Advanced Chemistry: Structure and Properties
|
|
- Alexis Mathews
- 7 years ago
- Views:
Transcription
1 ILLLINOIS MATHEMATICS & SCIENCE ACADEMY Teacher: Dave DeVol Advanced Chemistry: Structure and Properties August 2013 Unit 1: Molecular Structure and Intermolecular Forces Theme: Relate structure and properties of atoms, ions, and molecules The Bohr Model of the Hydrogen atom SSL 2.A,2.B,3.B,3.C,4.A,5.B The Quantum Mechanical Model of the atom HS-PS1-1 SSL 1.B,2.B SSL 3.B,3.C SSL 4.C Quantitatively and qualitatively relate wavelength of light in the H spectrum to energy levels (Bohr Model) Write the electron configuration and orbital diagram of an atom or ion, given the atomic number of the element. Write the four quantum numbers for each electron in an atom. For a given sublevel, describe the shape of the electron cloud. Bohr Model Lab Students make connections between atomic emission spectra and electron transitions between energy levels. Quantum Mechanics Packet Students relate quantum numbers to the periodic table and electron configurations. Bohr Model Quiz VSEPR/Quantum Numbers Quiz Quantum Numbers Homework Check VSEPR/Quantum Numbers Quiz Quantum Numbers Homework Check Explain the differences between the Bohr Model and Quantum Mechanical model of the atom. Describe and interpret the following periodic trends: ionization energy, atomic radius, electronegativity. Quantum Numbers Homework Check Students answer questions related to quantum numbers, electron configurations, and orbital diagrams. Bohr Lab Post-lab Quantum Numbers Homework Check 1 of 8
2 Chemical Bonding and VSEPR HS-PS1-1 SSL 1.A,1.B SSL 3.B,3.C SSL 4.A Explain why atoms bond together and the formation of ionic, polar covalent, and covalent bonds Name (given formula) or write formula (given name) of covalent and ionic compounds Naming Quiz September 2013 Unit 1: Molecular Structure and Intermolecular Forces (continued) Chemical Bonding and VSEPR (cont.) Given the formula of a molecule showing primarily covalent bonding, describe the bond polarity, molecular polarity, draw the Lewis dot structure, and describe the shape or geometry including bond angles. Construct models to determine molecular geometry. Molecular Models Activity Students draw Lewis structures of and build models of molecules, and predict molecular orientation, geometry, polarity, bond angles, and hybridization. VSEPR/Quantum Numbers Quiz VSEPR Lab Packet VSEPR Lab Packet Intermolecular forces HS-PS1-3 SSL 1.,1.B,1.C,1.D Differentiate between intermolecular and intramolecular forces. Melting Point/Boiling Point lab Students make predictions about the melting and boiling points of substances based on the structure of the molecule, then go into the lab and measure the actual melting 2 of 8
3 and boiling points. Given the formula of a molecule, Intermolecular Forces Demos identify the nature of the Students perform teacher intermolecular force as London supervised demos for the class. dispersion, dipole-dipole, or Topics: solubility, conductivity, hydrogen bonding. malleability, viscosity, and evaporation rate Properties of solids HS-PS1-3 SSL 3.B,3.C SSL 4.A,4.C Given the formula of a solid, classify it as metallic, ionic, molecular or macromolecular. Also, be able to identify the basic units within, the force holding them together, and predict the physical properties of the substance. Given an unknown solid substance, be able to determine enough information about its physical properties in the laboratory in order to classify it as metallic, ionic, molecular, or macromolecular. Attractive Forces Lab Students classify substances based on solubility, conductivity, and melting point. Categories are ionic binary, ionic polyatomic, ionic hydrate, molecular polar, molecular nonpolar, metallic, and network solid. Chapter 10 Study Guide Students reinforce concepts related to attractive forces and types of solids. Attractive Forces Lab Summary Attractive Forces Lab Summary Attractive Forces Lab Summary 3 of 8
4 October 2013 Unit 2: Stoichiometry and the Gas Laws Theme: Quantitative relationships in chemical equations due to conservation of mass Stoichiometric Calculations HS-PS1-2 HS-PS1-7 SSL 3.B The Gas Laws Calculate the molar mass and percent composition of a substance given its formula, or determine empirical and molecular formula given mass data or percent composition. Given a chemical equation, calculate masses of reactants and products and determine excess and limiting reactants. Use the ideal gas law and other gas laws to calculate pressure, volume, moles, or temperature. Describe the main assumptions of the kinetic molecular theory for gases. Mole Calculations Activity Students go to 10 different stations in the lab, make measurements, and perform calculations to introduce the concept of the mole and Avogadro s number. Hydrate Lab Students use stoichiometry to determine the formula of a hydrate. Carbonate/Bicarbonate Lab Students use stoichiometry and flame tests to identify an unknown carbonate or bicarbonate. Airbag Lab Students use the ideal gas law and stoichiometry to calculate the amounts of sulfuric acid and sodium bicarbonate to put inside a Ziploc bag in order to react and inflate the bag, but not pop it. Boyle s Law Mini-Lab Students use Logger Pro software and pressure sensors to investigate the relationship between pressure and volume of a gas. Mole Quiz Hydrate Lab Calculations/Summary Unit 2 Exam Carbonate/Bicarbonate lab calculations Carbonate/Bicarbonate lab Quiz Mole Quiz Unit 2 Exam Airbag calculations Unit 2 Exam Unit 2 Exam 4 of 8
