1: Atoms vs. ions
Potassium (K): 19 protons e ¯
19 e ¯
Potassium atom: K
Bridging nomenclature
18 e ¯
Potassium ion: K +
1
1: Atoms vs. ions
Chlorine (Cl): 17 protons e ¯
17 e ¯
Chlorine atom: Cl
Bridging nomenclature
18 e ¯
Chloride ion: Cl −
1: Molecules vs Polyatomic ions
Neutral Molecule Charged
Polyatomic Ion e ¯ e ¯
2-
O
S
S O O
O O
O
Sulfur trioxide molecule
SO
3
Bridging nomenclature
Sulfite ion
SO
3
2
¯
3
2
1

2: Ionic Bonding e ¯
Potassium atom: K
Bridging nomenclature
2: Ionic Bonding
Chlorine atom: Cl
4
Bridging nomenclature
2: Ionic Bonding
Potassium ion: K + KCl
Potassium Chloride
Chloride ion: Cl
−
Bridging nomenclature
6
5
2

3: Using the Periodic table: Main Group
Main Group Elements
Bridging nomenclature
3:Using the Periodic Table:Transition Group
Transition Metals
Form various cations by loss of electrons e.g. Fe 2+ / Fe 3+ ,
Cu + / Cu 2+
Cr 2+ / Cr 3+
Bridging nomenclature
8
4: Binary Compounds: Names, Formulae
RULE for formula continued: if cation has two or more possible charges
Roman numerals immediately after the cation to indicate its charge
These are typically Transition Metals
Cl
−
Cu 2+ Cl
−
Cu + Cl
−
CuCl
Copper (I) Chloride
Bridging nomenclature
CuCl
2
Copper (II) Chloride
9
7
3

4: Binary Compounds: Names, Formulae
RULE for formula continued: if cation has two or more possible charges
Roman numerals immediately after the cation to indicate its charge
These are typically Transition Metals
Fe 2+
O 2
− O 2
−
Fe 3+ O 2
−
Fe 3+
O 2
−
Fe
2
O
3
Iron (III) Oxide
Bridging nomenclature
FeO
Iron (II) Oxide
10
5: Covalent bonding
Electrons are shared , not transferred
Usually occurs between non-metals
H H
Bridging nomenclature
5: Covalent bonding: Diatomic Elements
Electrons are shared , not transferred
H H
Usually occurs between non-metals
Some elements are always sharing
Bridging nomenclature
12
11
4

5: Covalent bonding: Diatomic Elements
H
2
N
2
O
2
The Halogens
F
2
Cl
2
Br
2
I
2
At
2
Bridging nomenclature
13
6: Naming Binary Covalent Compounds
RULE for naming
Most metallic element / space / least metallic element
Bridging nomenclature
14
6: Using the Periodic Table
Non-metals
Metals
Bridging nomenclature
Metalloids
15
5

6: Using the Periodic Table
Naming order: Metal first, Non-Metal second
Periodic table
Least Metallic
Most Metallic
Metallic character decreases across and up PT
Bridging nomenclature
16
7: Binary Covalent Compounds
RULE for naming
Most metallic element / space / least metallic element
CO
Carbon (II) Oxide
Bridging nomenclature
17
7: Binary Covalent Compounds
RULE for naming continued
When more than one binary compound from the two elements is possible, use the prefixes mono-, di-, tri- etc.
Carbon mon oxide
CO
CO
2
Carbon di oxide
Bridging nomenclature
18
6

7: Binary Covalent Compounds
RULE for naming continued
When more than one binary compound from the two elements is possible, use the prefixes mono-, di-, tri- etc.
Sulfur di oxide
Bridging nomenclature
19
7: Naming: No Prefixes
RULE for naming continued
When more than one atom of an element is present in each molecule, it is not stated in the name when it is implied by what we know about combining capacities.
E.g.
Cl
−
Cu 2+ Cl
−
CuCl
2
Copper (II) Chloride
Copper (II) Dichloride
Bridging nomenclature
20
7: Naming: No Prefixes
RULE for naming continued
When more than one atom of an element is present in each molecule, it is not stated in the name when it is implied by what we know about combining capacities.
E.g.
Br − Aluminium Bromide
Aluminium (III) Tribromide
Bridging nomenclature
Br −
Al 3+
Br −
AlBr
3
21
7

