SUMMER WORK AP Chemistry Summer 2015 Dr. Kathleen Gorski, Chair, Science Department
|
|
- Albert Hoover
- 5 years ago
- Views:
Transcription
1 SUMMER WORK AP Chemistry Summer 2015 Dr. Kathleen Gorski, Chair, Science Department Topics equivalent to those in Sections 1-5 (see below) are expected to be mastered prior to the start of the school year. Pay special attention to the solubility rules, and be sure to know the common monatomic and polyatomic ions. Topics in sections 6 8, if covered, are typically in less depth during a first year high school chemistry class, but should be familiar to students. Less than two weeks are spent reviewing this material at the beginning of the school year. This material is covered in any secondary school chemistry class, so students should already be familiar with it. The summer assignment is meant to reinforce these topics as well as provide a brief introduction of simple related topics. All studies should be performed in English. All work done in class will be in English and students who do not prepare correctly will be at a great disadvantage. The summer assignment will be collected at the beginning of the first class of the year. The assignment is a requirement for enrollment in AP Chemistry. 1. Introduction: Matter and Measurement CLASSIFICATIONS OF MATTER: States of Matter, Pure Substances, Elements, Compounds, Mixtures PROPERTIES OF MATTER: Physical and Chemical Changes, Separation of Mixtures UNITS OF MEASUREMENT: SI Units, Length and Mass, Temperature, Derived SI Units, Volume, Density UNCERTAINTY IN MEASUREMENT: Precision and Accuracy, Significant Figures, Significant Figures in Calculations DIMENSIONAL ANALYSIS: Using Two or More Conversion Factors, Conversions Involving, Volume 2. Atoms, Molecules, and Ions THE ATOMIC THEORY OF MATTER THE DISCOVERY OF ATOMIC STRUCTURE: Cathode Rays and Electrons, Radioactivity, The Nuclear,Model of the Atom THE MODERN VIEW OF ATOMIC STRUCTURE: Atomic Numbers, Mass Numbers, and Isotopes ATOMIC WEIGHTS: The Atomic Mass Scale, Atomic Weight THE PERIODIC TABLE MOLECULES AND MOLECULAR COMPOUNDS: Molecules and Chemical Formulas, Molecular and Empirical Formulas, Picturing Molecules IONS AND IONIC COMPOUNDS: Predicting Ionic Charges, Ionic Compounds NAMING INORGANIC COMPOUNDS: Names and Formulas of Ionic Compounds, Names and Formulas of Acids, Names and Formulas of Binary Molecular Compounds SOME SIMPLE ORGANIC COMPOUNDS: Alkanes, Some Derivatives of Alkanes 3. Stoichiometry: Calculations with Chemical Formulas and Equations CHEMICAL EQUATIONS: Balancing Equations, Indicating the States of Reactants and Products SOME SIMPLE PATTERNS OF CHEMICAL REACTIVITY: Combination and Decomposition Reactions, Combustion Reactions FORMULA WEIGHTS: Formula and Molecular Weights, Percentage Composition from Chemical Formulas AVOGADRO S NUMBER AND THE MOLE: Molar Mass, Interconverting Masses and Moles, Interconverting Masses and Numbers of Particles EMPIRICAL FORMULAS FROM ANALYSES: Molecular Formulas from Empirical Formulas, Combustion Analysis QUANTITATIVE INFORMATION FROM BALANCED EQUATIONS LIMITING REACTANTS: Theoretical Yields 4. Reactions in Aqueous Solution GENERAL PROPERTIES OF AQUEOUS SOLUTIONS: Electrolytic Properties Ionic Compounds in Water, Molecular Compounds in Water, Strong and Weak Electrolytes PRECIPITATION REACTIONS: Solubility Guidelines for Ionic Compounds, Exchange (Metathesis) Reactions, Ionic Equations 1
2 ACIDS, BASES, AND NEUTRALIZATION REACTIONS: Acids Bases Strong and Weak Acids and Bases, Identifying Strong and Weak Electrolytes, Neutralization, Reactions and Salts, Neutralization Reactions with Gas Formation OXIDATION-REDUCTION REACTIONS: Oxidation and Reduction, Oxidation Numbers, Oxidation of Metals by Acids and Salts, The Activity Series CONCENTRATIONS OF SOLUTIONS: Molarity, Expressing the Concentration of an Electrolyte, Interconverting Molarity, Moles, and Volume Dilution SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS: Titrations 5. Thermochemistry THE NATURE OF ENERGY: Kinetic Energy and Potential Energy, Units of Energy, System and Surroundings, Transferring Energy, Work and Heat THE FIRST LAW OF