1. NAMING & FORMULA WRITING

2. Examine the number of valence electrons for each atom:
What do you notice?
IONS AND THEIR CHARGES

3. TREND:
-Elements in the same group have the same number of valence electrons
-Thus elements in the same group have similar reactivity
Examine the number of valence
electrons for each atom:
Example:
All alkali
metals
have one
valence
electron
IONS AND THEIR CHARGES

4. - Elements become stable by achieving 8 valence electrons (except for
hydrogen and helium, which achieve 2 electrons)
- Noble gases are non-reactive because they have 8 electrons
- This is called the Octet Rule
The number of valence
electrons can determine
reactivity:
IONS AND THEIR CHARGES

5. How many valence electrons
does each atom need to gain or
lose to achieve a full octet?
Alkali metals
lose 1
electron
Alkali earth
metals lose 2
electrons
Group 13
elements lose 3
electrons
Group 14 elements
lose or gain 4
electrons
IONS AND THEIR CHARGES

6. How many valence electrons
does each atom need to gain or
lose to achieve a full octet?
Group 14
elements lose or
gain 4 electrons
Group 15
elements gain
3 electrons
Group 16
elements gain
2 electrons
Halogens
gain 1
electron
Noble gases
already have
a full octet
IONS AND THEIR CHARGES

7. Ion charges based on family/group:
+1 +2 +3 +/-4 -3 -2 -1 N/A
IONS AND THEIR CHARGES

8. BINARY IONIC COMPOUNDS
MgCl2
magnesium chlorine
ide
= magnesium chloride
1) Naming:

9. Magnesium oxide
Mg O
2 2+ -
SIMPLIFY!!!
= MgO
2) Writing the chemical formula:
BINARY IONIC COMPOUNDS

10. PbI4
lead iodide
Pb I
41
Check charge on non-metal
ion to see if you need to
“un-simplify”
(IV)
= lead (IV) iodide
IONIC COMPOUNDS WITH MULTIVALENT METALS
1) Naming:

11. Copper (II) chloride
Cu Cl
2 1+ -
= CuCl2
2) Writing the chemical formula:
Copper (II) chloride
IONIC COMPOUNDS WITH MULTIVALENT METALS

12. Na2SO4
sodium sulfate
= sodium sulfate
1) Naming:
IONIC COMPOUNDS WITH POLYATOMIC IONS

13. Calcium chlorate
Ca ClO3
2 1+ -
= Ca(ClO3)2
2) Writing the chemical formula:
IONIC COMPOUNDS WITH POLYATOMIC IONS
( )

14. ACIDS
Polyatomic ions have modified names in acids
Polyatomic ion
name
Acid anion name Example
sulfate sulfuric H2SO4 sulfuric acid
chlorate chloric HClO3 chloric acid
carbonate carbonic H2CO3 carbonic acid
phosphate phosphoric H3PO4 phosphoric acid
ACIDS

15. H2SO4(aq)
Sulfuric acid
OXYACID
Most acids have hydrogen
HCl(aq)
Hydrochloric acid
BINARY ACID
ACIDS
1) Naming:

16. bromic acid
BrO3H
1 1+ -
= HBrO3(aq)
ACIDS
2) Writing the chemical formula:

17. mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
NAMING…
• Name both elements (change the
ending of the element on the right
to “ide”
• Put prefixes in front of the element
• Eliminate the prefix “mono” if it is
attached to the first element (the
element on the left)
WRITING THE FORMULA…
• Write the symbols of the elements
• Convert the prefixes to subscripts
MOLECULAR COMPOUNDSNON-METAL + NON-METAL
Prefixes
1
2
3
4
5
6
7
8
9
10

18. mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
Writing the name: PCl5
MOLECULAR COMPOUNDSNON-METAL + NON-METAL
phosphorus chlorine
ide
chloride
1
RULE #3: Eliminate the prefix “mono” if it is
attached to the first element (the element on the
left)
= phosphorus pentachloride

19. Writing the formula: sulfur tetroxide
MOLECULAR COMPOUNDSNON-METAL + NON-METAL
S O1 4
= SO4
Notice how “tetroxide” is NOT spelt as tetraoxide. The “a”
in the prefix is eliminated when its followed by an “o”