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CHM 110 General Chemistry

This course is designed for students majoring in technical areas other than chemistry. Topics include the metric system, structure of matter, nomenclature, reactions, gases, rates and equilibrium, solutions, acids, bases, and nuclear chemistry. Laboratory experiments are used to illustrate theory.

Credits

4

Prerequisite

Prerequisite: SSC 100 or concurrent

See Course Syllabus

Course Number and Title:

CHM 110 General Chemistry

Campus Location

  • Georgetown

Prerequisites

Prerequisite: SSC 100 or concurrent

Course Credits and Hours

4 credit(s)

3 lecture hours/week

2 lab hours/week

Course Description

This course is designed for students majoring in technical areas other than chemistry. Topics include the metric system, structure of matter, nomenclature, reactions, gases, rates and equilibrium, solutions, acids, bases, and nuclear chemistry. Laboratory experiments are used to illustrate theory.

Required Text(s)

Obtain current textbook information by viewing the campus bookstore - https://www.dtcc.edu/bookstores online or visit a campus bookstore. Check your course schedule for the course number and section.

Core Course Performance Objectives (CCPOs)

  1. Convert between English and International System (SI) of measurements. (CCC 2,6)
  2. Describe the structure of matter at the atomic and molecular level. (CCC 1, 2, 6)
  3. Describe types of chemical reactions and balance equations. (CCC 1, 2, 6)
  4. Contrast the properties of gases, liquids, solids, and solutions. (CCC 1, 2, 6)
  5. Perform stoichiometric and gas law calculations. (CCC 2, 6)
  6. Describe acids, bases, and buffers, and perform calculations used to evaluate them. (CCC 1, 2, 6)
  7. Describe simple organic compounds, including names, structures, formulas, and example reactions. (CCC 1, 2, 6)
  8. Discuss nuclear radiation, including nomenclature. (CCC 2, 6)
  9. Perform and analyze various laboratory activities related to chemistry. (CCC 1, 2, 3, 4, 5, 6)

See Core Curriculum Competencies and Program Graduate Competencies at the end of the syllabus. CCPOs are linked to every competency they develop.

Measurable Performance Objectives (MPOs)

Upon completion of this course, the student will:

  1. Convert between English and International System (SI) of measurements.
    1. Interpret scientific notation and prefixes for units of measure, and convert numbers to and from scientific notation.
    2. Name the abbreviations and the metric base units and SI units for mass, length, volume, time, and temperature.
    3. Convert physical quantities from one unit to another using conversion factors.
    4. Interpret the number of significant figures in a physical quantity, and round off numbers in calculations involving physical quantities.
    5. Define density and specific gravity, and use these quantities in calculations.
    6. Differentiate between potential and kinetic energy.
    7. Convert between temperatures scales.
    8. Define specific heat, and use it to calculate heat changes.
    9. Distinguish among the calorie, kilocalorie, Calorie, and joule.
    10. Use the factor-label method in problem analysis and estimation techniques in solving problems.
  2. Describe the structure of matter at the atomic and molecular level.
    1. Define matter, energy, and chemistry.
    2. Distinguish between physical and chemical changes.
    3. Describe the scientific method of investigation.
    4. Define and distinguish pure substances, elements, compounds, and mixtures.
    5. Name and give the symbols for selected elements.
    6. Name the major principles of modern atomic theory.
    7. Name the elements that exist as diatomic molecules.
    8. Name the three subatomic particles, and state their symbols, relative masses, charges, and location.
    9. Explain the composition of different atoms in terms of the number of protons, neutrons, and electrons.
    10. Identify isotopes of an element from their atomic composition.
    11. Define atomic number, mass number, and atomic weight, and distinguish among them.
    12. Describe the arrangement of elements in the periodic table; define periodicity, and give examples.
    13. Define period, group, metal, metalloid, nonmetal, alkali metal, alkaline earth metal, halogen, and noble gas, and distinguish among them.
    14. Describe the arrangement of electrons within shells and subshells of an atom, and write the electron configuration of an atom.
    15. Relate the position of an element in the periodic table to its electronic structure.
    16. Describe the relationship between atomic energy and electronic arrangement.
    17. Describe the relationship between absorption and release of energy by an electron and changes in energy level.
    18. Describe the octet rule, and discuss its significance.
    19. Draw electron dot structures for the first 20 elements.
    20. Define ion, cation, and anion.
    21. Write the symbols and names of the ions formed by elements in Groups 1A-8A.
    22. Define ionic bonding and covalent bonding, and distinguish between them.
    23. Define electronegativity, and describe the trends in electronegativity within periods and groups of the periodic table.
    24. Name and write formulas for ionic compounds.
    25. Discuss the properties of ionic compounds.
    26. Recognize and distinguish single, double, and triple covalent bonds.
    27. Predict the numbers of covalent bonds normally formed by the more common main group elements.
    28. Name and write formulas for molecular compounds.
    29. Discuss the properties of molecular compounds.
    30. Given two elements that are bonded and their electronegativities, determine whether the bond is ionic, polar covalent, or nonpolar covalent.
    31. Indicate the polarity of polar bonds with partial charge notation: δ+, δ-.
    32. Interpret molecular formulas, structural formulas, and Lewis structures.
    33. Draw Lewis structures and use valence shell electron pair repulsion (VSEPR) theory to predict molecular geometry.
    34. Use electronegativity and molecular geometry to predict bond and molecular polarity.
    35. Describe the differences in structure, composition, and properties of ionic and molecular compounds.
  3. Describe types of chemical reactions and balance equations.
    1. Explain the meaning and uses of the mole and Avogadro's number.
    2. Balance a chemical equation.
    3. Translate a written description of a chemical reaction into a balanced chemical equation and vice versa.
    4. Classify different types of reactions.
    5. Write the net ionic equation for a given reaction.
    6. Recognize and distinguish oxidation and reduction.
    7. Define heat of reaction.
    8. Define and distinguish between endothermic and exothermic processes.
    9. Describe how collisions and activation energy determine reaction rate.
    10. Predict the effects of changes in conditions on reaction rates.
    11. Interpret a reaction energy diagram.
    12. Describe the effect of a catalyst on a reaction.
    13. Describe what is occurring in a reaction that is at equilibrium.
    14. Write and use equilibrium constant expressions.
    15. Relate the magnitude of the equilibrium constant to the equilibrium position of a reaction.
    16. Use Le Chatelier's principle to predict the effect of changes in conditions on an equilibrium system.
  4. Contrast the properties of gases, liquids, solids, and solutions.
    1. Distinguish solids, liquids, and gases.
    2. Name and define the common units of pressure.
    3. State the assumptions of the kinetic theory of gases, and use them to explain gas behavior.
    4. Define and distinguish the principal intermolecular forces: hydrogen bond, dipole-dipole interaction, and London dispersion forces.
    5. Discuss the significance of hydrogen bonding.
    6. Describe the properties of liquids.
    7. Describe the relations among vapor pressure, temperature, and boiling point.
    8. Describe the characteristics and classification of solids.
    9. Apply the concepts of heat exchange, equilibrium, and vapor pressure to phase changes (changes of state).
    10. Perform calculations with heat of fusion and heat of vaporization.
    11. Describe the properties of solutions, and distinguish them from other mixtures.
    12. Explain how the nature of solute and solvent affect solubility.
    13. Describe the influence of temperature and pressure on solubility.
    14. Describe the process of solvation by water.
    15. Define and distinguish strong, weak, and nonelectrolytes.
    16. Define solution, suspension, and colloid, and distinguish among them.
    17. Define diffusion, osmosis, and dialysis, and distinguish among them.
    18. Define osmotic pressure, and discuss its significance.
  5. Perform stoichiometric and gas laws calculations.
    1. Given the formula of a compound, calculate its formula weight.
    2. Convert between molar and mass quantities of any element or compound.
    3. Perform mole and mass calculations using chemical equations.
    4. Define percentage yield for a reaction.
    5. State important gas laws and use them in calculations.
    6. Define partial pressure, and use Dalton's law of partial pressures.
    7. Define concentration.
    8. Define, use, and convert between percent concentration and molarity.
    9. State the result of a dilution, and explain how to make a desired dilution.
    10. Define and calculate the osmolarity of a solution.
  6. Describe acids, bases, and buffers, and perform calculations used to evaluate them.
    1. Describe the properties of acids, bases, and salts.
    2. Write the names and formulas for common acids and bases.
    3. Define and distinguish strong and weak acids and bases in terms of their electrolyte character.
    4. Define conjugate acid-base pairs, and determine the conjugate of a given acid or base.
    5. Discuss acid-base ionization constants.
    6. Write equations for neutralization reactions.
    7. Describe the amphiprotic behavior of water.
    8. Write the equation and equilibrium constant expression for the ionization of water.
    9. Define pH, and perform calculations with pH.
    10. Describe techniques used for measuring pH.
    11. Describe a titration experiment, and perform titration calculations.
    12. Describe the composition and action of buffer solutions.
    13. Describe the relationship between buffer composition and buffer pH.
  7. Describe simple organic compounds, including names, structures, formulas, and example reactions.
    1. Explain the significance of carbon compounds.
    2. Identify the principal functional group families of organic compounds.
    3. Draw structural formulas for and name important organic compounds.
    4. Compare the properties and reactions of organic and inorganic compounds.
    5. Describe the applications of organic compounds.
    6. Name and distinguish the principal types of biomolecules.
    7. Describe the structure of the major biomolecules.
  8. Discuss nuclear radiation, including nomenclature.
    1. Define radioactivity and the terms used to describe it.
    2. Describe the relationship between the energy of radiation and its frequency and wavelength.
    3. List the characteristics of alpha, beta, and gamma radiation.
    4. Describe the processes of alpha, beta, positron, and gamma emission.
    5. Define half-life, and perform decay calculations.
    6. Define ionizing radiation, and describe its properties and measurement.
    7. Describe the important factors in protection from radiation.
    8. Name and define common units for measuring radiation.
    9. Discuss nuclear fission and fusion.
  9. Perform and analyze various laboratory activities related to chemistry.
    1. Accurately measure length, volume, mass, density, and temperature of common materials using standard laboratory apparatus.
    2. Perform mathematical conversions with correct application of significant figures.
    3. Safely and accurately follow written and oral experimental instructions to obtain valid qualitative and quantitative data.
    4. Make accurate observations of physical and chemical changes, and record those observations in written forms.
    5. Recognize and report unusual or unexpected results when accurately following a written experimental procedure.
    6. Work effectively with a laboratory partner or as part of a small group.
    7. Observe and adhere to accepted good laboratory practices (GLP) for working safely in a laboratory.