THERMODYNAMICS: Internal Energy, Relating to Heat and Work, Endothermic and Exothermic Processes, State Functions, ENTHALPY ENTHALPIES OF REACTION CALORIMETRY: Heat Capacity and Specific Heat, Constant-Pressure Calorimetry, Bomb Calorimetry (Constant-Volume Calorimetry) HESS S LAW ENTHALPIES OF FORMATION: Using Enthalpies of Formation to Calculate Enthalpies of Reaction FOODS AND FUELS: Foods, Fuels, Other Energy Sources 6. Electronic Structure of Atoms THE W A VE NA TURE OF LIGHT QUANTIZED ENERGY AND PHOTONS: Hot Objects and the Quantization of Energy, The Photoelectric Effect and Photons LINE SPECTRA AND THE BOHR MODEL: Line Spectra, Bohr s Model, The Energy States of the Hydrogen Atom, Limitations of the Bohr Model THE W A VE BEHA VIOR OF MA TTER: The Uncertainty Principle QUANTUM MECHANICS AND ATOMIC ORBITALS: Orbitals and Quantum Numbers REPRESENTATIONS OF ORBITALS: The s Orbitals, The p Orbitals, The d and f Orbitals MANY-ELECTRON ATOMS: Orbitals and Their Energies, Electron Spin and the Pauli Exclusion Principle ELECTRON CONFIGURATIONS: Hund s Rule, Condensed Electron Configurations, Transition Metals, The Lanthanides and Actinides ELECTRON CONFIGURATIONS AND THE PERIODIC TABLE: Anomalous Electron Configurations 7. Periodic Properties of the Elements DEVELOPMENT OF THE PERIODIC TABLE EFFECTIVE NUCLEAR CHARGE SIZES OF ATOMS AND IONS: Periodic Trends in Atomic Radii, Periodic Trends in Ionic Radii IONIZATION ENERGY: Variations in Successive Ionization Energies, Periodic Trends in First Ionization Energies, Electron Configurations of Ions ELECTRON AFFINITIES METALS, NONMETALS, AND METALLOIDS: Metals, Nonmetals, Metalloids TRENDS FOR GROUP A AND GROUP A METALS: Group A - The Alkali Metals, Group A - The Alkaline Earth Metals TRENDS FOR SELECTED NONMETALS: Hydrogen, Group A - The Oxygen Group, Group A - The Halogens, Group A - The Noble Gases 8. Basic Concepts of Chemical Bonding LEWIS SYMBOLS AND THE OCTET RULE: The Octet Rule IONIC BONDING: Energetics of Ionic Bond Formation, Electron Configurations of Ions, of the s- and p-block Elements, Transition-Metal Ions COV ALENT BONDING: Lewis Structures Multiple Bonds BOND POLARITY AND ELECTRONEGATIVITY: Electronegativity, Electronegativity and Bond Polarity, Dipole Moments, Differentiating Ionic and Covalent Bonding DRAWING LEWIS STRUCTURES: Formal Charge and Alternative Lewis Structures RESONANCE STRUCTURES: Resonance in Benzene EXCEPTIONS TO THE OCTET RULE: Odd Number of Electrons, Less than an Octet of Valence Electrons, More than an Octet of Valence Electrons STRENGTHS OF COVALENT BONDS: Bond Enthalpies and the Enthalpies of Reactions, Bond Enthalpy and 2
3 Bond Length 9. Molecular Geometry and Bonding Theories MOLECULAR SHAPES THE VSEPR MODEL: Effect of Nonbonding Electrons and Multiple Bonds on Bond Angles, Molecules with Expanded Valence Shells, Shapes of Larger Molecules MOLECULAR SHAPE AND MOLECULAR POLARITY COVALENT BONDING AND ORBITAL OVERLAP HYBRID ORBITALS: sp Hybrid Orbitals, sp2 and sp3 Hybrid Orbitals, Hybrid Orbital Summary MULTIPLE BONDS: Resonance Structures, Delocalization, and Bonding Problems 1. (a) After the label fell off a bottle containing a clear liquid believed to be benzene, a chemist measured the density of the liquid to verify its identity. A 25.0-mL portion of the liquid had a mass of g. A chemistry handbook lists the density of benzene at 15 C as g/ml. Is the calculated density in agreement with the tabulated value? (b) An experiment requires 15.0 g of cyclohexane, whose density at 25 C is g/ml. What volume of cyclohexane should be used? (c) A spherical ball of lead has a diameter of 5.0 cm. What is the mass of the sphere if lead has a density of g.cm 3? (The volume of a sphere is (4/3)πr 3 where r is the radius.) 2. Gold is alloyed (mixed) with other metals to increase its hardness in making jewelry. (a) Consider a piece of gold jewelry that weighs 9.85 g and has a volume of cm 3. The jewelry contains only gold and silver, which have densities of 19.3 g/cm 3 and 10.5 g/cm 3, respectively. If the total volume of the jewelry is the sum of the volumes of the gold and silver that it contains, calculate the percentage of gold (by mass) in the jewelry. (b) The relative amount of gold in an alloy is commonly expressed in units of carats. Pure gold is 24 carat, and the percentage of gold in an alloy is given as a percentage of this value. For example, an alloy that is 50% gold is 12 carat. State the purity of the gold jewelry in carats. 