zumdahl chemistry 6th edition study guide solutions

zumdahl chemistry 6th edition study guide solutions

Shed the societal and cultural narratives holding you back and let step-by-step Chemistry textbook solutions reorient your old paradigms. NOW is the time to make today the first day of the rest of your life. Unlock your Chemistry PDF (Profound Dynamic Fulfillment) today. YOU are the protagonist of your own life. Let Slader cultivate you that you are meant to be! Please reload the page. Groups Discussions Quotes Ask the Author To see what your friends thought of this book,This book is not yet featured on Listopia.There are no discussion topics on this book yet.Some people fall in love. And some people fall in love with books about falling in love. Zumdahl, Susan Arena Zumdahl, Paul Kelter, Thomas J. Hummel Hardcover, 1,184 Pages, Published 2008 by Brooks Cole Unabridged ISBN-13: 978-0-547-12532-9, ISBN: 0-547-12532-1 General Chemistry (10th Edition) by Steve n S. Zumdahl, Susan A. Zumdahl, Donald J. Decoste, Gretchen Adams Hardcover, 900 Pages, Published 2017 by Brooks Cole Student Edition, International Edition ISBN-13: 978-1-305-95740-4, ISBN: 1-305-95740-7 Chemistry (2nd Edition) An Atoms First Approach by Steve n S. Zumdahl, Susan A. Zumdahl Hardcover, 1,216 Pages, Published 2015 by Cengage Learning International Edition ISBN-13: 978-1-305-07924-3, ISBN: 1-305-07924-8 Chemistry, Loose-Leaf Version (10th Edition) by Steve n S. Zumdahl, Susan A. Zumdahl, Donald J. Decoste Loose Leaf, Published 2017 by Brooks Cole ISBN-13: 978-1-305-95766-4, ISBN: 1-305-95766-0 Chemistry, Hybrid Edition (9th Edition) (with OWLv2, 4 terms (24 months) Printed Access Card) by Steve n S. Zumdahl, Susan A. Zumdahl Paperback, 944 Pages, Published 2013 by Brooks Cole International Edition ISBN-13: 978-1-285-18849-2, ISBN: 1-285-18849-7 Chemistry (9th Edition) by Steve n S. Zumdahl, Susan A. Zumdahl Hardcover, 1,200 Pages, Published 2013 by Cengage Learning Vqf ISBN-13: 978-1-133-61109-7, ISBN: 1-133-61109-5 Chemistry (1st Edition) An Atoms First Approach by Steve n S. Zumdahl, Susan A.

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Zumdahl Hardcover, 1,152 Pages, Published 2011 by Cengage Learning Clv ISBN-13: 978-0-8400-6532-2, ISBN: 0-8400-6532-9 Chemistry (6th Edition) Media Guide Update for Students by Steve n S. Zumdahl, Susan A. Zumdahl, Thomas J. Hummel Paperback, 448 Pages, Published 2013 by Brooks Cole Student Edition ISBN-13: 978-1-133-61199-8, ISBN: 1-133-61199-0 Chemistry (3rd Edition) An Atoms First Approach by Steve n S. Zumdahl, Susan A. Zumdahl, Donald J. Decoste Hardcover, 1,216 Pages, Published 2020 by Cengage Learning ISBN-13: 978-0-357-36336-2, ISBN: 0-357-36336-1 Chemistry 10th Edition by Steve n S. Zumdahl, Susan A. Zumdahl, Donald J. Decoste Hardcover, Published 2017 by Cengage ISBN-13: 978-1-305-95773-2, ISBN: 1-305-95773-3 Chemistry (2nd Edition) An Atoms First Approach, Loose-leaf Version by Steve n S. Zumdahl, Susan A. Zumdahl Loose Leaf, 1,216 Pages, Published 2015 by Brooks Cole ISBN-13: 978-1-305-63267-7, ISBN: 1-305-63267-2 Chemistry (2nd Edition) An Atoms First Approach, Hybrid Edition (with OWLv2 24-Months Printed Access Card) by Steve n S. Zumdahl, Susan A. Zumdahl, Robert Powell Paperback, 944 Pages, Published 2015 by Brooks Cole International Edition ISBN-13: 978-1-305-26453-3, ISBN: 1-305-26453-3 Chemistry - Custom Edition For Saddleback College, 8th Edition by Steve n S. Zumdahl, Susan A. Zumdahl Paperback, Published 2013 by Cengage Learning ISBN-13: 978-1-285-92317-8, ISBN: 1-285-92317-0 Chemistry Ace Edition Grades 9-12 (8th Edition) AP Edition by Steve n S. Zumdahl, Susan A. Zumdahl Hardcover, 1,168 Pages, Published 2007 by Cengage Learning International Edition ISBN-13: 978-0-547-05405-6, ISBN: 0-547-05405-X Chemistry Advanced Placement Seven th Edition (7th Edition) by Steve n S. Zumdahl, Susan A. Zumdahl Hardcover, 1,168 Pages, Published 2005 by Houghton Mifflin Company Student Edition ISBN-13: 978-0-618-71370-7, ISBN: 0-618-71370-0 Chemistry An Atoms First Approach (3rd Edition) Standalone Looseleaf Version by Steve n S. Zumdahl, Susan A.

