Midterm Exam III. CHEM 181: Introduction to Chemical Principles Solutions C HC N H 3 C. pka = 9.7
|
|
- Joel Charles
- 5 years ago
- Views:
Transcription
1 Midterm Exam III EM 181: Introduction to hemical Principles Solutions 1. For reference, here are the pk a values for four weak acids (not all resonance structures shown): N 3 N N pka = 3.5 pka = 9.7 pka = 4.8 pka = 16 Now consider this list of compounds (not all resonance structures shown): N N N 3 2 N N 1
2 (a) An unknown acid has a pk a of 9.9 and the following IR spectrum: i. Identify this compound from the list on page 2 (redraw the Lewis structure below). ii. ircle the most acidic proton of this compound. iii. Draw any resonance structures that are important in determining the acidity of this proton. iv. Label any peaks on the IR spectrum that you can assign (there will likely only be a few.) Just as important is that there are not peaks for either = or N stretches. 2
3 (b) An unknown acid has a pk a of 4.6 and the following IR spectrum: i. Identify this compound from the list on page 2 (redraw the Lewis structure below). ii. ircle the most acidic proton of this compound. iii. Draw any resonance structures that are important in determining the acidity of this proton. N N N Two minor structures (single/triple-bonded, with a 2 charge on one nitrogen) could be included, too. iv. Label any peaks on the IR spectrum that you can assign (try to label most.) The large peak at 2200 cm 1 can t be a =. Given how close it is to a N, it s a sensible guess that the N N stretch would be around here, too. (Note that bond orders are probably a little under 3 and a little over 1 for N N bonds.) 3
4 2. For each of the following, rank the compounds by most acidic (basic) to least acidic (basic). (a) Write strongest next to the strongest acid and weakest next to the weakest. (b) Write strongest next to the strongest acid and weakest next to the weakest. (c) Write strongest next to the strongest BASE and weakest next to the weakest BASE. (It is the N 2 group that acts as the base.) (d) Write strongest next to the strongest BASE and weakest next to the weakest BASE. (It is the N (or N) that acts as the base.) 4
5 3. Match the compounds on the following page to the 1 NMR spectra on this page. (All peaks are shown. Ignore very small spikes in the baseline, as well as the calibration peak at 0 ppm.) The data here are plotted with an integration trace (red) which lets you measure the area of each peak and makes it much easier to tell which peaks are real and which are blips of noise. Because you didn t have this information on the exam, we accepted two correct answers for #4. 5
6 4. Succinic acid, 4 6 4, is a diprotic acid: K a ( ) = K a ( ) = Aniline, 6 5 N 2, is a weak base: K b ( 6 5 N 2 ) = (a) If you start with a 0.1 M solution of aniline in water, and add succinic acid until 50% of the aniline is converted to its conjugate acid ( 6 5 N + 3 ), what is the p of the resulting solution? The important thing here is that there are equal quantities of aniline and its conjugate base (aniline + ) at equilibrium. So K b ( 6 5 N 2 ) = [ 6 5 N + 3 ][ ] [ 6 5 N 2 ] = [ 6 5 N + 3 ] [ 6 5 N 2 ] [ ] [ ] = At equilibrium, it also must be true that so K w = = [ + ][ ] [ + ][ ] = [ + ] = [ ] = = M p = log 10 [ + ] =
7 (b) At this point, what are the concentrations of the succinic acid and its two conjugate bases ( 4 6 4, 4 5 4, and )? We know the + concentration at equilibrium, and we can use that to figure out where the two acid equilibria lie for succinic acid: K a ( ) = [Succ ][ + ] [ 2 Succ] = [Succ ] [ 2 Succ] [Succ ] = 4.67 [ 2 Succ] K a ( ) = [Succ2 ][ + ] [Succ ] = [Succ2 ] 1.35 [Succ 10 5 ] [Succ 2 ] = 0.19 [Succ ] In other words, because we know the p, we also know the proportion of 2 Succ, Succ, and Succ 2 in solution at equilibrium. For every Succ we create, we must also create one aniline +, while we create two aniline + with every Succ 2. So the stoichiometry is [aniline + ] = [Succ ] + 2[Succ 2 ] and plugging in the above proportions lets us solve 0.05 = [Succ ] + 2[Succ 2 ] 0.05 = [Succ ] [Succ ] [Succ ] = M [Succ 2 ] = M [ 2 Succ] = M 7