3. The following diagram is a representation of 20 atoms of a fictitious element, which we will call nevadium (Nv). The red spheres are 293 Nv, and the blue spheres are 295 Nv. (a) Assuming that this sample is a statistically representative sample of the element, calculate the percent abundance of each element. (b) If the mass of 293 Nv is amu and that of 295 Nv is amu, what is the atomic weight of Nv? [Section 2.4] 4. Name the following ionic compounds: (a) Li 2 O, (b) FeCl 3, (c) NaClO, (d) CaSO 3, (e) Cu(OH) 2, (f) Fe(NO 3 ) 2 (g) Ca(CH 3 COO) 2, (h) Cr 2 (CO 3 ) 3, (i) K 2 CrO 4, (j) (NH 4 ) 2 SO Balance the following equations: (a) Li (s) + N 2 (g) à Li 3 N (s) (b) TiCl 4 (l) + H 2 O (l) à TiO 2 (s) + HCl (aq) (c) NH 4 NO 3 (s) à N 2 (g) + O 2 (g) + H 2 O (g) (d) Ca 3 P 2 (s) + H 2 O (l) à Ca(OH) 2 (aq) + PH 3 (g) (e) Al(OH) 3 (s) + H 2 SO 4 (aq) à Al 2 (SO 4 ) 3 (aq) + H 2 O (l) (f) AgNO 3 (aq) + Na 2 CO 3 (aq) à Ag 2 NO 3 (s) + Na 2 CO 3 (aq) (g) C 2 H 5 NH 2 (g) + O 2 (g) à CO 2 (g) + H 2 O (g) + N 2 (g) 6. Determine the formula weights of each of the following compounds: (a) nitric acid, HN 3 ; (b) KMnO 4 ; (c) Ca 3 (PO 4 ) 2 ; (d) quartz, SiO 2 ; (e) gallium sulfide, (f) chromium(iii) sulfate, (g) phosphorus trichloride. 7. Calculate the following quantities: (a) mass, in grams, of 1.50 x 10-2 mol of CdS (b) number of moles of NH 4 Cl in 86.6 g of this substance (c) number of molecules in x 10-2 mol C 6 H 6 (d) number of O atoms in 6.25 x 10-3 mol Al(NO 3 ) 3 3
4 8. (a) Combustion analysis of toluene, a common organic solvent, gives 5.86 mg of CO 2 and 1.37 mg of H 2 O. If the compound contains only carbon and hydrogen, what is its empirical formula? (b) Menthol, the substance we can smell in mentholated cough drops, is composed of C, H, and O. A g sample of menthol is combusted, producing g of CO 2 and g of H 2 O. What is the empirical formula for menthol? If menthol has a molar mass of 156 g/mol, what is its molecular formula? 9. The complete combustion of octane, C 8 H 18, the main component of gasoline, proceeds as follows: 2 C 8 H 18 (l) + 25 O 2 (g) à 16 CO 2 (g) + 18 H 2 O (g) (a) How many moles of O 2 are needed to burn 1.50 mol of C 8 H 18? (b) How many grams of O 2 are needed to burn 10.0 g of C 8 H 18? (c) Octane has a density of g/ml at 20 C. How many grams of O2 are required to burn 15.0 gal of C 8 H 18 (the capacity of an average fuel tank)? (d) How many grams of CO 2 are produced when 15.0 gal of C 8 H 18 are combusted? 10. Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) Cr 2 (SO 4 ) 3 (aq) + (NH 4 ) 2 CO 3 (aq) à (b) Ba(NO 3 ) 2 (aq) + K 2 SO 4 (aq) à (c) Fe(NO 3 ) 2 (aq) + KOH (aq) à 11. Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) H 2 SO 3, (b) C 2 H 5 OH (ethanol), (c) NH 3, (d) KClO 3, (e) Cu(NO 3 ) (a) Starting with solid sucrose, C 12 H 22 O 11, describe how you would prepare 250 ml of a M sucrose solution. (b) Describe how you would prepare ml of M C 12 H 22 O 11 starting with 3.00 L of 1.50 M C 12 H 22 O You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion (CrO 4 2- ) and the oxalate ion (C 2 O 4 2- ). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na 2 CrO 4 Yellow B (NH 4 ) 2 C 2 O 4 Colorless C AgNO 3 Colorless D CaCl 2 Colorless When these solutions are mixed, the following observations are made: Expt Number Solutions Mixed Result 1 A + B No precipitate, yellow solution 2 A + C Red precipitate forms 3 A + D Yellow precipitate forms 4 B + C White precipitate forms 5 B + D White precipitate forms 6 C + D White precipitate forms (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments. 14. Calculate ΔE and determine whether the process is endothermic or exothermic for the following cases: (a) q = kj and w = 840 J; (b) a system releases 66.1 kj of heat to its surroundings while the surroundings do 44.0 kj of work on the system; (c) the system absorbs 7.25 kj of heat from the surroundings while its volume remains constant (assume that only P-V work can be done). 15. Using values from any table of enthalpies, calculate the value of ΔH for each of the following reactions: (a) CaO (s) 2 HCl (g) à CaCl 2 (s) + H 2 O (g) (b) 4 FeO (s) + O2 (g) à 2 Fe 2 O 3 (s) (c) 2 CuO (s) + NO (g) à Cu 2 O (s) + NO 2 (g) (d) 4 NH 3 (g) + O 2 (g) à 2 N 2 H 4 (g) + 2 H 2 O (l) 4
