Chapter 2: Acids and Bases
|
|
|
- Meryl Hopkins
- 5 years ago
- Views:
Transcription
1 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 about a Brønsted-Lowry base is true? A) The net charge may be zero, positive, or negative. B) All Brønsted-Lowry bases contain a lone pair of electrons or a π bond. C) All Brønsted-Lowry bases contain a proton. D) The net charge may be zero or positive. 3. Which of the following compounds is both a Brønsted-Lowry acid and base? A) I, II B) I, III C) II, IV D) I, IV 4. Which of the following species cannot act as both a Brønsted-Lowry acid and base? - - A) HCO 3 B) HSO 4 C) HO - - D) H 2 PO 4 5. Which of the following species is not a Brønsted-Lowry base? A) BF 3 B) NH 3 C) H 2 O D) PO Which of the following statements about Brønsted-Lowry acids and bases is true? A) Loss of a proton from a base forms its conjugate acid. B) Loss of a proton from an acid forms its conjugate base. C) Gain of a proton by an acid forms its conjugate base. D) Brønsted-Lowry acid-base reactions always result in the transfer of a proton from a base to an acid. 7. Which of the following species is the conjugate base of methanol, CH 3 OH? + A) CH 3 OH 2 B) CH 3 O - - C) CH 3 D) CH 4 8. Which of the following species is the conjugate base of the hydronium ion, H 3 O +? A) H 3 O B) H 2 O - C) H 2 O D) HO - 9. Which of the following species is the conjugate acid of ammonia, NH 3? A) H 4 N B) H 3 N + C) H 2 N - D) H 4 N + Page 1
2 10. Which is the conjugate acid in the following reaction? 11. Which is the conjugate base in the following reaction? 12. Which is the conjugate acid in the following reaction? 13. Which is the conjugate base in the following reaction? 14. Which of the following statements about acid strength is true? A) The stronger the acid, the further the equilibrium lies to the left. B) The stronger the acid, the smaller the K a. C) The stronger the acid, the larger the pk a. D) The stronger the acid, the smaller the pk a. 15. Which of the following compounds is the strongest acid? 16. Which of the following compounds is the strongest acid? A) CH 3 OH B) BrCH 2 OH C) CH 3 NH 2 D) CH 3 Cl Page 2
3 17. Which of the following compounds is the weakest acid? A) HF B) HCl C) HBr D) HI 18. Which of the following compounds is the weakest acid? A) H 2 S B) PH 3 C) HCl D) SiH Which of the following species is the strongest base? A) HO - B) H 2 N - C) CH 3 COO - D) Cl Which of the following ranks the compounds in order of increasing basicity, putting the least basic first? A) CH 3 NH 2 < CH 3 OH < CH 4 C) CH 4 < CH 3 NH 2 < CH 3 OH B) CH 3 OH < CH 3 NH 2 < CH 4 D) CH 4 < CH 3 OH < CH 3 NH Consider the following molecule with protons labeled, I-III. Rank these protons in order of decreasing acidity, putting the most acidic A) I > II > III B) I > III > II C) III > II > I D) III > I > II 22. Rank the following compounds in order of increasing acidity, putting the least acidic A) III < I < IV < II C) II < I < IV < III B) III < IV < I < II D) III < I < II < IV 23. Rank the following compounds in order of increasing acidity, putting the least acidic A) I < IV < III < II C) II < III < IV < I B) I < III < IV < II D) II < IV < III < I Page 3
4 24. Rank the following compounds in order of decreasing acidity, putting the most acidic A) IV > II > III > I C) I > II > IV > III B) III > II > IV > I D) III > IV > II > I 25. Rank the following compounds in order of decreasing acidity, putting the most acidic A) IV > II > III > I C) III > IV > II > I B) IV > III > II > I D) III > IV > I > II 26. Rank the following conjugate bases in order of increasing basicity, putting the least basic A) II < I < III B) II < III < I C) I < II < III D) I < III < II 27. Rank the following conjugate bases in order of decreasing basicity, putting the most basic A) II > I > III B) I > II > III C) III > I > II D) III > II > I 28. Which of the following is the strongest base? A) CH 3 COCH 3 B) CH 3 COOH C) NH 3 D) H 2 O Page 4
5 29. What is the direction of equilibrium when acetylene (C 2 H 2 ) reacts with H 2 N - in an acid-base reaction? A) Left B) Right C) Neither D) Cannot be determined 30. What is the direction of equilibrium when acetylene (C 2 H 2 ) reacts with ethoxide (CH 3 CH 2 O - ) in an acid-base reaction? A) Left B) Right C) Neither D) Cannot be determined 31. Which of the following statements explain why H 2 O is a stronger acid than CH 4? A) H 2 O can form hydrogen bonds while CH 4 cannot. B) H 2 O forms a less stable conjugate base, HO -. C) CH 4 forms a more stable conjugate base, CH 3 -. D) H 2 O forms a more stable conjugate base, HO Which of the following statements explain why HBr is a stronger acid than HF? A) Br - is more stable than F - because Br - is larger than F -. B) Br - is less stable than F - because Br - is larger than F -. C) Br - is more stable than F - because Br - is less electronegative than F -. D) Br - is less stable than F - because Br - is less electronegative than F Which of the following compounds has the lowest pk a? A) H 2 O B) H 2 S C) NH 3 D) CH Which of the following concepts can be used to explain the difference in acidity between acetic acid (CH 3 COOH) and ethanol (CH 3 CH 2 OH)? A) Hybridization B) Electronegativity C) Resonance D) Size 35. Which of the following concepts can be used to explain the difference in acidity between acetylene (C 2 H 2 ) and ethylene (C 2 H 4 )? A) Size B) Resonance C) Inductive effect D) Hybridization 36. Which of the following concepts can be used to explain the difference in acidity between ethanol (CH 3 CH 2 OH) and 2-fluoroethanol (FCH 2 CH 2 OH)? A) Size B) Inductive effect C) Resonance D) Hybridization Page 5
6 37. Rank the following compounds in order of decreasing acidity, putting the most acidic A) I > II > III B) III > II > I C) II > III > I D) III > I > II 38. Which of the following statements about Lewis acids is true? A) Lewis acids are proton donors. B) Lewis acids are proton acceptors. C) Lewis acids are electron pair donors. D) Lewis acids are electron pair acceptors. 39. Which of the following statements about Lewis bases is true? A) Lewis bases are electron pair acceptors. B) Lewis bases are electron pair donors. C) Lewis bases are proton donors. D) Lewis bases are proton acceptors. 40. Which of the following is a Lewis acid but not a Brønsted-Lowry acid? A) CH 3 OH B) H 2 O C) CH 3 COOH D) BF Which of the following species can be both Lewis acid and Lewis base? A) I, III, IV B) I, II, IV C) II, III, IV D) I, II, III 42. What is the correct classification of the following compound? CH 3 -O-CH 3 A) Brønsted-Lowry acid and Lewis acid. C) Brønsted-Lowry base. B) Brønsted-Lowry base and Lewis base. D) Lewis base. 43. Identify the Lewis acid in the following reaction. Page 6
7 44. Identify the Lewis base in the following reaction. 45. Which of the following compounds is not a Lewis acid? A) AlCl 3 B) HCl C) H 2 O D) CBr What is the role of methylchloride (CH 3 Cl) in the following reaction? A) Lewis acid C) Brønsted-Lowry acid B) Lewis base D) Brønsted-Lowry base 47. What is the electrophilic site in the following compounds? A) I = Carbon; II = carbon; III = boron. C) I = Carbon; II = oxygen; III = boron. B) I = Chlorine; II = carbon; III = boron. D) I = Carbon; II = carbon; III = fluorine. 48. What is the nucleophilic site in the following compounds? A) I = Hydrogen; II = π electrons in bond; III = nitrogen. B) I = Oxygen; II = carbon; III = nitrogen. C) I = Hydrogen; II = carbon; III = carbon. D) I = Oxygen; II = π electrons in bond; III = nitrogen. Page 7
8 Answer Key 1. D 2. B 3. B 4. C 5. A 6. B 7. B 8. C 9. D 10. C 11. D 12. D 13. C 14. D 15. D 16. B 17. A 18. D 19. B 20. D 21. C 22. B 23. A 24. D 25. B 26. A 27. C 28. C 29. B 30. A 31. D 32. A 33. B 34. C 35. D 36. B 37. D 38. D 39. B 40. D 41. A 42. B 43. B 44. A Page 8
9 45. D 46. B 47. A 48. D Page 9
Acid-Base Chemistry & Organic Compounds. Chapter 2
Acid-Base Chemistry & Organic Compounds Chapter 2 Brønsted Lowry Acids & Bases! Brønsted-Lowry Acid: Proton (H + ) Donor! Brønsted-Lowry Base: Proton (H + ) Acceptor! General reaction: HA + B: A - + BH
Acids and Bases. Acids and Bases
BrØnsted-Lowry A BrØnsted-Lowry acid is a proton donor. A BrØnsted-Lowry base is a proton acceptor. H + = proton BrØnsted-Lowry Some molecules contain both hydrogen atoms and lone pairs and thus, can act
Full 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
Chapter 2 Lecture Outline
Organic Chemistry, Second Edition Janice Gorzynski Smith University of Hawai i Chapter 2 Lecture Outline Prepared by Rabi Ann Musah State University of New York at Albany Copyright The McGraw-Hill Companies,
Chapter 3 Acids and Bases"
Chapter 3 Acids and Bases BrØnsted-Lowry Acids and Bases A BrØnsted-Lowry acid is a proton donor. A BrØnsted-Lowry base is a proton acceptor. H + = proton Acids and Bases Reactions of BrØnsted-Lowry Acids
CHEM 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:
Chapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
Many 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
Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
Topic-1 Lowry - Bronsted and Lewis theory of acids and bases with examples and applications
Topic-1 Lowry - Bronsted and Lewis theory of acids and bases with examples and applications VERY SHORT ANSWER QUESTIONS 1. What is bronsted acid and base give one example? Strength of bronsted acids and
