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UGA CHEM 2211 - Acids and Bases Overview
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CHEM 2211 1st Edition Lecture 4 Outline of Last Lecture I Chapter 1 over view of structure and bonding Outline of Current Lecture II Practice questions a Answers and explanations III Chapter two Acids and Bases a Defining types of Acids and Bases b 3 definitions IV Strengths of Acids and Bases V pKa and pH a Definitions and equations Current lecture notes II Practice questions 1 What is the hybridization of a double bonded O atoms i Example C CH2 O b SP c SP2 d SP3 i Answer and explanation will be in order after last question 2 Of the gas phase halogen compounds formula HX which has the weakest bond a HF b HCl c HBr d HI Question 1 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 Answer is C Why Count the number of electron domains occupied two lone pair domains and one double bond domain o 3 total domains SP2 hybridization Question 2 Answer is D Why o The weakest bond will be made by the longest bond length o Bond length increases as atomic radius increases o Iodine is the largest atom in the group causing it to have the longest bond length III Chapter two Acids and Bases Types of acids and bases Arrhenius Acid a hydronium ion donor Base a hydroxide ion donor Bronsted Lowrey Acid hydronium ion donor Base lone pair donor o NH3 Lewis Acid lone pair donor Base lone pair acceptor Example of Lewis Acid and base BH3 NH3 BH3NH3 This reaction is a lewis acid adduct IV Strengths of Acids and Bases Acids and bases can be either strong or weak Strong acids HCl HBr HI HClO3 HClO4 H2SO4 Strong Bases Strong bases can be found in groups 1 and 2 on the periodic table A1 and A2 hydroxides Ex NaOH and Ca OH 2 KOH Weak acids and bases Weak acids o Anything else besides the strong acids atoms combined with H Weak bases o Anything else besides the strong base atoms Water can be either an acid of base depending on what it is acting with General equations for acids and bases What you used in general chemistry looked like this o HA aq H2O l A aq H3O aq Strong acid and base o HA B A BH Base o B H2O HB OH Note single arrow shows reaction goes to completion Double headed arrow shows equilibrium can be reached between reactants and products V pKa and pH pH measure of acidity on a scale from 0 14 scale can go as high as 16 between 0 and 7 is acidic 7 is neutral water Between 7 and 14 is basic Ex table to the right Equation for pH pH log H H molarity Molarity moles liters mol L pKa Acidity of a given hydrogen atom Lower the pKa the more acidic it is Equation for pKa pKa log Ka Ka is the acid dissociation constant It is determined by aqueous products aqueous reactants o Ex HA H2O H3O Ao a b c d Reactant a is aq Products c and d are aq Ka So H3O A HA Ka Ka also determines which side is predominate in a double headed arrow reaction like this one If Ka is less than 1 o Reactants are predominate If Ka is greater than 1 o Products are predominate


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UGA CHEM 2211 - Acids and Bases Overview

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