5 16. (a) Calculate the energy of a photon of electromagnetic radiation whose frequency is 6.74 x s -1. (b) Calculate the energy of a photon of radiation whose wavelength is 322 nm. (c) What wavelength of radiation has photons of energy 2.87 x J. 17. Bohr s model can be used for hydrogen-like ions ions that have only one electron, such as He + and Li 2+. (a) Why is the Bohr model applicable to He + ions but not to neutral He atoms? (b) The ground-state energies of H, He +, and Li 2+ are tabulated as follows: Atom or ion H He + Li 2+ Ground-state energy x J x J x J By examining these numbers, propose a relationship between the ground-state energy of hydrogen-like systems and the nuclear charge, Z. (c) Use the relationship you derive in part (b) to predict the ground-state energy of the C 5+ ion. 18. Write the Lewis symbol for atoms of each of the following elements: (a) Al, (b) Br, (c) Ar, (d) Sr. 19. Which of the following bonds are polar: (a) B F, (b) Cl Cl, (c) Se O, (d) H I? Which is the more electronegative atom in each polar bond? 20. Draw the Lewis structures for each of the following ions or molecules. Identify those that do not obey the octet rule, and explain why they do not: (a) SO 3 2-, (b) AlH 3, (c) N 3-, (d) CH 2 Cl 2, (e) SbF
CHEM 1364 Detailed Learning Outcomes Fall 2011 Buckley
CHEM 1364 Introduction: Matter and Measurement (Chapter 1) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Classification of matter Given sufficient information be able
More informationChemistry 111 Syllabus
Chemistry 111 Syllabus Chapter 1: Chemistry: The Science of Change The Study of Chemistry Chemistry You May Already Know The Scientific Method Classification of Matter Pure Substances States of Matter
More informationMiami Dade College CHM 1045 First Semester General Chemistry
Miami Dade College CHM 1045 First Semester General Chemistry Course Description: CHM 1045 is the first semester of a two-semester general chemistry course for science, premedical science and engineering
More informationCHEM 121 Lecture Planner
CHEM 121 Lecture Planner Lecture Lecture 1 Lecture 2 Lecture 3 Lecture 4 Lecture 5 Topics The Scientific Method Theories & Laws Quantitative Measurements vs Qualitative Measurements Accuracy & Precision
More informationChemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
More informationContents. 1 Matter: Its Properties and Measurement 1. 2 Atoms and the Atomic Theory Chemical Compounds Chemical Reactions 111
Ed: Pls provide art About the Authors Preface xvii xvi 1 Matter: Its Properties and Measurement 1 1-1 The Scientific Method 2 1-2 Properties of Matter 4 1-3 Classification of Matter 5 1-4 Measurement of
More informationChemistry 152: Introduction to General Chemistry
Chemistry 152: Introduction to General Chemistry Dr. Namphol Sinkaset Final Exam Study Guide Chapter 1: The Chemical World 1. The scientific method Chapter 2: Measurement and Problem Solving 1. SI units
More informationChemistry Curriculum Map
Timeframe Unit/Concepts Eligible Content Assessments Suggested Resources Marking Periods 1 & 2 Chemistry Introduction and Problem Solving using the Scientific Method Approach Observations Hypothesis Experiment
More informationMARLBORO CENTRAL SCHOOL DISTRICT-CURRICULUM MAP. Subject: AP Chemistry 2015/16
MARLBORO CENTRAL SCHOOL DISTRICT-CURRICULUM MAP Subject: AP Chemistry 205/6 Title or Topics (Unit organizing idea) Concepts (understandings) Tasks (What students actually do) Major Assessments (Tests,
More informationLearning Objectives for Chemistry 173
Learning Objectives for Chemistry 173 Glenbrook North High School Academic Year, 2017-2018 This outline provides a comprehensive list of the topics and concepts you will learn in this course. For each
More informationChemistry 1-2E Semester I Study Guide
Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound
More informationPhET Interactive Chemistry Simulations Aligned to an Example General Chemistry Curriculum
PhET Interactive Chemistry Simulations Aligned to an Example General Chemistry Curriculum Alignment is based on the topics and subtopics addressed by each sim. Sims that directly address the topic area
More informationFinal Exam Review Chem 101
Final Exam Review Chem 101 1. Know your nomenclature. a) Know how to go from the name to the formula. b) Know how to go from the formula to the name. 1. Ionic compounds (binary and ternary) a. Example:
More informationReview for Chemistry Final Exam [Chapters 1-9 & 12]
Name: Block: Date: Chapter 1 Matter and Change Review for Chemistry Final Exam [Chapters 1-9 & 12] 1-1. Define the terms matter and atom. 1-2. Define the terms element and compound and list some examples
More informationStudents are required to bring these definitions HAND written on separate 3 in X 5 in index cards by chapters, the first week of school
Students are required to bring these definitions HAND written on separate 3 in X 5 in index cards by chapters, the first week of school 2015-2016 Have a Great Summer!!! Ms. Charles LAB SAFETY/Vocabulary
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationMemorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
More informationHADDONFIELD PUBLIC SCHOOLS Curriculum Map for Accelerated Chemistry
Curriculum Map for Accelerated Chemistry 1st Marking Period 5.1.12.A.1, 5.1.12.A.2,, 5.1.12.A.3,, 5.1.12.B.1, 5.1.12.B.2, 5.1.12.B.3, 5.1.12.B.4, 5.1.12.C.1, 5.1.12.C.2, 5.1.12.C.3,, 5.1.12.D.1, 5.1.12.D.2,
More informationObjective #1 (80 topics, due on 09/05 (11:59PM))
Course Name: Chem 110 FA 2014 Course Code: N/A ALEKS Course: General Chemistry (First Semester) Instructor: Master Templates Course Dates: Begin: 06/27/2014 End: 06/27/2015 Course Content: 190 topics Textbook:
More informationStudy guide for AP test on TOPIC 1 Matter & Measurement
Study guide for AP test on IC 1 Matter & Measurement IC 1 Recall a definition of chemistry Understand the process and stages of scientific (logical) problem solving Recall the three states of matter, their
More information(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide:
1. Name each of the following compounds: (a) Ca(OCl) 2 : ; (b) (NH 4 ) 3 PO 4 : ; (c) K 2 Cr 2 O 7 : ; (d) HBrO 2 : ; (e) PF 5 : ; (f) B 2 O 3 : ; (g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (i) Na 2 C 2 O 4
More informationRegents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY
Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence
More informationChemistry 11 Unit 1 Safety in the Laboratory. Chemistry 11 Unit 2 Introduction to Chemistry
Unit 1 Safety in the Laboratory Safety Equipment Activities Tour of the Lab reviewing where the emergency safety equipment is. A review of the operation of lab safety equipment. Read pages 1-5 of Student
More informationUpdated: Page 1 of 5
A. Academic Division: Health Sciences B. Discipline: Science MASTER SYLLABUS 2018-2019 C. Course Number and Title: CHEM1210 Chemistry I D. Course Coordinator: Assistant Dean: Melinda S. Roepke, MSN, RN
More informationSecond Semester Chemistry Study Guide
Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on
More informationVOCABULARY. Set #2. Set #1
VOCABULARY Set #1 1. Absolute zero 2. Accepted value 3. Accuracy 4. Celsius scale 5. Conversion factor 6. Density 7. Dimensional analysis 8. Experimental value 9. Gram 10. International system of units
More informationCHM 111 Final Fall 2012
Name Part I. Multiple Choice 1. Consider the following specific heats of metals. Metal copper cobalt chromium gold silver CHM 111 Final Fall 2012 Specific Heat 0.385 J/(g C) 0.418 J/(g C) 0.447 J/(g C)
More informationSection EXAM III Total Points = 150. November 15, Each student is responsible for following directions. Read this page carefully.
Name Chemistry 11100 Test 66 Section EXAM III Total Points = 150 TA Thursday, 8:00 PM November 15, 2012 Directions: 1. Each student is responsible for following directions. Read this page carefully. 2.
