Common use of Chemistry Clause in Contracts

Chemistry. a minimum 8 credits A student should meet this requirement by successfully completing General Chemistry I and II for majors as part of the Transfer Credit Framework (see Appendix B). Successful completion of comparable coursework will at the minimum yield competency in: • Presenting the scientific method. • Classifying matter on the basis of physical and chemical properties. • Classifying matter on the basis of physical and chemical changes. • Listing the common SI units of measurement, the values of selected prefixes, and the use of dimensional analysis to interconvert units of measurement. • The use of the rules for significant figures for calculation problems. • Describing the structure of the atom in terms of subatomic particles; writing the isotopic symbol for any isotope of a given element or ion. • Describing the basic features of the periodic table. • Writing formulas of ionic or covalent compounds from their names and from their names writing their formulas. • Writing and balancing a chemical reaction. • Classifying reactions into various types such as combination, decomposition, single replacement, double replacement, oxidation-reduction, acid-base, precipitation and gas forming reactions. • The use of the mole concept to calculate the molar mass, the number of moles from the mass of a sample, the number of atoms or molecules and molarity of solutions. • Applying the mole concept to the determination of mass %, empirical and molecular formulas. • Applying the mole concept to reaction stoichiometry calculations including limiting reagent and percent yield. • The use of kinetic molecular theory to account for the properties of gases and the gas laws (Xxxxxx, Xxxxxxx, Xxxxxxxx, etc.). • The use of gas laws to calculate the pressure, volume, temperature or number of moles from appropriate data. • The use of the Ideal gas law to determine the density or molar mass of a gas and the stoichiometry of reactions involving gases. • Calculating of the partial pressure or mole fractions from the appropriate data of gas mixtures. • Explaining how the properties of real gases differ from an Ideal Gas. • Explaining the role of heat in chemical reactions (Thermodynamic Laws). • Performing calorimetric calculations and use enthalpy tables or Xxxx’x Law to determine the heat of a reaction. • Explaining the relationships between the properties of electromagnetic radiation with respect to wavelength, frequency, energy and spectral region and being able to calculate the energy, frequency or wavelength from appropriate data. • Comparing and contrasting the Xxxx and quantum theories of atomic structure and how they account for location of electrons in atoms and spectral lines. • Explaining the characteristics of atomic orbitals and the quantum numbers associated with them. • Writing the electronic configuration of atoms and ions. • The use of the periodic table to predict the physical and chemical properties of elements, including atomic radii, ionization energy and electron affinity. • Writing Xxxxx structures for neutral atoms, ions, ionic and covalent compounds. • The use of Xxxxx structures and VSPER theory to predict electronic and molecular geometries. • The use of the principle of electronegativity to describe the characteristics of polar covalent bonds. • The use of polar and covalent bonds and VSEPR to determine the overall polarity of a molecule. • The use of valence bond theory and molecular geometry to determine the hybridization of atoms. • Comparing and contrasting valence bond, molecular orbital and metallic bonding theories and how each accounts for molecular structures and properties. • Comparing the differences between the state of matter and the changes of state that occur. • Describing the major types of intermolecular forces and use them to explain the properties of solids and liquids such as boiling point, melting point, surface tension and viscosity. • Describing how intermolecular forces determine solubility of polar and nonpolar substances. • Calculating the concentration of solutions in molarity, molality, normality, mole fraction, or percent by mass and be able to interconvert between them. • Listing the colligative properties of solutions (freezing point depression, boiling point elevation, vapor pressure lowering and osmotic pressure) and performing calculations involving them. • Determining rate laws and order of a reaction from experimental data using the initial rates or graphical methods. • The use of collision theory to explain the concept of activation energy and the effect of temperature on reaction rates and use the Arrhenius equation to calculate the activation energy. • The use of elementary steps to link the mechanism of a reaction to the rate law. • Explaining how a catalyst affects a reaction. • Stating and applying LeChatlelier’s Principle to a reaction at equilibrium. • Calculating the value of an equilibrium constant from experimental data and use equilibrium constants to predict quantities of all species at equilibrium. • Stating and applying the Arrenhius, Bronsted-Xxxxx and Xxxxx acid-base theories to acid-base reactions. • Performing equilibrium calculations for pH, Ka and buffer systems. • Explaining the concept of solubility product constant, complex ion equilibrium, the common ion effect and write the Ksp and Keq expressions. • Calculating the molar solubility of a species and determining if a precipitate will form. • Discussing the fundamental laws of thermodynamics, free energy and entropy. • Performing thermodynamics calculations to predict the spontaneity of a chemical reaction and its equilibrium constant. • Discussing and applying the principles of electrochemistry including writing and balancing redox reactions. • Calculating cell potentials. • Calculating free energy and equilibrium constants from cell potentials. • Applying the above-mentioned competencies in a collaborative laboratory environment.

