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This 4 page Study Guide was uploaded by Alexandria Bauch on Monday October 26, 2015. The Study Guide belongs to CHEM0110 at University of Pittsburgh taught by AdrianMichael in Fall. Since its upload, it has received 14 views. For similar materials see /class/229438/chem0110-university-of-pittsburgh in Chemistry at University of Pittsburgh.
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Date Created: 10/26/15
Chemistry 0110 Spring Term 2010 Study Outline for Exam 1 Study Outline Exam 1 covers Chapters l4 There will be 10 multiple choice questions 75 short answer questions and 75 problems The exam will last for the whole class period 75 min Some of the multiple choice questions will test your knowledge of basic facts Others will require numerical work and problem solving e g nding the number of moles produced in a reaction titration calculations etc Practice these types of calculations make sure the units cancel properly check your signi cant gures do the calculations more than once etc Correct answers to numerical problems have the correct number of signi cant gures and correct units What you need for the exam an electronic calculator no laptops palm pilots cell phones etc and a couple pencils and a good eraser just in case What you will be given A periodic table and for the exam a copy of the solubility rules in Table 41 Things you are expected to know The periodic table provided with the exam will be monochrome it will not be colorcoded to show metals nonmetals and metalloids 7 you are supposed to know which is which The names and symbols of the rst 36 elements you do not need to memorize atomic numbers or atomic weights 7 this information will be on the periodic table The SI units Table 12 and pre xes Table 13 highlighted pre xes only The charges on common ions 7 Table 24 Table 25 Table 26 for the main group elements you can gure this out from the periodic table For the transition metals you need to know how to use the roman numeral nomenclature The names formula and charge of the common polyatomic ions 7 Table 26 Without being able to do this you will have a dif cult time with questions about balancing reactions assigning oxidation numbers etc The Greek pre xes in Table 27 The nomenclature for simple ionic and molecular substances including hydrates and acids Know how to apply the solubility rules for ionic compounds 7 Table 4 l the table will be provided you do not need to memorize the rules although you should have given yourself ample practice in using them The common strong acids and bases in Table 43 The rules for assigning oxidation numbers in Table 45 However on this test the oxidation number of oxygen is 72 in its compounds ie we will not deal with peroxides and the oxidation number of hydrogen is 1 in its compounds ie we will not deal with hydrides For rule 5 the oxidation number of the halogens is 71 except when bonded to oxygen ie in the oxoanions of Table 26 You do not need to memorize the activity series of Table 46 if it is needed for a problem it will be provided 7 but know how to use it Know the de nition of molarity p 156 and be able to use it in numerical problems concerning dilutions and titrations General advice again review the Checklist Summary of Facts and Concepts and list of Operational Skills listed at the end of each chapter Chapter 1 Chemistry and Measurement Chapter 1 contains very preliminary information but you must understand the material in this chapter to have a good foundation for your study in Chapter 24 Be able to state and use the Law of Conservation of Mass be able to do calculations as in Example 11 Distinguish between elements compounds and mixtures know the difference between chemical and physical properties We did not cover this material during week 1 but now that you ve read Chapters 24 the material in Chapter 1 should be clear to you Know about significant figures 7 the exam can include problems just about sig figs 7 answers to all problems on the exams must have the correct significant figures for full credit Know the SI units and prefixes be able to derive units from the SI units 7 density volume etc Be able to use the dimensional analysis also known as the factorlabel method for calculations Chapter 2 Atoms 39 39 and Ions Quite a lot of class time was spent on the structure of the atom and how experiments by Thompson Millikan Rutherford and others contributed to the discovery of atomic structure There will be questions about this on the exam Be prepared to explain the Crookes tube and the cathode ray and how they helped demonstrate the existence of subatomic particles You should know about nuclear structure isotopes and be able to calculate atomic weights from isotopic abundance data Example 23 Be able to use and explain the Mass Number and Atomic Number Understand and use the atomic mass unit amu Using the periodic table the one you will have during the exam will NOT be in color be able to identify main group and transition metal elements identify metals nonmetals and metalloids nd the number of valance electrons of elements explain and predict the charge on ions of main group elements in periods 13 Be able to explain Coulomb s Law and what it means about the reactivity of elements Be able to use the Noble gas concept to explain the formation of simple molecules ie understand the tendency of atoms to gain lose or share electrons in order to attain Noble gas 7 like electron clouds Identify substances as being ionic or molecular Be able to draw Lewis structures ie show the single double or triple bonds between atoms of simple molecules hydrogen oxygen nitrogen chlorine methane carbon dioxide etc Know and use the rules for naming simple compounds Section28 Be able to balance simple chemical equations Chapter 3 Calculations with Chemical Formulas and Equations The material in Chapter 3 is very important Basically you should be able to do all the types of calculations discussed in Chapter 3 Calculate molar masses Know what a mole is including the de nition of the atomic mass unit Be able to interconvert between grams of substance and moles of substance Calculate mass percentages from a formula Determine empirical formula from mass percentage information Determine molecular formula from empirical formula molecular weight information Calculate amount of reagents consumed or products made during chemical reactions Predict limiting reagents and theoretical yields Chapter 4 Chemical Reactions Be able to identify and explain electrolytes and nonelectrolytes strong electrolytes and weak electrolytes soluble and insoluble compounds NB you will only be asked about compounds discussed in the chapter 7 you are not expected to know about all existing compounds Identify whether precipitation reactions occur when ionic substances are mixed use the solubility rules Understand full molecular reactions complete ionic reactions and net ionic reactions identify spectator ions Understand and identify Arrhenius acids and bases BronsteadLowry acids and bases Identify strong acids and bases 7 assume all others are weak Reactions of acids and bases with water and with each other neutralization reactions forming salt water and sometimes gas Recognize redox reactions Be able to assign oxidation numbers to atoms in a reaction Identify what is being oxidized and what is being reduced Identify the oxidizing agent and reducing agent in a redox reaction Balance simple redox reactions Be able to do calculations with molarity interconvert between mass volume and molarity do dilution calculations graVimetric analysis volumetric analysis calculations for titrations
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