1. Chapter 24:Chemical Compounds

2. 24.1 – Ionic and Covalent Compounds

3. Properties of Ionic Compounds
Form crystals
Crystal lattice – the regular pattern in which a crystal is arranged

4. Properties of Ionic Compounds
Have high melting points and boiling points

5. Properties of Ionic Compounds
Very soluble
When dissolved in water, conduct electricity well

6. Properties of Covalent Compounds
Low melting points and low boiling points

7. Properties of Covalent Compounds
Low solubility
Poor conductivity

8. 24.2 Acids and Bases Properties of acids: Properties of bases:
Tastes sour
Reacts with metals and carbonates
Turns blue litmus paper red
Conduct Electric current
Properties of bases:
Tastes bitter
Feels slippery
Turns red litmus paper blue
Conduct electric current

9. Uses of Acids and Bases

10. 24.3 Solutions of Acids and Bases
Acids produce hydrogen (H+) ions in water
HCl = hydrochloric acid
HNO3 = nitric acid
H2CO3 = carbonic acid
H2SO4 = sulfuric acid
HC2H3O2 = acetic acid
H3PO4 = phosphoric acid

11. Acids and Bases in Solution
Bases produce hydroxide ions (OH-) in water
Some bases do not contain OH-, but will react with water to form OH-
NaOH – sodium hydroxide
KOH – potassium hydroxide
Ca(OH)2 – calcium hydroxide
Al(OH)3 – aluminum hydroxide
NH3 – ammonia
CaO – calcium oxide

12. Strength of Acids and Bases
Strength = how well the acid or base forms ions
pH = power of hydrogen; range of values to measure H+ concentration
0-6.9 is a low pH = high H+, low OH-, acid
7 is a neutral pH = H+ and OH- are equal
is a high pH = low H+, high OH-, base

13. Each unit of the pH scale represents a tenfold change in acidity!

15. Acid-Base Rxns Acid + Base  salt + water Neutralization Rxn
A salt is an ionic compound formed from the positive ion of a base and the negative ion of an acid
Examples:
HCl + NaOH  ?
HCl + KOH  ?

16. Acid, Base, Salt or Neither?
NH4OH
H3PO4
NH4Cl
H2O
HC2H3O2
H2SO4
NaCl
CO2
Mg(OH)2
NH3