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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

  • Dover
  • Georgetown
  • Wilmington
  • Stanton

Effective Date

202351

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.

Additional Materials

None 

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.

Disclaimer

None 

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. Interpret the number of significant figures in a physical quantity, and round off numbers in calculations involving physical quantities.

  4. Define density and specific gravity, and use these quantities in calculations.

  5. Convert between temperature scales.

  6. Distinguish among the calorie, kilocalorie, Calorie, and joule.

  7. Define specific heat, and use it to calculate heat changes.

  8. Use the factor-label method for problem-solving.

  1. Describe the structure of matter at the atomic and molecular level.

    1. Define matter, energy, and chemistry.

    2. Differentiate between potential and kinetic energy.

    3. Distinguish between physical and chemical changes.

    4. Describe the scientific method of investigation.

    5. Define and distinguish pure substances, elements, compounds, and mixtures.

    6. Name and give the symbols for selected elements.

    7. Name the major principles of modern atomic theory.

    8. Name the elements that exist as diatomic molecules.

    9. Describe the structure of the atom and the characteristics of the subatomic particles. 

    10. Define atomic number, mass number, atomic weight, and isotopes.

    11. Describe the arrangement of elements in the periodic table; define periodicity, and give examples.

    12. Define electronegativity, and describe the trends in electronegativity within periods and groups of the periodic table.

    13. Describe electron configuration, and its relationship to the periodic table.

    14. Describe the relationship between absorption and release of energy by an electron and changes in energy level.

    15. Describe the octet rule, and draw electron dot structures for the first 20 elements.

    16. Write the symbols and names of the cations and anions formed by elements in Groups 1A-8A.

    17. Define ionic and covalent bonds and discuss the properties of ionic compounds and molecular compounds.

    18. Name and write the formulas for ionic and covalent compounds. 

    19. Recognize and distinguish single, double, and triple covalent bonds.

    20. Determine whether bonds are ionic, polar covalent, or nonpolar covalent.

    21. Differentiate molecular and structural formulas, draw Lewis structures, and use VSEPR theory to predict molecular geometry.

    22. Use electronegativity and molecular geometry to predict bond and molecular polarity.

  2. Describe types of chemical reactions and balance equations.

    1. Explain the meaning and uses of the mole and Avogadro’s number.

    2. Translate a written description of a chemical reaction into a balanced chemical equation and vice versa.

    3. Classify different types of reactions.

    4. Write the net ionic equation for a given reaction.

    5. Differentiate between oxidation and reduction.

    6. Define heat of reaction.

    7. Differentiate between endothermic and exothermic processes.

    8. Describe the factors that affect activation energy, and reaction rates.

    9. Interpret a reaction energy diagram.

    10. Define equilibrium, write and use equilibrium constant expressions.

    11. Use Le Chatelier’s principle to predict changes of a system at equilibrium.

  3. Contrast the properties of gases, liquids, solids, and solutions.

    1. Describe the characteristics and properties of 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. Explain how vapor pressure, temperature, and boiling point relate to liquids.

    6. Apply the concepts of heat exchange, equilibrium, and vapor pressure to phase changes (changes of state).

    7. Perform calculations with heat of fusion and heat of vaporization.

    8. Differentiate between a solution, suspension, and colloid.

    9. Explain how temperature, pressure and the properties of a solute and solvent affect solubility.

    10. Define and distinguish strong, weak, and nonelectrolytes.

    11. Define diffusion, osmosis, dialysis, and osmotic pressure.

  4. Perform stoichiometric and gas laws calculations.

  1. Given the formula of a substance, determine its molar mass.

  2. Perform mole and mass calculations using chemical equations.

  3. Define and calculate percentage yield for a reaction.

  4. State important gas laws and use them in calculations.

  5. Define partial pressure, and use Dalton’s law of partial pressures.

  6. Define, use, and convert between units of concentration and molarity.

  7. Describe dilution and perform dilution calculations.

  1. 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. Write equations for neutralization reactions.

  6. Discuss acid-base ionization constants and write the equilibrium constant expression for the ionization of water.

  7. Describe the amphoteric behavior of water.

  8. Define pH, perform calculations and describe techniques for measuring pH.

  9. Describe a titration experiment, and perform titration calculations.

  10. Describe the composition of buffers and their role in maintaining pH.

  1. Describe simple organic compounds, including names, structures, formulas, and example reactions.

  1. Explain the significance of carbon compounds.

  2. Identify the principal functional groups of organic compounds.

  3. Draw structural formulas and name important organic compounds.

  4. Compare the properties and reactions of organic and inorganic compounds.

  5. Describe and compare the structures of the major biomolecules.

  1. 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, positron, 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 common units for measuring radiation.

  9. Discuss nuclear fission and fusion.

  1. Perform and analyze various laboratory activities related to chemistry.

  1. Safely and accurately follow written and oral experimental instructions to obtain valid qualitative and quantitative data.

  2. Accurately measure length, volume, mass, density, and temperature of common materials using standard laboratory apparatus.

  3. Perform mathematical conversions with correct application of significant figures.

  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.

Academic Integrity

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Attendance

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Cell phone/Electronic Device

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Tuition Adjustment Policy

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