1. Chemical Names and Formulas

2. Review
What are ionic compounds?
What are covalent compounds?

3. Relate the forming of compounds to orbital diagrams
Good Examples to use:
NaCl
CaCl2
H2O

4. Always ask this question
Is it ionic or covalent?
Two nonmetals= covalent
Metal and a nonmetal = ionic
Look at the periodic table

6. Naming Molecules
What are molecules?

7. Molecular Nomenclature
CO2
Carbon dioxide
Carbon monoxide CO
What about water?
H2O
Dihydrogen monoxide

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

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

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

13. Naming Ionic compounds
What are ionic compounds?

14. Ionic Nomenclature sodium chloride magnesium nitrate
Charges are called oxidation number
magnesium nitrate
copper(II) chloride
Na+ Cl-
 NaCl
Mg2+ NO3-
 Mg(NO3)2
Cu2+ Cl-
 CuCl2

15. Ionic Nomenclature NO PREFIXES Depends on charges
Charges are called oxidation numbers

16. Ionic Nomenclature – Binary Compounds
potassium chloride
calcium chloride
K+ Cl-
 KCl
Ca2+ Cl-
 CaCl2

17. Ionic Nomenclature – Binary Compounds
NaBr
sodium bromide

18. Ionic Nomenclature Ionic Names
Write the names of both ions, cation first.
Overall charge must equal zero.
Change ending of monatomic ions to -ide.
Polyatomic ions have special names.
Stock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

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

20. Polyatomic Ions
A polyatomic ion is a covalent molecule that has an ionic charge.
Poly = many
Atomic = atoms
Ion = charged particle

21. Polyatomic Ions Examples: Sulfate = SO4-2 Nitrate = NO3-1
Phosphate = PO4-3
Chlorate = ClO3-1
Carbonate = CO3-2
Notice the ending has changed to –ate.

22. Ionic Nomenclature Consider the following:
Does it contain a polyatomic ion?
-ide  no
-ate, -ite,  yes
Does it contain a Roman numeral?
Check the table for metals not in Groups 1 or 2.

23. Ionic Nomenclature – Polyatomic compounds
magnesium nitrate
Mg2+ NO3-
 Mg(NO3)2

24. Ionic Nomenclature – Polyatomic compounds
Na2CO3
sodium carbonate

25. Transition Metals May have more than one charge
For element with more than one charge write the charge using Roman numerals and put it in parenthesis after the elements name
Example:
FeSO4
 Iron (II) Sulfate

26. Ionic Nomenclature – Transition Metals
copper(II) chloride
Cu2+ Cl-
 CuCl2

27. Ionic Nomenclature – Transition Metals
SnCO3 tin(II) carbonate

28. Practice
Practice ions and molecules before adding acids

29. Naming Acids

30. Definition Acid Compound that forms H+ in water.
Formula usually begins with ‘H’.
All of ours will start with ‘H’.
Examples:
HCl, HNO3, H2SO4

31. Acid Names
4.) If the root has a prefix, keep it.

32. Acid names HBr H2CO3 H2SO3 Other Hydrogen Bromide hydrobromic acid
Hydrogen Carbonate
carbonic acid
H2SO3
Hydrogen Sulfite
sulfurous acid
Other
HClO
Hydrogen Hypochlorite
hypochlorous acid
HClO4
Hydrogen Perchlorate
perchloric acid

33. Acid Formulas hydrofluoric acid sulfuric acid nitrous acid -ide  HF
-ate
 H2SO4
-ite
 HNO2