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

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

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

4. Science 10 Review
A. The Atom
 
proton p+
positive charge
 
neutron n0
zero charge
 
electron e–
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

5. mass number =
# protons + # neutrons
# neutrons =
mass number - # protons
isotope =
atoms with the same # of protons but a different # of neutrons (different mass numbers)
eg) carbon-12 
carbon-14 
6 p+, 6 n0
6 p+, 8 n0

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

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

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

9. D. Ions
ions are
particles or groups of particles that have a net charge (either positive or negative)
neutral atoms are unstable if
their valence level is not full
atoms will strive to satisfy the in order to become stable…in other words, they strive to have
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+, Ca2+, Fe3+
non-metals 
take e- and become negative ions
eg) Cl-, P3-, O2-

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

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

13. Your Assignment: pgs 1-3 in workbook

14. E. Elements
metals exist as
single atoms
eg) Li(s), Cu(s), Hg(l)
nonmetals and hydrogen
do not exist as single atoms – MUST MEORIZE! H2 N2 O2 F2 P4 S8
Cl2
Br2 I2

15. Try These:
1. Cu(s) =
2. O2(g) =
Al(s) =
4. fluorine gas =
5. barium =
6. nitrogen gas =
copper
oxygen gas
aluminum
F2(g)
Ba(s)
N2(g)

16. F. Ionic Compounds
metals + nonmetals or polyatomic ions
eg) K+, Be2+ or metals
eg) Fe3+, Fe2+
monovalent
multivalent
charges on the ions are the result of
taking or giving e-
to go from formula to name:
name of first ion,
then brackets for charge if multivalent,
then name for second ion
i.e. first element ( ) second element-ide
eg) AlCl3 =
aluminum chloride
Fe2O3 =
iron (III) oxide

17. Try These:
1. Zn3P2 =
2. NaNO3 =
3. NiF3 =
4. MnO2 =
5. Cr2(SO4)3 =
zinc phosphide
sodium nitrate
nickel (III) fluoride
manganese (IV) oxide
chromium (III) sulphate

18. to go from name to formula: write the symbol for each ion,
then add subscripts to balance charges
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 =
LiBr
Na3PO4
Mg3N2
(NH4)2SO4
Ca3(PO4)2

19. ionic compounds containing in their structure water
Hydrated Compounds
ionic compounds containing in their structure
water
water is represented by in the formula where is the number of water molecules
“xH2O” x
prefixes:
1 = 6 =
2 = 7 =
3 = 8 =
4 = 9 =
5 = =
mono
hexa di
hepta
tri
octa
nona
tetra
penta
deca

20. to go from name to formula: give the for the first part of the compound, then name the part as
ionic name
“xH2O”
prefix + “hydrate”
eg) NaF3H2O =
CuSO45H2O =
sodium fluoride trihydrate
copper (II) sulphate pentahydrate

21. to go from name to formula: first part is the
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
same as before
“xH2O” x
eg) iron (III) nitrate nonahydrate =
sodium chlorate tetrahydrate =
nickel (II) sulphite heptahydrate =
Fe(NO3)39H2O
NaClO34H2O
NiSO37H2O

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. to go from formula to name:
name of first element (including prefix if necessary),
then name for second element with “ide” ending (including prefix)
i.e. ___first element ___second element -ide
eg) N2O =
CO2 =
P4O10 =
dinitrogen monoxide
carbon dioxide
tetraphosphorus decaoxide
to go from name to formula:
write the symbol for each element,
then use the prefixes to determine the subscripts
eg) carbon monoxide =
carbon tetrachloride = CO
CCl4

25. remember the please memorize:
NH3(g)=
H2O(l) =
H2S(g) =
HF, HCl, HBr, HI =
CH4(g)=
CH3OH(l) =
C2H6(g)=
C2H5OH(l) =
C6H12O6(s)=
C12H22O11(s)=
O3(g)=
H2O2(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
aqueous (aq)
hydrogen
Rules
1. hydrogen becomes acid
2. hydrogen becomes acid
3. hydrogen becomes acid
____ide
hydro___ic
____ate
_______ic
____ite
______ous

27. Try These: 1. hydrogen iodide = 2. hydrogen phosphate =
3. hydrogen nitrite =
4. hydrogen sulphite =
hydroiodic acid
HI(aq)
phosphoric acid
H3PO4(aq)
nitrous acid
HNO2(aq)
sulphurous acid
H2SO3(aq)

28. Your Assignment: pgs 5-7 in workbook

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

30. aq s s aq aq aq aq aq aq s Try These: 1. NaCH3COO( ) 6. CaCO3( )
2. BaSO4( ) FeSO4( )
3. KOH( ) (NH4)2S( )
4. Pb(NO3)4( ) Pb(SO4)2( )
5. Hg(CH3COO)2( ) Ca3(PO4)2( ) aq s s aq aq aq aq aq aq s

31. J. Chemical Reactions
vs.
endothermic
exothermic
reaction types:
1. hydrocarbon combustion
C?H? O2(g)  CO2(g) H2O(g)
eg) CH4(g) O2(g)  CO2(g) H2O(g)
2. simple composition
element + element  compound
eg) 2 Mg(s) O2(g)  2 MgO(s)

32. compound  element + element eg) 2 H2O(l)  2 H2(g) + O2(g)
3. simple decomposition
compound  element + element
eg) 2 H2O(l)  2 H2(g) O2(g)
4. single replacement
element + compound  element + compound
eg) Cu(s) AgNO3(aq)  2 Ag(s) + Cu(NO3)2(aq)
5. double replacement
compound + compound  compound + compound
eg) Pb(NO3)2(aq) KI(aq)  2 KNO3(aq) + PbI2(s)

33. Balancing Reactions
law of conservation of matter says that
matter cannot be created or destroyed, it can only change forms
we must chemical equations to conserve matter
balance
CH4 (g) + O2(g)  2
CO2(g) + H2O(g) 2 4 2
C2H6 (g) O2(g)  7
CO2(g) H2O(g) 6

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

35. Potassium iodide solution is added to lead (II) nitrate solution.
Predicting Reactions
Try the following:
Potassium iodide solution is added to lead (II) nitrate solution. 2
KI(aq)  2
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) AgNO3(aq)  2 Ag(s) + Cu(NO3)2(aq)
Chlorine gas is bubbled through a solution of sodium
phosphide
6 Cl2(g) Na3P(aq)  P4(s) NaCl(aq)

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

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

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 =
number
6.02 x 1023 “items”
1. Molar Mass
sum of the
individual atomic masses for each element in a compound
eg) CO2 =
Al(OH)3 =
Cu(ClO3)2 =
44.01 g/mol
78.01 g/mol
g/mol

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

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

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

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