CHEM 1405 Introductory Chemistry I

CHEM 1405
Introductory Chemistry I

Western Texas College

Basic Course Information
1. Lecture—Survey course introducing chemistry. Topics may include inorganic, organic, biochemistry, food/physiological chemistry, and environmental/consumer chemistry. Designed for allied health students and for students who are not science majors.
2. Lab—the required laboratory activities will reinforce the lecture material.
3. Any required prerequisites: None
4. Required grade for enrolling in the next course in this sequence: Need a C or higher in CHEM 1405 in order to take CHEM 1407
Student Learning Outcomes:
1. Lecture
  1. Define the fundamental properties of matter.
  2. Classify matter, compounds, and chemical reactions.
  3. Determine the basic nuclear and electronic structure of atoms.
  4. Identify trends in chemical and physical properties of the elements using the Periodic Table.
  5. Describe the bonding in and the shape of simple molecules and ions.
  6. Solve stoichiometric problems.
  7. Write chemical formulas.
  8. Write and balance equations.
  9. Use the rules of nomenclature to name chemical compounds.
  10. Define the types and characteristics of chemical reactions.
  11. Use the gas laws and basics of the Kinetic Molecular Theory to solve gas problems.
  12. Determine the role of energy in physical changes and chemical reactions.
  13. Convert units of measure and demonstrate dimensional analysis skills.
2. Lab
  1. Use basic apparatus and apply experimental methodologies used in the chemistry laboratory.
  2. Demonstrate safe and proper handling of laboratory equipment and chemicals.
  3. Conduct basic laboratory experiments with proper laboratory techniques.
  4. Make careful and accurate experimental observations.
  5. Relate physical observations and measurements to theoretical principles.
  6. Interpret laboratory results and experimental data, and reach logical conclusions.
  7. Record experimental work completely and accurately in laboratory notebooks and communicate experimental results clearly in written reports.
  8. Design fundamental experiments involving principles of chemistry.
  9. Identify appropriate sources of information for conduction laboratory experiments involving principles of chemistry.
Testing Requirements
1. Campus
  1. Students are not allowed to use their book or notes of any kind while taking their proctored tests and exams. A periodic table will be provided.
  2. Students are allowed to use a calculator.
2. Online
  1. The midterm and final exam must be proctored by an approved testing organization. (Ask your instructor for more details.)
  2. Students are not allowed to use their book or notes of any kind while taking their proctored tests and exams. A periodic table will be provided.
  3. Students are allowed to use a calculator.
Course Requirements
1. Campus/Online
  1. Lecture: homework assignments; weekly quizzes; midterm and final exam
  2. Lab: lab reports; final exam
  3. Quizzes and exams are timed.
Information on Books and Other Course Materials
1. Required Book: Introductory Chemistry w/Mastering Chemistry, 6th Edition. Tro. 2018. Pearson Prentice Hall. (ISBN:) 9780134290812
2. Required Access Code: MasteringChemistry access code is bundled with book.
3. Required Lab Book (ON-CAMPUS ONLY): Laboratory Manual for Introductory Chemistry: Concepts and Critical Thinking, 6th Edition. Charles H. Corwin, American River College. 2013. Pearson (ISBN: 9780321750945)
4. Required Lab Kit (ONLINE ONLY): Intro Chemistry Custom Lab Kit. Hands On Learning. (SKU: Kit LP-2820-CK-01) (ISBN: 2818560391975)
5. Calculators: scientific calculator
Grading Breakdown:
1. Campus/Online
  Lecture Homework                 10%
  Lecture Quizzes                      10%
  Lecture Midterm                      25%
  Lecture Final Exam                 25%
  Lab Reports                             15%
  Lab Final Exam                       15%
2. A final semester grade will be based as follows:
  A = 89.5% and above
  B = 79.5 – 89.49
  C = 69.5 – 79.49
  D = 59.5 – 69.49
  F = 59.49% and below
  I = Incomplete (failure to complete the requirements of the course)
Other Policies, Procedures and important dates. Please refer to the WTC Catalog for the following:
1. Campus Calendar
2. Final exam schedule
3. How to drop a class
4. Withdrawal information
5. Student Conduct/Academic Integrity
6. Students with disabilities
Course Content

