1. Chapter 6 Nomenclature of Inorganic Compounds
Objectives:
Distinguish between common and systematic names of compounds
Review differences between elements and ions
Be able to write formula from names of compounds
Understand binary compounds
Name compounds containing polyatomic ions
Name and recognize acids

2. Common and Systematic Names
Common Names
Arbitrary
Not based on chemical composition
Historically associated with a physical or chemical property
Not consistent among languages or disciplines
Systematic names
Identify the chemical composition
Devised by IUPAC

3. Elements and Ions Diatomic molecules Polyatomic Ion
2 atoms of same element
H2, O2, N2, F2, Cl2, Br2, I2
Polyatomic
3 or more atoms of same element
Sulfur (S8) and Phosphorus (P4)
Ion
Charged particle
Positive (cation)
Negative (anion)
IUPAC – international union of pure and applied chemistry 1921 – still meets regularly
Diatomic – just normal name
Polyatomic – more than 2
ion

4. Elements and Ions Naming cations Naming anions
Same as element but add the word ion
Potassium ion
Naming anions
Stem of the parent name with ending changed to –ide
Add the word ion
Oxide ion
Commonly formed ions – figure 6.2 pg 107
Need to know figure 6.2 by memory
Should be familiar after chapter 11

5. Writing Formulas from Names of Compounds
Chemical compounds must have a net charge of zero
Compare charges of ions formed from elements
“Trade” charges and rewrite as subscript on opposite ion
Write with lowest possible whole numbers

6. Writing Formulas from Names of Compounds
Write formulas for
Sodium and chlorine
Aluminum and oxygen
Na1+
Cl1-
NaCl
Al2O3
Al3+
O2-

7. Writing Formulas from Names of Compounds
Write formulas for the following
Calcium chloride
Calcium will form Ca2+
Chlorine will form Cl1-
Formula is CaCl2
Magnesium oxide
Magnesium will form Mg2+
Oxygen will form O2-
Formula is MgO

8. Writing Formulas from Names of Compounds
Barium phosphide
Barium will form Ba2+
Phosphorus will form P3-
Formula is Ba3P2
Sodium sulfide
Sodium will form Na+
Sulfur will form S2-
Formula is Na2S

9. Binary Compounds Contain only two different elements
Often metal with nonmetal (binary ionic compound)

10. Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation
Name of cation is left the same
Name of anion is changed (-ide)
Write formulas for the following compounds
Strontium chloride
Strontium is Sr2+ and Chlorine is Cl-
Calcium sulfide
Calcium is Ca2+ and Sulfur is S2-
SrCl2
CaS

11. Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations
Metals in the center of the periodic table
Iron can be Fe2+ or Fe3+
Stock System
Use Roman Numeral to designate charge of cation
Copper (II) Chloride is CuCl2
Tin (IV) Oxide is SnO2
-ous and –ic endings are also sometimes used
-ous and –ic endings are OLD SYSTEM – should know common ones such as iron and copper…others almost always listed in Stock System
Ferrous = 2+
Ferric = 3+
Cuprous = +
Cupric = 2+

12. Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations
Write the name for each of the following compounds
PbI2
Fe2O3
CuO
TiF4
Lead (II) Iodide
Iron (III) Oxide
Copper (II) Oxide
Titanium (IV) Fluoride

13. Binary Compounds Containing Two Nonmetals
Not ionic bonds - Molecular (covalent)
Different system of naming
Element that occurs first in the series below is written and named first
Si, B, P, H, C, S, I, Br, N, Cl, O, F
Usually given to you…first element listed always named first
Second element retains –ide ending

14. Binary Compounds Containing Two Nonmetals
Prefix is attached to each element to indicate the number of atoms of that element in the molecule
Mono (1) never used for first element
Prefix
Meaning
Mono 1
Hexa 6 Di 2
Hepta 7
Tri 3
Octa 8
Tetra 4
Nona 9
Penta 5
Deca 10

15. Binary Compounds Containing Two Nonmetals
Examples:
N2O is dinitrogen monoxide (drop “o”)
S2F10 is disulfur decofluoride
You try:
P2O5
CBr4
NH3
Diphosphorus pentoxide
Carbon tetrabromide
Nitrogen trihydride

16. Acids Derived from Binary Compounds
Hydrogen compounds – form acids in water
Write symbol of H first, then the rest
Shows it is an acid
Naming
Take stem of nonmetal
Add prefix hydro-
Add suffix –ic
Add the word acid
Not ALL hydrogen compounds form acids – methane (CH4), ammonia (NH3) – H written after another

17. Acids Derived from Binary Compounds
H2S
Hydrogen sulfide (if not in water)
Hydrosulfuric acid
HCl
Hydrogen chloride (if not in water)
Hydrochloric acid
Figure 6.4 on page 115
VERY HELPFUL FOR NAMING BINARY COMPOUNDS

18. Naming Compounds Containing Polyatomic Ions
Must be able to recognize common polyatomic ions
Table 6.6 (pg 116)

19. Naming Compounds Containing Polyatomic Ions
Usually end in –ate or –ite (but not always)
-ate indicates
-ite indicates
Nitrate is NO3-
Nitrite is NO2-
Hypo-
(if more than two varieties)
ClO- hypochlorite
ClO2- chlorite
ClO3- chlorate
ClO4- hyperchlorate
or perchlorate

20. Naming Compounds Containing Polyatomic Ions
Need to recognize polyatomic ions in Table 6.6
Hydroxide (OH-)
Cyanide (CN-)

21. Naming Compounds Containing Polyatomic Ions
Naming follows binary compound rules

22. Naming Acids Oxy-acids
Inorganic compounds containing hydrogen, oxygen, and one other element
Change ending of polyatomic ion
Add the word “acid”
See figure 6.5 page 120
HC2H3O2
Hydrogen & acetate ion
Acetic acid

23. Homework Questions #1,3,6 Paired Exercises #7-25 odd
Additional Exercise #34 & 36
Remember: Quiz next class 