1. ACIDS and BASES

2. Properties of Acids

3. Properties of Bases

4. Naming Acids and Bases For Acids We can use Table K to help us with naming Acids are polar covalent and will give off hydrogen ions Two types of acids exist

5. Binary Acids Contain Hydrogen and 1 other (non-metal) element All Binary acids begin with the prefix HYDRO All Binary acids end with –ic acid Example: HCl will be named: HYDROchlorIC acid

6. Ternary Acids Give away H+ ions when dissolved in water Feature Oxygen containing polyatomic ions with Hydrogen NO 3 SO 4 If the Polyatomic ends with (ate) we call this an IC ACID Example: H2SO4 SO4 = Sulfate So Acid is Sulfuric Acid

7. Naming Continued If the polyatomic ends with ITE we name this an OUS acid. Example: H2SO3 Would be named: Sulfurous Acid Notice that in all cases NO HYDRO is used to name a ternary acid. Most can be found in Table K

8. Naming Bases

9. Steps to Follow Bases are usually ionic compounds (Metal and non- metal) that release OH- ions in solution. Consist of a group 1 or 2 metal with hydroxide Therefore we just follow regular naming rules for ionic compounds when naming most NaOH consists of sodium and hydroxide Name: Sodium Hydroxide Metal keeps its name, and polyatomic OH ions keep theirs as well. Table L gives a list of common bases and names

10. The Nature of the Hydrogen Ion Has No Electron when it is ionized (H+) So it looks for something to bind to for stability In water it attaches itself to the water molecule and forms an H3O+ ion (hydronium) Creates an ion complex with acid like properties This is why you can indicate the presence of an acid with either the H+ ion or the H3O+ ion

11. Illustration of Hydronium Ion

12. Nature of the Hydroxide Ion OH- is what makes many bases basic Given off when a basic compound is placed into water The more OH- (hydroxide ions) that you release in water, the stronger you are in terms of base strength (higher pH 10-14) If H+ ions are present, OH- ions will bind with it to form water (basis of neutralization)