5 November 2013 Unit 3: Solutions, Colligative Properties, Spectrophotometry Theme: The structure of the solute(s) and solvent(s) affects the properties of the solution Factors that affect solubility HS-PS1-3 SSL 1.A,1.B SSL 3.B Predict the solubility of a solute in different solvents. Predict how changes in pressure and/or temperature affect solubilities of solids, liquids and gases. The colligative properties HS-PS1-3 Predict the vapor pressure, freezing point, boiling point, or osmotic pressure of a solution of known concentration. Determine the molar mass of an unknown solute by freezing point depression or boiling point elevation. Define electrolyte and be able to determine whether a solute is an electrolyte or a nonelectrolyte. Colligative Properties Investigation Students evaluate solute effects on freezing point depression and boiling point elevation in an openended investigation. Freezing Point (Antifreeze) Lab Students determine the effects of commercially available antifreeze on the freezing and boiling point of water, and use their data to estimate the molar mass of the antifreeze. Solutions Homework Check Antifreeze Lab Write-up Solutions Quiz Antifreeze Lab Write-up Solutions Quiz Compare colligative properties of nonelectrolytes to electrolytes. Solutions Homework Check Solutions Quiz 5 of 8
6 Dilution series and spectrophotometry Prepare a solution of known concentration and create a dilution series. Solution preparation activity Students perform the necessary calculations and then prepare a solution of known concentration. They then measure the conductivity of the solutions. Use a spectrophotometer and/or colorimeter to create a standard curve, and determine the concentration of an unknown solution. Spectrophotometry Lab Students perform a dilution series, construct a standard curve, determine concentration of an unknown, and create an absorption spectrum of two different colored solutions. Solutions Homework Check Solutions Homework Check Spectrophotometry Lab Summary 6 of 8
7 December 2013 Unit 4: Kinetics Theme: Collision Theory and the factors that affect reaction rates Factors that affect reaction rates HS-PS1-5,5.B Predict the effect of changes in concentration, temperature, and the addition of a catalyst on the rate of reaction, and explain these effects using collision theory. Reaction Rate Lab I Students investigate the effects of concentration, temperature, and surface area on the reaction between hydrochloric acid and calcium carbonate. Reaction Rate Lab I Post-lab Unit 4 Exam Reaction orders Potential Energy Diagrams SSL 3.B Be able to determine the order of a reaction, given the initial rate as a function of concentration of reactants, or reactants as a function of time. Generate or interpret graphic representations of zero, first, or second order reactions. Interpret a potential energy diagram and identify Delta H, Ea, Ea, the location of the activated complex, and the effect of a catalyst. Reaction Rate Lab II Pre-lab Reaction Rate Lab II Students collect data and perform the necessary calculations to determine the order and rate constant of a chemical reaction. Method of Initial Rates Packet The method of initial rates and graphical representation of different orders is reinforced by working problems. Reaction Rate Lab II (Determination of Ea) Students calculate the activation energy for a reaction using data collected in the lab. Reaction Rate Lab II Summary Unit 4 Exam Unit 4 Exam 7 of 8
8 Reaction Mechanisms SSL 3.B Unit 4 Exam Determine whether a proposed mechanism is consistent with an observed rate law. If it is not, suggest a mechanism that is consistent. Reaction Mechanisms Analogy An analogy to the University of Illinois Assembly Hall is discussed to develop the idea of rate limiting step and zero order reactions. Reaction Mechanisms Practice Problems Students practice the concepts of reaction mechanisms. Note: Most Content, Skills and Processes that are assessed on unit exams are also assessed on the semester final exam. 8 of 8
Keystone Exams: Chemistry Assessment Anchors and Eligible Content. Pennsylvania Department of Education www.education.state.pa.
