1. Stock System-New Naming System
Some metal elements can form two or more cations with a different charge. The stock system denotes the specific ion by putting the charge in ( ).
Example:
Iron (II) has a + 2 charge
Iron (III) has a +3 charge

2. Other common examples Lead (II) has a +2 charge
Lead (IV) has a +4 charge
Tin (II) has a + 2 charge
Tin (IV) has a +4 charge
Copper (I) has a +1 charge
Copper (II) has a +2 charge

3. Old Nomenclature-Don’t have to memorize these
Copper (I) – cuprous
Copper (II) – cupric
Iron (II) – ferrous
Iron (III) – ferric
Tin (II) – stannous
Tin (IV) – stannic
Lead (II) – plumbous
Lead (IV) – plumbic

4. Naming ionic compounds
Nomenclature-naming system
Positive ions is first, then negative ion
Ex: sodium chloride NaCl

5. Practice Write formulas for the following: Copper (II) Sulfate
CuSO4
Iron (III) oxide
Fe2O3
Zinc (II) sulfide
ZnS
Vandium (IV) chloride
VCl4
Cobalt (III) Nitrite
Co(NO3)3

6. Practice -

7. Compounds containing Polyatomic ions
Treat the polyatomic ion as a single atom
Always put polyatomic ion in parentheses if there is more than 1 of them
Example: ammonium chloride
NH4Cl
Practice
Barium Nitrate
Ba(NO3)2
FeSO4
iron (II) sulfate

8. Naming Molecular Compounds
Old way of naming Molecular Compounds requires the Use of prefixes. (memorize These)
1 = mono
2 = di
3 = tri
4 = tetra
5 = penta
6 = hexa
7 = hepta
8 = octa
9 = nona
10 = deca

9. Naming Binary Molecular Compounds: Compounds with 2 elements
The least EN Atom goes first
C,P,N,H,S,I,Br,Cl,O,F
The element is given a prefix if it contributes more than one element to the molecule.
The second element: Combine a prefix with the root of that element with -ide at the end.
Dioxide, pentoxide
This is true for most molecules containing 2 elements
The o or a at the end of a prefix is usually dropped when the name of the element begins with a vowel

10. Practice CO Carbon Monoxide CO2 Carbon Dioxide CCl4
Carbon TetraChloride
SiF4-
Silicon Tetraflouride
Nitrogen Monoxide NO
N2O3
Dinitrogen Trioxide
Phosphorus Trichloride
PCl3

11. Acids
Oxyacid-Acids that contain hydrogen, Oxygen and another atom (usually a non-metal)
H3PO4: Phosphoric Acid
HNO2: Nitrous Acid
Usually made from polyatomic ions and the addition of enough Hydrogens to balance out the ion.

12. Acids Naming: Practice HNO2 Sulfuric Acid
Decide which polyatomic Ion is being used and use that rootword
Polyatomic ions that end in
ate  ic
ite  ous
Rootword(ic or ous) and Add Acid
Practice
HNO2
Nitrous Acid
Sulfuric Acid
H2SO4

13. Acids
Binary Acids-Acids that consist of 2 elements: usually Hydrogen and one of the Halogens (there are others)
HCl: Hydrochloric Acid
HF: Hydroflouric Acid
Naming:
Hydro goes first
Add the name of the second atom with ic at the end
H2S
Hydrosulfuric Acid
Hydrobromic Acid
HBr

14. Acids-Practice HI CH3COOH Sufurous Acid Carbonic Acid H2CO3
Hydroiodic Acid
CH3COOH
Acetic Acid
Sufurous Acid
H2SO3
Carbonic Acid
H2CO3

15. Using Chemical Formulas
Subscript indicates how many moles of that atom or polyatomic ion are in 1 mole of that compound.
KNO3
Na2SO4
Ca(OH)2
(NH4)2SO3

16. Using Chemical Formulas
Formula mass-sum of all the average atomic masses of all elements in compound.
Ex: H2SO4
2 Hydrogen 2 x = 2.02
1 Sulfur x =32.07
4 Oxygen x = total = OR
EX: NaCl
1 sodium ion
1 Chloride ion
total=

17. Practice
(NH4)3(PO4)
Al2O3
Na2O

18. Molar Mass as a Conversion Factor
Converting between moles and grams with compounds.
1st calculate formula mass of given compound. (unit gram/mole)
2nd convert either by multiplying or dividing by the formula mass
molesgrams (x) by formula mass
Gramsmoles (divide) formula mass

19. Practice What is the mass of 4.5 moles of Ca(CO3)?
4.5 x 102 g Ca(CO3)
What is the mass of 2.0 moles of Na(NO3)?
1.7 x 102 g Na(NO3)
How many moles are contained in 25.0 grams of AgCl?
.174 mol AgCl
How many moles are contained in 5.0 grams of ZnCl2?
.037 mol ZnCl2

20. Percent Composition
Gives the percent by molar mass of each element in a compound.
1st calculate the total molar mass of the compound
H2SO4
2 H x =
1 S x = 32.07
4 O x = 64.00
98.09

21. continued 2nd Divide each individual atoms mass by the total mass.
3rd Multiply each by 100 (or move decimal two places to the right)
2 H x = /98.16 = =2.05%
1 S x = 32.07/98.16 = =32.7%
4 O x = 64.00/98.16 = =65.2%
Check to make sure % adds to 100
(or close to 100)
More Practice Pg 244 Practice Problems
ZnSO4•7H2O
42.85%

22. Determining Chemical Formulas
Empirical formula-symbols of elements in compound showing the smallest whole number ratio.
Convert percents of elements in a compound into formula.

23. How to: 1st change % to grams 2nd convert grams to moles
3rd divide each by the least
Ex: Determine the formula of a compound made up of the following percents:
% Na
% S
% O

24. Practice problems 1-3 p.247

25. Molecular formulas Actual formula of a molecular compound
C2H4 simplifies to CH2
C3H6 simplifies to CH2
C2H4 (ethene) and C3H6 (cyclopropane)

26. How the empirical formula relates to the molecular formula:
EF = empirical formula
MF = molecular formula
X( EF) = (MF)
1st solve for x
X= (MF)/(EF)
HINT-BIG NUMBER ALWAYS GOES ON TOP
Multiply (EF) by x to get the molecular formula

27. Example
The empirical formula of a cpd of phosphorus and oxygen was found to be P2O5. the molar mass of this cpd is g/mol. What is the cpd’s molecular formula?

28. Practice Problems 1-2 p. 249

29. Give the formula for the following:
1. potassium oxide
2. lithium phosphide
3. aluminum chloride
4. calcium bromide
5. iron(II)oxide
6. iron(III)oxide
7. tin(IV)fluoride
8. copper(II)chloride
9. lead (II) sulfide
10. magnesium chloride

30. Determine the molecular formula:
1. Emperical formual = CH, molar mass = 78 g/mole
2. Emperical formula = NO2, molar mass = g/mol
3. Mesitylene has an empirical formula of C3H4. What is the molecular formula(mass 121)?