Chemistry. a minimum 8 credits A student should meet this requirement by successfully completing General Chemistry I and II for majors as part of the Transfer Credit Framework (see Appendix B). Successful completion of comparable coursework will at the minimum yield competency in: •  Presenting the scientific method. •  Classifying matter on the basis of physical and chemical properties. •  Classifying matter on the basis of physical and chemical changes. •  Listing the common SI units of measurement, the values of selected prefixes, and the use of dimensional analysis to interconvert units of measurement. •  The use of the rules for significant figures for calculation problems. •  Describing the structure of the atom in terms of subatomic particles; writing the isotopic symbol for any isotope of a given element or ion. •  Describing the basic features of the periodic table. •  Writing formulas of ionic or covalent compounds from their names and from their names writing their formulas. •  Writing and balancing a chemical reaction. •  Classifying reactions into various types such as combination, decomposition, single replacement, double replacement, oxidation-reduction, acid-base, precipitation and gas forming reactions. •  The use of the mole concept to calculate the molar mass, the number of moles from the mass of a sample, the number of atoms or molecules and molarity of solutions. •  Applying the mole concept to the determination of mass %, empirical and molecular formulas. •  Applying the mole concept to reaction stoichiometry calculations including limiting reagent and percent yield. •  The use of kinetic molecular theory to account for the properties of gases and the gas laws (Xxxxxx, Xxxxxxx, Xxxxxxxx, etc.). •  The use of gas laws to calculate the pressure, volume, temperature or number of moles from appropriate data. •  The use of the Ideal gas law to determine the density or molar mass of a gas and the stoichiometry of reactions involving gases. •  Calculating of the partial pressure or mole fractions from the appropriate data of gas mixtures. •  Explaining how the properties of real gases differ from an Ideal Gas. •  Explaining the role of heat in chemical reactions (Thermodynamic Laws). •  Performing calorimetric calculations and use enthalpy tables or Xxxx’x Law to determine the heat of a reaction. •  Explaining the relationships between the properties of electromagnetic radiation with respect to wavelength, frequency, energy and spectral region and being able to calculate the energy, frequency or wavelength from appropriate data. •  Comparing and contrasting the Xxxx and quantum theories of atomic structure and how they account for location of electrons in atoms and spectral lines. •  Explaining the characteristics of atomic orbitals and the quantum numbers associated with them. •  Writing the electronic configuration of atoms and ions. •  The use of the periodic table to predict the physical and chemical properties of elements, including atomic radii, ionization energy and electron affinity. •  Writing Xxxxx structures for neutral atoms, ions, ionic and covalent compounds. •  The use of Xxxxx structures and VSPER theory to predict electronic and molecular geometries. •  The use of the principle of electronegativity to describe the characteristics of polar covalent bonds. •  The use of polar and covalent bonds and VSEPR to determine the overall polarity of a molecule. •  The use of valence bond theory and molecular geometry to determine the hybridization of atoms. •  Comparing and contrasting valence bond, molecular orbital and metallic bonding theories and how each accounts for molecular structures and properties. •  Comparing the differences between the state of matter and the changes of state that occur. •  Describing the major types of intermolecular forces and use them to explain the properties of solids and liquids such as boiling point, melting point, surface tension and viscosity. •  Describing how intermolecular forces determine solubility of polar and nonpolar substances. •  Calculating the concentration of solutions in molarity, molality, normality, mole fraction, or percent by mass and be able to interconvert between them. •  Listing the colligative properties of solutions (freezing point depression, boiling point elevation, vapor pressure lowering and osmotic pressure) and performing calculations involving them. •  Determining rate laws and order of a reaction from experimental data using the initial rates or graphical methods. •  The use of collision theory to explain the concept of activation energy and the effect of temperature on reaction rates and use the Arrhenius equation to calculate the activation energy. •  The use of elementary steps to link the mechanism of a reaction to the rate law. •  Explaining how a catalyst affects a reaction. •  Stating and applying LeChatlelier’s Principle to a reaction at equilibrium. •  Calculating the value of an equilibrium constant from experimental data and use equilibrium constants to predict quantities of all species at equilibrium. •  Stating and applying the Arrenhius, Bronsted-Xxxxx and Xxxxx acid-base theories to acid-base reactions. •  Performing equilibrium calculations for pH, Ka and buffer systems. •  Explaining the concept of solubility product constant, complex ion equilibrium, the common ion effect and write the Ksp and Keq expressions. •  Calculating the molar solubility of a species and determining if a precipitate will form. •  Discussing the fundamental laws of thermodynamics, free energy and entropy. •  Performing thermodynamics calculations to predict the spontaneity of a chemical reaction and its equilibrium constant. •  Discussing and applying the principles of electrochemistry including writing and balancing redox reactions. •  Calculating cell potentials. •  Calculating free energy and equilibrium constants from cell potentials. •  Applying the above-mentioned competencies in a collaborative laboratory environment.