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Zumdahl, Donald J. DeCoste Published by Cengage Inc ISBN-13: 978-0-357-36356-0, ISBN: 0-357-36356-6 Chemistry (6th Edition) by Steve n S. Zumdahl, Susan A. Zumdahl Hardcover, 1,102 Pages, Published 2002 by Brooks Cole ISBN-13: 978-0-618-22156-1, ISBN: 0-618-22156-5 Chemistry Study Guide by Paul B. Kelter, Steve n S. It can only be used once.Please only buy this code if your instructor has an active Sapling course. This could be because we removed or broke something or maybe the address you used is incorrect. We suggest that you check that the web address (URL) is typed correctly and reload the page. And by having access to our ebooks online or by storing it on your computer, you have convenient answers with Zumdahl Chemistry 6th Edition Answers. To get started finding Zumdahl Chemistry 6th Edition Answers, you are right to find our website which has a comprehensive collection of manuals listed. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. The online questions are identical to the textbook questions except for minor wording changes necessary for Web use. Whenever possible, variables, numbers, or words have been randomized so that each student receives a unique version of the question. This list is updated nightly.All rights reserved. Instructors get the flexibility to define mastery thresholds and manage student learning aids down to the question level giving students the support they need to learn when they need it. WebAssign provides extensive content, instant assessment, and superior support. The text gives students the tools to become critical thinkers: to ask questions, to apply rules and models, and to evaluate the outcome. The authors emphasize a thoughtful, logical approach rather than simply memorizing procedures.

Recently retired from his long-time position as Director of Undergraduate Programs at the University of Illinois, he has received numerous awards for his contributions to chemical education. These include the National Catalyst Award in recognition of his contribution to chemical education, the University of Illinois Teaching Award, the UIUC Liberal Arts and Sciences Advising Award, and the School of Chemical Sciences Teaching Award (five times). He earned his B.S. in Chemistry from Wheaton College (IL), and his Ph.D. from the University of Illinois. She has taught science and mathematics at all levels, including middle school, high school, community college, and university. She is past director of the Merit Program for Emerging Scholars in Chemistry at the University of Illinois. In addition, she spearheaded the development of a sophisticated web-based electronic homework system for chemistry and is co-author on several chemistry textbooks. At UIUC he has developed chemistry courses for nonscience majors, preservice secondary teachers, and preservice elementary teachers. He teaches courses in introductory chemistry and the teaching of chemistry and has received the School of Chemical Sciences Teaching Award four times. Don has led workshops for secondary teachers and graduate student teaching assistants, discussing the methods and benefits of getting students more actively involved in class. When not involved in teaching and advising, Don enjoys spending time with his wife and three children. Instructors get the flexibility to define mastery thresholds and manage student learning aids down to the question level giving students the support they need to learn when they need it. When not involved in teaching and advising, Don enjoys spending time with his wife and three children. Recently retired from his long-time position as Director of Undergraduate Programs at the University of Illinois, he has received numerous awards for his contributions to chemical education.