Assessment Anchors and Pennsylvania Department of Education www.education.state.pa.us 2010 PENNSYLVANIA DEPARTMENT OF EDUCATION General Introduction to the Keystone Exam Assessment Anchors Introduction
More informationChemistry. The student will be able to identify and apply basic safety procedures and identify basic equipment.
Chemistry UNIT I: Introduction to Chemistry The student will be able to describe what chemistry is and its scope. a. Define chemistry. b. Explain that chemistry overlaps many other areas of science. The
More informationForensic Science Standards and Benchmarks
Forensic Science Standards and Standard 1: Understands and applies principles of scientific inquiry Power : Identifies questions and concepts that guide science investigations Uses technology and mathematics
More informationBergen Community College Division of Mathematics, Science and Technology Department of Physical Sciences
Semester and year: Course Number: Meeting Times and Locations: Instructor: Office Location: Phone: Office Hours: Email Address: Bergen Community College Division of Mathematics, Science and Technology
More informationAAHS-CHEMISTRY FINAL EXAM PREP-REVIEW GUIDE MAY-JUNE 2014 DR. GRAY CLASS OF 2016
AAHS-CHEMISTRY FINAL EXAM PREP-REVIEW GUIDE MAY-JUNE 2014 DR. GRAY CLASS OF 2016 UNIT I: (CHAPTER 1-Zumdahl text) The Nature of Science and Chemistry 1. Explain why knowledge of chemistry is central to
More informationTitle: General Chemistry I. Department: Credits: 5 Lecture Hours:4 Lab/Studio Hours:3
Code: CHEM-101 Title: General Chemistry I Institute: STEM Department: Chemistry Course Description:The student will investigate the fundamental concepts of chemistry from a theoretical approach and participate
More informationCHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING
CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING Essential Standard: STUDENTS WILL UNDERSTAND THAT THE PROPERTIES OF MATTER AND THEIR INTERACTIONS ARE A CONSEQUENCE OF THE STRUCTURE OF MATTER,
More informationAP Chemistry Semester One Study Guide
AP Chemistry Semester One Study Guide Unit One: General Chemistry Review Unit Two: Organic Nomenclature Unit Three: Reactions Unit Four: Thermochemistry Unit Five: Electronic Structure of the Atom Unit
More informationCHEMISTRY II FINAL EXAM REVIEW
Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas
More informationCHAPTER 6 Chemical Bonding
CHAPTER 6 Chemical Bonding SECTION 1 Introduction to Chemical Bonding OBJECTIVES 1. Define Chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding.. 4. Explain
More informationPrentice Hall. Chemistry (Wilbraham) 2008, National Student Edition - South Carolina Teacher s Edition. High School. High School
Prentice Hall Chemistry (Wilbraham) 2008, National Student Edition - South Carolina Teacher s Edition High School C O R R E L A T E D T O High School C-1.1 Apply established rules for significant digits,
More informationA Teaching Portfolio for General Chemistry Harry Pang, Ph.D.
