1. Formula Writing and Nomenclature

2. What is an ion? An ion is a ______________.
It may be a ____ or ___charge.
Lose electrons  cation (+)
Gain electrons  anion (-)
charged particle. + -

3. Why do atoms gain or lose electrons?
To become more ______.
Electrons come from ___________.
One ion ______ e- and the other _____e- to form a _____.
stable
other atoms
loses
gains
bond

4. Do ions follow rules? YES!
Octet Rule: _____________
Tendency of valence electrons to rearrange to form a ________________ .
THE MAGIC NUMBER=________
The Rule of 8
stable/full valence shell
Happy Ion

5. Opposites attract! NaF
Examples: +1 Na F -1 -1 8
Opposites attract! NaF

6. Do ions follow rules? YES!
Duet Rule:___________
For atoms so small their valence shell is the ______ energy level which can only hold ___________.
The Rule of 2
first
two electrons

7. Examples: H can gain ___ e- to form _____.
H can lose ____ e- to form_____.
Li loses _____ e- to form _____.
Be loses ____ e- to form _____.
B loses _____ e- to form _____. 1
H-1 1
H+1 1
Li+1 2
Be+2 3
B+3

8. Writing Formulas All compounds have a charge of zero.
When writing formulas, all ions have to add up to zero.

9. IUPAC
IUPAC- International Union of Pure and Applied Chemists (created this naming system)

10. Forming Binary Ionic Compounds
Binary = two elements
Ionic = one metal and one nonmetal
Transfer of electrons
Not called molecules!

11. Writing Binary Ionics Write each ion (metal first)
Crisscross the charges
Drop the + and –
Write numbers as subscripts

12. Binary Ionic Compounds
Example:
magnesium chloride
Mg+2
Cl-1
MgCl2

13. Why does this work?
MgCl2 means…
Cl-1
Mg+2
Cl-1

14. Binary Ionic Compounds
Example:
barium oxide
Ba+2
O-2
BaO
Ba2O2

15. Practice Sodium bromide Calcium fluoride Magnesium oxide Lithium oxide
Aluminum oxide
Magnesium fluoride
Potassium iodide
Aluminum sulfide
NaBr
CaF2
MgO
Li2O
Al2O3
MgF2 KI
Al2S3

16. Forming Ternary Ionics
Contain 3 or more elements
Combination of a metal and a polyatomic ion (Table E)

18. Writing Ternary Ionics
Write each ion (positive first)
Crisscross the charges
Drop the + and –
Write numbers as subscripts
Keep polyatomic ions in parentheses if more than 1
Never change a polyatomic ion!!!!!

19. Ternary Ionic Compounds
Example:
ammonium chloride
NH4+1
Cl-1
NH4Cl

20. Ternary Ionic Compounds
Example:
lithium carbonate
Li+1
CO3-2
Li2CO3

21. Ternary Ionic Compounds
Example:
calcium hydroxide
Ca+2
OH-1
Ca(OH)2

22. Why does this work?
Ca(OH)2 means…
OH-1
Ca+2
OH-1

23. Practice Magnesium hydroxide Potassium sulfate Sodium phosphate
Calcium nitrate
Mg(OH)2
K2SO4
Na3PO4
Ca(NO3)2

24. Stock System for Ionics
Some metals can have more than one oxidation state (i.e. transition metals)
Use roman numerals
Examples:
Copper (I) chloride
Cu+1
Cl-1
CuCl
Copper (II) chloride
CuCl2
Cu+2
Cl-1

25. Practice Mercury (II) oxide Vanadium (V) bromide Copper (I) oxide
Tin (IV) bromide
HgO
VBr5
Cu2O
SnBr4

26. Forming Molecular Compounds
Composed of two non-metals
Electrons are shared so no ions are formed (covalent bonding).
Called molecules
Prefix system- tells you how many atoms of each element

27. Prefixes prefix meaning Mono- 1 Di- 2 Tri- 3 Tetra- 4 Penta- 5 Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10

28. Molecular Compounds CO CO2 PCl3 PCl5 CCl4 Examples Carbon monoxide
Carbon dioxide
Phosphorous trichloride
Phosphorous pentachloride
Carbon tetrachloride CO
CO2
PCl3
PCl5
CCl4

29. Practice Phosphorous trichloride Dichlorine monoxide
Sulfur tetrafluoride
Dinitrogen trioxide
Iodine monochloride
PCl3
Cl2O
SF4
N2O3
ICl

30. Naming Ionic Compounds
Ionic Compounds (formula units)- Metal and non-metal
Write cation name first (use roman numerals if more than one oxidation state). 1.
Write the first syllable of the anion and add –ide. OR just name the polyatomic ion. 2.

31. Examples: Ionics LiBr Na2SO4 CuCl2 lithium bromide sodium sulfate
copper (II) chloride

32. Naming Molecular Cmpds
Molecular Compounds (molecules)- two non-metals
Use prefix system on first element (except Mono). 1.
Use prefix system on the second element (including mono) and add –ide ending. 2.

33. Examples: Molecular N2O5 CO PCl3 Dinitrogen pentoxide Carbon monoxide
Phosporous trichloride

34. Empirical Formulas vs. Molecular Formulas
Compounds exist with a definite ratio of atoms (ex: water has 2 H per 1 O)
Empirical formula: lowest whole number ratio
Molecular formula: actual formula (can be empirical also).

35. Examples C2H8 is a molecular formula (can be reduced).
CH4 is an empirical formula (can’t be reduced).