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He earned his B.S. in Chemistry from Wheaton College (IL), and his Ph.D. from the University of Illinois. All Rights Reserved. The Curved-arrow Notation 4 Introduction To Alkenes. Structure And Reactivity 5 Addition Reactions Of Alkenes 6 Principles Of Stereochemistry 7 Cyclic Compounds. Stereochemistry Of Reactions 8 Nonconvalent Intermolecular Interactions 9 The Chemisrty Of Alkyl Halides 10 The Chemisrty Of Alcohols And Thiols 11 The Chemistry Of Ethers, Epoxides, Glycols, And Sulfides 12 Introduction To Spectroscopy. Infrared Spectroscopy And Mass Spectrometry 13 Nuclear Magnetic Resonance Spectroscopy 14 The Chemistry Of Alkynes 15 Dienes, Resonance, And Aromaticity 16 The Chemistry Of Benzene And Its Derivatives 17 Allylic And Benzylic Reactivity 18 The Chemistry Of Aryl Halides, Vinylic Halides, And Phenols. Transition-metal Catalysis 19 The Chemistry Of Aldehydes And Ketones.The book is used at a wide variety of schools, such as UC Berkeley, Caltech, Colorado, Cornell, Duke, Harvard, Illinois, Maryland, Purdue, Yale, Wisconsin, and many more. This edition provides students with more health examples drawn from modern medical practice, as well as many cutting-edge topics from modern synthetic organic chemistry. Sample Solutions for this Textbook We offer sample solutions for Organic Chemistry homework problems. See examples below: Show more sample solutions add The given atom is sodium. The electronic configuration of sodium is, 1s22s22p63s1 It belongs to the. Lewis acids are electron donor, whereas Lewis bases are electron pair accepter. In water molecule. The given compound is, Figure 1 The bond with higher percentage of s-character has electron density. In acid catalyzed hydration reaction, nucleophile goes to the more substituted carbon of the alkene. The structure of the given compound is shown below as, Figure 1 Four different groups are attached. The given leftmost figure of chair conformation of cyclohexane is shown as, Figure 1 The model of.

The given compound is (CH3)2CHCH2?F. It contains four carbon atoms. Fluorine is attached to the.The name of the compound sodium isopropoxide indicates that the compound is organic salt. The cation. The oxygen is the most electronegative species followed by sulphur and least electronegative is. Alkynes are hydrocarbons containing at least one carbon-carbon triple bond. The triple bonded. In (E)-1, 3, 5-hexatriene, the combination of 6 2p orbitals provides the information of 6 molecular. Aromatic compounds are those compounds which contains at least one aromatic ring. The naming of. The structure of a given compound is shown below. Figure 1 In Figure 1, there are five allylic. The structure of given compounds is shown below Figure 1 The SN2 reaction is a nucleophilic. Isobutrylaldehyde is a compound containing 4 carbon atoms and aldehyde as a functional group. In the. The given compound contains four carbon atom hydrocarbon chain which is identified by butyric acid. In 5?cyanopentanoic acid, there is a five carbon chain. At one end of the chain there will be a. In diethyl malonate the methylene group is surrounded by two carbonyl groups as shown below. Figure. The name N-isopropylaniline indicates that it consists of the structure of aniline compound. One. The structure of the given molecule is shown below. Figure 1 In the Fischer projection, the. In the given name cyclohexyl thiobenzoate, the cyclohexyl is the alkyl group which is bonded to the. The name of the given compound 4?(dimethylamino)pyridine suggest that it contains a pyridine ring. The name of the peptide is triptophylglycylisoleucylaspartic acid. This peptide is made up of four. The given reaction is an example of an electrocyclic reaction. This is because of in this. Check out a sample textbook solution. All Rights Reserved. Download Student Solutions Manual for Chemical Principles Sixth(6th) Edition by Zumdahl.

