CHEM 102 1nd Edition Lecture 22Outline of Last Lecture I. Example of Le Chatelier’s PrincipleII. Effect of a CatalystIII. Application of Le Chatelier’sIV. Relationship Between ΔG and KOutline of Current Lecture I. ArrheniusII. Bronsted-LowryIII. Dissociation vs IonizationIV. Hydronium IonsV. Strong and Weak AcidsVI. Strong and Weak BasesVII. Strong ElectrolytesVIII. Acid and Bond StrengthIX. Binary AcidsX. Acid Strength and KCurrent LectureI. Arrhenius- Acids produce H+- Bases produce OH-II. Bronsted-Lowry- Acids donate H+- Bases receive H+III. Dissociation vs Ionization- Dissociation – solid ionic compound separates into ions in solution- Ionization – molecular compound separates into ions in solutionIV. Hydronium ions- Hydrogen ions in water do not stay as hydrogen ions- They combine with water- Create H3OV. Strong and Weak Acids These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Acids produce H+ in aqueous solution- Strong acids: completely ionize or almost completely- Weak acids: only ionize slightly (reversible reaction)- Bases ionize the sameVI. Strong Acids and Bases- Acids HCl HBr HClO4 HClO3 HNO3 H2SO4- Strong Bases LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2VII. Strong Electrolytes- Strong acids HCl HNO3 H2SO4 HClO3 HClO4 HBr HI- Strong Bases NaOH LiOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2- Soluble SaltsVIII. Acid and Bond Strength- Larger radius; weaker bond between H and anion Weaker bond means more ionizable More ionizable means stronger acid- Higher electronegativity difference; weaker bonds between H and nonmental More polar means more ionizable More ionizable means weaker bond Weaker bon means stronger acidIX. Binary Acids- H and a nonmetal- When going down a family Weakest bond means largest NM and the strongest acid H20 <H2S H2Se < H2Te HF < HCl < HB < HI- Across a period Weakest bond in the most electronegative and the strongest acid SiH4 < PH3 < H2S < HClX. Acid Strength and K- Natural tendency lies in the direction of the weakest acid and base- When K < 1, reactants are favored, so weakest are the reactants- When K > 1, weakest are the
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