Students will relate atomic structure to chemical systems, calculate the amount of material used in chemical reactions, use the periodic table as an aid to understanding chemical systems and interpret chemical reactions. 5 hrs. lecture/wk. Note: An honors contract is available. Contact the Honors Program Office, COM 201, for more information.
Prerequisite or corequisite: MATH 171 or assessment test and Corequisite: CHEM 125
Refer to the instructor's course syllabus for details about any supplies that may be required.
Upon successful completion of this course, the student should be able to:
- Describe matter and its measurement, including calculations done on measurements.
- Demonstrate an understanding of basic chemical nomenclature.
- Explain concepts of basic atomic theory and relate the theory to the periodic table.
- Write chemical reactions and solve problems involving chemical stoichiometry.
- Describe the nature of aqueous solutions and reactions occurring in aqueous solution.
- Apply concepts of thermochemistry to physical and chemical changes.
- Describe the electronic structure of atoms and relate the electronic structure to atomic properties.
- Demonstrate an understanding of chemical bonding and its application to molecular structure.
- Describe the properties of solids, liquids and gases and relate those properties to intermolecular forces.
Content Outline and Competencies:
I. Describe Matter and Its Measurement, Including Calculations Done on Measurements A. Distinguish among the three states of matter (solid, liquids and gases). B. Distinguish among elements, compounds and mixtures. C. Distinguish between physical and chemical properties and physical and chemical changes. D. State the basic units of measurement for length, mass, volume and temperature in the SI system. E. Give the numerical equivalent of selected SI prefixes. F. Convert temperatures between Fahrenheit, Celsius and Kelvin scales. G. Express numerical answers to the correct number of significant figures. H. Solve problems using dimensional analysis, including conversion of units. I. Solve problems involving density. II. Demonstrate an Understanding of Basic Chemical Nomenclature A. Write the name and symbol for selected elements. B. Write the name and symbol for selected polyatomic ions. C. Compare and contrast molecular compounds and ionic compounds. D. Write names and formulas for the following types of compounds: ionic compounds, binary molecular compounds and acids. III. Explain Concepts of Basic Atomic Theory and Relate the Theory to the Periodic Table A. Recall the basic ideas in Dalton's atomic theory. B. Summarize the experiments of J.J. Thomson, Robert Millikan and Ernest Rutherford that characterized the structure of the atom. C. Describe atoms in terms of electrons, protons and neutrons. D. Given the isotopic masses and fractional abundances for a naturally occurring element, calculate its atomic weight. E. Identify the following areas of the periodic table: metals, nonmetals and metalloids; main groups, transition metals, inner transition metals; alkali metals, alkaline earth metals, halogens and noble gases. F. Describe the formation of cations and anions and use the periodic table to predict the charges of monoatomic ions. IV. Write Chemical Reactions and Solve Problems Involving Chemical Stoichiometry A. Calculate the molecular mass of a compound from its formula. B. Solve problems relating the mass of a compound to the number of moles of a compound. C. Solve problems relating the mass of a compound to the number of molecules. D. Calculate the percent composition of a compound from its formula. E. Determine the empirical formula of a compound from its percent composition. F. Determine the molecular formula of a compound from its empirical formula and molecular mass. G. Write a balanced chemical equation given the reactants and products. H. Predict the product of the combustion reactions of hydrocarbons and simple compounds having C, H and O. I. Identify chemical reactions by type: combination, decomposition, combustion. J. Solve problems relating grams and moles of substances in balanced chemical equations. K. Calculate theoretical yield and percent yield when actual yield is given. L. Recognize the limiting reagent in a reaction and do calculations with limiting reagent. V. Describe the Nature of Aqueous Solutions and Reactions Occurring in Aqueous Solution A. Explain how to make solutions of given concentration. B. Explain how to dilute solutions to a specified volume or concentration. C. Solve solution stoichiometry problems. D. Distinguish among strong, weak and nonelectrolytes in solution. E. Write balanced complete and net ionic equations. F. List the common acids and bases and classify each as a strong or weak electrolyte. G. Assign oxidation numbers to atoms in molecules and ions. H. Recognize oxidation-reduction reactions and identify oxidizing and reducing agents. I. Balance simple oxidation-reduction reactions by the half-reaction method. VI. Apply Concepts of Thermochemistry to Physical and Chemical Changes A. Recognize and illustrate the law of conservation of energy. B. Distinguish between a system and its surroundings and describe the energy changes in a system and its surroundings during a given reaction. C. State the first law of thermodynamics. D. Solve problems involving enthalpies for physical and chemical changes. E. Solve calorimetry and heat capacity problems. F. Calculate enthalpy changes using Hess' law and measured enthalpies