CHM 130 Fundamental Chemistry with Lab (Title Change ONLY effective Oct. 2013) Course Package

Transcription

1 Fundamental Chemistry with Lab (Title Change ONLY effective Oct. 2013) Course Package Effective Spring 2005 Modified 4/3/2009 effective Fall 2009

2 COURSE INFORMATION Title Fundamental Chemistry Number CHM130 Catalog Course Description. Fundamental chemistry covers principles of inorganic chemistry designed for programs requiring a year or less of chemistry, and for students proceeding on to one semester of organic chemistry. Credit hours 04 Lecture hours 03 Lab hours 03 Prerequisites ENG 085, ENG 089 and MAT 031 or appropriate score on assessment. Identify any risk management Risk of minor physical injury (skin laceration) due to glass breakage issues. Writing Across the Curriculum Rationale: Mohave Community College firmly supports the idea that writing can be used to improve education; students who write in their respective content areas will learn more and retain what they learn better than those who don t. Courses in the core curriculum have been identified as Writing Across the Curriculum courses. Suggested minimum standards for the Writing Across the Curriculum component are as follows: 1. The writing assignments should total words. For example, a single report which is 1500 words in length could fulfill the requirement, or a series of essay questions and short papers (example: four -375 word assignments) which total 1500 words could meet the requirement. 2. The writing component will represent at least 10% of a student s final grade in the course. Is this a course identified as a Writing Across the Curriculum course? Yes No Contact person(s) Farah Farah (KNG), Jan Parrott (BHC), Doyle Wilson (HAV), Kris Hansen (NMC) - 2 -

3 Intended Course Outcomes Course Goals 1. Introduce students to the perspectives and values of chemistry and the major principles and theories upon which these are based. 2. Promote scientific literacy using the developments, methods and technologies of chemistry. 3. Demonstrate the ability to communicate an understanding of the interrelationships between chemical principles and concepts. 4. Facilitate critical thinking skills through direct experience with the methods and processes of inquiry (the scientific method). 5. Recognize the important contributions that chemistry has made and continues to make in today s society. Course Competencies and Objectives Competency 1 Students will be able to describe the science of chemistry. Objective 1.1 Devise a working definition of chemistry. Objective 1.2 Solve problems using a scientific approach. Objective 1.3 Demonstrate an understanding of the scientific method. Objective 1.4 Interpret the content of the textbook in order to aid in acquiring information about chemistry. Competency 2 Students will be able to perform chemical measurements and calculations. Objective 2.1 Convert numbers written in decimal notation to scientific notation and vise versa. Objective 2.2 List the Systeme Internationale (SI-an international system for standardizing measures) system prefixes and their meanings. Objective 2.3 Identify the names of the principle SI units of length, volume, and mass. Objective 2.4 Perform measurements of length, volume, and mass. Objective 2.5 Explain why there is uncertainty in measurements. Objective 2.6 Restate the rules for determining the correct number of significant figures and the correct number of significant figures to use in a calculation. Objective 2.7 Solve problems using dimensional analysis. Objective 2.8 Convert temperatures from one scale of measure to another, specifically, Celsius, Fahrenheit, or Kelvin. Objective 2.9 Calculate the density, volume, or mass, if given any two items. Competency 3 Students will be able to define matter and energy

4 Objective 3.1 Define matter. Objective 3.2 State the distinguishing characteristics of the three states of matter. Objective 3.3 State the difference between physical or chemical properties and physical or chemical changes. Objective 3.4 Define elements and compounds and give examples of each. Objective 3.5 Determine whether a substance is a pure substance or a mixture, whether it is homogeneous or heterogeneous. Objective 3.6 Describe how distillation and filtration are used to separate a mixture. Objective 3.7 Identify the relative amounts of energy associated with the three states of matter and which units are commonly used when discussion heat energy. Objective 3.8 Solve problems involving energy, mass, specific heat and temperature change. Competency 4 Understand the Basic Chemical Foundations: Elements, Atoms, and Ions. Objective 4.1 List which elements are common on earth and describe their relative abundance. Objective 4.2 List the names and symbols for common elements. Objective 4.3 State Dalton s atomic theory. Objective 4.4 Interpret chemical formulas. Objective 4.5 Identify the structure of the atom according to modern concepts. Objective 4.6 Define the term isotope. Objective 4.7 Write and interpret symbols for isotopes. Objective 4.8 Identify what the symbols and numbers on a periodic table mean, what the major families of elements are, and where to they are located on the periodic table. Objective 4.9 Describe the natural states of the elements. Objective 4.10 Describe the meaning of the term ion. Objective 4.11 Identify compounds that contain ions. Competency 5 Describe the nomenclature of compounds Objective 5.1 Name compounds that contain a metal and a nonmetal. Objective 5.2 Name binary compounds that contain only nonmetals (type III). Objective 5.3 List the names, formulas, and charges for the common polyatomic ions and how to name compounds which contain polyatomic ions. Objective 5.4 State the names of the common acids and how to name less common acids. Objective 5.5 Write the chemical formula of a compound given the name. Competency 6 Identify Chemical Reactions - 4 -

