Chapter 6 Nomenclature of Inorganic Compounds

1. Chapter 6Nomenclature 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 • 2 atoms of same element • Polyatomic • 3 or more atoms of same element • Ion • Positive • Negative

4. Elements and Ions • Naming cations • Same as • Naming anions • Stem of the parent name with • Add • Commonly formed ions – figure 6.2 pg 107

5. Writing Formulas from Names of Compounds • Chemical compounds must have a net charge of • Compare charges of ions formed from elements

6. Writing Formulas from Names of Compounds • Write formulas for • Sodium and chlorine • Aluminum and oxygen

7. Writing Formulas from Names of Compounds • Write formulas for the following • Calcium chloride • Calcium will form • Chlorine will form • Formula is • Magnesium oxide • Magnesium will form • Oxygen will form • Formula is

8. Writing Formulas from Names of Compounds • Barium phosphide • Barium will form • Phosphorus will form • Formula is • Sodium sulfide • Sodium will form • Sulfur will form • Formula is

9. Binary Compounds • Contain only • Often

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 • Calcium sulfide

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 • Stock System • Use Roman Numeral to designate • Copper • Tin • -ous and –ic endings are also sometimes used

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

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 • Second element

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

15. Binary Compounds Containing Two Nonmetals • Examples: • N2O is • S2F10 is • You try:

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

17. Acids Derived from Binary Compounds • H2S • HCl Figure 6.4 on page 115 VERY HELPFUL FOR NAMING BINARY COMPOUNDS

18. Naming Compounds ContainingPolyatomic Ions • Polyatomic ion • Similar to naming binary compounds • Must be able to recognize common polyatomic ions • Table 6.6 (pg 116)

19. Naming Compounds ContainingPolyatomic Ions • Usually end in • Hyper- or per- indicates • -ate indicates • -ite indicates • Nitrate is • Nitrite is • Hypo- indicates ClO- hypochlorite ClO2- chlorite ClO3- chlorate ClO4- hyperchlorate or perchlorate

20. Naming Compounds ContainingPolyatomic Ions • Need to recognize polyatomic ions in Table 6.6

21. Naming Compounds ContainingPolyatomic Ions • Naming follows binary compound rules • NaHCO3 • See page 118

22. Naming Acids • Oxy-acids • Inorganic compounds containing hydrogen, oxygen, and one other element • Hydrogen is the • Second part is a • Change ending of polyatomic ion • Add the word “acid” • HC2H3O2 • Hydrogen & acetate ion • Acetic acid