1. Unit 5: Bonding Nomenclature! (Is a fancy word for naming things)
There are 3 types of compounds you need to know how to name & write formulas for:
Ionic (we already learned that!)
Molecular (aka Covalent)
Acid (a special type of covalent)

2. A. Ionic FORMULAS
Write each ion, cation first. Don’t show charges in the final formula.
Overall charge must equal zero.
If charges cancel, just write symbols.
If not, use subscripts to balance charges.
Use parentheses to show more than one polyatomic ion.
Roman numerals indicate the ion’s CHARGE

3. A. Ionic NOMENCLATURE Write the names of both ions, cation first.
Change ending of monatomic ions to -ide.
Polyatomic ions have special names. Don’t change endings!
Use Roman numerals to show the ion’s charge (except s-block, Ag, Zn, Al).
Overall charge must equal zero.

4. A. Ionic Nomenclature Consider the following:
Does it contain a polyatomic ion?
-ide, 2 elements  no
-ate, -ite, 3+ elements  yes
Does it contain a Roman numeral?
Check the table for metals not in Groups 1 or 2.
No prefixes!

5. A. Ionic Nomenclature
Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

6. A. Ionic Nomenclature potassium chloride magnesium nitrate
copper(II) chloride
K+ Cl-
 KCl
Mg2+ NO3-
 Mg(NO3)2
Cu2+ Cl-
 CuCl2

7. A. Ionic Nomenclature NaBr Na2CO3 sodium bromide FeCl3
sodium carbonate
iron(III) chloride

8. B. Molecular Nomenclature
Prefix System (binary compounds)
1. Less e-neg atom comes first.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the second element to -ide.

9. B. Molecular Nomenclature
PREFIX
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
NUMBER 1 2 3 4 5 6 7 8 9 10

10. B. Molecular Nomenclature
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride

11. B. Molecular Nomenclature
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10

12. B. Molecular Nomenclature
Remember the Seven Diatomic Elements!
Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

13. C. ACIDS! Acids Compounds that form H+ in water.
Formulas usually begin with ‘H’.
Examples:
HCl – hydrochloric acid
HNO3 – nitric acid
H2SO4 – sulfuric acid

14. C. Acid Nomenclature

15. C. Acid Nomenclature

16. C. Acid Nomenclature HBr H2CO3 H2SO3 2 elements, -ide
 hydrobromic acid
3 elements, -ate
 carbonic acid
3 elements, -ite
 sulfurous acid

17. C. Acid Nomenclature hydrofluoric acid sulfuric acid nitrous acid
2 elements
 H+ F-
 HF
3 elements, -ic
 H+ SO42-
 H2SO4
3 elements, -ous
 H+ NO2-
 HNO2