1. Nomenclature International naming system
Unit 4
Nomenclature
International naming system

2. [ ] Types of Bonding Ionic Bonding – between a metal & non-metal
Transfer of e- resulting in a positive ion and a negative ion that are attracted to each other.
Metal – outer energy level (valence orbitals) are emptied
Non – metal – outer energy level (valence orbitals) fill to have the configuration of the next Noble gas.
Covalent Bonding: between Non-metals Sharing of e- in such a way as to complete the outer energy level (valence orbitals) of both (all) atoms. All atoms end up with the e- configuration of Noble gases. [ ]

3. Rules for a molecular formula for an ionic compound
A molecule is made of a positive and negative charged ion.
The positive ion is written first.
The negative ion is written second.
(+) + (-) = 0, the total charge on a molecule must equal zero. Use subscripts to indicate the number of each ion to use.

4. Inorganic binary compounds type I
one atom type (+) cations maintain atom name
one atom type (-) anions change name (-ide)
(+) cation is followed by the (-) anion
Example: NaCl
Sodium chloride
CaF2

5. Inorganic type II – some anions form multiple charges
(the Transition metals)
Use Roman numerals to indicate charge
example: CuCl – copper (I) chloride,
CuCl2 – copper (II) chloride
Or/ higher charge name ends with (-ic) while lower charge name ends with (-ous) example: FeCl3 ferric chloride
FeCl2 ferrous chloride
SnI4
SnI2
2 naming methods: new
&
old

6. Binary Covalent type III – 2 nonmetals
1st element in formula named first with full element name
2nd element named as if anion, end with –ide
Prefixes used to denote number of atoms present
Mono is never used for 1st element
mono hexa - 6
di hepta - 7
tri octa
tetra nona
penta dec

7. Examples: CO
Carbon monoxide
CO2
N2O4

8. Polyatomic – must memorize the names!
Oxy anions: elements with oxygen acting as polyatomic ions
Large number of oxygen (-ate)
Small number of oxygen (-ite)
More than large number of oxygen (per-)
Less than small number of oxygen (hypo-)
Example: perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO1-1
There are a few polyatomic ions without oxygen !

9. MgSO4
MgSO3
LiNO2
LiNO3

10. Naming Acids – when dissolved in H2O they produce free protons (H+)
If anion does not contain oxygen
Use prefix (hydro-) with suffix (-ic) on the anion
example H2S hydrosulfuric acid
If anion does contain oxygen
If anion ends in (-ate) use root name with (-ic) H2SO4 sulfuric acid
If anion ends in (-ite) use root name with (-ous) H2SO3 sulfurous acid
When multiple oxyanion use
Example HClO4 perchlorate perchloric acid
HClO3 chlorate chloric acid
HClO2 chlorite chlorous acid
HClO hypochlorite hypochlorous acid

11. HCl
HNO3
HNO2

12. Combining ions to form compounds and write formulas.
1. Positive and negative ions combine to form neutral compounds.
2. When writing formulas, write the positive ions first. Write the negative ions second.
3. The electrical charge for a compound must be neutral (zero).
Examples:
Sodium chloride
Barium sulfide
Zinc iodide
Nickel phosphate
Ammonium carbonate

13. Writing Formula’s Oxide O-2 Iodide I-1 Sulfate SO4-2 Cyanide CN-1
Hydrogen
H+1
Barium
Ba+2
Chromium
Cr+3

14. Review 1. Potassium chloride Lead (II) iodide Calcium nitrate
Nitrogen dioxide
Acetic acid
2. MgO
CoCl2
(NH4)2S CO
HBr

15. Periodic Table Crossword
Down 2. Affinity 8. Ramsey 14. Ionization 34. Actinide 37. Mosely
Across 6. Carbon 12. Transition 33 Lanthanide

16. Crystals
All solids form geometric figures in which the atoms and molecules are arranged in a regular repeating pattern.
Solid geometric figures are called crystals. Crystals have plane surfaces that are at definite angles to one another.
There are 6 crystal structures.

17. Cubic Tetragonal
Monoclinic Orthorhombic
Triclinic Hexagonal

18. Crystal shape lab PbS FeS2 ZrSiO4 Ca6Al3OH or F(SiO4)5 SiO2 CaCO3 S
1. Cr2K2(SO4)4.24H2O
PbS
FeS2
ZrSiO4
Ca6Al3OH or F(SiO4)5
SiO2
CaCO3 S
BaSO4
CaSO4.2H2O
Ni(NH4)2(SO4)2.6H2O
CuSO4.5H2O