of reaction. G. Calculate standard enthalpies of reaction from standard enthalpies of formation. H. Determine the enthalpy of reaction using bond energies. VII. Describe the Electronic Structure of Atoms and Relate the Electronic Structure to Atomic Properties A. Solve problems relating frequency, wavelength and energy of electromagnetic radiation. B. Explain the essential feature of Planck's quantum theory. C. Discuss how line spectra give evidence of energy quantization. D. Describe the wave mechanical model of the atom. E. Describe s and p orbitals and recognize d orbitals. F. Write a set of quantum numbers for any particular electron. G. Write the electron configuration of elements up to atomic number 57. H. Write electron configurations for ions of main group and transition elements. I. Relate position on the periodic table to electron configuration and quantum numbers. J. Describe the scientific contributions of Planck, Einstein, de Broglie, Bohr, Schrodinger, Heisenberg, Pauli and Mendeleyev. K. Apply Periodic Trends in atomic radii to predict relative size of an atom. L. Predict relative first ionization energies from periodic trends. M. Explain the observed changes in value of the successive ionization energies for a given atom. N. Describe the periodic trends in metallic and nonmetallic behavior. O. Describe the general differences in chemical reactivity between metals and nonmetals. VIII. Demonstrate an Understanding of Chemical Bonding and its Application to Molecular Structure A. Determine the number of valence electrons for an atom and write its Lewis symbol. B. Recognize when the octet rules applies to the arrangement of electrons in the valence shell. C. Predict the relative size of anions and cations formed from an atom. D. Use electronegativity differences between bonding atoms to classify bonds as non-polar, polar covalent or ionic. E. Draw Lewis structures for atoms, ions and covalent compounds, recognizing when multiple bonds, resonance structures, expanded valence shells, incomplete valence shells and odd electrons are needed. F. Relate the number of electron pairs in the valence shell of an atom in a molecule to the geometrical arrangement around that atom. G. Predict molecular geometry using the VSEPR model. H. Predict whether a molecule can have a net dipole moment from the molecular shape and the electronegativity of the atoms involved. I. Describe covalent bonding using valance bond theory. J. Describe sp, sp2 and sp3 hybrid orbitals. K. Describe the bonding in a double and triple bond. IX. Describe the Properties of Solids, Liquids and Gases and Relate Those Properties to Intermolecular Forces A. Compare and contrast gases, liquids and solids. B. Convert between torr, mm Hg, standard atmosphere and Pascal. C. Demonstrate an understanding of the gas laws (Charles', Boyle's ideal, etc.) by working problems with them. D. List the points of the kinetic molecular theory and describe how this theory explains the common gas laws. E. Work stoichiometry problems involving gases and the gas laws. F. Describe how the relative rates of diffusion and effusion of two gases depend on their molar masses (Graham's law). G. Describe how a real gas differs from an ideal gas. H. Employ the kinetic molecular model to explain the differences between the gas, liquid and solid states. I. Recognize where dipole-dipole forces, hydrogen bonding and London dispersion forces are important. J. Qualitatively explain the relationship between intermolecular forces and properties of liquids and solids. K. Draw a phase diagram of a substance given proper data and use a phase diagram to predict the phases present at a given temperature and pressure. L. Given heating/cooling curves, calculate the heat associated when a given substance changes from one condition to another. M. Compare and contrast crystalline and amorphous solids. N. Categorize crystalline solids as ionic, molecular, covalent network and metallic solids.
Method of Evaluation and Competencies:
Evaluation of student mastery of course competencies will be accomplished using the following methods:
All exams will be taken in class (no take home exams will be given). 60% of grade 3-6 Unit exams 20% of grade Final exam 20% of grade Quizzes and homework 100% Final grades will be determined with the following percentage scores: A = 90% - 100% B = 80% - 89% C = 70% - 79% D = 60% - 69% F = 0% - 59%
- Computer Literacy Expectations: Students will need basic word processing and Internet searching skills for the completion of some papers, exercises and projects.
- Students entering physical science classes should be aware that they may be in close contact with potentially hazardous chemicals and equipment. Students should assume responsibility in conducting themselves in a manner to minimize such hazards.
If you are a student with a disability, and if you will be requesting accommodations, it is your responsibility to contact Access Services. Access Services will recommend any appropriate accommodations to your professor and his/her director. The professor and director will identify for you which accommodations will be arranged.
JCCC provides a range of services to allow persons with disabilities to participate in educational programs and activities. If you desire support services, contact the office of Access Services for Students With Disabilities (913) 469-8500, ext. 3521 or TDD (913) 469-3885. The Access Services office is located in the Success Center on the second floor of the Student Center.