A Teaching Portfolio for General Chemistry Harry Pang, Ph.D. Table of Content I. Teaching Philosophy II. Critical Thinking Practices III. Course Syllabus IV. Student Evaluation V. Final Report I. My Teaching
More informationSTATE UNIVERSITY OF NEW YORK COLLEGE OF TECHNOLOGY CANTON, NEW YORK COURSE OUTLINE CHEM 150 - COLLEGE CHEMISTRY I
STATE UNIVERSITY OF NEW YORK COLLEGE OF TECHNOLOGY CANTON, NEW YORK COURSE OUTLINE CHEM 150 - COLLEGE CHEMISTRY I PREPARED BY: NICOLE HELDT SCHOOL OF SCIENCE, HEALTH, AND PROFESSIONAL STUDIES SCIENCE DEPARTMENT
More informationCOURSE SYLLABUS CHEM 103: General Chemistry- Fall 2010 University of Wisconsin-Eau Claire
COURSE SYLLABUS CHEM 103: General Chemistry- Fall 2010 University of Wisconsin-Eau Claire Instructor Dr. Sudeep Bhattacharyay Office P-452 Office Phone 715 836 2278 Office Hours By appointment E-mail bhattas@uwec.edu
More informationSTUDENT COURSE INFORMATION
STUDENT COURSE INFORMATION FANSHAWE COLLEGE OF APPLIED ARTS AND TECHNOLOGY HEALTH SCIENCES JANUARY 2010 CHEM-1004 -- CHEMISTRY I Duration: 45 total course hours Credit Units: 3.00 *NOTE: The hours may
More informationIntroduction to Chemistry. Course Description
CHM 1025 & CHM 1025L Introduction to Chemistry Course Description CHM 1025 Introduction to Chemistry (3) P CHM 1025L Introduction to Chemistry Laboratory (1) P This introductory course is intended to introduce
More informationChemistry. Essential Question: How can one explain the structure, properties, and interactions of matter?
Chemistry Special Note for the 2014-15 School Year: In 2013, the Maryland State Board of Education adopted the Next Generation Science Standards (NGSS) that set forth a vision for science education where
More informationName Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular
More informationSoutheastern Louisiana University Dual Enrollment Program--Chemistry
Southeastern Louisiana University Dual Enrollment Program--Chemistry The Southeastern Dual Enrollment Chemistry Program is a program whereby high school students are given the opportunity to take college
More informationChapter 13 - LIQUIDS AND SOLIDS
Chapter 13 - LIQUIDS AND SOLIDS Problems to try at end of chapter: Answers in Appendix I: 1,3,5,7b,9b,15,17,23,25,29,31,33,45,49,51,53,61 13.1 Properties of Liquids 1. Liquids take the shape of their container,
More informationThe Mole Concept. The Mole. Masses of molecules
The Mole Concept Ron Robertson r2 c:\files\courses\1110-20\2010 final slides for web\mole concept.docx The Mole The mole is a unit of measurement equal to 6.022 x 10 23 things (to 4 sf) just like there
More information3/5/2014. iclicker Participation Question: A. MgS < AlP < NaCl B. MgS < NaCl < AlP C. NaCl < AlP < MgS D. NaCl < MgS < AlP
Today: Ionic Bonding vs. Covalent Bonding Strengths of Covalent Bonds: Bond Energy Diagrams Bond Polarities: Nonpolar Covalent vs. Polar Covalent vs. Ionic Electronegativity Differences Dipole Moments
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationMolar Mass of Butane
Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures
More informationKinetic Molecular Theory. Chapter 5. KE AVE and Average Velocity. Graham s Law of Effusion. Chapter 7. Real Gases
hapter 5 1. Kinetic Molecular Theory. 2. Average kinetic energy and velocity. 3. Graham s Law of Effusion. 4. Real gases and the van der Waals equation. Kinetic Molecular Theory The curves below represent
More informationQUEENSBOROUGH COMMUNITY COLLEGE CHEMISTRY DEPARTMENT COURSE SYLLABUS CH-151: GENERAL CHEMISTRY I
QUEENSBOROUGH COMMUNITY COLLEGE CHEMISTRY DEPARTMENT COURSE SYLLABUS CH-151: GENERAL CHEMISTRY I Pre-requisites: MA-119 and MA-121 or Departmental permission Hours: 3 Class Hours 3 Laboratory Hours 1 Recitation
More informationInstructional Notes/Strategies. GLEs. Evidence / Assessments of learning Knowledge/Synthesis. Resources # SI-1 (E)
Lafayette Parish School System Curriculum Map Honors Chemistry (Pearson) Unit 1: Introduction to Chemistry Time Frame 1 week August 15 August 21, 2011 Unit Description - This unit focuses on Why It Is
More informationThe content is based on the National Science Teachers Association (NSTA) standards and is aligned with state standards.