8 5. Decanoic acid ( ) has a K a of It is a white solid that is only slightly soluble in water K sp ( ) = M If 85 g (0.5 mole) of decanoic acid is added to 1 L of water, what is the lowest p at which all of it will dissolve? Assume that p is changed by adding strong base (e.g. Na), the solution volume does not change, either when adding base or adding decanoic acid, and The reactions are is completely soluble in water. Dec(s) Dec(aq) Dec(aq) Dec (aq) + + (aq) The equilibrium expressions are Dec(aq) = M = [Dec (aq)][ + (aq)] [Dec(aq)] Stoichiometry is So Dec(aq) + Dec (aq) = 0.5 M = [Dec (aq)][ + (aq)] [Dec(aq)] = [ + (aq)] [ + (aq)] = M p =
Midterm Exam III. CHEM 181: Introduction to Chemical Principles November 25, 2014 Answer Key
Midterm Exam III EM 181: Introduction to hemical Principles ovember 25, 2014 Answer Key 1. For reference, here are the pk a values for three weak acids: 3 pk a = 7.2 pk a = 4.8 pk a = 15 ow consider this
More informationFinal Exam. CHEM 181: Introduction to Chemical Principles Answer Key. 1. The major resonance structure of 1,4-diazepine is shown below:
Final Exam EM 181: Introduction to hemical Principles Answer Key 1. The major resonance structure of 1,4-diazepine is shown below: or Show all reasonable resonance structures; label them as major (if equivalent
More informationFinal Exam. CHEM 181: Introduction to Chemical Principles December 14, 2015 Answer Key N C S C
Final Exam EM 181: Introduction to hemical Principles December 14, 2015 Answer Key 1. The compound 4 5 NO has the connectivity shown below O N On the next page: Draw all reasonable resonance structures
More informationCHEM 109A Organic Chemistry
CHEM 109A Organic Chemistry https://labs.chem.ucsb.edu/zakarian/armen/courses.html Chapter 2 Acids and Bases Central to Understanding Organic Chemistry Draw the conjugate acid of each of the following:
More informationChemistry 1A, Fall 2007 KEY Midterm Exam #2 October 16, 2007 (90 min, closed book)
Chemistry 1A, Fall 2007 KEY Midterm Exam #2 ctober 16, 2007 (90 min, closed book) ame: SID: GSI ame: ame The test consists of 6 short answer questions and a page of multiple choice questions. Put your
More informationLearning Guide for Chapter 7 - Organic Reactions I
Learning Guide for Chapter 7 - rganic Reactions I I. Introduction to Reactions II. Principles of Kinetics III. Principles of Thermodynamics IV. Nucleophiles and Electrophiles V. Acids and Bases What a
More informationChapter 2: Acids and Bases
1. Which of the following statements is a correct definition for a Brønsted-Lowry acid? A) Proton acceptor C) Electron pair acceptor B) Electron pair donor D) Proton donor 2. Which of the following statements
More information**YOU ARE NOT ALLOWED TO TAKE SPARE COPIES OF THIS EXAM FROM THE TESTING ROOM**
EM 233, Fall 2017 Midterm #3 Ian R. Gould MPLETE TIS SETIN : Up to TW PINTS will be removed for incorrect/missing information! PRINTED FIRST NME answer key PRINTED LST NME Person on your LEFT (or Empty
More informationCovalent bonds can have ionic character These are polar covalent bonds
Polar Covalent Bonds: Electronegativity Covalent bonds can have ionic character These are polar covalent bonds Bonding electrons attracted more strongly by one atom than by the other Electron distribution
More informationChem 2061 Final Exam. Fall Andy Aspaas, Instructor. Thursday, December 15, Instructions: Please print: Last name: First name:
Please print: Last name: First name: hem 2061 Final Exam Fall 2005 Andy Aspaas, Instructor Thursday, December 15, 2005 Instructions: You may start as soon as you arrive. The exam was designed to be finished
More informationCHM 233 : Fall 2018 Quiz #10 - Answer Key
M 233 : Fall 2018 Quiz #10 - nswer Key Question 1 M20a Which of the following is The strongest Bronsted cid? R- 2 is a carboxylic acid and R-S 3 is a solfonic acid, you will want to draw these two as Lewis
More informationHomework - Chapter 1 Chem 2310
omework - hapter 1 hem 2310 ame I. Introduction to rganic hemistry 1. Explain in your own words what organic chemistry is, and what it is useful for. 2. Why do you think the field of study that you are
More informationChemistry 14C Fall 2015 Final Exam Part B Page 1
Chemistry 14C Fall 2015 Final Exam Part B Page 1 Uric acid is a normal metabolic product derived from purine nucleosides. Gout is a painful arthritic condition in which excess uric acid precipitates as
More informationChemistry 250A -- Exam #1 Answer Key -- September 23, 2008 (There are 5 pages.)
