1. Acids and Bases

2. HCl(aq) → H+ (aq) + Cl- (aq)
Acids
Sour tasting
Excellent conductors of electricity
Acids are corrosive
Very reactive (They readily combine with other substances such as metals)
Acids can be very harmful if the pH value is low enough
They are water soluble
HCl(aq) → H+ (aq) + Cl- (aq)
**All acids contain hydrogen (H+) ion in a combined form
For Example: Sulfuric acid H2(SO4) and Hydrochloric acid (HCl)

3. Binary Acids
Begin with a hydrogen (H) atom and one other element (For example: HCl and HF)
When naming binary acids;
Hydro is always used as the prefix
Next add the stem name of the second element
Add “ic acid” to the stem name of the second element
Then you add (aq) to the end of the chemical formula because this always occurs in an aqueous solution
For Example
HCl(aq) would be Hydrochloric acid
H2S(aq) would be Hydrosulfuric acid

4. Oxy Acids
Begin with a hydrogen (H) atom reacting with a polyatomic ion (For example: Sulfuric acid H2(SO4)(aq) and Carbonic acid H2(CO3)(aq)
When naming oxy acids;
The stem of the polyatomic ion is always written first
Next, the ending “ate” is dropped from the end of the polyatomic ion and it is replaced with “ic acid”.
Then you add (aq) to the end of the chemical formula because this always occurs in an aqueous solution
For Example
H2(SO4)(aq) would be Sulfuric acid
H2(CO3)(aq) would be Carbonic acid

5. H2(SO4)(aq) would be Sulfuric acid1+ 2-
H (SO4) 1 2
H2(SO4)(aq)
H2(CO3)(aq) would be Carbonic acid 2- 1+
H (CO3) 2 1
H2(CO3)(aq)

6. Dilute nitric acid H(NO3) and sulfuric H2(SO4)
Acid Rain
Sulfur dioxides and nitrogen oxides released into the atmosphere lead to air pollution and acid rain
When water combines with sulfur dioxide and nitrogen oxides they form precipitation
Dilute nitric acid H(NO3) and sulfuric H2(SO4)

7. Acid Rain

8. Bases Alkaline Bitter tasting Good conductor of electricity
Slippery in aqueous solution
When dissolved in water hydroxide ions (OH)- are released For example: Na(OH)(aq) → Na+(aq) + (OH)-(aq)
Bases react with proteins

9. The majority of bases are compounds that contain hydroxide ions (OH)-
The majority of bases are compounds that contain hydroxide ions (OH)- . For Example, K(OH).
However, substances containing bicarbonate (HCO3) react with water to form (OH)- and are therefore also bases
When naming bases;
First you write the element bonding with the hydroxide ion or bicarbonate ion
Next, you write hydroxide or bicarbonate depending on the chemical formula.
Then you add (aq) to the end of the chemical formula because this always occurs in an aqueous solution
For Example: K(OH)(aq) would be Potassium hydroxide
Ca(OH)2(aq) would be Calcium hydroxide
Na(HCO3)(aq) would be Sodium Bicarbonate

10. K(OH)(aq) would be Potassium hydroxide1+ 1+
K (OH) 1 1
K(OH)(aq)
Ca(OH)2(aq) would be Calcium hydroxide 2+ 1-
Ca (OH) 1 2
Ca(OH)2(aq)
Na(HCO3)(aq) would be Sodium Bicarbonate 1+ 1+
Na (HCO3) 1 1
Na(HCO3)(aq)

11. Reactions of Metals
Metals follow certain patterns of chemical behaviour:
They react in presence of oxygen to form metal oxides (a.k.a basic oxides or basic anhydrides)
Metal oxides are solids
Metal oxides react in water to form bases

12. For Example … Calcium burns in oxygen to yield Calcium oxide
Ca(s) + O2(g) → CaO(s)
Calcium oxide reacts with water to form Calcium hydroxide
CaO(s) + H2O(l) → Ca(OH)(aq)

13. Reactions of Nonmetals
Nonmetals also follow certain patterns of chemical behaviour:
They react in oxygen to form nonmetal oxides (a.k.a acidic oxides)
Nonmetal oxides are often gases or liquids
Nonmetal oxides react in water to form acids

14. Sulfur trioxide then can react with water to form Sulfuric acid
For Example …
Sulfur can react with oxygen to produce Sulfur trioxide
S (g) + O2 (g) → SO3 (g)
Sulfur trioxide then can react with water to form Sulfuric acid
SO3 (g) + H2O(l) → H2SO4(aq)