Literacy Advantage Physical Science Physical Science Literacy Advantage offers a tightly focused curriculum designed to address fundamental concepts such as the nature and structure of matter, the characteristics
More informationChapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
More informationStates of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas
More informationWhat You Need To Know for the Chemistry Regents Exam
Name: What You Need To Know for the Chemistry Regents Exam The Test The Chemisty Regents Exam is broken down into three sections: Part A: 35 mulitple choice questions from all units covered over the course
More informationChemistry Diagnostic Questions
Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to
More informationChapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
More informationSummer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More informationScience Standard Articulated by Grade Level Strand 5: Physical Science
Concept 1: Properties of Objects and Materials Classify objects and materials by their observable properties. Kindergarten Grade 1 Grade 2 Grade 3 Grade 4 PO 1. Identify the following observable properties
More information5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C
1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationCHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry
CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,
More informationChemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
More informationCHEM 110 A Chemistry I
Columbia College Online Campus P a g e 1 CHEM 110 A Chemistry I Early Fall Session (15-51) Monday, August 17 Saturday, October 10, 2015 Course Description Fundamental course in the principles of chemistry.
More informationCHM 111 - General Chemistry I Lecture Fall 2014
CHM 111 - General Chemistry I Lecture Fall 2014 Dr. Stuart T. Gentry Holroyd 329 215-951-1259 gentry@lasalle.edu Class Postings, Lecture Notes, and PowerPoint Slides Available on Canvas and at www.lasalle.edu/~gentry
More informationGetting the most from this book...4 About this book...5
Contents Getting the most from this book...4 About this book....5 Content Guidance Topic 1 Atomic structure and the periodic table...8 Topic 2 Bonding and structure...14 Topic 2A Bonding....14 Topic 2B
More informationRANGER COLLEGE CREDIT HOURS: 3 HRS/WK LECTURE & 3 HRS/WK LAB. LEC/LAB/HRS/WK COMBINATION: 4 credit hours total
RANGER COLLEGE COURSE NUMBER AND TITLE: Chemistry 1411 General Chemistry I CREDIT HOURS: 3 HRS/WK LECTURE & 3 HRS/WK LAB LEC/LAB/HRS/WK COMBINATION: 4 credit hours total INSTRUCTOR: Kimberlea M. Adams
More informationCHAPTER 6 REVIEW. Chemical Bonding. Answer the following questions in the space provided.
Name Date lass APTER 6 REVIEW hemical Bonding SETIN 1 SRT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence
More informationChemistry Assessment Unit AS 1
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]
More informationWhich substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationKINETIC MOLECULAR THEORY OF MATTER
KINETIC MOLECULAR THEORY OF MATTER The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids, liquids,
More informationChapter 14 Solutions
Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute
More informationIn the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
More informationCHEM 120 Online Chapter 7
CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases
More informationPV (0.775 atm)(0.0854 L) n = = = 0.00264 mol RT -1-1
catalyst 2 5 g ¾¾¾¾ 2 4 g 2 g DH298 = rxn DS298 C H OH( ) C H ( ) + H O( ) 45.5 kj/mol ; = 126 J/(K mol ) ethanol ethene water rxn 1 atm 760 torr PV (0.775 atm)(0.0854 L) n = = = 0.00264 mol RT -1-1 (0.08206
More informationFreezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version
Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version Freezing point depression describes the process where the temperature at which a liquid freezes is lowered by adding another
More informationChem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
More informationWRIGHT COLLEGE PROGRAM/DISCIPLINE ASSESSMENT FORM
Program/Discipline: Chemistry 201 Instructional Manager: Kevin Li Semester/Year: Fall/2012 Assessment Coordinator: Kris Ochwat Department Chair: Doris Espiritu Email: kochwat@ccc.edu Plan Title: The Improvement
More informationStructure, Polarity & Physical Properties
tructure, Polarity & Physical Properties upplemental packet handouts 92-96 I. Lewis structure, stability, and bond energies A. ydrogen, oxygen, and nitrogen are present in the atmosphere as diatomic molecular
More informationVCE CHEMISTRY UNIT 2 Environmental Chemistry SAMPLE COURSE OUTLINE
VCE CHEMISTRY UNIT 2 Environmental Chemistry SAMPLE COURSE OUTLINE Week Area of Study Key knowledge Possible activities Key skills 1 1 Water Role of water in maintaining life in the environment unique
More informationLaboratory 11: Molecular Compounds and Lewis Structures
Introduction Laboratory 11: Molecular Compounds and Lewis Structures Molecular compounds are formed by sharing electrons between non-metal atoms. A useful theory for understanding the formation of molecular
More information7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter
7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed
More informationAP CHEMISTRY 2009 SCORING GUIDELINES
AP CHEMISTRY 2009 SCORING GUIDELINES Question 6 (8 points) Answer the following questions related to sulfur and one of its compounds. (a) Consider the two chemical species S and S 2. (i) Write the electron
More informationA mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
Chemistry I ATOMIC BONDING PRACTICE QUIZ Mr. Scott Select the best answer. 1) A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is
More informationPart B 2. Allow a total of 15 credits for this part. The student must answer all questions in this part.
