1. WHMIS  workplace hazardous materials information system  all chemicals are treated with  WHMIS has been developed to provide guidelines for of reactive materials respect handling, storage and disposal  MSDS is a material safety data sheet

2. compressed gas corrosive flammable and combustible poisonous and infectious material causing immediate and serious toxic effects

3. biohazardous infectious material oxidizing material dangerously reactive material poisonous and infectious causing other toxic effects

4. A. The Atom    proton neutron electron p+p+ n0n0 e–e– zero charge positive charge negative charge  electrons are found in a cloud region around the nucleus  nucleus contains the protons and neutrons which make up most of mass of atom Science 10 Review

5.  mass number =  isotope = # protons + # neutrons atoms with the same # of protons but a different # of neutrons (different mass numbers) eg) carbon-12  carbon-14  6 p +, 6 n 0 6 p +, 8 n 0 # neutrons = mass number - # protons

6. B. Periodic Table  arranged in and  group number =  period number = groups (columns) periods (rows) number of outer level (valence) e - number of energy levels occupied by e - Ex. Na Group number = Period number = 1 3 This info is helpful for drawing Energy Level Diagrams

7. C. Energy Level Diagrams  atoms are which means that the  maximum number of e - : 3 rd level = 2 nd level = 1 st level = electrically neutral # of p + = # of e - 8 e - 2 e -

8. Examples 11 p + Na 3 p + Li 2 e - 8 e - 1 e - 2 e - 1 e -

9. D. Ions  ions are  neutral atoms are unstable if  atoms will strive to satisfy the in order to become stable…in other words, they strive to have particles or groups of particles that have a net charge (either positive or negative) their valence level is not full octet rule a full valence level and do so by giving away or taking e -

10.  metals  give away e - and become positive ions eg) Na +, Ca 2+, Fe 3+ take e - and become negative ions  non-metals  eg) Cl -, P 3-, O 2-

11. Examples 11 p + Na 2 e - 8 e - 1 e - 2 e - 8 e - 11 p + Na + sodium atomsodium ion

12. 17 p + Cl 2 e - 8 e - 7 e - 2 e - 8 e - 17 p + Cl – chlorine atomchloride ion 8 e -

13. Your Assignment: 1. Draw argon and neon and compare to Na + and Cl – 2. pgs 1,2 in workbook

14. E. Elements  metals exist as  nonmetals and hydrogen single atoms eg) Li (s), Cu (s), Hg (l) do not exist as single atoms – flagpole! H2H2 N2N2 O2O2 F2F2 P4P4 S8S8 Cl 2 Br 2 I2I2

15. Try These: 1. Cu (s) = 2. O 2(g) = 3.Al (s) = 4. fluorine gas = 5. barium = 6. nitrogen gas = copper oxygen gas aluminum F 2(g) Ba (s) N 2(g)

16. F. Ionic Compounds   eg) K +, Be 2+ or metals eg) Fe 3+, Fe 2+ monovalentmultivalent  charges on the ions are the result of taking or giving e -  to go from formula to name:name of first ion, eg)AlCl 3 =aluminum chloride metals + nonmetals or polyatomic ions then name for second ion then brackets for charge if multivalent, Fe 2 O 3 =iron (III) oxide i.e. first element ( ) second element-ide

17. Try These: 1. Zn 3 P 2 = 2. NaNO 3 = 3. NiF 3 = 4. MnO 2 = 5. Cr 2 (SO 4 ) 3 = nickel (III) fluoride manganese (IV) oxide zinc phosphide chromium (III) sulphate sodium nitrate

18.  to go from name to formula: write the symbol for each ion, eg)calcium sulphide = iron (II) hydroxide = CaS Fe(OH) 2 Try These: 1. lithium bromide = 2. sodium phosphate = 3. magnesium nitride = 4. ammonium sulphate = 5. calcium phosphate = Na 3 PO 4 Mg 3 N 2 (NH 4 ) 2 SO 4 then add subscripts to balance charges Ca 3 (PO 4 ) 2 LiBr

19. Hydrated Compounds  ionic compounds containing in their structure  water is represented by in the formula where is the number of water molecules  prefixes: 1 = 6 = 2 = 7 = 3 = 8 = 4 = 9 = 5 = 10 = water “  xH 2 O” mono di tri tetra penta hexa hepta octa nona deca x

20.  to go from name to formula: give the for the first part of the compound, then name the part as eg) NaF  3H 2 O = CuSO 4  5H 2 O = ionic name “  xH 2 O” prefix + “hydrate” sodium fluoride trihydrate copper (II) sulphate pentahydrate

21.  to go from name to formula: first part is the …look up the symbol for each ion then balance the charges using subscripts, then for the hydrate part…add where is the number given in the prefix eg) iron (III) nitrate nonahydrate = sodium chlorate tetrahydrate = nickel (II) sulphite heptahydrate = Fe(NO 3 ) 3  9H 2 O NaClO 3  4H 2 O NiSO 3  7H 2 O same as before “  xH 2 O” x

22. Your Assignment: pgs 3,4 in workbook

23. G. Molecular Compounds     nonmetals only e - are shared therefore no ions are formed no charges involved use prefixes in naming

