1. Review of Atomic Model You should be able to:
Name and write formula for most chemical compounds
Write, balance and predict products for most chemical equations

2. Anything that has mass and takes up space, or volume.
Matter:
Anything that has mass and takes up space, or volume. Na
NaCl
NaCl +
H2O
NaCl +
Pepper

3. Elements are pure substances containing one type of atom – found on the Periodic Table.
The atom is the smallest part that retains all the properties of that element.
protons (p+)
neutrons (no)
electrons (e-)
Charge
Mass
Location
+1.6 x C
-1.6 x C
1.67 x g
9.11 x g
Nucleus
Orbit clouds

4. A “staircase” on every Periodic Table separates the metals from the non-metals (with metalloids in between)

5. Can be qualitative or quantitative
Physical properties
Testing or measuring these traits will NOT change the original composition (what it is made of)
Can be qualitative or quantitative
quality
quantity
State/phase – solid, liquid or gas (at room temperature)
Hardness – how easy it is to scratch or dent
Viscosity – how easy it flows
Melting point – unique temperature needed to change from solid into liquid
Boiling point – unique temperature needed to change from liquid into gas

6. Other examples of Physical Properties:
Lustre – shiny (opposite – dull)
Malleability – how easy to bend or flatten
(opposite – brittle)
Ductility – how easy to pull into a wire
Solubility – how well it dissolves in water
Conductivity – how well it transfers heat/electricity
Quantitative traits require a measurement – melting point Qualitative traits don’t need one – state

7. Trait describes if substance reacts chemically
Chemical properties
Trait describes if substance reacts chemically
Testing or measuring these traits WILL change the original composition (will create something new)
Reactivity – does it react quickly?
Combustibility – does it ignite or burn?
Corrosion – does it react with acids?
Oxidation – does it react with air?
Toxicity – does it react with the body?
Testing a chemical property requires a chemical reaction that will alter what you test:
wood  ash

8. Anything that changes what it “looks like” NOT “what it is”
Physical Change
A change in shape or state of a substance
- crushing, cutting, folding, smashing, melting, boiling…
No evidence of a new material forming H O
Anything that changes what it “looks like” NOT “what it is”

9. A chemical reaction has happened!
Chemical change
A change in the properties of a substance
**Means a new substance is formed
A chemical reaction has happened!
Evidence of a chemical change (and chemical reaction):
A change in colour
A change in smell
3. Fizzing or bubbling
(new gas being made)

10. This new solid is called a precipitate
4. A new solid forms from a mixture of liquids or the mixture goes cloudy
This new solid is called a precipitate
A change in energy
Exothermic: energy is released (product)
Endothermic: energy is absorbed (reactant)
“Energy” could be light, heat, sound – think of the most obvious change in energy reaction – an EXPLOSION!

11. Testing the property can cause a…
Physical properties
Chemical properties
Testing the property can cause a…
Physical change
Chemical change
Δ colour
Δ smell
Δ energy
Gas bubbles
Precipitate
State or
shape
NO Reaction
Chemical Reaction
Same substance with
same properties
New substance with
new properties

12. Number of protons and neutrons (p+ + no)
We will not be building Bohr diagrams this course, but you should remember how do use these numbers
Number of protons (p+)
[OR electrons (e-) since atoms are neutral]
Remember electrons are so small as to be essentially “massless” – the whole mass of the atom is really just the number of p+ and no in the nucleus
Number of protons and neutrons (p+ + no)

13. Atoms that have the same number of protons but a different number of neutrons are called Isotopes.
At Mass = 1
At Number = 1
At Mass = 2
At Number = 1
At Mass = 3
At Number = 1
These are ALL considered Hydrogen
– based on the proton number

14. An atom that has lost or gained an electron is called an ion
Atoms can either gain or lose electrons
Gain - negatively charged ion
Lose - positively charged ion H
neutral atom H+
positive ion
(cation) H-
negative ion
(anion)
An atom that has lost or gained an electron is called an ion

15. Octet rule: atoms react to acquire a full outer shell:
Called valence shell
Gain an e- from another atom
Lose an e- to another atom
Share an e- with another atom
Ionic bond
Covalent bond
Note
Metals typically lose e-
Non-metals typically gain e-

16. NOTE
These numbers might be called “combining capacity” “valences” or “charges” +1 +3 -3 -2 -1 +2
+4/-4
Non-metals
gain e-
Metals lose e-
Remember: The number of the column is equal to the valence electron number. Know that and you figure out the number of electrons lost or gained – the ionic charge

17. Mg Cl Cl S Cl Cl MgCl 2 SCl 2 ionic compound covalent compound - +2 -
metal
non-metal
non-metal
non-metal
MgCl 2
SCl 2
ionic compound
covalent compound - +2 Mg Cl Cl S - Cl Cl
Gain / lose – called a “formula unit”
Sharing – called a “molecule”
A compound has different characteristic properties than the atoms which form it.