ame: 1 hemistry 250 -- Exam #1 nswer Key -- September 23, 2008 (There are 5 pages.) 1. (15 pts) Show the major product(s) from the following acid-base reactions. If there is no reaction then say o Reaction.
More informationChapter 2: Acids and Bases
hapter 2: Acids and Bases 32 hapter 2: Acids and Bases Problems 2.1 Write each acid- reaction as a proton-transfer reaction. Label which reactant is the acid and which the, as well as which product is
More informationHOMEWORK PROBLEMS: POLAR BONDS, RESONANCE, ACIDS & BASES 1. Which of the following molecules is the most polar?
CEM 31 MEWRK PRBLEMS: PLAR BDS, RESACE, ACIDS & BASES 1. Which of the following molecules is the most polar? 2. Trans-dichlorodifluoroethylene, C 2 Cl 2 2, has a number of polar bonds but no net dipole
More information216 S10-Exam #1 Page 2. Name
216 S10-Exam #1 Page 2. Name I. (3 points) Arrange the following four compounds in order of their R f values when analyzed by thinlayer chromatography (TLC) on silica gel-coated plates using C 2 Cl 2 as
More informationChem 14C Lecture 1 Spring 2017 Final Exam Part B Page 1
Chem 14C Lecture 1 Spring 2017 Final Exam Part B Page 1 1. (2) Write the letter of the structure that best fits the following 13 C-NMR spectrum: 51 ppm (doublet), 44 ppm (triplet), 27 ppm (quartet), 26
More informationChemistry 2541, Fall 2017 Midterm Exam 1 (100 points)
hemistry 2541, all 2017 Midterm Exam 1 (100 points) Important notes: - Please use the provided Scantron form for your answers; you can keep the sheet with the questions and can use it as scratch paper
More informationAmino acids have the general structure: All amino acids have at least two acidic protons. One is the proton
Worksheet rganic Acids and Bases II Amino Acids Acids are proton donors in aqueous solutions: A + 2 3 + + A - acid base conjugate conjugate base acid The strength of an acid is measured by the [ 3 + ]
More information1. methyl 2. methylene 3. methine 4. primary 5. secondary 6. tertiary 7. quarternary 8. isopropyl
hem 201 Sample Midterm Beauchamp Exams are designed so that no one question will make or break you. The best strategy is to work steadily, starting with those problems you understand best. Make sure you
More informationChemistry 201. MW 12pm 1:15pm Examination #1 July 20 th Bronco ID. Question Score Possible Points. 1 (17pts) 2 (28pts) 3 (14pts) 4...
Chemistry 201 MW 12pm 1:15pm Examination #1 July 20 th 2016 Name Bronco ID. Question Score Possible Points 1 (17pts) 2 (28pts) 3 (14pts) 4... (22pts) 5 (19pts). Total (100pts) 1. Read each question carefully.
More informationC h a p t e r T h r e e: Acids and Bases. 17, 21-Dimethylheptatriacontane, a sex attractant pheromone of the tsetse fly
C h a p t e r T h r e e: Acids and Bases 17, 21-Dimethylheptatriacontane, a sex attractant pheromone of the tsetse fly CM 321: Summary of Important Concepts YConcepts for Chapter 3: Acids and Bases I.