No part of this work may be reproduced or transmitted in any form or by any means, electronic or mechanical, including photocopying and recording, or by any information storage or retrieval system without the prior written permission of Houghton Mifflin Company unless such copying is expressly permitted by federal copyright law. Address inquiries to College Permissions, Houghton Mifflin Company, 222 Berkeley Street, Boston, MA 02116. This “Solutions Guide” can be very valuable if you use it properly. The way NOT to use it is to look at an exercise in the book and then immediately check the solution, often saying to yourself, “That’s easy, I can do it.” Developing problem solving skills takes practice. Don’t look up a solution to a problem until you have tried to work it on your own. If you are completely stuck, see if you can find a similar problem in the Sample Exercises in the chapter. Only look up the solution as a last resort. If you do this for a problem, look for a similar problem in the end of chapter exercises and try working it. The more problems you do, the easier chemistry becomes. It is also in your self interest to try to work as many problems as possible. Most exams that you will take in chemistry will involve a lot of problem solving. If you have worked several problems similar to the ones on an exam, you will do much better than if the exam is the first time you try to solve a particular type of problem. No matter how much you read and study the text, or how well you think you understand the material, you don’t really understand it until you have taken the information in the text and applied the principles to problem solving. You will make mistakes, but the good students learn from their mistakes. In this manual we have worked problems as in the textbook. We have shown intermediate answers to the correct number of significant figures and used the rounded answer in later calculations. Thus, some of your answers may differ slightly from ours.

When we have not followed this convention, we have usually noted this in the solution. The most common exception is when working with the natural logarithm (ln) function, where we usually carried extra significant figures in order to reduce round-off error. In addition, we tried to use constants and conversion factors reported to at least one more significant figure as compared to numbers given in the problem. For some problems, this required the use of more precise atomic masses for H, C, N, and O as given in Chapter 3. This practice of carrying one extra significant figure in constants helps minimize round-off error. We are grateful to Claire Szoke for her outstanding effort in preparing the manuscript of this manual. We also thank Estelle Lebeau for her careful accuracy review and Jim Madru for his thorough copyediting of the Solutions Manual. We also are grateful to Don DeCoste for his assistance in creating solutions to some of the problems in this Solutions Guide. TJH SSZ v CHAPTER 2 ATOMS, MOLECULES, AND IONS Development of the Atomic Theory 18. Law of conservation of mass: mass is neither created nor destroyed. The total mass before a chemical reaction always equals the total mass after a chemical reaction. Law of definite proportion: a given compound always contains exactly the same proportion of elements by mass. For example, water is always 1 g hydrogen for every 8 g oxygen. Law of multiple proportions: When two elements form a series of compounds, the ratios of the mass of the second element that combine with 1 g of the first element always can be reduced to small whole numbers. For CO2 and CO discussed in section 2.2, the mass ratios of oxygen that react with 1 g carbon in each compound are in a 2: 1 ratio. 19. From Avogadro’s hypothesis (law), volume ratios are equal to molecule ratios at constant temperature and pressure. The formula of X is ClF3 for a balanced reaction. 20. a.