Part B 2 Allow a total of 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 3 Mg(s) N 2 (g) Mg 3 N 2 (s). Allow credit even if the coefficient 1 is
More informationIndiana's Academic Standards 2010 ICP Indiana's Academic Standards 2016 ICP. map) that describe the relationship acceleration, velocity and distance.
.1.1 Measure the motion of objects to understand.1.1 Develop graphical, the relationships among distance, velocity and mathematical, and pictorial acceleration. Develop deeper understanding through representations
More informationChemistry Ch 15 (Solutions) Study Guide Introduction
Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual
More informationLAGUARDIA COMMUNITY COLLEGE CITY UNIVERSITY OF NEW YORK NATURAL SCIENCES DEPARTMENT
LAGUARDIA COMMUNITY COLLEGE CITY UNIVERSITY OF NEW YORK NATURAL SCIENCES DEPARTMENT SCC 110: Foundations of Chemistry Course Coordinator: Dr. Nalband S. Hussain Office: M 210 E-mail: nhussain@lagcc.cuny.edu
More informationChapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?
Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently
More informationKINETIC THEORY OF MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature
1 KINETIC TERY F MATTER - molecules in matter are always in motion - speed of molecules is proportional to the temperature TE STATES F MATTER 1. Gas a) ideal gas - molecules move freely - molecules have
More informationAP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
More informationMole Notes.notebook. October 29, 2014
1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the
More informationChapter 4 Practice Quiz
Chapter 4 Practice Quiz 1. Label each box with the appropriate state of matter. A) I: Gas II: Liquid III: Solid B) I: Liquid II: Solid III: Gas C) I: Solid II: Liquid III: Gas D) I: Gas II: Solid III:
More informationChemistry 13: States of Matter
Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties
More informationExam 4 Practice Problems false false
Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids
More informationDetermination of Molar Mass by Freezing-Point Depression
DETERMINATION OF MOLAR MASS BY FREEZING-POINT DEPRESSION 141 Determination of Molar Mass by Freezing-Point Depression OBJECTIVES: Gain familiarity with colligative properties of nonelectrolyte solutions
More informationPractice Multiple Choice Questions:
Practice Multiple Choice Questions: 1) Which of the following is NOT a laboratory safety rule? a) You should never mix acids with bases b) You should tie back your long hair c) You should never add water
More informationEXPERIMENT 1: Survival Organic Chemistry: Molecular Models
EXPERIMENT 1: Survival Organic Chemistry: Molecular Models Introduction: The goal in this laboratory experience is for you to easily and quickly move between empirical formulas, molecular formulas, condensed
More information2. Why does the solubility of alcohols decrease with increased carbon chain length?
Colligative properties 1 1. What does the phrase like dissolves like mean. 2. Why does the solubility of alcohols decrease with increased carbon chain length? Alcohol in water (mol/100g water) Methanol
More informationAP CHEMISTRY 2006 SCORING GUIDELINES
AP CHEMISTRY 2006 SCORING GUIDELINES Question 6 6. Answer each of the following in terms of principles of molecular behavior and chemical concepts. (a) The structures for glucose, C 6 H 12 O 6, and cyclohexane,
More informationMolecular Geometry & Polarity
Name AP Chemistry Molecular Geometry & Polarity Molecular Geometry A key to understanding the wide range of physical and chemical properties of substances is recognizing that atoms combine with other atoms
More informationCHEMISTRY 103 - GENERAL CHEMISTRY Calvin College Whoever can be trusted with very little can also be trusted with much.