8: Naming: Polyatomic ions
• Ions that themselves are composed of two or more atoms with covalent bonding
• Formulae are written like molecular formulae with superscripted charge
+
NH
4
+
H
Cl
−
Ammonium ion
N
H
H
H
4
Ammonium chloride
Bridging nomenclature
22
8: Naming: Polyatomic ions
• If the polyatomic ion is present more than once, brackets are required in the formula
¯
NO
3
¯
O
O
O
3
3
¯
Fe 3+
N
O O
O
O
N
N
O
¯
O
Bridging nomenclature
23
8: Naming: Polyatomic ions
SO
4
2-
2
4
3
O
O
S
O
O
O
S
O
2Al 3+
O
O
Al 3+
S
O
O
Bridging nomenclature
O
2-
2-
O
24
8

9: CHEMICAL EQUATIONS:
Representing chemical change
• Chemical change results in pure substances transforming into other pure substances.
• A chemical reaction occurs when at least one chemical involved changes its elemental composition
Bridging nomenclature
25
9: Equation Components
“+” used if there is more than one reactant or product
“React together to yield”
HCl + NaOH
H
2
O + NaCl
REACTANTS
Species that exist before the reaction occurs
Bridging nomenclature
PRODUCTS
Species formed from the reaction
26
9: Law of conservation of Mass
• During a reaction there is no detectable gain or loss of mass i.e.
mass is conserved
• Cannot make / destroy atoms
• Same number and type of atoms at beginning and end of reaction
HCl + NaOH
H
2
O + NaCl
Bridging nomenclature
27
9

10: Coefficients: Indicating how many of each component
A coefficient indicates more than one molecule of that species
2 HCl + Ca(OH)
2
2 H
2
O + CaCl
2
N.B.: HCl and H
2
O formulae unchanged
Bridging nomenclature
28
10: Coefficients vs. Formulae subscripts
2 Cl Cl
Bridging nomenclature
Cl Cl
29
H
10: Coefficients: Indicating how many of each component
2 HCl + Ca(OH)
2
2 H
2
O + CaCl
2
H Cl
O
H H
H Cl O
+
H H
+
O
¯
Ca 2+
¯
O H Cl ¯ Ca 2+ Cl ¯
Bridging nomenclature
30
10

10: Balancing chemical equations:
1. Write the unbalanced equation showing the reactants and the products
2. Adjust the coefficients on each side to give equal numbers of atoms of each element
3. Adjust the coefficients on each side to give equal numbers of charges on each side
4. In 2 and 3, Do not change formulae
Bridging nomenclature
31
10: Balancing chemical equations
Solid mercury(II) oxide decomposes on heating to liquid mercury metal and oxygen gas
2 HgO
(s)
2 Hg
(l)
+ O
2(g)
32 Bridging nomenclature
10: Balancing chemical equations
Solid zinc sulfide is reacted with oxygen gas to produce zinc oxide and sulfur dioxide
2 ZnS
(s)
3
2(g)
→
2 ZnO
(s)
2
2(g)
Bridging nomenclature
33
11

10: Balancing chemical equations
Zn 2+ S 2
−
2 ZnS
(s)
O
+ O
2(g)
O
Zn 2+
O 2
−
→ 2 ZnO
Zn 2+
(s)
O 2 −
Zn 2+ S 2
−
O O
O
2
2(g)
S
O
O O
S
O O
Bridging nomenclature
34
10: Balancing chemical equations
Propane gas is reacted with oxygen gas to produce liquid water and carbon dioxide.
C
3
H
8(g)
5
2(g)
→ 3 CO
2(g)
4
2
O
(l)
35 Bridging nomenclature
10: Balancing chemical equations
Sulfuric acid in aqueous solution is reacted with calcium hydroxide solution to produce water and solid calcium sulfate
H
2
SO
4(aq)
+ Ca(OH)
2(aq)
→
H
2
O
(l)
+ CaSO
4(s)
H
2
SO
4(aq)
+ Ca(OH)
2(aq)
→
2 H
2
O
(l)
+ CaSO
4(s)
Bridging nomenclature
36
12

10: Balancing chemical equations
Sodium hydroxide solution is reacted with dilute phosphoric acid to produce sodium phosphate and water
NaOH
(aq)
+ H
3
PO
4(aq)
→
Na
3
PO
4(aq)
+ H
2
O
3 NaOH
(aq)
+ H
3
PO
4(aq)
→
Na
3
PO
4(aq) 2
O
Bridging nomenclature
37
10: Indicating state of reactants, products
NaCl
(aq) means common salt – sodium chloride, dissolved in water
NaCl
(l) means common salt – raised to a temperature high enough for the salt to melt
>801C
HCl
(g)
HCl
(aq) is hydrogen chloride gas is hydrochloric acid
Bridging nomenclature
38
13