NH 3 (aq) + HF (aq) F (aq) + NH 4. NaOH (aq) + H 2 O (l) NaOH (aq) + H 2 O (l) KOH (aq) + H 2 CO 3 (aq) KHCO 3 (aq) + H 2 O (l)
Quiz 2.1 Acid-Base Definitions 1. The conjugate base of H 3O + is: A. H 3O B. H 2O C. H 3O D. H 3O + E. HO 2. What is the conjugate acid of C 6H 5NH 2? A. C 6H 5NH 3 + B. C 6H 5NH C. C 6H 5NH 4 + D. C
Acid / Base Properties of Salts
Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,
ORGANIC - 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
2. 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!
1.10 Structural formulas
1.10 Structural formulas It shows which atoms are bonded to which. There are two types of structural formulas, complete Lewis structures and condensed structural formulas. In addition, there are several
Acids and Bases: Molecular Structure and Acidity
Tutorial Contents A. Introduction B. Resonance C. Atomic Radius D. Electronegativity E. Inductive Effect F. Exercises G. Exercise Solutions Acids and Bases: Molecular Structure and Acidity Review the Acids
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
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.
HA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
![HA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]](/thumbs/87/96059823.jpg "HA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]")
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
Chapter 16. Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius
Contents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
Many 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
ORGANIC - BROWN 8E CH.4 - ACIDS AND BASES.
!! www.clutchprep.com CONCEPT: FREE ENERGY DIAGRAMS Atoms save energy by forming bonds. Free energy diagrams show overall changes in potential energy during reactions. Free energy diagrams give us information
Chapter 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
Lecture 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
Aqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
Chapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
Chapter 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
NATURE OF ACIDS & BASES
General Properties: NATURE OF ACIDS & BASES ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species
3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates
Reactions in Aqueous Solutions I: Acids, Bases & Salts
10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER GOALS 1. Properties of Aqueous Solutions of Acids and Bases 2. The Arrhenius Theory 3. The Hydronium Ion (Hydrated Hydrogen Ion) 4. The
Chem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
Acid-Base Strength. Chapter 6. Monday, November 2, 2015
Acid-Base Strength Chapter 6 Monday, November 2, 2015 Acid-Base Strength We ve seen that the reactivity of acids and bases can be viewed through the HSAB Model or the EC Model. Both of these models try
Chapter 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
Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter
Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties
Chapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
Chemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
Chapter 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
Chapter 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.
Name Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
Covalent 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
Chapter 15: Acids and Bases Arrhenius Definitions:
Chapter 15: Acids and Bases Arrhenius Definitions: Acids and Bases s - compounds that produce an increase in [H + ] when dissolved in water bases - compounds that produce an increase in [OH ] when dissolved
Chapter 3 An Introduction to Organic Reactions: Acids and Bases
There are 4 types of Organic Reactions Chapter 3 An Introduction to Organic Reactions: SUBSTITUTION: ADDITION: X Y + A X A + Y Example Example A B + X Y A B X Y ELIMINATION There are 4 Types of Organic
Chapter 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
Chapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
The best things in life aren t things
Chemistry 132 NT The best things in life aren t things Anon 1 2 Chem 132 NT Acids and Module 2 Acid and Base s Relative s of Acids and Acidbase indicator dye. 3 1 Review Arrhenius ConceptAcids H+ donors
CHEMICAL EQUILIBRIUM -3
CHEMICAL EQUILIBRIUM -3 1. Arrhenius neutralisation involves 1. formation of dative bond. formation of water by the combination of H + with OH - 3. transfer of proton 4.all of these. NH 3 is not a base
Two atoms share electrons to make a covalent bond. The differenceof the electronegativites of those two atoms determines how polar that bond is.