Evaluation Criteria/Policies

The grade will be determined using the Delaware Tech grading system:

90-100 = A
80-89 = B
70-79 = C
0-69 = F
Students should refer to the Catalog/Student Handbook for information on the Academic Standing Policy, the Academic Integrity Policy, Student Rights and Responsibilities, and other policies relevant to their academic progress.

Core Curriculum Competencies (CCCs are the competencies every graduate will develop)

  1. Apply clear and effective communication skills.
  2. Use critical thinking to solve problems.
  3. Collaborate to achieve a common goal.
  4. Demonstrate professional and ethical conduct.
  5. Use information literacy for effective vocational and/or academic research.
  6. Apply quantitative reasoning and/or scientific inquiry to solve practical problems.

Students in Need of Accommodations Due to a Disability

We value all individuals and provide an inclusive environment that fosters equity and student success. The College is committed to providing reasonable accommodations for students with disabilities. Students are encouraged to schedule an appointment with the campus Disabilities Support Counselor to request an accommodation needed due to a disability. The College's policy on accommodations for persons with disabilities can be found in the College's Guide to Requesting Academic Accommodations and/or Auxiliary Aids Students may also access the Guide and contact information for Disabilities Support Counselors through the Student Resources web page under Disabilities Support Services, or visit the campus Advising Center.

Minimum Technology Requirements

Minimum technology requirements for online, hybrid, video conferencing and web conferencing courses.

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Tuition Adjustment Policy

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