Chapter 1: The Chemical World	1.1 Sand and Water 1.2 Chemicals Compose Ordinary Things 1.3 The Scientific Method: How Chemists Think 1.4 Analyzing and Interpreting Data 1.5 A Beginning Chemist: How to Succeed
Chapter 2: Measurement and Problem Solving	2.1 he Metric Mix-Up: A $125 Million Unit Error 2.2 Scientific Notation: Writing Large and Small Numbers 2.3 Significant Figures: Writing Numbers to Reflect Precision 2.4 Significant Figures in Calculations 2.5 The Basic Units of Measurement 2.6 Problem Solving and Unit Conversion 2.7 Solving Multistep Unit Conversion Problems 2.8 Unit Conversion in Both the Numerator and Denominator 2.9 Density 2.10 Numerical Problem-Solving Strategies and the Solution map
Chapter 3: Matter and Energy	3.1 In Your Room 3.2 What is Matter? 3.3 Classifying Matter According to Its State: Solid, Liquid, and Gas 3.4 Classifying Matter According to Its Composition: Elements, Compounds, and Mixtures 3.5 Differences in Matter: Physical and Chemical Properties 3.6 Changes in Matter: Physical and Chemical Changes 3.7 Conservation of Mass: There is No New Matter 3.8 Energy 3.9 Energy and Chemical and Physical Change 3.10 Temperature: Random Motion of Molecules and Atoms 3.11 Temperature Changes: Heat Capacity 3.12 Energy and Heat Capacity Calculations
Chapter 4: Atoms and Elements	4.1 Experiencing Atoms at Tiburon 4.2 Indivisible: The Atomic Theory 4.3 The Nuclear Atom 4.4 The Properties of Protons, Neutrons, and Electrons 4.5 Elements: Defined by Their Numbers of Protons 4.6 Looking for Patterns: The Periodic Law and the Periodic Table 4.7 Ions: Losing and Gaining Electrons 4.8 Isotopes: When the number of Neutrons Varies 4.9 Atomic Mass: The Average Mass of an Element’s Atoms
Chapter 5: Molecules and Compounds	5.1 Sugar and Salt 5.2 Compounds Display Constant Composition 5.3 Chemical Formulas: How to Represent Compounds 5.4 A Molecular View of Elements and Compounds 5.5 Writing Formulas for Ionic Compounds 5.6 Nomenclature: Naming Compounds 5.7 Naming Ionic Compounds 5.8 Naming Molecular Compounds 5.9 Naming Acids 5.10 Nomenclature Summary 5.11 Formula Mass: The Mass of a Molecule or Formula Unit
Chapter 6: Chemical Composition	6.1 How Much Sodium? 6.2 Counting Nails by the Pound 6.3 Counting Atoms by the Gram 6.4 Counting Molecules by the Gram 6.5 Chemical Formulas as Conversion Factors 6.6 Mass Percent Composition of Compounds 6.7 Mass Percent Composition from a Chemical Formula 6.8 Calculating Empirical Formulas for Compounds 6.9 Calculating Molecular Formulas for Compounds
Chapter 7: Chemical Reactions	7.1 Grade School Volcanoes, Automobiles, and Laundry Detergents 7.2 Evidence of a Chemical Reaction 7.3 The Chemical Equation 7.4 How to Write Balanced Chemical Equations 7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water 7.6 Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid 7.7 Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations 7.8 Acid-Base and Gas Evolution Reactions 7.9 Oxidation-Reduction Reactions 7.10 Classifying Chemical Reactions
Chapter 8: Quantities in Chemical Reactions	8.1 Climate Change: Too Much Carbon Dioxide 8.2 Making Pancakes: Relationships between Ingredients 8.3 Making Molecules: Mole-to-Mole Conversions 8.4 Making Molecules: Mass-to-Mass Conversions 8.5 More Pancakes: limiting Reactant, Theoretical Yield, and Percent Yield 8.6 Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants 8.7 Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
Chapter 9: Electrons in Atoms and the Periodic Table	9.1 Blimps, Balloons, and Models of the Atom 9.2 Light: Electromagnetic Radiation 9.3 The Electromagnetic Spectrum 9.4 The Bohr Model: Atoms with Orbits 9.5 The Quantum-Mechanical Model: Atoms with Orbitals 9.6 Quantum-Mechanical Orbitals and Electron Configurations 9.7 Electron Configurations and the Periodic Table 9.8 The Explanatory Power of the Quantum-Mechanical Model 9.9 Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
Chapter 10: Chemical Bonding	10.1 Bonding Models and AIDS Drugs 10.2 Representing Valence Electrons with Dots 10.3 Lewis Structures of Ionic Compounds: Electrons Transferred 10.4 Covalent Lewis Structures: Electrons Shared 10.5 Writing Lewis Structures for Covalent Compounds 10.6 Resonance: Equivalent Lewis Structures for the Same Molecule 10.7 Predicting the Shapes of Molecules 10.8 Electronegativity and Polarity: Why Oil and Water Don’t Mix
Chapter 11: Gases	11.1 Extra-Long Straws 11.2 Kinetic Molecular Theory: A Model for Gases 11.3 Pressure: The Result of Constant Molecular Collisions 11.4 Boyle’s Law: Pressure and Volume 11.5 Charles’s Law: Volume and Temperature 11.6 The Combined Gas Law: Pressure, Volume, and Temperature 11.7 Avogadro’s Law: Volume and Moles 11.8 The Ideal Gas Law: Pressure, Volume, Temperature, and Moles 11.9 Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen 11.10 Gases in Chemical Reactions

Last Modified: August 25, 2017