CHEM 1405, CHEM 1405L

Introductory Chemistry I

CHEM 1405; CHEM 1405L

Updated August 24, 2012

  • State Approval Code: 4005015103
  • Semester Credit Hours: 4
  • Lecture Hours per Week: 3
  • Lab Hours per Week: 3
  • Contact Hours per Semester: 90

Catalog Description

An introductory course in inorganic chemistry that relates the
principles and concepts of chemistry to man and his environment. This course is a
basic introduction to chemistry, with chemical calculations, making it appropriate for
health science students. (Lab Fee)

Course Curriculum

Basic Intellectual Compentencies in the Core Curriculum

  • Reading
  • Writing
  • Speaking
  • Listening
  • Critical thinking
  • Computer literacy

Perspectives in the Core Curriculum

  • Establish broad and multiple perspectives on the individual in relationship to the larger society and world in which he/she lives, and to understand the responsibilities of living in a culturally and ethnically diversified world.
  • Stimulate a capacity to discuss and reflect upon individual, political, economic, and social aspects of life in order to understand ways in which to be a responsible member of society.
  • Recognize the importance of maintaining health and wellness.
  • Develop a capacity to use knowledge of how technology and science affect their lives.
  • Develop the ability to make aesthetic judgments.
  • Use logical reasoning in problem solving.
  • Integrate knowledge and understand the interrelationships of the scholarly disciplines.

Core Components and Related Exemplary Educational Objectives

Mathematics

  • To apply arithmetic, algebraic, geometric, higher-order thinking, and statistical methods to modeling and solving real-world situations.
  • To represent and evaluate basic mathematical information verbally, numerically, graphically, and symbolically.
  • To expand mathematical reasoning skills and formal logic to develop convincing mathematical arguments.
  • To use appropriate technology to enhance mathematical thinking and understanding and to solve mathematical problems and judge the reasonableness of the results.
  • To interpret mathematical models such as formulas, graphs, tables and schematics, and draw inferences from them.
  • To recognize the limitations of mathematical and statistical models.
  • To develop the view that mathematics is an evolving discipline, interrelated with human culture, and understand its connections to other disciplines.

Natural Sciences

  • To understand and apply method and appropriate technology to the study of natural sciences.
  • To recognize scientific and quantitative methods and the differences between these approaches and other methods of inquiry and to communicate findings, analyses, and interpretation both orally and in writing.
  • To identify and recognize the differences among competing scientific theories.
  • To demonstrate knowledge of the major issues and problems facing modern science, including issues that touch upon ethics, values, and public policies.
  • To demonstrate knowledge of the interdependence of science and technology and their influence on, and contribution to, modern culture.

Instructional Goals and Purposes

Panola College's instructional goals include 1) creating an academic atmosphere in which students may develop their intellects and skills and 2) providing courses so students may receive a certificate/an associate degree or transfer to a senior institution that offers baccalaureate degrees.

General Course Objectives

1. Understand and be able to explain the general principles, laws, and theories of chemistry that are discussed and presented throughout the semester
2. Use critical thinking and logic in the solution of problems
3. Apply learned chemistry skills to new situations
4. Demonstrate an understanding of chemistry through technological advancement
5. Apply chemical principles in the laboratory setting
6. Develop independent and cooperative learning skills
7. Recognize and acquire attitudes that are characteristic of the successful worker regardless of the major field of study
8. Develop an awareness of the value of chemistry in our daily living