Chapter 2: Polar covalent bonds; Acids and bases The reactivity of organic compounds is often defined by the polarities of the covalent bonds in the molecule. Polar covalent bonds: an intermediate between
ORGANIC CHEMISTRY. Meaning of Organic?
ORGANIC CHEMISTRY Meaning of Organic? Initially scientists believed there was a special force in living organisms -this was assumed the unique component of organic material In 1828 Wöhler synthesized urea
Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You
D. Ammonia can accept a proton. (Total 1 mark)
1. Which statement explains why ammonia can act as a Lewis base? A. Ammonia can donate a lone pair of electrons. B. Ammonia can accept a lone pair of electrons. C. Ammonia can donate a proton. D. Ammonia
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good
Properties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
Chapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
Essential Organic Chemistry, 3e (Bruice) Chapter 2 Acids and Bases: Central to Understanding Organic Chemistry
Essential Organic Chemistry Canadian 3rd Edition Bruice TEST BANK Full downdoad at: https://testbankreal.com/download/essential-organic-chemistrycanadian-3rd-edition-bruice-test-bank/ Essential Organic
Full file at
Essential Organic Chemistry, 2e (Bruice) Chapter 2 Acids and Bases 1) Which of the following is not a conjugate acid-base pair? A) B) C) HSO- 4, H2SO4 D) -OH, O2- E) NO3 -, NO2-2) Which is defined as a
11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
Chapter 16 Acid Base Equilibria
Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar
Chapter 2 Acids and Bases. Arrhenius Acid and Base Theory. Brønsted-Lowry Acid and Base Theory
hapter 2 Acids and Bases A significant amount of chemistry can be described using different theories of acids and bases. We ll consider three different acid-base theories (listed in order of increasing
ACID BASE EQUILIBRIUM
ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric
ACID-BASE REACTIONS & THE ph SCALE
Introduction ACID-BASE REACTIONS & THE ph SCALE In acid-base reactions in aqueous solution, the active agents are commonly the hydronium ion H 3 0 + or the hydroxide ion OH. The range of concentrations
Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
Chapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
[H ] [OH ] 5.6 " 10
![[H ] [OH ] 5.6 10](/thumbs/73/68396449.jpg "[H ] [OH ] 5.6 10")
Howemork set solutions 10: 11.1 Table 11.5 of the tet contains a list of important Brønsted acids and bases. (a) both, base, (c) acid, (d) base, (e) acid, (f) base, (g) base, (h) base, (i) acid, (j) acid.
Double Bond: C 2 H 4. An sp 2 hybridized C atom has one electron in each of the three sp 2 lobes
Double Bond: C 2 H 4 An sp 2 hybridized C atom has one electron in each of the three sp 2 lobes Top view of the sp 2 hybrid Side view of the sp 2 hybrid + the unhybridized p orbital 1 Double Bond: C 2
Chapter 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)
Why do I care, Dr. P?
Chapter 2- Polar Covalent Bonds; Acids and Bases Ashley Piekarski, Ph.D. Why do I care, Dr. P? In Chapter 1, we studied valence bond theory which uses hybrid orbitals to account for the observed shapes
CHE2060 Lecture 5: Acid-base chemistry. CHE2060 Lecture 5: Acid-base chemistry
CHE2060 Lecture 5: Acid-base chemistry 5.1 Acids & bases: overview & basics 5.2 Acid & base strength 5.3 Equilibrium acid-base reactions 5.4 The leveling effect of solvents 5.5 Estimation of acidity by
Organic Chemistry. Second Edition. Chapter 3 Acids and Bases. David Klein. Klein, Organic Chemistry 2e
Organic Chemistry Second Edition David Klein Chapter 3 Acids and Bases 3.1 Conjugate Acids and Bases Brønsted-Lowry definition A conjugate acid results when a base accepts a proton A conjugate base results
Organic Chemistry I Dr Alex Roche Organic chemistry is the chemistry of Carbon and its compounds. Organic molecules constitute the essence of life (fats, sugars, proteins, DNA), and also permeate our everyday
Acid-Base Chemistry. There are a couple of ways to define acids and bases Brønsted-Lowry acids and bases. Lewis acids and bases
Acid-Base Chemistry There are a couple of ways to define acids and bases Brønsted-Lowry acids and bases Acid: H + ion donor Base: H + ion acceptor Lewis acids and bases Acid: electron pair acceptor Base:
Chapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Practice test 2013 Multiple Choice Identify the choice that best completes the statement or answers the question. Important constants For Water H fus = 6.01 kj/mol or 334 J/g H vap =
Acids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).
CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).
BIOB111_CHBIO - Tutorial activity for Session 6:
BIOB111_CHBIO - Tutorial activity for Session 6: General topics for the week: Acids and Bases ph and buffer Interactive animations are used to reinforce the understanding Instructions- interactive animations:
Chapter 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
Talk n Acids & Bases... Lady Dog! Definitions
Talk n Acids & Bases... Lady Dog! Definitions So far in this course, we have looked at processes in chemistry that deal with, or are best explained by, ionic salts or molecules. Now we will turn our attention
Acids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
Chapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1
Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.
SCH4U Chapter 8 review
Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic
Chapter 15. Properties of Acids. Structure of Acids 7/3/08. Acid and Bases
Chapter 15 Acid and Bases Properties of Acids! Sour taste! React with active metals! React with carbonates, producing CO 2! Change color of vegetable dyes!blue litmus turns red! React with bases to form
Acid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
CHEM Dr. Babb s Sections Exam #3 Review Sheet
CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry
6.2 Electron Movements in Brønsted Acid Base Reactions. Copyright 2018 by Nelson Education Limited 1
6.2 Electron Movements in Brønsted Acid Base Reactions Copyright 2018 by Nelson Education Limited 1 Recall: Brønsted Acid Base Reactions often simply termed acid base reactions Recall: H + does not actually
HW #5: 5.28, 5.34, 5.36, 5.38, 5.46, 5.52, 5.54, 5.58, 5.68, 5.72, 5.74, 5.76, 5.78, 5.80
Chemistry 121 Lectures 11 & 12: Chemical Equations; Balancing Chemical Equations; Classes of Chemical Reactions: Precipitation, Acid-Base, and Redox Reactions Chapter 5 in McMurry, Ballantine, et. al.
Chap 16 Chemical Equilibrium HSU FUYIN
Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen
Chapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
Brønsted-Lowry Acid-Base Model. Chapter 13 Acids and Bases. The Nature of H + Outline. Review from Chapter 4. Conjugate Pairs
Brønsted-Lowry Acid-Base Model William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 13 Acids and Bases Brønsted-Lowry Johannes Brønsted (1879-1947) Thomas Lowry (1874-1936)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The effect of a catalyst on a chemical reaction is to. A) increase the entropy change
T8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2.
![T8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2.](/thumbs/89/100188411.jpg "T8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2.")
T8-1P1 [212 marks] 1. Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2 2. Which of the following is correct? A. A weak acid is a proton donor and
Models of Acids and Bases. Acid-Base Equilibrium Conjugate Acid/Base Pairs QUESTION: 3.1 6/21/12. Acids & Bases/ Organic Chemistry
Chapter 3 Models of Acids and Bases Structure and Bonding Acids and Bases Acids & Bases/ Organic Chemistry Dr. Ron Rusay Fall 2012! Arrhenius: Acids produce H + & bases produce OH ion in aqueous solutions."
CH 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
Definition Arrhenius ( ) acid and base (1887) Acid A molecule ionizes in water to form a solution
1 Acids and bases Definition Arrhenius (1859-197) acid and base (1887) Acid A molecule ionizes in water to form a solution containing H ions Base A molecule ionizes in water to form a solution containing
Acids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H ], (also thought of as hydronium ion, H O ) when dissolved in water. Acids
Chapter 1: Structure and Bonding
1. What is the ground-state electronic configuration of a carbon atom? A) 1s 2, 2s 2, 2p 5 B) 1s 2, 2s 2, 2p 2 C) 1s 2, 2s 2, 2p 6 D) 1s 2, 2s 2, 2p 4 2. What is the ground-state electronic configuration
General 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
2. 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.: