Acids and Bases

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)

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

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

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

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)

Acid Rain

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

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

K(OH)(aq) would be Potassium hydroxide 1+ 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)

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

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)

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

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)