A. The Atom

proton

neutron

electron

p+

n

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 n6 p+, 8 n

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-

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-

Your Assignment: pg 1 in workbook

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 2,3 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! (SHPON)

eg) H2(g), O2(g), P4(s), S8(s)

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, then brackets for charge if multivalent, then name for second ion eg) AlCl3 =

CuSO45H2O =

aluminum chloride copper (II) sulphate pentahydrate

metals + nonmetals or polyatomic ions

Try These:

1. NiF3 =

2. MnO2 =

3. Na3PO410H2O =

4. Zn3P2 =

5. Cr2S3 =

6. MgCl26H2O =

nickel (III) fluoride

manganese (IV) oxide

sodium phosphate decahydrate

zinc phosphide

chromium (III) sulphide

magnesium chloride hexahydrate

to go from name to formula: write the symbol for each ion, then add subscripts to balance charges

eg) calcium sulphide = iron (III) oxide =

CaS Fe2O3

Try These:

1. sodium phosphate =

2. vanadium (IV) sulphide dihydrate =

3. magnesium nitride =

4. ammonium sulphate =

Na3PO4

VS22H2O

Mg3N2

(NH4)2SO4

Your Assignment: pgs 4,5 in workbook

***pg 4 #18 cupric = Cu2+

pg 5 #24 –3- water = trihydrate

G. Molecular Compounds

nonmetals only

e- are shared therefore no ions are formed

no charges involved

use prefixes in naming

eg) N2O =

CO2 =

P4O10 =

dinitrogen monoxide carbon dioxide

to go from formula to name: name of first element (including prefix if necessary), then name for second element with “ide” ending (including prefix)

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

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

_________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

Your Assignment: pgs 6,7 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)

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)

Your Assignment: pgs 9-10

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

Your Assignment: pgs 9-10 - balancing

Your Assignment: 1. pg 10 #1, 2, 11, 13, 14 – predicting, states, balancing, reaction type

2. pg 11

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

Your Assignment: pgs 12,13 in workbook

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/mol

230.45 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 molM = 110.27 g/molm = ?

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

Your Assignment: pgs 14,15 in workbook