More information2. Acids and Bases (text )
2009, Department of hemistry, The University of Western ntario 2.1 2. Acids and Bases (text 2.1 2.6) Acid-base reactions are one of the most important reaction types in organic chemistry and biology, e.g.:
More informationExam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]=
Chem 101B Study Questions Name: Chapters 14,15,16 Review Tuesday 3/21/2017 Due on Exam Thursday 3/23/2017 (Exam 3 Date) This is a homework assignment. Please show your work for full credit. If you do work
More informationNow, the excess strong base will react: HA + OH - A - + H 2 O Start mol End mol
Chemistry Spring 016 Exam 3: Chapters 8-10 Name 80 Points Complete problem 1 and four of problems -6. CLEARLY mark the problem you do not want graded. You must show your work to receive credit for problems
More informationChemistry 14C Spring 2016 Final Exam Part B Page 1
hemistry 14 Spring 2016 Final Exam Part B Page 1 In lecture we discussed the possibility that the first cells may have been formed in boiling mud puddles, which have been shown (in the lab) to produce
More informationChem 5 PAL Worksheet Acids and Bases Smith text Chapter 8
D.CHO3HE.KOHB.NHC.CHC3OHHCl3F.H.CHHCH3COG.H2HCHEM 5 PAL Worksheet Acids and Bases Fall 2017 Chem 5 PAL Worksheet Acids and Bases Smith text Chapter 8 Many substances in the body are acids and bases. Many
More informationExam (6 pts) Show which starting materials are used to produce the following Diels-Alder products:
Exam 1 Name CHEM 212 1. (18 pts) Complete the following chemical reactions showing all major organic products; illustrate proper stereochemistry where appropriate. If no reaction occurs, indicate NR :
More informationChemistry 250B Final Exam Answer Key December 19, 2008
Name: NSWER KEY 1 hemistry 250 Final Exam nswer Key ecember 19, 2008 Show non-zero formal charges on all atoms for all structures. There are 11 pages. 1. (42 pts) omplete the following reactions. Show
More informationFull file at https://fratstock.eu
1. From the list below, pick the one species that cannot act as both a Bronsted-Lowry acid and base. A) HCO3 D) OH B) H2SO4 E) HPO4 2 C) H2PO4 2. From the list below, pick the one species that is not a
More informationChemistry 2331H Friday, December 6. Workshop 30 Using IR, MS and NMR Data for Structure Elucidation
Chemistry 2331H Friday, December 6 Workshop 30 Using IR, MS and NMR Data for Structure Elucidation Fragrance chemists frequently use spectroscopic tools to try to determine what molecules are responsible
More informationAMINES. 4. From your knowledge of the effects involved, predict or explain experimental results. Important areas include:
AMINES A STUDENT SHOULD BE ABLE TO: 1. Give the IUPAC or common name given the structure, and draw the structure given the name of amines and common nitrogen heterocycles (pyrrole, pyridine, purine, pyrimidine,
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationPractice Hour Examination # 1-1
CHEM 346 Organic Chemistry I Fall 2013 Practice Hour Examination # 1-1 Solutions Key Page 1 of 12 CHEM 346 Organic Chemistry I (for Majors) Instructor: Paul J. Bracher Practice Hour Examination # 1-1 Monday,
More informationChapter 16: Applications of Aqueous Equilibrium Part 2. Acid-Base Titrations
Chapter 16: Applications of Aqueous Equilibrium Part 2 Acid-Base Titrations When you add an acid and a base together, a neutralization rxn occurs. In the lab, we do neutralization rxns all the time as
More informationCHM 112 Dr. Kevin Moore
CHM 112 Dr. Kevin Moore Reaction of an acid with a known concentration of base to determine the exact amount of the acid Requires that the equilibrium of the reaction be significantly to the right Determination
More informationLecture 21 Cations, Anions and Hydrolysis in Water:
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 21 Cations, Anions and ydrolysis in Water: 1. ydration.energy 2. ydrolysis of metal cations 3. Categories of acidity and observable behavior
More informationOrganic Chemistry Peer Tutoring Department University of California, Irvine
Organic Chemistry Peer Tutoring Department University of California, Irvine Arash Khangholi (akhangho@uci.edu) Cassandra Amezquita (camezqu1@uci.edu) Jiana Machhor (jmachhor@uci.edu) OCHEM 51A Professor
More informationChemistry 232 PRACTICE Midterm 2 September / October 2010 Your name:
1 You will need to be able to show picture ID to take the test. D NT PEN TIS TEST UNTIL EVERYNE AS NE I encourage following instructions: ten (10) points will be deducted if items 1 to 4 below are not
More informationName: 1: /33 Grade: /100 2: /33 3: /33 +1 free point. Midterm Exam I. CHEM 181: Introduction to Chemical Principles September 20, 2012 Answer Key
ame: 1: /33 Grade: /100 2: /33 3: /33 +1 free point Directions: Do all three problems. Midterm Exam I EM 181: Introduction to hemical Principles eptember 20, 2012 Answer Key how all of your work neatly
More informationtert-butyl alcohol n-butyl alcohol methyl propyl ether (c) Explain briefly why n-butyl alcohol has a much higher bp than methyl propyl ether.
1. (15 points) Three 4 10 isomers are shown below, along with their boiling points. ( 3 ) 3 3 2 2 2 3 2 2 3 tert-butyl alcohol n-butyl alcohol methyl propyl ether bp: 82 118 39 (a) Based on their boiling
More informationMany Organic compounds are acids or bases (or both) Many Organic compounds undergo acid-base reactions
Objective 4 Intro to Reactivity 1: identify acids and bases using Lewis definition. Use curved arrows to show how base reacts with acid. Relate strength to pk a. Determine direction of equilibrium. Use
More informationKEY I. (28 points) i) NOTE: sp-hybridized carbanions make good nucleophiles for substitution reactions. Product A C C CH 3. Product B.
I. (8 points) Page 1 A. omplete the following as necessary NT: sp-hybridized carbanions make good nucleophiles for substitution reactions NaN N Na Na (optional) i equivalents of Product A Product B a)
More informationLecture Presentation. Chapter 16. Acid Base Equilibria. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 16 Acid Base Equilibria John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius An acid is a substance that, when dissolved in water, increases
More informationCHEMISTRY 102 Fall 2010 Hour Exam III. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
1. My answers for this Chemistry 10 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml of 0.30 M HCN by 0.10
More informationCH 15 Summary. Equilibrium is a balance between products and reactants
CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationCEM 351, Fall 2010 Midterm Exam 1 Friday, October 1, :50 2:40 p.m. Room 138, Chemistry
Name (print) Signature Student # EM 351, Fall 2010 Midterm Exam 1 Friday, ctober 1, 2010 1:50 2:40 p.m. Room 138, hemistry Wright N. Swers 1.(20 2.(20.. 3.(20 4.(20 5.(20 6.(20 Section Number (2 pts extra
More informationChemistry 222. Start mol End mol
Chemistry Spring 019 Exam 3: Chapters 8-10 Name 80 Points Complete problem 1 and four of problems 6. CLEARLY mark the problem you do not want graded. You must show your work to receive credit for problems
More informationFifth Exam CHEM 1A Summer 2017
ifth Exam EM 1A Summer 2017 Name: Last KEY irst Instructions: Read every problem carefully. Gauge your time. Use the proper number of significant figures on your results. Don t just believe the calculator,
More informationChapter Bonding. Atoms trying to attain the stable configuration of a noble (inert) gas - often referred to as the octet rule
Chapter 1 1.2-1.3 Bonding Atoms trying to attain the stable configuration of a noble (inert) gas - often referred to as the octet rule 1.2 Ionic Bonding - Electrons Transferred 1.3 Covalent Bonding - Electrons