5 Objective 6.1 Identify the evidence that a chemical reaction has occurred. Objective 6.2 Write chemical equations. Objective 6.3 Balance chemical equations. Competency 7 Identify Reactions in Aqueous Solutions Objective 7.1 Describe reactions in aqueous solutions. Objective 7.2 Predict whether a reaction will occur. Objective 7.3 Identify reactions in which a solid forms. Objective 7.4 Identify reactions that form water: acids and bases. Objective 7.5 Identify reactions of metals with nonmetals: oxidation-reduction. Objetcive 7.6 Classify reactions as precipitation, acid-base, or oxidationreduction. Competency 8 Determine Chemical Composition. Objective 8.1 Describe the concept of counting by weighing. Objective 8.2 Solve problems to determine the number of atoms in a given mass of a substance. Objective 8.3 Define the term mole. Objective 8.4 Calculate the number of moles of a substance and the number of units of a substance. Objective 8.5 Calculate the molar mass of any molecule. Objective 8.6 Calculate the percent composition of a compound given the formula of a molecule. Objective 8.7 Explain the distinction between an empirical formula and a molecular formula. Objective 8.8 Calculate the empirical formula of a compound. Objective 8.9 Calculate the molecular formula of a compound. Competency 9 Determine Chemical Quantities. Objective 9.1 Interpret and apply information given in a balanced chemical equation, in terms of moles. Objective 9.2 Use the mole-mole relationship as a conversion factor to calculate moles of reactants and products. Objective 9.3 Calculate the mass of the product produced. Objective 9.4 Calculate the percent yield. Competency 10 Describe the Modern Atomic Theory. Objective 10.1 Describe how electromagnetic radiation is characterized. Objective 10.2 Recognize the different types of electromagnetic radiations. Objective 10.3 Identify what happens when a hydrogen atom in an excited state loses energy. Objective 10.4 Explain the Bohr model of an atom. Objective 10.5 Explain how the wave mechanical model of the atom describes - 5 -

6 the location of an electron. Objective 10.6 State the physical shapes, relative distance from the nucleus, and labels (symbols) for the orbitals of hydrogen through the third principles energy level. Objective 10.7 Explain what a probability map of an orbital represents. Objective 10.8 Recognize that electron spin limits the number of electrons in each orbital to two. Objective 10.9 Write electron configurations, box diagrams, and short-hand for the elements using the periodic table. Objective Analyze the relationship between the arrangements of atoms in the periodic table and the arrangement of electrons in orbitals. Objective Recognize the atomic trends that exist in the periodic table. Competency 11 Describe Chemical Bonding. Objective 11.1 Identify the different types of bonds which can form between atoms. Objective 11.2 Explain why different kinds of bonds form. Objective 11.3 Describe covalent bonds in terms of electro negativity. Objective 11.4 Determine which molecules will be polar-based on bond polarity and dipole moments. Objective 11.5 Analyze stable electron configurations and charges on ions. Objective 11.6 Explain ionic bonding and the structure of ionic compounds. Objective 11.7 Examine the relationship between the size of an anion or cation. Objective 11.8 Draw Lewis Structures of molecules. Objective 11.9 Draw Lewis Structures of molecules with double and triple bonds. Objective Determine the molecular structure, electron arrangement, and the bond angles between pairs of atoms for a given molecule. Objective State the premise of the Valence Shell Electron Pair Repulsion (VSEPR) model. Competency 12 Discuss the Behavior of Gases Objective 12.1 Describe how a barometer can used to measure atmospheric pressure. Objective 12.2 Apply the common units for measuring pressure and for converting units. Objective 12.3 Use Boyle s law to calculate the new volume or new pressure of a gas. Objective 12.4 Use Charles law to calculate the new volume or new temperature of a gas. Objective 12.5 Use Avogadro s law to calculate the new volume or new number of moles of a gas. Objective 12.6 Apply the ideal gas law to solve many gas law problems. Objective 12.7 Apply Dalton s law of partial pressures to calculate the total pressure of a mixture of gases or the partial pressure of one gas in a mixture. Objective 12.8 Differentiate between a law and a model