The composition of a substance depends on the numbers of atoms of each element making up the compound (depends on the formula of the compound) and not on the composition of the mixture from which it was formed. b. Avogadro’s hypothesis (law) implies that volume ratios are equal to molecule ratios at constant temperature and pressure. The atomic masses of H and Na are close. Something must be wrong about the assumed formulas of the compounds. It turns out that the correct formulas are H2O, Na2O, and MgO. The smaller discrepancies result from the error in the assumed atomic mass of H. The Nature of the Atom 24. Deflection of cathode rays by magnetic and electrical fields led to the conclusion that they were negatively charged. The cathode ray was produced at the negative electrode and repelled by the negative pole of the applied electrical field. ? particles are electrons. Each of these particles has a mass approximately 1800 times greater than that of an electron. The combination of the protons and the neutrons in the nucleus makes up the bulk of the mass of an atom, but the electrons make the greatest contribution to the chemical properties of the atom. 29. If the plum pudding model were correct (a diffuse positive charge with electrons scattered throughout), then.This was not the case because a few of the.Rutherford reasoned that the large deflections of these.Ions, on the other hand, have electrons added to form anions (negatively charged ions) or electrons removed to form cations (positively charged ions). b. The sharing of electrons between atoms is a covalent bond. An ionic bond is the force of attraction between two oppositely charged ions. c. A molecule is a collection of atoms held together by covalent bonds. A compound is composed of two or more different elements having constant composition. Another difference is that molecules do not necessarily have to be compounds. H2 is two hydrogen atoms held together by a covalent bond.

The mass number is the sum of the number of protons plus neutrons in the nucleus. The atomic mass is the actual mass of a particular isotope (including electrons). As we will see in Chapter 3, the average mass of an atom is taken from a measurement made on a large number of atoms. The average atomic mass value is listed in the periodic table. 32. a. Metals: Mg, Ti, Au, Bi, Ge, Eu, and Am. Nonmetals: Si, B, At, Rn, and Br. b. Si, Ge, B, and At. The elements at the boundary between the metals and the nonmetals are B, Si, Ge, As, Sb, Te, Po, and At. Aluminum has mostly properties of metals, so it is generally not classified as a metalloid. 33. a. The noble gases are He, Ne, Ar, Kr, Xe, and Rn (helium, neon, argon, krypton, xenon, and radon). Radon has only radioactive isotopes. In the periodic table, the whole number enclosed in parentheses is the mass number of the longest-lived isotope of the element. b. promethium (Pm) and technetium (Tc) 34. Carbon is a nonmetal. Silicon and germanium are called metalloids as they exhibit both metallic and nonmetallic properties. Tin and lead are metals. Thus metallic character increases as one goes down a family in the periodic table. CHAPTER 2 36. 5 a. Cobalt is element 27. The major difference is that CrCl3 contains a transition metal (Cr) that generally exhibits two or more stable charges when in ionic compounds. We need to indicate which charged ion we have in the compound. This is generally true whenever the metal in the ionic compound is a transition metal. ICl3 is made from only nonmetals and is a covalent compound. Predicting formulas for covalent compounds is extremely difficult. Because of this, we need to indicate the number of each nonmetal in the binary covalent compound. The exception is when there is only one of the first species present in the formula; when this is the case, mono- is not used (it is assumed). 44. a. Dinitrogen monoxide is correct. N and O are both nonmetals resulting in a covalent compound.

We need to use the covalent rules of nomenclature. The other two names are for ionic compounds. b. Copper(I) oxide is correct. With a metal in a compound, we have an ionic compound. Because copper, like most transition metals, forms at least a couple of different stable charged ions, we must indicate the charge on copper in the name. Copper oxide could be CuO or Cu2O, hence why we must give the charge of most transition metal compounds. Dicopper monoxide is the name if this were a covalent compound, which it is not. c. Lithium oxide is correct. Dilithium monoxide would be the name if Li2O were a covalent compound (a compound composed of only nonmetals). Iron(III) chloride is correct. b. This is a covalent compound so use the covalent rules. Nitrogen dioxide is correct. c. This is an ionic compound, so use the ionic rules. Calcium oxide is correct. Aluminum sulfide is correct. e. This is an ionic compound, so use the ionic rules. Iron(III) phosphate is correct. g. This is a covalent compound, so use the covalent rules. Sodium peroxide is correct. Note that sodium oxide would be Na2O. 53. i. HNO3 is nitric acid, not nitrate acid. Nitrate acid does not exist. j. H2S is hydrosulfuric acid or dihydrogen sulfide or just hydrogen sulfide (common name). H2SO4 is sulfuric acid. a. nitric acid, HNO3 b. perchloric acid, HClO4 d. sulfuric acid, H2SO4 e. phosphoric acid, H3PO4 c. acetic acid, HC2H3O2 Additional Exercises 54. a. The smaller parts are electrons and the nucleus. The nucleus is broken down into protons and neutrons, which can be broken down into quarks. For our purpose, electrons, neutrons, and protons are the key smaller parts of an atom. b. All atoms of hydrogen have 1 proton in the nucleus. Different isotopes of hydrogen have 0, 1, or 2 neutrons in the nucleus. The number of neutrons can be the same for a hydrogen atom and a helium atom. Tritium (3H) and 4He both have 2 neutrons.