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
More informationHour Examination # 2
CHEM 347 Hour Examination # 2 Spring 2014 Page 1 of 8 CHEM 347 rganic Chemistry II (for Majors) Instructor: Paul J. Bracher Hour Examination # 2 Wednesday, March 5 th, 2014 5:30 8:30 p.m. Student Name
More information**YOU ARE NOT ALLOWED TO TAKE SPARE COPIES OF THIS EXAM FROM THE TESTING ROOM**
EM 233, Fall 2016 Midterm #3 Ian R. Gould MPLETE TIS SETI : Up to TW PITS will be removed for incorrect/missing information! PRITED FIRST AME Answer Key Person on your LEFT (or Empty or Aisle) Person on
More informationCHEMISTRY 101 EXAM 3 FORM 3M
CHEMISTRY 101 EXAM 3 SECTIONS 572-580 Dr. Joy Heising Directions: FORM 3M November 20, 2001 1. This examination consists of two parts: 17 multiple choice questions (6 points each) in Part 1 and 4 free
More informationCHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA. For Review
CHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA For Review 1. A common ion is an ion that appears in an equilibrium reaction but came from a source other than that reaction. Addition of a common ion
More informationUCI DEPARTMENT OF ORGANIC CHEMISTRY PEER TUTORING REVIEW SESSION FEEDBACK EVALUATION
UCI DEPARTMENT OF ORGANIC CHEMISTRY PEER TUTORING REVIEW SESSION FEEDBACK EVALUATION Quarter: Fall Date: 12/07/18 Class: Rychnovsky Final Review Tutors Names: Ying Chow, Hannah Nguyen, Joshua Torosyan
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationCHM235 Fall 04 Exam 1 September 22, 2004
M235 Fall 04 Exam 1 September 22, 2004 125 points + bonus 1. (25-30 points) Draw Lewis Structures for these molecules: (a) The skeleton of is squaric acid (formula = 4 2 3 ) is shown below Add pi bonds
More informationHour Examination # 3
CHEM 343 Principles of Organic Chemistry II Summer 2014 Exam # 3 Solutions Key Page 1 of 8 CHEM 343 Principles of Organic Chemistry II Summer 2014 Instructor: Paul J. Bracher Hour Examination # 3 Tuesday,
More informationHomework - Review of Chem 2310
omework - Review of Chem 2310 Chapter 1 - Atoms and Molecules Name 1. What is organic chemistry? 2. Why is there an entire one year course devoted to the study of organic compounds? 3. Give 4 examples
More informationGeneral Chemistry II CHM 1046 E Exam 2
General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of
More informationOrganic Chemistry II KEY March 27, 2013
rganic Chemistry II KEY March 27, 2013 Exam 2: VERSI C 1. Rank the dienophiles from most reactive to least reactive in the Diels Alder reaction (most>least) E I II III IV > II > III > IV b) III > I > II
More informationChapter 02 - Polar Covalent Bonds; Acids and Bases
Exhibit 2-1 Give the corresponding letter of the term that best matches the given definition. a. Brønsted-Lowry Acid f. Ionic Bond b. Brønsted-Lowry Base g. Covalent Bond c. Lewis Acid h. Polar-Covalent
More information4. NMR spectra. Interpreting NMR spectra. Low-resolution NMR spectra. There are two kinds: Low-resolution NMR spectra. High-resolution NMR spectra
1 Interpreting NMR spectra There are two kinds: Low-resolution NMR spectra High-resolution NMR spectra In both cases the horizontal scale is labelled in terms of chemical shift, δ, and increases from right
More informationLS1a Midterm Exam 1 Review Session Problems
LS1a Midterm Exam 1 Review Session Problems 1. n aqueous mixture of a weak acid and its conjugate base is often used in the laboratory to prepare solutions referred to as buffers. ne commonly used acid
More informationOrganic Chemistry II KEY March 27, Which of the following reaction intermediates will form the fastest in the reaction below?
rganic Chemistry II KEY March 27, 2013 Exam 2: VERSI D 1. Which of the following reaction intermediates will form the fastest in the reaction below? C 1 equiv a 2 a) IV b) III c) II d) II & III e) I I.
More informationORGANIC - CLUTCH CH. 3 - ACIDS AND BASES.