7 Objective 12.9 Outline the parts of the Kinetic Molecular Theory and how the Kinetic Molecular Theory explains gas behavior. Objective Apply the appropriate gas law or the molar volume of an ideal gas to solve stoichiometric problems. Competency 13 Identify Properties of Liquids and Solids. Objective 13.1 List the properties of water and its phase changes. Objective 13.2 Discuss the phase changes of water using the heating/cooling curve. Objective 13.3 Differentiate between intra molecular and intermolecular forces. Objective 13.4 Use molar heat fusion and molar heat of vaporization to calculate the energy required to melt of form ice, to boil water, and to condense steam. Objective 13.5 Compare and contrast dipole-dipole interaction, hydrogen bonding, and London dispersion forces between molecules. Objective 13.6 Explain how the intermolecular forces play a role in changes of the physical state, that is, from liquid to solid or liquid to gas. Objective 13.7 Discuss the concept of vapor pressure and predict whether a molecule will have a large or small vapor pressure. Objective 13.8 List the properties of different types of solids. Objective 13.9 Describe what types of bonding occur in different crystalline solids and how bonding in metals account for the different properties of different metals. Competency 14 Determine the Concentrations of Solutions Objective 14.1 Define the term solubility. Objective 14.2 Explain how intermolecular forces affect the solubility of molecules. Objective 14.3 Define terms associated with concentration of a solution. Objective 14.4 Calculate the mass percent of a solution. Objective 14.5 Calculate the moles of solute in a solution and the molarity of a solution. Objective 14.6 Calculate the amount of concentrated stock solution needed to prepare a diluted solution. Objective 14.7 Perform solution stoichiometric calculations using the balanced equations for a neutralization (acid-base) reaction to determine the amount of reactant needed to neutralized (react with) another reactant. Objective 14.8 Calculate normality, equivalents, or volume of a solution and use the calculations to determine how much acid or base is needed to react with a given amount of acid or base solution. Competency 15 Determine Properties of Acids and Bases. Objective 15.1 Compare the Arrhenius model of acids and bases to the Bronsted- Lowry model of acids and bases. Objective 15.2 Identify a conjugate acid-base pair. Objective 15.3 State the properties of weak and strong acids

8 Objective 15.4 Explain how water can be both an acid and a base and how the ion-product derived. Objective 15.5 Interpret the ph scale and calculate the ph or the poh. Objective 15.6 Calculate the hydrogen ion and the hydroxide ion concentrations given the ph or the poh. Objective 15.7 Determine the ph of a strong acid solution of known molarity. Objective 15.8 Identify the characteristics of a buffer and how a buffer works to resist changes in ph. Competency 16 Understand Equilibrium. Objective 16.1 Describe how the collision model explains how chemical reactions occur. Objective 16.2 List what factors can change the rate of a chemical reaction and why these factors cause a change in the rate of reaction. Objective 16.3 Define the term equilibrium. Objective 16.4 Characterize the phrase equilibrium constant. Objective 16.5 Write an equilibrium expression for a balanced chemical equation. Objective 16.6 Write an equilibrium expression for a heterogeneous equilibrium reaction. Objective 16.7 Apply Le Chatelier s Principle to predict the effect of changes in concentration, volume, or temperature has on equilibrium. Objective 16.8 Apply the equilibrium constant to calculate concentrations of reactants products or the equilibrium constant itself. Objective 16.9 Define the nature of the solubility product and its use. Competency 17 Understand Oxidation-Reduction Reactions and Electrochemistry. Objective 17.1 Define oxidation and reduction reactions, and identify oxidationreduction reactions between a metal and nonmetal. Objective 17.2 Assign oxidation states to all atoms in molecules and in ions. Objective 17.3 Determine which elements are oxidized and which elements are reduced. Objective 17.4 Determine which species is the oxidizing agent and which is the reducing agent. Objective 17.5 Balance oxidation-reduction reactions by the half-reaction method. Objective 17.6 Define the term electrochemistry. Objective 17.7 Describe how lead cell and how common dry cell batteries work. Objective 17.8 Explicate how corrosion occurs and what means are available to combat corrosion. Objective 17.9 Explain how electrolysis is used to produce a chemical reaction which does not occur naturally. Competency 18 Define Radioactivity and Nuclear Energy