More informationUnit 1: Chemical Foundations: Lab Skills, Properties of Matter, Scientific Measurement, and Dimensional Analysis
Curriculum at a Glance Chemistry Honors Level: 400 Grades 10-12 The curriculum for the Chemistry Honors 400 course is designed to provide higher performing students a strong, fundamental understanding
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationCourse Title: Academic chemistry Topic/Concept: Chapter 1 Time Allotment: 11 day Unit Sequence: 1 Major Concepts to be learned:
Course Title: Academic chemistry Topic/Concept: Chapter 1 Time Allotment: 11 day Unit Sequence: 1 1. Nature of chemistry 2. Nature of measurement 1. Identify laboratory equipment found in the lab drawer
More informationGeneral Chemistry, in broad strokes. I. Introduction to chemistry, matter, measurements, and naming -- The Language of Chemistry
General Chemistry, in broad strokes. I. Introduction to chemistry, matter, measurements, and naming -- The Language of Chemistry II. Stoichiometry -- The Numerical Logic of Chemistry III. A survey of chemical
More informationAP Chemistry Summer Review Assignment
Name: Period: Chem I Teacher/year: AP Chemistry Summer Review Assignment Due on the FIRST DAY OF SCHOOL! A. Chemical Foundations 1. The beakers shown below have different precisions. a. Label the amount
More informationExplain the emission of electromagnetic radiation in spectral form in terms of the Bohr model
Name Chemistry Review Chm.1.1 Matter:Properties and Change Chm. 1.1.1 Chm. 1.1.2 Chm. 1.1.3 Chm. 1.1.4 Analyze the structure of atoms, isotopes, and ions. Analyze an atom in terms of the location of electrons.
More informationStoichiometry. Percent composition Part / whole x 100 = %
Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)
More informationCHEM 130 Final Review
CHEM 130 Final Review Chapter Chp 1 Chemistry Define Introduction Scientific approach Describe Theory, natural law Distinguish between theory & law Chp 2 Scientific notation Conversions between standard
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationBIG IDEA TWO. October 13, 2016
BIG IDEA TWO October 13, 2016 Topics to Cover in Big Idea 2 1. Ionic, metallic, and covalent bonds 2. Polarity and dipole moment 3. Intermolecular forces (IMF): 4. Lewis dot structures 5. Resonance forms
More information1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
More informationExample: How many significant figures are in the measured number ml? (5)
Chem 143 Final Exam Study Guide 1.) Know significant figures. Example: How many significant figures are in the measured number 0.0012030 ml? (5) 2.) Know how to use dimensional analysis. Example: A pipe
More informationCHEM 1411 SAMPLE FINAL EXAM
PART I - Multiple Choice (2 points each) CHEM 1411 SAMPLE FINAL EXAM 1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following expresses this distance in meters? A. 1.34
More informationFirst Semester Review Worksheet
First Semester Review Worksheet 1. Determine the number of significant figures in each of the numbers below a. 1000 b. 4.567 c. 2030 d. 0.0240 e. 0.02677 f. 200.00 g. 4.65 x 10 4 h. 100.300 2. Convert
More informationFall 2014 Inorganic Chemistry CHM3610. Prerequisite Knowledge Assessment Quiz General Chemistry I and II Quantitative Analytical Organic I/II
Fall 2014 Inorganic Chemistry CHM3610 Name: Year Taken Prerequisite Knowledge Assessment Quiz General Chemistry I and II Quantitative Analytical Organic I/II University/College Last name(s) of Professor(s)
More informationCurriculum Guide Chemistry
Chapter 1: Introduction to Chemistry Why is chemistry important in using dominion science? Is chemistry necessary in all aspects of life? How can a chemist advance science for the kingdom of God? 1 Lesson
More informationNCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE
UNIT Atomic Structure & Properties Periodic Table Bonding Chemical Reactions Moles / Stoichiometry Acids and Bases 15 Days 11 Days 16 Days 16 Days 26 Days 9 Days S T A N D A R D S H.1P.1 Explain how atomic
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationNOTE: This practice exam contains more than questions than the real final.
NOTE: This practice exam contains more than questions than the real final. 1. The wavelength of light emitted from a green laser pointer is 5.32 10 2 nm. What is the wavelength in meters? 2. What is the
More information4. Draw a concept map showing the classifications of matter. Give an example of each.
Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationgenerate testable Students will be able to investigations. Biology 1 2 (can be conclusions. reveal relationships identify sources of error higher.