!! www.clutchprep.com CONCEPT: OVERVIEW OF CHEMICAL REACTIONS There are 4 types of common chemical reactions that we need to be familiar with in organic chemistry 1. Acid-Base Reactions: Two molecules
More informationHomework for Chapter 7 Chem 2310
omework for Chapter 7 Chem 2310 Name I. Introduction to Reactions 1. Explain why the following fits the definition of a chemical reaction. C 3 Na C 3 Na 2. Using the chemical reaction above, give all compounds
More informationCHM 152 Final Exam Review
CHM 152 Final Exam Review Kinetics Chapter 12 End-of-Chapter Suggested problems: 1, 2, 3, 4, 6, 7, 9, 11, 13, 14, 15, 17, 19, 21, 25, 29, 31, 33 (graphing), 37, 39, 41, 47, 51, 53, 57, 63, 67, 68, 69,
More informationCHAPTER 2: RESONANCE THEORY
CAPTER 2: RESACE TERY The Basics. Use the Rules for writing acceptable contributing structures for this exercise (some hydrogens have been added for clarity) 1. For each example, add curved arrows to the
More informationChapter 1 Atomic and Molecular Structure
Name Date PEP Organic Chemistry Think About It: What is organic chemistry? Chapter 1 Atomic and Molecular Structure Describe some of the ways that ancient civilizations have taken advantage of organic
More informationChapter 1 Introduction and Review
Chapter 1 Introduction and Review Concept to review: It is your responsibility to review the following concepts before the first class to ensure success in understanding new concepts: Atomic structure
More informationToday. Solubility The easiest of all the equilibria. Polyprotic Acids determining something about an unknown by reacting it with a known solution
Today Solubility The easiest of all the equilibria Polyprotic Acids determining something about an unknown by reacting it with a known solution Solubility Equilibria Mg(OH)2 (s) Mg 2+ (aq) + 2OH - (aq)
More informationName Final Exam Spring 2002 Page (16 points) Acetylsalicylic acid, the molecule pictured here, is better known as aspirin.
Name Final Exam Spring 2002 Page 1 1. (16 points) Acetylsalicylic acid, the molecule pictured here, is better known as aspirin. 1 A D 2 B 3 4 Describing the bonding in aspirin, acetylsalicylic acid. (a)
More informationToday. Complex Equilibria. Approximations when do your previous formulas fail?
Today Complex Equilibria Approximations when do your previous formulas fail? In short hand notation what is dimethylamine? A. HA B. A - C. B D. BH + Amines are like ammonia with other substituents instead
More informationpotassium formate? In short hand notation what is dimethylamine? Today Complex Equilibria Approximations when do your previous formulas fail?
In short hand notation what is dimethylamine? Today Complex Equilibria A. HA Approximations when do your previous formulas fail? B. A - C. B D. BH + Amines are like ammonia with other substituents instead
More informationChapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Often, there are many equilibria going on in an aqueous solution. So, we must determine the dominant equilibrium (i.e. the equilibrium reaction
More informationChapter 02 - Polar Covalent Bonds; Acids and Bases. Exhibit 2-1
Exhibit 2-1 Organic Chemistry 9th Edition McMurry TEST BANK Full clear download at: https://testbankreal.com/download/organic-chemistry-9th-edition-mcmurry-test-bank/ Organic Chemistry 9th Edition McMurry
More informationFinal Exam. Your lab section and TA name: (if you are not in a lab section write no lab ) Instructions:
CHEM 232 Final Exam May 10, 2014 RedID number: Signature: Your lab section and TA name: (if you are not in a lab section write no lab ) Instructions: 1. In fairness to all, do not open this test until
More informationChapter 15, Applications of Aqueous Equilibria
Chapter 15, Applications of Aqueous Equilibria We will focus on 3 areas: 1) titrations 2) buffers (incl. the Henderson- Hasselbalch Transformation), 3) solubility equilibria. 1 I. Neutralization Reactions
More informationChapter 8. Acidity, Basicity and pk a
Chapter 8 Acidity, Basicity and pk a p182 In this reaction water is acting as a base, according to our definition above, by accepting a proton from HCl which in turn is acting as an acid by donating a
More informationAqueous Equilibria: Acids and Bases