Specific Course Objectives

1. Describe and demonstrate the scientific method.
2. Describe and demonstrate good laboratory behavior.
3. Describe the safety criteria and safety features of your lab.
4. Identify from the lab drawer any specific item of glassware and its proper use and function.
5. Describe the proper use of an analytical balance.
6. Define and distinguish between the terms precision, uncertainty, and accuracy.
7. Make and record measurements to the proper instrument precision.
Determine correct number of significant figures
Adjust calculated answers to correct number of significant figures
8. Give the metric units for mass, length, and volume.
9. Perform American to metric conversion equivalents for mass, length, and volume. Write conversion factors
10. Give the exponential numerical equivalents for the metric prefixes: nano, micro, milli, centi, deci, deca, hecta, kilo, and mega
11. Distinguish between mass and weight.
12. Distinguish between heat and temperature.
13. Use the unit analysis(factor-label) method in good written form to perform conversion calculations.
Density problems % problems
14. Define, distinguish, and correctly classify examples of:
a. Physical and chemical properties of matter
b. pure substances,elements, compounds, and mixtures
c. metals, nonmetals, and metalloids
d. solid, liquid, and gaseous phases of matter
e. atoms, ions, and molecules
f. homogeneous and heterogeneous materials
15. Write the names and symbols for common chemical elements. See list.
16. Give the correct symbols for the seven common elements that exist as diatomic molecules.
17. Identify the purpose and broad organization of the chemical periodic table.
18. Write the symbols for the common monoatomic ions, recognizing the ion charge from the periodic chart.
19. Identify energy as kinetic or potential.
Explain and use the formula E = m x sp.ht. x Dt. Clearly define the quantity represented by each symbol and the proper units of measurement for the quantity. Use the formula to compute information from a calorimetry experiment.
Perform temperature conversions Use energy to calculate nutrition values
Know and describe the six phase changes, melting point, freezing point
Perform calculations using heat of fusion and heat of vaporization
20. Write a thorough description of the development of thought shaping early theory of atomic structure.
21. Describe the present day simple electron-proton-neutron model for a manyelectron atom.
22. Explain how an atom acquires a net charge to become an ion.
23. Define: isotope, atomic number, atomic mass (weight), and atomic mass unit.
24. Give the name, symbol, and charge for some common polyatomic ions. See list.
25. Write the correct formulas for all compounds, given the names; write the correct names for compounds, given the formulas.
26. Define and distinguish between:
a. Binary and ternary compounds
b. common and systematic chemical names
27. Describe the energy level nature for the electrons in many-electron atoms.
28. Describe the historical discovery of electron energy levels and give an overview of the theoretical development, Define atomic orbital.
29. Write electron configurations (spdf) for the first twenty elements of the periodic chart.
30. Relate the electron configurations of elements to their position in the periodic chart (row and column).
31. Draw Lewis dot diagrams for representative elements.
32. Define ionization potential, electron affinity, and electronegativity.
Use electronegativity to determine polarity
33. Describe the periodic trends in the properties of elements in the periodic chart.
34. Define and give examples of ionic and covalent bonds. Identify compounds as ionic or covalent.
35. Draw Lewis structures for simple molecules.
Predict three dimensional shape of molecules
Describe attractive forces between ions, polar molecules and nonpolar molecules
36. Define: atomic mass, formula mass, molar mass, empirical formula molecular formula, Avogadro’s number.
37. Given the formula for a substance, determine its percent composition by mass for each element in the formula.
38. Given the composition of a pure substance by mass or percent weight, determine its empirical formula.
39. Given the empirical formula and the molecular weight, determine the molecular formula for a given compound.
40. Use the unit analysis method to convert between grams, molecules, atoms, and moles of a substance.
41. Describe what a “chemical equation” is and explain why it is an important tool in the study of chemistry.
42. Explain what we mean by each of the following: reactants, products, coefficients, balanced equation, word equation, skeleton equation.
43. Name and describe four types of chemical reactions.
Write balanced chemical equations
44. Explain what is meant by a “combustion reaction”. Explain why we say that hydrogen is combustible but will not support combustion. Cite experimental evidence.
45. Calculate related amounts in chemical reactions from balanced chemical equations
a. Given reactant moles, find product mass or moles.
b. Given reactant mass, find product mass or moles.
c. Given one reactant or product amount, find related reactant or product amount.
d. Given two or more reactant amounts, determine and correctly use limiting reactant information.
e.Given percent yield, determine related reactant or product amount.
46. State and solve problems using Boyle's Law, Charles Law, Guy-Lussac's Law, Avogadro’s Law and the Combined Gas Law. 47. State and apply Graham's Law for rates of diffusion.
48. State and apply Dalton's Law of Partial Pressures.
49. State and solve problems using the Ideal Gas Law
50. Recognize the values for STP and molar volume at STP.
51. Solve stoichiometry problems involving gas volumes.
52. Compare ideal gases and real gases.
53. Using the Kinetic Molecular Theory distinguish among gases, liquids, and solids.
54. Define: evaporation, vapor pressure, surface tension, boiling point, freezing point, and melting point.
55. Describe the importance of hydrogen bonding.
56. Distinguish between hygroscopic, deliquescent, and efflorescent substances.
57. List important sources of air and water pollution.
58. Describe the operation of a typical municipal water purification system.
59. Define solubility and describe the solvation process; define saturated and unsaturated.
60. Define molarity; solve problems computing moles, mass, and concentrations of solutions.
61. Solve stoichiometry problems for reacting solutions.
62. Define equivalence and normality; be able to relate molarities and normalities.
63. Given appropriate constants, calculate boiling and freezing point changes due to colligative properties.
64. Define acids and bases. Give typical reactions, especially neutralization reactions.
65. Describe the titration process.
66. Given concentration of acids or bases, calculate the pH and the pOH.
67. Distinguish between spontaneous and nonspontaneous reactions.
68. Use the collision theory to explain how the rate of a chemical reaction is influenced by temperature, catalyst, concentration, and particle size of reactants.
69. Define chemical equilibrium in terms of a reversible reaction and predict the equilibrium position of a reaction from a given Keq value.
70. State LeChatelier's principle and use it to predict changes in the equilibrium position due to changes in concentration and temperature.
71. Describe how buffer solutions control pH in biological systems.
72. Define oxidation and reduction reactions; describe an oxidizing agent and a reducing agent.
73. Predict reactivity of ionic compounds by comparing metal cations' activity .
74. Balance redox equations.
75. Describe alpha, beta, and gamma radiation.
Write equations showing mass number and atomic numbers for radioactive decay
Describe detection and measurement of radiation
Perform half-life calculations
76. Differentiate between fission and fusion.
77. Describe the biological effects of radioactive substances.
Describe the use of radioisotopes in medicine

General Description of Each Lecture or Discussion

Students will be required to participate in and complete the following:
1. Students will participate in lecture activities including discussions, quizzes and in class assignments
2. Students will turn in assigned homework problems and questions
3. Students may participate in optional cooperative learning groups
4. Students will participate in laboratory experiments and turn in laboratory reports
5. Students will complete four unit exams and one comprehensive final exam
6. Students will participate in a service learning project

Methods of Instruction/Course Format/Delivery

Lecture, class discussion, lecture activities, chapter reading, homework problem assignments and laboratory experimentation and reports

Assessment

The following components will be used to calculate a final grade for each student:
1. Homework - for the course will consist mainly of problems and questions from the text. Homework will be completed and turned in using an online system called Sapling Learning. This online access pass MUST be purchased separately online. This system is separate from Canvas.

For homework to be most useful in preparing for in class work and exams, it must be submitted by the date due. Late work is not accepted.

2. Lecture Activities – are exercises performed in class as a participation in the lesson, quizzes and optional participation in chemistry seminars. No late or makeup work will be accepted for lecture activities except in the case of student participation in a Panola College student activity that has been approved by the college.
Study Groups - are recommended to encourage peer tutoring and cooperative learning. Groups will form by student choice and meet at times chosen by the group. Reports of study group activity will be turned in to me once a month for extra credit in the lecture activities grade portion.


3. Laboratory Experiments – Laboratory experiments will be performed in order to apply the general principles, laws and theories of chemistry learned during lecture. Experimental results will be recorded and submitted on the forms found
in the lab manual. Lab expectations will be discussed in the laboratory orientation by your lab instructor. Course information states additional rules and expectations that must be followed and the consequences that will result.

The grade of 100 possible points for each laboratory experiment is broken down as follows:

  1. 10 points for showing up on time with the pre-lab assignment complete and an up to date MSDS notebook containing all required safety information. This is your ticket in the door and you will not begin an experiment without it.
  2. 40 points for conducting the experiment, adhering to all safety and equipment use rules, completing the experiment, cleaning up your lab station, and disposing of all waste, trash according to instructions given. All of these items must be complete before leaving lab.
  3. 50 points for the report sheet you turn in. It must be complete, legible, and information must be properly presented and clearly explained when necessary. All work must be shown when necessary.

4. Unit Exams – Four unit exams are given throughout the semester that are worth 100 points each. Each written exam will be given during a regular lecture class period. No one coming in late may start an exam after the first person has left and extra time will not be given. One unit exam may be made up at the end of the semester at a time designated by the instructor. The make up exam is comprehensive and all essay/problems.  Online students will take proctored written exams at one of the three testing centers offered by Panola College. 
A tentative schedule for unit exams is as follows (see the lecture schedule for dates):
Unit I Chapters 1, 2
Unit II Chapters 3, 4, 5
Unit III Chapters 6, 7
Unit IV Chapters 8, 9, 10


5. Final Exam – is also comprehensive and will be administered according to the posted final exam schedule in December. No one coming in late may start a final exam after the first person has left. Anyone late for the final will not be allowed any additional time to complete it.


6. Attendance – is expected at all lectures and labs. Class attendance is monitored and recorded. See the handbook for rules concerning allowed absences.  If the role sheet has already been turned into me, you are absent.  Tardies disrupt instruction and need to be avoided to the best of your ability.

Mandatory Project:

Each student will complete the following project during the semester:

Participate in a service learning project by volunteering for 4 hours in an area that can be related to chemistry. (Everything relates to chemistry.) You are responsible for finding the place of service, but help will be provided and you will be in contact with me and the chosen mentor to determine your role.

  1. All volunteer work must be approved in advance by me. More information will be provided in the next couple of weeks.
  2. You will serve in whatever capacity they need you.
  3. You will write a reflection paper about the experience to turn in to me.
  4. All volunteer work, reflections and presentations must be completed by the due date.

Additional instructions and due dates will be provided at a later time. This project is worth 250 points and is a part of your laboratory grade.

I reserve the right to make any changes to this syllabus according to what is deemed best for student learning and success in CHEM 1405.

My Philosophy:
I believe chemistry is a core discipline essential to a college education regardless of major or career choice. Recognizing a broad range of interests, preparations, and future needs among chemistry students, this course is designed to allow each student
to individually select topics for various assignments in order to further develop possible career choices. Every attempt on my part is made to ensure your area of interest is discussed. Please let me know if there is a topic that particularly interests you. Organization is a key to success in this course. I highly recommend a notebook or three ring binder to keep up with all assignments, quizzes, homework and exams. For example, if there is a problem with the homework system and you can show me your work, I am able to give you credit.

Canvas:
This course is available on Canvas and will contain useful information like conversion charts and formulas, specific course objectives by chapter for test review, assignments, laboratory experiments, copies of handouts, tutorial sites and ACS
information.

Letter grades are as follows:
A 90 - 100
B 80 - 89
C 70 - 79
D 60 - 69
F Below 60
The final grade will be determined as follows:
1. Homework and Quizzes 20%
2. Labs 25%
3. Unit Exams 40%
4. Final Exam 15%

Text, Required Readings, Materials, and Supplies

1. General, Organic, and Biological Chemistry 4th ed. By Karen Timberlake. (The Panola College Bookstore offers a condensed version designed for this course)

2. Introduction to Chemistry in the Laboratory. Amy Calhoun

3. Scientific calculator (does NOT need to be graphing)

4. OPTIONAL- Study guide: A Visual Analogy Guide to Chemistry

Helpful Links