Assuming neutral atoms, then the number of electrons will be 1 for hydrogen and 2 for helium. CHAPTER 2 ATOMS, MOLECULES, AND IONS 9 d. Water (H2O) is always 1 g hydrogen for every 8 g of O present, whereas H2O2 is always 1 g hydrogen for every 16 g of O present. These are distinctly different compounds, each with its own unique relative number and types of atoms present. e. A chemical equation involves a reorganization of the atoms. Bonds are broken between atoms in the reactants, and new bonds are formed in the products. The number and types of atoms between reactants and products do not change. Because atoms are conserved in a chemical reaction, mass is also conserved. 55. A compound will always have a constant composition by mass. The solid residue must have come from the flask. 61. In the case of sulfur, SO42.However, they are all related to other ions and acids named in the text that contain a same group element. Because HClO4 is perchloric acid, HBrO4 would be perbromic acid. Because ClO3? is the chlorate ion, KIO3 would be potassium iodate. Since ClO2? is the chlorite ion, NaBrO2 would be sodium bromite. The number of protons corresponds to the atomic number. Thus this is element 51, antimony. There are 3 fewer electrons than protons. The anion has one-third the number of protons of the cation which corresponds to 17 protons; this is element 17, chlorine. The name of the compound is antimony(III) chloride. The Roman numeral is used to indicate the charge of Sb because the predicted charge is not obvious from the periodic table. 66. a. This is element 52, tellurium. Te forms stable 2? charged ions in ionic compounds (like other oxygen family members). The heavier elements have significantly more neutrons than protons in their nuclei. Because this element forms anions, it is a nonmetal and will be a halogen because halogens form stable 1! charged ions in ionic compounds. From the halogens listed, chlorine, with an average atomic mass of 35.45, fits the data.

The two isotopes are 35Cl and 37Cl, and the number of electrons in the 1! ion is 18. Note that because the atomic mass of chlorine listed in the periodic table is closer to 35 than 37, we can assume that 35Cl is the more abundant isotope. This is discussed in Chapter 3. Challenge Problems 68. Because the gases are at the same temperature and pressure, the volumes are directly proportional to the number of molecules present. Let’s consider hydrogen and oxygen to be monatomic gases and that water has the simplest possible formula (HO). Because they have the same formula, their mass percent composition will be identical. However, these are different compounds with different properties because the atoms are bonded together differently. These compounds are called isomers of each other. b. When wood burns, most of the solid material in wood is converted to gases, which escape. Although the compounds are composed of different isotopes, their properties are similar because different isotopes of the same element have similar properties (except, of course, their mass). 70. For each experiment, divide the larger number by the smaller. The answer to part d depends on which (if any) of experiments 1 and 3 have a formula of XY in the compound. If the number of protons equals the number of neutrons, we have 22 protons in the molecule. In terms of balanced equations, Avogadro’s hypothesis (law) implies that volume ratios will be identical to molecule ratios. Assuming one molecule of octane reacting, then 1 molecule of CxHy produces 8 molecules of CO2 and 9 molecules of H2O. There are many possible correct answers for the balanced equations. This is just one possibility. This is consistent with two isotopes, differing in mass by two mass units. The peak at 157.84 corresponds to a Br2 molecule composed of two atoms of the lighter isotope. The intensities of the highest and lowest masses tell us the two isotopes are present at about equal abundance.