Honors Chemistry Essential Questions: 1. How can one explain the structure, properties, and interactions of matter? Communication of Scientific Information Anchor Standard 1: Students will be able to design,
More informationSpanish Fork High School Unit Topics and I Can Statements AP Chemistry
Spanish Fork High School 2014-15 Unit Topics and I Can Statements AP Chemistry Properties of Elements I can describe how mass spectroscopy works and use analysis of elements to calculate the atomic mass
More informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationREVIEW OF BASIC CHEMISTRY ANSWER KEY
REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F
More informationSolid Gas Liquid Plasma
Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and
More informationSectional Solutions Key
Sectional Solutions Key 1. For the equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + 188 kj, the number of moles of sulfur trioxide will increase if: a. the temperature of the system is increased (at constant
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationName: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What
More informationChemistry: The Central Science Twelfth Edition, AP* Edition 2012
A Correlation of The Central Science Twelfth Edition, AP* Edition 2012 to the AP* Chemistry Topics I. Structure of Matter A. Atomic theory and atomic structure 1. Evidence for the atomic theory SECTIONS:
More informationThree (3) (Qatar only) The expected learning outcome is that the student will be able to:
Course Information for 2014-2015 COURSE NUMBER: COURSE TITLE: CH1120 Chemistry COURSE DESCRIPTION: This in an introductory course designed to give students knowledge and understanding of the fundamental
More informationCP Chemistry Midterm Topic List
CP Chemistry Midterm Topic List Converting SI Units (Kilo, Hecto, Deca, Base Unit, Deci, Centi, Milli) Scientific Notation Precision versus Accuracy Properties of Matter Classification of Matter (Element/Compound/Mixture)
More informationChem 101 General Chemistry Practice Final Exam
Name h = 6.626 x 10-34 J s (Planck s Constant) c = 3.00 x 10 8 m/s (speed of light) R H = 1.097 x 10-7 m -1 (Rydberg Constant) Chem 101 General Chemistry Practice Final Exam Multiple Choice (5 points each)
More informationChemistry 11 Course Review
Introduction to Chemistry 1. 0.0006 mm =? µm Chemistry 11 Course Review 6. A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/ml. 2. 0.054 ml =? nl 3. 3.5 µg/l =? mg/ml
More informationAP Chemistry Common Ion Effect; 16.6 ionization constants, will. Equilibria with Weak Acids and and the preparation of buffer
Instructional Unit Acid-Base Equibria 16.1 Acid-Ionizaation Equilibria; Students will perform Students will distinguish Oral response, written 3.1.12C, 16.2 Polyprotic Acids; 16.3 Base- calculations involving
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationEnfield Public Schools. Advanced (AP/UCONN) Chemistry (0297) Curriculum Writers: Patrick Smith William Schultz
Enfield Public Schools Advanced (AP/UCONN) Chemistry (0297) Curriculum Writers: Patrick Smith William Schultz November 2007 Lab Safety 1. Basic safety rules must be followed in the Advanced Chemistry laboratory.
More informationChemistry 231 Fall 2014 Oregon State University Final Exam December 8, 2014 Drs. Nafshun, Watson, Nyman, Barth, Burand
Chemistry 231 Fall 2014 Oregon State University Final Exam December 8, 2014 Drs. Nafshun, Watson, Nyman, Barth, Burand Instructions: You should have with you several number two pencils, an eraser, your
More informationChemistry Final Review 2017
Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,
More information14. Use reactions 1 and 2 to determine the value of H (in kj) for reaction 3.
11. A 2.85 g sample of a food substance was burned in a calorimeter that had a heat capacity of 9.84 kj/ C. The temperature of the calorimeter increased from 22.51 C to 35.66 C. Calculate the amount of
More informationChemistry Final Exam: Practice Problems
Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence
More informationChemistry 1411 Practice Exam 2, Chapters 5-8 Brown
Chemistry 1411 Practice Exam 2, Chapters 5-8 Brown Some constants and equations: E = q + w q = C p T Heat = m T Cs h = 6.626 X 10 34 J. s c = 2.998 X 10 8 m/s R H = 2.18 X 10 18 J E = (2.18 X 10 18 J)(1/n
More informationReactions. Chapter 3 Combustion Decomposition Combination. Chapter 4 Reactions. Exchange reactions (Metathesis) Formation of a precipitate
Reactions Chapter 3 Combustion Decomposition Combination Chapter 4 Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte Single Displacement
More informationGENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016
GENERAL CHEMISTRY I CHEM 1411 SYSTEM FINAL EXAM VERSION A Fall 2016 Departmental Final Exam General Chemistry I, CHEM 1411 Fall 2016 VERSION A Part I: 35 Multiple Choice (2 pts each). Directions: Select
More informationFirst Semester Review AP Chemistry 7 points DUE AT EXAM (Thurs., 1/25/18) Date:
First Semester Review Name: AP Chemistry 7 points DUE AT EXAM (Thurs., 1/25/18) Date: The AP Chemistry Semester Exam on January 25, 2018, will cover textbook Chapters 3 through 10, our labs, and any additional
More informationNorwich City Schools AP Chemistry
Topic: Structure of Matter Students will use inquiry based methods to investigate scientific concepts Students will examine and investigate the structure, properties, and interactions of matter. Students
More informationAP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
More informationOxnard Union High School District Chemistry Pacing Plan SEMESTER 1
Oxnard Union High School District 2013-2014 Chemistry Pacing Plan SEMESTER 1 Unit and Number of Weeks Introduction to Chemistry 1 ½ weeks CA State Standard & Sub Concepts Investigation & Experimentation
More informationCHEM Final Exam Name
CHEM 10060 Final Exam Name Conversion factors: 1 mile = 1.61 km, 1 in. = 2.54 cm, 1 kg = 2.205 lb, 1 lb = 454 g 1 L = 1.057 qt., 1 qt. = 946 ml, 4.184 J = 1 cal, 32 oz. = 1 qt., 4 qt. = 1 gallon, 2 pt.
More informationCHEM 1310 Reading Day Study Session. 2. How many atoms of nitrogen are in g Ba(NO3)2?