24. eg)N 2 O = CO 2 = P 4 O 10 = dinitrogen monoxide carbon dioxide  to go from formula to name: then name for second element with “ide” ending (including prefix) tetraphosphorus decaoxide  to go from name to formula: write the symbol for each element, eg)carbon monoxide = carbon tetrachloride = CO CCl 4 name of first element (including prefix if necessary), then use the prefixes to determine the subscripts i.e. ___first element ___second element -ide

25.  remember the memorizers?????? NH 3 (g)= H 2 O(l) = H 2 S(g) = HF, HCl, HBr, HI = CH 4 (g)= CH 3 OH(l) = C 2 H 6 (g)= C 2 H 5 OH(l) = C 6 H 12 O 6 (s)= C 12 H 22 O 11 (s)= O 3 (g)= H 2 O 2 (l)= ammonia water hydrogen sulphide no prefixes methane methanol ethane ethanol glucose sucrose ozone hydrogen peroxide

26. H. Acids  always have as the state and always have Rules 1. hydrogen becomes acid 2. hydrogen becomes acid 3. hydrogen becomes acid aqueous (aq) hydrogen ____idehydro___ic ____ate_______ic ____ite______ous

27. Try These: 1. hydrogen iodide = 2. hydrogen phosphate = 3. hydrogen nitrite = 4. hydrogen sulphite = hydroiodic acid phosphoric acid nitrous acid sulphurous acid HI (aq) H 3 PO 4(aq) HNO 2(aq) H 2 SO 3(aq)

28. Your Assignment: pgs 5-7 in workbook

29. I. States  acids –  elements –  molecular compounds –  ionic compounds always (aq) can be (s), (l) or (g)…see periodic table can be (s), (l), or (g) - If not in a solution always (s) - If in a solution either (s) or (aq)…look up on the solubility chart

30. Try These: 1. NaCH 3 COO( )6. CaCO 3 ( ) 2. BaSO 4 ( )7. FeSO 4 ( ) 3. KOH( )8. (NH 4 ) 2 S( ) 4. Pb(NO 3 ) 4 ( )9. Pb(SO 4 ) 2 ( ) 5. Hg(CH 3 COO) 2 ( )10. Ca 3 (PO 4 ) 2 ( ) aq s s s

31. J. Chemical Reactions  vs.  reaction types: endothermicexothermic 1. hydrocarbon combustion 2. simple composition C ? H ? + O 2(g)  CO 2(g) + H 2 O (g) eg) CH 4(g) + 2 O 2(g)  CO 2(g) + 2 H 2 O (g) element + element  compound eg) 2 Mg (s) + O 2(g)  2 MgO (s)

32. 5. double replacement 4. single replacement 3. simple decomposition compound  element + element eg) 2 H 2 O (l)  2 H 2(g) + O 2(g) element + compound  element + compound eg) Cu (s) + 2 AgNO 3(aq)  2 Ag (s) + Cu(NO 3 ) 2(aq) compound + compound  compound + compound eg) Pb(NO 3 ) 2(aq) + 2 KI (aq)  2 KNO 3(aq) + PbI 2(s)

33.  law of conservation of matter says that  we must chemical equations to conserve matter matter cannot be created or destroyed, it can only change forms balance CH4 (g) + O2(g)  CO2(g) + H2O(g) C2H6 (g) + O2(g)  CO2(g) + H2O(g) 23 27 4 6 Balancing Reactions

34. Your Assignment: pg 8, 1 st half p. 9

35. Try the following: Potassium iodide solution is added to lead (II) nitrate solution. KI (aq) +  + 22 Predicting Reactions Pb(NO3)2(aq)KNO3(aq)PbI2(s) NOTE: -SR and DR reactions always happen in solutions so for ionic compounds check solubility table -Composition and decomposition do NOT happen in solutions so ionic compounds are (s)

36. Predicting: single replacement Copper metal is added to a solution of silver nitrate Cu (s) + 2 AgNO 3(aq)  2 Ag (s) + Cu(NO 3 ) 2(aq) Chlorine gas is bubbled through a solution of sodium phosphide 6 Cl 2(g) + 4 Na3P (aq)  P 4(s) + 12 NaCl (aq)

37. Your Assignment: pg 2 nd half p. 9

38. K. Significant Digits  any digit from is significant  are significant eg)  are not significant eg) 1-9 trailing zeros  counted objects and constants are not included in sig digs “sandwich” zeros leading zeros 6.3800, 12 000 2.04, 1005.002 0.0065

39.   /  :  +/  : multiply or divide then round answer to the lowest number of sig digs add or subtract then round answer to the lowest number of decimal places

40. L. The Mole  it is a =number6.02 x 10 23 “items” 1. Molar Mass  sum of the eg)CO 2 = Al(OH) 3 = Cu(ClO 3 ) 2 = 44.01 g/mol 78.01 g/mol 230.45 g/mol individual atomic masses for each element in a compound

41. 2. Mole/Mass Calculations n = m M where: n = m = M = number of moles in mol mass in g molar mass in g/mol m = nM

42. Example 1 How many moles are in 8.06 g of magnesium oxide? m = 8.06 g M = 40.31 g/mol n = ? n = m M = 8.06 g 40.31 g/mol = 0.1999503 mol = 0.200 mol

43. Example 2 What is the mass of 0.677 mol of potassium sulphide? n = 0.677 mol M = 110.27 g/mol m = ? m = nM = (0.677 mol)(110.27 g/mol) = 74.65…g = 74.7 g

44. Your Assignment: p. 10 & 1st half p. 11 Your Review Assignment: finish p. 11 – p. 13