We will use both ideas to show how these conversion factors can be used. In practice, the NO produced in the third step is recycled back continuously into the process in the second step. If this is taken into consideration, then the conversion factor between mol NH3 and mol HNO3 turns out to be 1: 1; that is, 1 mol of NH3 produces 1 mol of HNO3. The product formed in the reaction is NO2; the other species present in the product representtation is excess O2. Therefore, NO is the limiting reactant. In the following table we have listed three rows of information. The “Initial” row is the number of molecules present initially, the “Change” row is the number of molecules that react to reach completion, and the “Final” row is the number of molecules present at completion. STOICHIOMETRY 35 An alternative method to solve limiting-reagent problems is to assume that each reactant is limiting and then calculate how much product could be produced from each reactant.The actual yield is 3 mol of acetaminophen compared with a theoretical yield of 4 mol of acetaminophen. In 1 hour, the 1000.Similarly, we would expect the formula of a Group 6A element with Al to be Al2X3. The volume of a gas is proportional to the number of molecules of gas. Challenge Problems 95. When the discharge voltage is low, the ions present are in the form of molecules. Therefore, the gas mixture contains 16O16O, 16O18O, and 40Ar. To determine the CHAPTER 3 STOICHIOMETRY 43 percent composition of each isotope, we use the relative intensity data from the high discharge data to determine the percentage that each isotope contributes to the total relative intensity. However, OF(g) is not a stable compound. We know that water is a product, so one of the elements in the compound is hydrogen. Balance the aspirin synthesis reaction to determine the formula for salicylic acid. We must have fewer moles of M than moles O present in If MO is the formula of the oxide, then M has a molar mass of the formula.

Some possibilities are MO2, M2O3, MO3, etc. It is a guessing game as to which to try. Let’s assume an MO2 formula. Therefore, the mol O to mol M ratio must be between 2 and 3. Some reasonable possibilities are 2.25, 2.33, 2.5, 2.67, and 2.75 (these are reasonable because they will lead to whole number formulas). The other choices for the O: M mole ratios between 2 and 3 do not give as reasonable results. Only statement b is true. A concentrated solution can also contain a nonelectrolyte dissolved in water, for example, concentrated sugar water. Acids are either strong or weak electrolytes. Some ionic compounds are not soluble in water, so they are not labeled as a specific type of electrolyte. 11. a. Polarity is a term applied to covalent compounds. Polar covalent compounds have an unequal sharing of electrons in bonds that results in unequal charge distribution in the overall molecule. Polar molecules have a partial negative end and a partial positive end. These are not full charges as in ionic compounds but are charges much smaller in magnitude. Water is a polar molecule and dissolves other polar solutes readily. The oxygen end of water (the partial negative end of the polar water molecule) aligns with the partial positive end of the polar solute, whereas the hydrogens of water (the partial positive end of the polar water molecule) align with the partial negative end of the solute. These opposite charge attractions stabilize polar solutes in water. This process is called hydration. Nonpolar solutes do not have permanent partial negative and partial positive ends; nonpolar solutes are not stabilized in water and do not dissolve. b. KF is a soluble ionic compound, so it is a strong electrolyte. Similarly: 75.0 ppm standard, dilute 7.50 mL of the 1000.0 ppm stock to 100.0 mL. 50.0 ppm standard, dilute 5.00 mL of the 1000.0 ppm stock to 100.0 mL. 25.0 ppm standard, dilute 2.50 mL of the 1000.0 ppm stock to 100.0 mL. 10.0 ppm standard, dilute 1.00 mL of the 1000.