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CHM 110 General Chemistry

This course will include matter and measurement, the periodic table, nomenclature, chemical reactions, states of matter, solutions, rates of reactions, equilibrium, acid/base, nuclear and organic chemistry. In the lab, a strong emphasis is placed on chemical laboratory skills in correlation with lecture topics.

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

202451

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 will include matter and measurement, the periodic table, nomenclature, chemical reactions, states of matter, solutions, rates of reactions, equilibrium, acid/base, nuclear and organic chemistry. In the lab, a strong emphasis is placed on chemical laboratory skills in correlation with lecture topics.

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. Perform numeric measurements to correctly solve chemical math problems.  (CCC 1, 2,6)

  2. Describe the structure of matter at the atomic and molecular level. (CCC 1, 2, 6)

  3. Analyze the different types of chemical reactions.  (CCC 1, 2, 6)

  4. Contrast the properties of gases, liquids, solids, and solutions. (CCC 1, 2, 6)

  5. Perform molar, 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 properties, names, structures, and formulas.  (CCC 2, 6)

  8. Explain nuclear radiation and decay.  (CCC 1, 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.  Perform numeric measurements to correctly solve chemical math problems. 
    1. Convert numbers to and from scientific notation.
    2.  Interpret the number of significant figures in a physical quantity to maintain the correct number of significant figures when performing calculations.
    3. Use dimensional analysis (the factor-label method) to convert between scientific units of measure including units of energy, length, volume, pressure, and mass.
    4. Perform calculations to calculate temperature, density, heat energy, and specific heat.
  2. Describe the structure of matter at the atomic and molecular level.
    1. Define key terms related to matter, energy, atomic structure, the periodic table, periodic trends, bonding, and electron arrangement.
    2. Identify the differences between physical and chemical changes.
    3. Explain differences between elements, compounds, and mixtures.
    4. Identify the composition of different atoms, ions, and isotopes in terms of the number of protons, neutrons, and electrons.
    5. Identify periodic trends in atomic radius, ionization energy, electronegativity, and valence electrons.
    6. Describe the arrangement of electrons within shells and subshells of an atom via electron configurations and location on the periodic table. 
    7. Describe the differences in structure, composition, and properties of ionic and molecular compounds.
    8. Name ionic and covalent compounds using proper IUPAC nomenclature.
    9. Write chemical formulas for ionic and covalent compounds.
    10. Draw Lewis structures for atoms and molecules.
    11. Determine whether bonds are ionic, polar covalent, or nonpolar covalent using electronegativity.
    12. Use valence shell electron pair repulsion (VSEPR) theory to predict molecular geometry and polarity.
  3. Analyze the different types of chemical reactions.
    1. Translate a written description of a chemical reaction into a balanced chemical equation and vice versa.
    2. Classify reaction types.
    3.  Write equations for neutralization reactions.
    4. Differentiate between endothermic and exothermic processes.
    5. Interpret a reaction energy diagram.
    6. Describe the factors that affect activation energy, and reaction rates.
    7. Write equilibrium constant expressions.
    8. Use Le Chatelier’s principle and equilibrium constants to predict changes in a system.
  4. Contrast the properties of gases, liquids, solids, and solutions.
    1. Describe the properties of solids, liquids, and gases including those that explain their specific behaviors.  
    2. Describe the properties of intermolecular forces: hydrogen bond, dipole-dipole interaction, and London dispersion forces.
    3. Identify the types of intermolecular forces present between molecules.
    4. Apply the concepts of heat exchange, equilibrium, and phase changes mathematically and conceptually.
    5. Describe the properties of solutions.
    6.  Explain the influence of temperature, pressure, and nature of the solute and solvent on solubility.
    7. Write the net ionic equation for a given reaction.
    8. Describe the colligative properties and their significance.
  5. Perform molar, stoichiometric, and gas law calculations. 
    1. Explain the meaning and uses of the mole and Avogadro’s number.
    2. Convert between molar and mass quantities of any element or compound.
    3. Perform different types of stoichiometric calculations using chemical equations.
    4. Convert between common units of pressure.
    5. Perform gas law calculations.
    6. Perform solution calculations including percent concentrations, molarity, and dilutions.
  6. Describe acids, bases, and buffers, and perform calculations used to evaluate them. 
    1. Differentiate between strong and weak acids and bases, and their salts.
    2. Write the names and formulas for common acids and bases.
    3. Define pH, titration, conjugate acid-base pairs, and amphoteric.
    4. Perform calculations with pH including titration calculations.
    5. Describe techniques used for measuring pH including titrations.
    6. Perform calculations using water’s equilibrium expression.
    7. Describe the composition and action of buffer solutions.
  7. Describe simple organic compounds, including properties, names, structures, and formulas.
    1. Compare the properties of organic and inorganic molecules.
    2. Draw and name basic organic compounds.
    3. Identify functional groups within organic compounds.
    4. Describe the structures and properties of major biomolecules. 
  8. Explain nuclear radiation and decay.  
    1. Describe the relationship between the energy of radiation and its frequency and wavelength.
    2. Write nuclear equations for alpha, beta, and gamma radiation. 
    3. Identify the characteristics, processes and protection needed for alpha, beta, and gamma radiation. 
    4. Define half life, and perform decay calculations.
    5. Contrast nuclear fission and fusion.
  9. Perform and analyze various laboratory activities related to chemistry.
    1. Describe the scientific method of investigation.
    2. Safely and accurately follow experimental procedures, adhere to good laboratory practices (GLP), and obtain valid qualitative and quantitative data.
    3. Measure length, volume, mass, density, and temperature of common materials using standard laboratory apparatus.
    4. Perform mathematical conversions with correct application of significant figures.
    5. Report the results of your experimental findings.
    6. Perform lab experiments effectively with a partner or in a small group. 

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 all distance education type 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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