CHEMISTRY 103 - GENERAL CHEMISTRY Calvin College Whoever can be trusted with very little can also be trusted with much. Luke 16:10a Instructor: Herb Fynewever Office: DeVries Hall 229 herb.fynewever@calvin.edu
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More informationARIZONA Science Standards High School Chemistry: Matter and Change 2005
ARIZONA Science Standards High School Chemistry: Matter and Change 2005 OBJECTIVES Strand 1: Inquiry Process Concept 1: Observations, Questions, and Hypotheses Formulate predictions, questions, or hypotheses
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationUnit 1 Measurement, Matter and Change
Unit 1 Measurement, Matter and Change Part one: Scientific Measurement 1. Apply the rules of safety in the Chemistry laboratory 2. Distinguish between quantitative and qualitative measurements 3. Distinguish
More informationScience 20. Unit A: Chemical Change. Assignment Booklet A1
Science 20 Unit A: Chemical Change Assignment Booklet A FOR TEACHER S USE ONLY Summary Teacher s Comments Chapter Assignment Total Possible Marks 79 Your Mark Science 20 Unit A: Chemical Change Assignment
More informationPhysical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
More informationPhase diagram of water. Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure.
Phase diagram of water Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure. WATER Covers ~ 70% of the earth s surface Life on earth
More informationCHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS
1 CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS The Chemical Equation A chemical equation concisely shows the initial (reactants) and final (products) results of
More information(1) e.g. H hydrogen that has lost 1 electron c. anion - negatively charged atoms that gain electrons 16-2. (1) e.g. HCO 3 bicarbonate anion
GS106 Chemical Bonds and Chemistry of Water c:wou:gs106:sp2002:chem.wpd I. Introduction A. Hierarchy of chemical substances 1. atoms of elements - smallest particles of matter with unique physical and
More informationAP CHEMISTRY 2013 SCORING GUIDELINES
AP CHEMISTRY 2013 SCORING GUIDELINES Question 4 (15 points) For each of the following three reactions, write a balanced equation for the reaction in part (i) and answer the question about the reaction
More informationUnit 3: Quantum Theory, Periodicity and Chemical Bonding. Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular Forces
onour Chemistry Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 10: Chemical Bonding II Molecular Geometry & Intermolecular orces 10.1: Molecular Geometry Molecular Structure: - the three-dimensional
More informationElectrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set
Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You
More informationChapter 13: Properties of Solutions
Chapter 13: Properties of Solutions Problems: 9-10, 13-17, 21-42, 44, 49-60, 71-72, 73 (a,c), 77-79, 84(a-c), 91 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component(s)
More informationProperties and Classifications of Matter
PS-3.1 Distinguish chemical properties of matter (including reactivity) from physical properties of matter (including boiling point, freezing/melting point, density [with density calculations], solubility,
More informationGENERAL CHEMISTRY II Lecture & Recitation
Howard University Department of Chemistry Fall 2010 GENERAL CHEMISTRY II Lecture & Recitation Chem 004, Section 04, CRN 82454; Section 05, CRN 82456; Section 06, CRN 82458 4 Credit Hours Course Time &
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions 11.1 Solution Composition A. Molarity moles solute 1. Molarity ( M ) = liters of solution B. Mass Percent mass of solute 1. Mass percent = 1 mass of solution C. Mole
More information1 What is the angular momentum quantum number (l) value for the 3p sublevel? A 1
1 What is the angular momentum quantum number (l) value for the 3p sublevel? 1 2 3 4 ORRET: For the 3p sublevel, the principal quantum number (n) is 3 and the angular momentum quantum number (l) is 1.
More informationChemical Bonds. Chemical Bonds. The Nature of Molecules. Energy and Metabolism < < Covalent bonds form when atoms share 2 or more valence electrons.
The Nature of Molecules Chapter 2 Energy and Metabolism Chapter 6 Chemical Bonds Molecules are groups of atoms held together in a stable association. Compounds are molecules containing more than one type
More informationCHEMISTRY BONDING REVIEW
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
More information