9 Objective 18.1 Name and describe the types of radioactive decay. Objective 18.2 Balance a nuclear equation. Objective 18.3 Explain how elements can undergo nuclear transformations when bombarded with small particles. Objective 18.4 Outline common detection methods for detecting radioactivity. Objective 18.5 Express the concept of half-life time. Objective 18.6 Explain how dating by radioactivity can be used to determine the age of artifacts. Objective 18.7 Identify the medical applications of radioactivity. Objective 18.8 Describe nuclear energy and nuclear reactors. Objective 18.9 Explain how nuclear fission occurs. Objective Explain how nuclear fusion occurs. Objective Describe how radiation damages human tissue. Objective Describe the types of damage that can occur to human tissue with exposure to radioactivity. Competency 19 Define the Basics of Organic Chemistry (optional) Objective 19.1 Identity the types of bonds formed when a carbon atom bonds to one or more atoms. Objective 19.2 List the formulas for the first ten alkanes. Objective 19.3 List the formulas for structural isomers of alkanes. Objective 19.4 Name alkanes systematically and write correct structures from the names. Objective 19.5 State the major components of petroleum and how they are used. Objective 19.6 Describe the reactions alkanes undergo. Objective 19.7 Name alkenes and alkynes and describe addition reactions. Objective 19.8 Recognize and draw a common feature of aromatic hydrocarbons. Objective 19.9 List the aromatic hydrocarbons. Objective Recognize each of the aromatic functional groups. Objective Name and classify alcohols. Objective List the properties and uses of the common alcohols. Objective List the properties and uses of common aldehydes. Objective List the properties and uses of common uses of ketones. Objective Name the aldehydes and ketones. Objective List structures and properties of the common carboxylic acids and esters. Objective Describe the two basic ways that polymers are made from monomers. Objective Draw a section of polymer given the monomers

10 Teacher s Guide Course Materials and Equipment Textbook(s) Title Introductory Chemistry: A Foundation 6th Edition Publisher Cengage ISBN Title Introductory Chemistry: A Foundation Study Guide (optional) Publisher Cengage ISBN Title Publisher Introductory Chemistry: A Foundation Solution Guide (optional) Cengage Software Equipment ISBN Title Laboratory Textbook Chemical Education Resources, Brooks/ Cole Publisher Thomson Learning ISBN Mastering Chemistry, Practice Problems Falcon Software, Inc ISBN Standard chemistry laboratory equipment. Other Writing Across the Curriculum This course will include a component that meets the Writing Across the Curriculum requirements. This may consist of a term paper or laboratory report that is written following standard scientific guidelines (American Chemical Society). Learning Units Learning Unit Topic 1: Introduction, Measurements and Calculations Competency: 1 Objectives:

11 A. Lecture Activities: Review syllabus Review methodology Give a minutes chemistry diagnostic quiz. Use examples to relate chemistry in real life. Lecture demonstration 1. (a safe and fun demonstration of your choice). B. Labotratory Activities: Review safety rules. Review laboratory equipment and uses. Watch lab safety video. Show the students where to find things in the laboratory. Perform practicing safety in the chemistry laboratory experiment (lab textbook). Learning Unit Topic 2: Measurements and Calculations Competency: 2 Objectives: the Quiz over Learning Unit Topic (15-20 minutes quiz) that can be also given at the beginning of the lab period or the end of a ecture period. B. Laboratory Activities: Safety quiz. Lab equipment quiz. Dimensional analysis lab. Lab demonstration 1. PROP 383 Density of Liquids and Solids. MISC 490 Using Exponential