18. I Have No Bright Or Clever Friends
Diatomic Elements:
Elements that are most commonly found in a
covalent bond with itself (not as single atoms)
I Have No Bright Or Clever Friends
I H N Br O Cl F2
NOTE
“Greediest” elements that must have a full octet, so they covalently bond with themselves when alone – BUT when bonded to another element there is no longer a reason to be diatomic

19. Notice: oxygen is not diatomic in a bond…
Chemical formula gives the following information:
The different elements in the compound
The number of atoms in the compound
Notice: oxygen is not diatomic in a bond…

20. Remember the subscript applies to what is directly in front of it
Brackets: subscripts outside a bracket multiply by everything inside the bracket. 3
Mg(NO3)2 1 1
Coefficient: total # of molecules present O N Mg O N
Remember the subscript applies to what is directly in front of it
Mg: 1 · 3 = 3
N: 1 · 2 · 3 = 6
O: 3 · 2 · 3 = 18

21. Writing Ionic Compound Formula
1. Write the symbol of the metallic element first.
2. Place the combining capacity (charge) of one element
as a subscript of the other element.
3. Leave subscripts with a value of 1 out.
4. Reduce the subscripts if possible.
beryllium combines with chlorine + 2 - 1
Be Cl
Be Cl2 1

22. Naming Ionic Compounds
1. Write the full name of the metal ion first.
2. Name the non-metal ion dropping the ending and
adding the suffix “ide.”
beryllium combines with chlorine
BeCl2
beryllium
chlor
ide

23. Here is an example of “reducing” the subscripts
Magnesium combines with Sulfur + 2 - 2
Mg S
Mg S
magnesium
sulph
ide
Here is an example of “reducing” the subscripts

24. Transition metals

25. Transition metals can give away different numbers of electrons.
To avoid confusion:
Brackets are used to show the number of electrons the Transition metal is giving away.

26. Fe Cl Fe Cl FeCl2 FeCl3 Iron (III) chloride Iron (II) chloride + 2 - 1
1. Write the symbol of the metallic element first.
2. Place the combining capacity (charge) of one element
as a subscript of the other element.
3. Leave subscripts with a value of 1 out.
4. Reduce the subscripts if possible.

27. Pb O PbO lead oxide (IV) +4 -2 Write the name of the ionic compound: +1
Pb O
PbO 1 2 2
lead oxide
(IV)
Remember: Always look at the anion to see if it has been reduced. If it has, so has the metal.

28. Al(C2H3O2)3 Polyatomic Ions (poly = many)
Groups of covalently bonded atoms that act as ions.
Polyatomic ions function as one unit with one ionic charge – gain or lose electrons.
Al(C2H3O2)3
Aluminum Acetate
Note the ending (not “ide”) – the ending is the clue that it is polyatomic and NOT a plain element

29. There are a few “ides” BUT they are obviously not elements

30. Mg NO3 Mg(NO3) magnesium nitrate Write the name of the ionic compound:+ - 1
Mg NO3
Mg(NO3) 2
magnesium nitrate
We get the valences (charges) and criss-cross – just like building any ionic compound

31. Ni(NO3)2
magnesium sulfate
KMnO4
iron (III) hydroxide
Ca(C2H3O2)2
silver chromate
PbCO3
tin (IV) sulfate
Na2HPO4
ammonium nitrite
nickel (II) nitrate
MgSO4
potassium permanganate
Fe(OH)3
calcium acetate
Ag2CrO4
lead (II) carbonate
Sn(SO4)2
sodium hydrogen phosphate
NH4NO2

32. Prefix Number of Atoms mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta7
octa 8
nona 9
deca 10
Memorize this…

33. Writing Covalent Compound Formula
1. Write the symbol of each element.
2. Use a subscript to show the number of atoms as indicated by the prefix.
*Do NOT reduce covalent bonds
Prefix
Number of Atoms
mono 1 di 2
tri 3
tetra 4
penta 5
hexa 6 di
phosphorus oxide
penta
P O 2 5

34. Naming Covalent Compounds
1. Write the first non-metal with the appropriate prefix.
*We don’t use “mono” for the first non-metal
2. Write the second non-metal with the appropriate prefix and add the suffix “ide.”
N O 2 4
Prefix
Number of Atoms
mono 1 di 2
tri 3
tetra 4
penta 5
hexa 6 di
nitrogen
tetra
oxide
dinitrogen tetroxide

35. OCl2 oxygen dichloride MgCl2 CuCl2 magnesium chloride
Does it have a metal?
YES (ionic)
Polyatomic
NO (covalent)
Find charges
Criss-cross
Don’t change ending
Is it a transition?
NO charges
NO criss-cross
Use prefixs
Ends in “ide”
Fe(NO3)2
iron (II) nitrate NO
Find charges
Criss-cross
Ends in “ide”
YES
Find charges
(reverse) Criss-cross
Use Brackets
Ends in “ide”
OCl2
oxygen dichloride
MgCl2
magnesium chloride
CuCl2
copper (II) chloride

36. reactants products 2 + A + 2 B C
Chemical reaction – substances react to produce one or more new substances.
Chemical equation – contains all necessary information about a reaction. 2 +
reactants products
A B C

