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 amaterial safety data sheet

compressed gas corrosive

flammable and combustible

poisonous and infectious

material causing immediate and serious toxic

effects

biohazardous infectious material

oxidizing material

dangerously reactive material

poisonous and infectious causing other

toxic effects

A. The Atom

proton

neutronelectron

p+

n0

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

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 n0

6 p+, 8 n0

# neutrons = mass number - # protons

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 =

13

This info is helpful for drawing Energy Level

Diagrams

C. Energy Level Diagrams

atoms are which means that the

maximum number of e-: 3rd level =   2nd level =   1st level =

electrically neutral # of p+ = # of e-

8 e- 8 e- 2 e-

Examples

11 p+

Na

3 p+

Li

2 e-

8 e-

1 e-

2 e-

1 e-

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-

metals give away e- and become positive ions

eg) Na+, Ca2+, Fe3+

take e- and become negative ions

non-metals

eg) Cl-, P3-, O2-

Examples

11 p+

Na

2 e-

8 e-

1 e-

2 e-

8 e-

11 p+

Na+

sodium atom sodium ion

17 p+

Cl

2 e-

8 e-

7 e-

2 e-

8 e-

17 p+

Cl–

chlorine atom chloride ion

8 e-

Your Assignment: 1. Draw argon and neon and compare to Na+ and Cl–

2. pgs 1,2 in workbook

E. Elements

metals exist as

nonmetals and hydrogen

single atoms

eg) Li(s), Cu(s), Hg(l)

do not exist as single atoms – flagpole!

H2

N2 O2 F2

P4 S8 Cl2

Br2

I2

Try These:

1. Cu(s) =

2. O2(g) =

3. Al(s) =

4. fluorine gas =

5. barium =

6. nitrogen gas =

copper

oxygen gas

aluminum

F2(g)

Ba(s)

N2(g)

F. Ionic Compounds

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,

eg) AlCl3 =aluminum chloride

metals + nonmetals or polyatomic ions

then name for second ion then brackets for charge if multivalent,

Fe2O3 =iron (III) oxide

i.e. first element ( ) second element-ide

Try These:

1. Zn3P2 =

2. NaNO3 =

3. NiF3 =

4. MnO2 =

5. Cr2(SO4)3 =

nickel (III) fluoride

manganese (IV) oxide

zinc phosphide

chromium (III) sulphate

sodium nitrate

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 =

Na3PO4

Mg3N2

(NH4)2SO4

then add subscripts to balance charges

Ca3(PO4)2

LiBr

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

“xH2O”

mono

di

tri

tetra

penta

hexa

hepta

octa

nona

deca

x

to go from name to formula: give the for the first part of the compound, then name the part as

eg) NaF3H2O =

CuSO45H2O =

ionic name

“xH2O” prefix + “hydrate”

sodium fluoride trihydrate

copper (II) sulphate pentahydrate

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(NO3)39H2O

NaClO34H2O

NiSO37H2O

same as before

“xH2O”x

Your Assignment: pgs 3,4 in workbook

G. Molecular Compounds

nonmetals only

e- are shared therefore no ions are formedno charges involved

use prefixes in naming

eg) N2O = CO2 =P4O10 =

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 CCl4

name of first element (including prefix if necessary),

then use the prefixes to determine the subscripts

i.e. ___first element ___second element -ide

remember the memorizers??????

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

ethanolglucose

sucrose

ozone

hydrogen peroxide

H. Acids always have as the

state and always have

Rules1. hydrogen becomes acid2. hydrogen becomes acid3. hydrogen becomes acid

aqueous (aq)hydrogen

____ide hydro___ic

____ate _______ic____ite ______ous

Try These:

1. hydrogen iodide =

2. hydrogen phosphate =

3. hydrogen nitrite =

4. hydrogen sulphite =

hydroiodic acid

phosphoric acid

nitrous acid

sulphurous acid

HI(aq)

H3PO4(aq)

HNO2(aq)

H2SO3(aq)

Your Assignment: pgs 5-7 in workbook

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

Try These:

1. NaCH3COO( ) 6. CaCO3( )

2. BaSO4( ) 7. FeSO4( )

3. KOH( ) 8. (NH4)2S( )

4. Pb(NO3)4( ) 9. Pb(SO4)2( )

5. Hg(CH3COO)2( ) 10. Ca3(PO4)2( )

aq

s

aq

aq

aq

s

aq

aq

aq

s

J. Chemical Reactions

vs.

reaction types:

endothermic

exothermic

1. hydrocarbon combustion

2. simple composition

C?H? + O2(g) CO2(g) + H2O(g)

eg) CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

element + element compound eg) 2 Mg(s) + O2(g) 2 MgO(s)

5. double replacement

4. single replacement

3. simple decomposition compound element +

element eg) 2 H2O(l) 2 H2(g) + O2(g)

element + compound element + compound eg) Cu(s) + 2 AgNO3(aq) 2 Ag(s) + Cu(NO3)2(aq)

compound + compound compound + compound eg) Pb(NO3)2(aq) + 2 KI(aq) 2 KNO3(aq) + PbI2(s)

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)

2 3

2 7 4 6

Balancing Reactions

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

Try the following:

Potassium iodide solution is added to lead (II) nitrate solution.

KI(aq) + + 2 2

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)

Predicting: single replacement

Copper metal is added to a solution of silver nitrate

Cu(s) + 2 AgNO3(aq) 2 Ag(s) + Cu(NO3)2(aq)Chlorine gas is bubbled through a solution of sodiumphosphide

6 Cl2(g) + 4 Na3P(aq) P4(s) + 12 NaCl(aq)

Your Assignment: pg 2nd half p. 9

K. Significant Digits

any digit from is significant

are significant eg)

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

/ :

+/ :

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

L. The Mole

it is a = number 6.02 x 1023 “items”

1. Molar Mass sum of the

eg) CO2 =Al(OH)3 =Cu(ClO3)2 =

44.01 g/mol78.01 g/mol230.45 g/mol

individual atomic masses for each element in a compound

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

Example 1

How many moles are in 8.06 g of magnesium oxide? m = 8.06 gM = 40.31 g/moln = ?

n = m M = 8.06 g 40.31 g/mol = 0.1999503 mol = 0.200 mol

Example 2

What is the mass of 0.677 mol of potassium sulphide?n = 0.677 mol

M = 110.27 g/molm = ?

m = nM = (0.677 mol)(110.27 g/mol) = 74.65…g = 74.7 g

Your Assignment: p. 10 & 1st half p. 11

Your Review Assignment: finish p. 11 – p. 13