1. 1

2. Nomenclature
Names and formulas

3. Using Flow Charts

7. Ionic Formulas
Ions combine in small, whole number proportions so that the sum of oxidation numbers will be zero!
Cations retain the name of the element and always comes first.
Anions keep the root name but add “ide” ending.

8. Examples… Lithium + chlorine magnesium + bromine Lithium Chloride
aluminum + oxygen
Lithium Chloride
Magnesium Bromide
Aluminum Oxide

9. Transition Metals
Some of the transition metals have variable oxidation numbers.
(They have more than one.)
Roman numerals are used to indicate oxidation numbers for elements with variable oxidation states.
Roman numerals are always positive!

10. Examples… Nickel (III) oxide Nickel (II) oxide Ni2O3 Fe2O3 FeO NiO
Iron (III) Oxide
Iron (II) Oxide

11. Polyatomic Ions
a group of atoms that stay together and have one oxidation number.
They combine like single atom ions, so that the total charge must be zero.
No name change here

12. Examples… Na 1+ and SO4 2- Ca 2+ and OH1- NH4 1+ and O2-
NH4 1+ and PO4 3-
Sodium Sulfate
Calcium Hydroxide
Ammonium Oxide
Ammonium Phosphate

13. POLYATOMIC IONS (charged building blocks) Polyatomic ions are mostly made of two non-metals.
Ions with -1 charge
perbromate BrO4-1
bromate BrO3-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
acetate C2H3O2-1
Permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1

14. Name Origins “ate” suffix most common bromate BrO3-1
“ite” suffix 1 oxygen less
than “ate”
bromite BrO2-1
“hypo” prefix 1 oxygen less
than “ite”
hypobromite BrO-1
“per” prefix 1 oxygen more
than “ate
perbromate BrO4-1

15. Name Covalent Bounds Covalent Bonds NO2 CO2 PO3 SF4 SO3
Between 2 or more non-metals
NO2
CO2
PO3
SF4
SO3

16. Naming Molecules The least electronegative element comes first.
Increases Left to Right
Decreases top to bottom
2. A prefix is always used for the first and second element to indicate quantity and the suffix “ide” is applied

17. The ability of an atom to attract the electrons of another
Electronegativity
The ability of an atom to attract the electrons of another
atom when bonded
INCREASING
DECREASING

18. Prefixes to Know 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa
7 = hepta
(NEVER use the prefix Mono on the first element )

19. Examples… PCl3 NH3 P2O5 I4O7 SCl6 PO5 H2O phosphorus trichloride
nitrogen trihydride
diphosphorus pentoxide
tetraiodine heptoxide
sulfur hexachloride
phosphorus pentoxide
dihydrogen monoxide
NH3
P2O5
I4O7
SCl6
PO5
H2O

20. Examples… CO2 CO SO3 N2O3 N2O5 AlCl3 Carbon Dioxide Carbon Monoxide
Sulfur Trioxide
Dinitrogen Trioxide
Dinitrogen Pentaoxide
Aluminum Trichloride