37. (l) = liquid (g) = gas (s) = solid *(aq) = aqueous
At this level it is expect that you can decipher chemical reactions as word equations:
Hydrogen gas and oxygen gas react to form
water vapour
H O H2O 2
(g) 2
(g)
(g)
diatomic
State (phase) of the substance is always shown as small subscripts after the compound formula:
(l) = liquid (g) = gas (s) = solid *(aq) = aqueous
*Aqueous means this compound has dissolved in water

38. H2 (g) + O2 (g) H2O (g) 2 2 The Law of Conservation of Mass
(balancing equations):
In any chemical reaction matter cannot be created or destroyed.
H2 (g) + O2 (g) H2O (g) 2 2 H H O H H O O H H H H O
was
This equation is unbalanced because the atoms are not conserved from one side (reactants) to the other (products)

39. Rules for Balancing Equations
Coefficients
(phase/state)
Subscripts
H2 (g) + 1O2 (g) H2O (g) 2 2
Coefficients indicate the ratio of the substances in the chemical reaction.
“Two molecules of hydrogen react with one molecule of oxygen to yield two molecules of water.”
Coefficients of 1 are not typically written
Rules for Balancing Equations
You cannot change the formula of any reactant or product.
2. You can only change the coefficients in front
of the reactants and products.

40. 2 HCl + MgBr2 MgCl2 + HBr 2 Balanced H: 1 H: 1 (2) = 2 (2) = 2
Cl: Cl: 2
Mg: 1 Mg: 1
Br: Br: 1
(2) = 2
(2) = 2
(2) = 2
(2) = 2
Balancing Tips:
Find a way to track it that is meaningful to YOU.
Balance metals first, then non-metals.
Balance single elements last.
Check and recount all the atoms.
Prepare for trial and error.

41. 2 LiI + MgO MgI2 + Li2O Balanced
Try using a system (here are dots) to track balanced atoms
– when all reactants have dots, it’s balanced! 2
LiI + MgO MgI2 + Li2O
Balanced
Balancing Tips:
Find a way to track it that is meaningful to YOU.
Balance metals first, then non-metals.
Balance single elements last.
Check and recount all the atoms.
Prepare for trial and error.

42. 2 2 Balanced K(NO3) + Mg Mg(NO3)2 + K Balancing Tips:
Find a way to track it that is meaningful to YOU.
Balance metals first, then non-metals.
If polyatomic ion is intact on both sides – balance as a whole unit.
Balance single elements last.
Check and recount all the atoms.
Prepare for trial and error.

43. Balanced 2 K2O + Cl KCl + O (s) 2 2 (g) 4 2 (g)
Solid potassium oxide and chlorine gas react to produce potassium chloride and oxygen gas. + +
potassium oxide
chlorine
Potassium chloride
oxygen 2
K2O Cl KCl + O
(s) 2 2
(g) 4 2
(g)
Balanced
Strategies:
Isolate the reactants and products (look for key words)
Write the reactants, reform (re-criss cross) the products
The goal is to be able to convert any written equation to an actual equation
Balance and include phases/states (if given)

44. Many reactions are similar.
Chemists have classified 5 types of reactions
BIG PICTURE IDEA:
If you know the reactants - you can guess the type of reaction AND predict the products
Synthesis reactions
Decomposition reactions
Single replacement reactions
Double replacement reactions
Combustion reactions

45. You have to “re-criss cross” the product valences too
Synthesis Reactions (Combination):
2 or more substances react to form a single substance.
A + B  C
You have to “re-criss cross” the product valences too 2
K Cl KCl
Fe O Fe2O3 2 4 3 2

46. Decomposition products can be hard to predict
Decomposition Reactions:
A single compound splits apart, into two or more simpler compounds.
C  A + B
Decomposition products can be hard to predict
CO CO O2
Al2S Al S 2 2 2 3

47. You have to “re-criss cross” the product valences too
Single Replacement Reactions:
One element replaces another element in a compound.
More active elements replace less active elements.
A + BC  AC + B
You have to “re-criss cross” the product valences too 2 2
I CuCl Cl CuI
Ba K(NO3) K Ba(NO3)2 2 2

48. You have to “re-criss cross” the product valences too
Double Replacement Reactions:
2 compounds split and exchange positive ions
AB + CD  AD + CB 2 2
BaF LiBr BaBr LiF
HCl AlBr3 HBr AlCl3 3 3
You have to “re-criss cross” the product valences too

49. CxHy + O2  CO2 + H2O 8 7 3 5 3 4 C7H6O + O2 CO2 + H2O
(Carbon) Combustion Reactions:
Oxygen reacts with a carbon compound to produce water, carbon dioxide and heat.
CxHy + O2  CO H2O
Combustion reactions ALWAYS react with oxygen to produce carbon dioxide and water
C7H6O O CO H2O
C3H O CO H2O 8 7 3 5 3 4

50. Synthesis A + B  C
Decomposition C  A + B
Single replacement A + BC  B + AC
Double replacement AC + BD  AD + BC
Carbon Combustion CxHy + O2  CO2 + H2O