CHEM 1310 Reading Day Study Session 1. The only two significant isotopes of group 3A element gallium are 69 Ga (68.9256amu) and 71 Ga (70.9247 amu). What are the natural abundances of the two isotopes?
More informationSection 4: Aqueous Reactions
Section 4: Aqueous Reactions 1. Solution composition 2. Electrolytes and nonelectrolytes 3. Acids, bases, and salts 4. Neutralization ti reactions 5. Precipitation reactions 6. Oxidation/reduction reactions
More informationAnglo-Chinese School (Independent) International Baccalaureate Diploma Programme Scheme Of Work Year 5 Chemistry HL
Topic 1 Quantitative Chemistry Topic 11 Measurement and Data Processing Topic 9 Redox equation 1.1 The mole concept and Avogadro s constant a) Determine the number of particles and the amount of substance
More informationSpanish Fork High School Unit Topics and I Can Statements Honors Chemistry
Spanish Fork High School 2014-15 Unit Topics and I Can Statements Honors Chemistry Module 1 I Can: Module 2 I Can: Distinguish between elements, compounds, and mixtures Summarize the major experimental
More informationCHEMISTRY 121 Review Problems
CHEMISTRY 121 Review Problems 1. Fill in the blanks with the correct symbols for the elements. An atom having a half-filled 2p subshell. An atom having a total of 6 electrons in its n = 3 principal quantum
More informationCHEMISTRY HONORS LEOCE Study Guide
BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4 CHEMISTRY HONORS CHEMISTRY AND SCIENTIFIC MEASUREMENT TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3 ESSENTIAL QUESTION: How is measurement
More informationCHAPTER Describing Chemical Reactions Reactants Products. New substances produced The arrow means yields TYPES OF EQUATIONS.
CHAPTER 11 Chemical Reactions 11.1 Describing Chemical Reactions Reactants Products New substances produced The arrow means yields Where do Chemical Reactions occur? Everywhere!!! In living organisms In
More informationName Date IB Chemistry HL-II Summer Review Unit 1 Atomic Structure IB 2.1 The nuclear atom
Name Date IB Chemistry HL-II Summer Review Unit 1 Atomic Structure IB.1 The nuclear atom 1. State the number of protons, neutrons, and electrons in each of the following: a. 65 Cu b. 15 N 3- c. 137 Ba
More informationAE Chemistry Midterm Study Guide
Name Date Define Chemistry AE Chemistry Midterm Study Guide Since chemistry studies matter what is the definition of matter. What is the Law of Conservation of Matter? What is energy, what are the two
More informationChemistry B Final Exam Review Packet Winter 2017
Chemistry B Final Exam Review Packet Winter 2017 The final exam will count as approximately 15% of your final grade in Chemistry B. Exam Format: Multiple choice ~35 questions Free Response/Calculations:
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationIntroductory College Chemistry
Introductory College Chemistry This course covers the topics shown below. Students navigate learning paths based on their level of readiness. Institutional users may customize the scope and sequence to
More informationChem 127, Final Exam December 14, 2001
I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (8 points) Fill in the empty boxes with the appropriate symbol, number, word or charge. Nuclear
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationName Pd SN Date Chemistry Review Packet- Spring 2014
Name Pd SN Date Chemistry Review Packet- Spring 2014 1.1.1 Draw pictures to illustrate the differing isotopes and ions of a given element. 1.1.1 Which atomic symbol represents an isotope of sulfur with
More informationATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY Note: For all questions referring to solutions, assume that the solvent is water unless otherwise stated. 1. The nuclide is radioactive and decays by the
More informationChemistry 151 Spring Section 01 MWF 9:10-10:00 am - MWF 9:10-10:00 am. Course Name: Course Code: N/A
Course Name: Chemistry 151 Spring 2018 - Section 01 MWF 9:10-10:00 am - MWF 9:10-10:00 am Course Code: N/A ALEKS Course: General Chemistry (First Semester) Instructor: Prof. Hascall Course Dates: Begin:
More informationCourse Title. All students are expected to take the College Board Advanced Placement Exam for Chemistry in May.
Course Title ERHS Chemistry A (AP) Description/ Target group This is two-semester laboratory course of inorganic chemistry, designed for college bound students entering the fields of science and engineering,
More informationPlum Borough School District
Course Chemistry (A) 413 Grade(s) 10 Unit/Lesson Unit 1: Measurement and Data Interpretation Overview Qualititative and quantitative observations, rules of measurement, significant figures, scientific
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationChemistry Curriculum Map. Embedded in all standards. Chm Chm Chm Chm Writing:
Six weeks Unit Unit Focus Chemistry Essential Standards Literacy in Science &Technical Subjects/ 8 Mathematical Practices First Introductory Chemistry Material - Density - Significant Digits - Metric Conversion
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More information