 3 O2(g)

15. Balance this equation Al(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2(g)

16. Balance this equation Hg(OH)2(s) + H3PO4(aq)  Hg3(PO4)2(s) + H2O(l)

17. Balance this equation CuO(s) + NH3(g)  Cu(s) + H2O(l) + N2(g)

18. NH3(g) + O2(g)  N2O4(g) + H2O(g)
Balance this equation
NH3(g) + O2(g)  N2O4(g) + H2O(g)
4 NH3(g) + 7 O2(g)  2 N2O4(g) + 6 H2O(g)

19. Cl2(g) + MgI2(aq)  MgCl2(aq) + I2(s)
Balance this equation
chlorine + magnesium iodide  magnesium chloride + iodine
Cl2(g) + MgI2(aq)  MgCl2(aq) + I2(s)

20. 2 NaCl(aq) + H2SO4(aq)  2 HCl(aq) + Na2SO4(aq)
Balance this equation
sodium chloride + sulfuric acid  hydrochloric acid + sodium sulfate
2 NaCl(aq) + H2SO4(aq)  2 HCl(aq) + Na2SO4(aq)

21. 2 KNO3(aq)  2 KNO2(aq) + O2(g)
Balance this equation
potassium nitrate decomposes into potassium nitrite and oxygen
2 KNO3(aq)  2 KNO2(aq) + O2(g)

22. 2 Bi(NO3)3(aq) + 3 CaI2(aq)  2 BiI3(aq) + 3 Ca(NO3)2(aq)
Balance this equation
bismuth (III) nitrate + calcium iodide  bismuth (III) iodide + calcium nitrate
2 Bi(NO3)3(aq) + 3 CaI2(aq)  2 BiI3(aq) + 3 Ca(NO3)2(aq)

23. Fe2O3(s) + 3 CO(g)  2 Fe(s) + 3 CO2(g)
Balance this equation
iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide
Fe2O3(s) + 3 CO(g)  2 Fe(s) + 3 CO2(g)

24. Homework:
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. Homework:
Read pgs. 55 – 57
pg. 57 Section 2.4 Questions #’s 1 – 7

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

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

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

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

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

38. Homework:
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