/3/014 Aqueous Equilibria: Acids and Bases Ch. 16 What is an? What is a? There are actually multiple definitions Arrhenius: Dealt with species in aqueous solutions. Most basic definition of acis. Acid:
More informationChemistry 201: General Chemistry II - Lecture
Chemistry 201: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 18 Study Guide Concepts 1. A buffer is a solution that resists changes in ph by neutralizing added acid or base. 2. Buffers are
More informationDepartment of Chemistry University of Texas at Austin
Titrations and Buffers Supplemental Worksheet KEY HINT: When calculating the ph of a solution use the following 3 steps Titrations The next six problems represent many points along a titration curve of
More informationLearning Guide for Chapter 7 - Organic Reactions I
Learning Guide for Chapter 7 - rganic Reactions I I. Introduction to Reactions II. Principles of Kinetics III. Principles of Thermodynamics IV. cleophiles and Electrophiles V. Acids and Bases What a chemical
More informationOrganic Chemistry II (CHE ) Examination I February 11, Name (Print legibly): Key. Student ID#:
rganic hemistry II (HE 232-001) Examination I February 11, 2009 Name (Print legibly): Key (last) (first) Student ID#: PLEASE observe the following: You are allowed to have scratch paper (provided by me),
More informationChapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) What is a dominant equilibrium? How do we define major species? Reactions between acids and bases 1. Strong Acids + Strong Base The reaction
More informationAcid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33
Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with
More informationChemistry II Unit 5b Practice Test
Practice for Unit 5b Exam 2013 1 Unit5Practicetest2013.odt Chemistry II Unit 5b Practice Test Reading: This material is covered in chapter 5 and chapter 12 in your book. Your notes and your molecular drawings
More informationAdvanced Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent. CHAPTER 14 ACIDS & BASES
Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 14 ACIDS & BASES Day Plans for the day Assignment(s) for the day 14.1 The Nature of Acids &
More informationDepartment of Chemistry University of Texas at Austin
Aqueous Equilibria Unit Activity Acids and Bases KEY PART I The following exercise will help you come to know acids and bases better. The following compounds are all acids: What common features would help
More informationTriprotic H3A, H2A -, HA 2-, A 3-
Today Quick solubility question Polyprotic Acids determining something about an unknown by reacting it with a known solution Silver Nitrate (AgNO3) and Potassium Chloride (KCl) are both soluble salts.
More information1.5 h; 100 points Signature UM ID # Problem Points Score GSI I 17 II 20 III 20 IV 19 V 24 Total
hemistry 10 First ame First Examination Last ame May 0, 01 please print clearly 1.5 h; 100 points ignature UM ID # PRIT TE FIRT LETTER F YUR LAT AME ERE: Problem Points core GI I 17 II 0 III 0 IV 19 V
More informationChapter 3. Acids and Bases
Chapter 3 Acids and Bases 3.1 Acids and Bases Brønsted-Lowry definition Acids donate a proton Bases accept a proton Recall from General Chemistry this classic example 3-2 3.1 Conjugate Acids and Bases
More informationChapter 14 Acid- Base Equilibria Study Guide
Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and
More informationAMINES. 3. From your knowledge of the effects involved, predict or explain experimental results. Important areas include:
AMINES A STUDENT SHOULD BE ABLE TO: 1. Name given the structure, and draw the structure given the name of amines and common nitrogen heterocycles (pyrrole and pyridine). Also, give the classification of
More informationChapter 2 Polar Covalent Bonds; Acids and Bases SAMPLE. Chapter Outline
Chapter 2 Polar Covalent Bonds; Acids and Bases Chapter utline I. Polar covalent bonds (Sections 2.1 2.3). A. Electronegativity (Section 2.1). 1. Although some bonds are totally ionic and some are totally
More information2. Polar Covalent Bonds: Acids and Bases
2. Polar Covalent Bonds: Acids and Bases Based on McMurry s Organic Chemistry, 6 th edition, Chapter 2 2003 Ronald Kluger Department of Chemistry University of Toronto 2.1 Polar Covalent Bonds: Electronegativity!
More information