1. Naming Polyatomic Ions
Didn’t you say we had to memorize these?
Lets look at the polyatomic ions and how they differ!!!

2. NO-1
Hyponitrite
NO2-1
Nitrite
NO3-1
Nitrate
NO4-1
Pernitrate

3. Acids
Acids are molecular compounds that form H+ when dissolved in water
Sour taste
Dissolve many metals
Like Zn, Fe, Mg, but not Au, Ag, Pt.
Formula generally starts with H
E.g., HCl, H2SO4.

4. Acids, Continued Contain H+1 cation and anion
In aqueous solution
Binary acids have H+1 and nonmetal
Oxyacids have H+1 and polyatomic

5. Naming Binary Acids Write a hydro- prefix.
Follow with the nonmetal name.
Change ending on nonmetal name to –ic.
Write the word acid at the end of the name.

6. Let’s try a Few
HBr HF HI

7. HBrO4 HBrO3 HBrO2 HBrO Naming Oxyacids Perbromic Acid Bromic Acid
Bromous Acid
HBrO2
Hypobromous Acid
HBrO

8. Practice─Name the Following
H2S
HClO3
HNO2

9. Writing Formulas for Acids
When name ends in acid, formulas starts with H.
Hydro- prefix means it is binary acid, no prefix means it is an oxyacid.
For an oxyacid, if ending is –ic, polyatomic ion ends in –ate; if ending is –ous, polyatomic ion ends in –ous.

10. Practice—What Are the Formulas for the Following Acids?
Chloric acid
Phosphoric acid
Hydrobromic acid

11. Tro's "Introductory Chemistry", Chapter 5

12. Lets Try a Few!! Potassium Chloride Aluminum Oxide Potassium Sulfide
Magnesium Hydroxide

13. Lets Try A few
HNO3
H2SO4
H2SO3

14. Formula Mass The mass of an individual molecule or formula unit
Also known as molecular mass or molecular weight
Sum of the masses of the atoms in a single molecule or formula unit
Whole = Sum of the parts.
Mass of 1 molecule of H2O
= 2(1.01 amu H) amu O = amu.

15. Practice—Calculate the Formula Mass of Al2(SO4)3.