12 Notation and Significant Figures (may be used as take home activity). Learning Unit Topic 3: Matter and Energy Competency: 3 Objectives: B. Laboratory Activities: THER 623 Estimating the calorie content of peanuts. PROP 621 Isolating the components of a three component mixture. Learning Unit Topic 4: Chemical Foundations: Elements, Atoms, and Ions Competency: 4 Objectives: Lecture demonstration 2. B. Laboratory Activities: Learning Unit Topic 5: Nomenclature Competency: 5 Objectives:

13 B. Laboratory Activities: MISC 629 Naming Inorganic Chemical Substances. Recitation 2. Learning Unit Topic 6: Chemical Reactions: An Introduction Competency: 6 Objectives: Lecture demonstration 3. B. Laboratory Activities: 1. MISC 614 Writing, Interpreting and Balancing Chemical Equations. REAC 422 Studying Chemical Reactions and Writing Chemical Equations. Learning Unit Topic 7: Reactions in Aqueous Solutions Competency: 7 Objectives: B. Laboratory Activities: REAC 405 Identifying Six Solutions by Their Interactions. Recitation

14 Lab demonstration 2. Learning Unit Topic 8: Chemical Composition Competency: 8 Objectives: Lecture and dscussion over B. Laboratory Activities: PROP 440 Identifying a liquid using physical properties. STOI 386 Determining the Empirical Formula of Copper Chloride. Learning Unit Topic 9: Chemical Quantities Competency: 9 Objectives: Lecture class over B. Laboratory Activities: Identifying six solutions by their interactions lab. Learning Unit Topic 10: Modern Atomic Theory Competency: 10 Objectives: B. Laboratory Activities: Single replacement reactions and relative reactivity lab

15 Learning Unit Topic 11: Chemical Bonding Competency: 11 Objectives: Lecture demonstration 4. B. Laboratory Activities: STRC 434 Writing Lewis Symbols and Lewis Structures lab. Learning Unit Topic 12: Gases Competency: 12 Objectives: B. Laboratory Activities: PROP 608 Calculating the Molar Volume of Carbon Dioxide. PROP 384 Charles's Law. Learning Unit Topic 13: Liquids and Solids Competency: 13 Objectives: B. Laboratory Activities: Recitation

16 Learning Unit Topic 14: Solutions Competency: 14 Objectives: B. Laboratory Activities: PROP 391 Solutions. Lab demonstration 3. Learning Unit Topic 15: Acids and Bases Competency: 15 Objectives: Lecture class over B. Laboratory Activities: ANAL 395 Titrating Vinegar. Learning Units Topic 16: Equilibrium Competency: 16 Objectives: Activities/ Assignmens: B. Laboratory Activities: ANAL 464 Comparing the resistance of buffered and unbuffered solutions. Learning Units Topic 17: Oxidation-Reduction

17 Reactions and Electrochemistry Competency: 17 Objectives: Activities/ Assignmens: Lecture class over Final review. B. Laboratory Activities: Liquid nitrogen and dry ice fun lab. REAC 456 Studying Oxidation- Reduction Reactions. Learning Units Topic 18: Radioactivity and Nuclear Energy Competency: 18 Objectives: Last problem set assignment due. Final exam (comprehensive) B. Laboratory Activities: Lab checkout. Course Assessment Information Description of Course Assessments (Essays, multiple choice, etc.) Each student will be assessed using all or some of the following assessment devices: quizzes, exams (midterm and final), homework assignments, research papers, laboratory reports, and participation in both lecture and laboratory sessions. This course includes a component that meets the requirements for Writing Across the Curriculum for this college. Writing assignments may include term papers or laboratory reports that follow standard scientific guidelines established by the American

18 Chemical Society. Are exams standardized in your department? Yes No Where can faculty members locate or access the exams for this course? Are the exams required by the department? Yes NO See contact people listed above for information regarding laboratory report guidelines. A published test bank accompanies the instructional materials