CHM 111H - General and Inorganic Chemistry I - HonorsCredits: 5
Emphasizes an in-depth study of the theories and principles of atomic structure bonding, stoichiometry, states of matters, and properties of solutions. Required for students who intend to enroll for more than one year of chemistry. Meets the needs of chemistry majors. Practices intellectual curiosity and applies it in independent ways to deepen understanding of course material. Provides opportunities to engage in independent intellectual inquiry to foster deeper learning. Credit may be earned in either CHM 111 or CHM 111H, but not in both.
Prerequisite(s): READING LEVEL 4, WRITING LEVEL 4, MATH LEVEL 5 and CHM 101W with a minimum grade of C or high school chemistry or permission of the Honors Office
Corequisite(s): None
Lecture Hours: 60 Lab Hours: 45
Meets MTA Requirement: Natural Science Lab
Pass/NoCredit: Yes
Outcomes and Objectives 1. Manipulate fundamental principles and terminology in the study of matter and its changes.
A. Define physical properties of matter and give examples.
B. Recognize the states of matter and give examples.
C. Explain the changes between states using Kinetic Molecular Theory.
D. Understand and manipulate the relationship between density, volume, mass, and specific gravity.
E. Explain the terms atom, element, molecule, compound, mixture and their interrelationships.
F. Differentiate between and give examples of physical and chemical properties and changes.
G. Identify elemental symbols.
2. Understand and apply proper measurement techniques and manipulations of measured numbers.
A. Manipulate units of English, Metric, and SI systems, and interconvert them.
B. Use dimensional analysis to carry out unit conversions and other calculations.
C. Explain the difference between precision and accuracy and demonstrate proper use of
significant digits in calculations.
D. Explain, convert between and measure temperature using the F, C, and K scales.
3. Demonstrate an understanding of the organization and information contained in the periodic table.
A. Recognize trends and predict elemental behavior based on the element's position in the periodic table.
B. Explain the difference between the atomic number and atomic mass from information contained in the periodic table.
C. Identify the location of groups, periods, and series.
D. Utilize the periodic table to predict the properties of elements and the formation.
4. Describe and explain the accepted theory of atomic structure.
A. Describe electrons, protons, neutrons, and the general structure of the atom.
B. Define isotope and give the mass number, number of neutrons, and number of electrons for a specific isotope.
C. Calculate the atomic mass of an element from isotopic abundances.
5. Understand the basic characteristics of compounds and their formation.
A. Differentiate between cations and anions and how they are formed.
B. Understand the difference between structural and molecular formulas.
C. Categorize ionic, covalent, and coordinate covalent bonds.
D. Understand the describe the properties of ionic and molecular compounds.
6. Converse and read fluently in the language of chemistry.
A. Name and write correct formulas for ionic and molecular compounds, including acids and bases.
B. Associate the names of common polyatomic ions with their formulas.
7. Apply the basic concepts of molar calculations.
A. Understand and calculate the molar mass of a compound.
B. Calculate the number of moles of an element or a compound from a given mass and the converse.
C. Determine the % composition of elements compounds.
D. Determine empirical and molecular formulas of a compound.
8. Explain the principles of chemical reactions.
A. Complete, balance, and interpret the three types of chemical equations (single replacement, double replacement,
oxidation-reduction).
B. Identify the oxidizing and reducing agents in an oxidation-reduction reaction.
C. Predict the solubility of ionic and non-ionic compounds in water.
D. Explain the difference between an electrolyte and non-electrolyte.
E. Predict what species will form when a compound dissolves in water.
F. Write and balance molecular, ionic, and net-ionic equations for an indicated reaction.
G. Determine the oxidation numbers for all elements or for each atom in a compound.
Outcome 9: Use the principles of stoichiometry.
A. Calculate the mass or moles of a reactant or product from the mass or moles of another reactant or product using a
balanced chemical equation.
B. Determine which of two reactants is the limiting reactant.
C. Calculate and explain the differences between actual yield, theoretical yield, and percent yield.
D. Explain and calculate molarity.
E. Prepare solutions of a known concentration through serial dilution.
F. Solve the stoichiometric problems using solution concentrations.
G. Explain how to carry out a titration and the preparation of a standard solution.
10. Understand basic concepts of energy in chemical reactions.
A. Describe the difference between potential and kinetic energy, and between heat energy and temperature.
B. Describe how to perform and calculate information from calorimetry experiments.
C. Recognize the terminology exothermic, endothermic, system, surroundings, and enthalpy.
D. Interconvert the units of calories and joules.
E. Understand the basis of the first law of thermodynamics.
11. Understand atomic structure.
A. Recognize and manipulate the symbols and equations for wavelength, frequency, wave
amplitude, and node.
B. Recognize and apply the Rydberg equation, Planck’s equation.
C. Understand the deBroglie equation, and the Bohr equation in the appropriate calculations.
D. Describe the probability of finding an electron in the region described by a wave equation as an orbital.
E. Discuss the implications of the Heisenberg uncertainty principle.
F. Describe the allowed energy states of an electron in an atom using the quantum numbers n, l, ml, and ms.
12. Understand electronic structure of elements and its relationship to chemical periodicity.
A. Classify substances as either paramagnetic or diamagnetic.
B. Understand that no orbital can be assigned more than 2 electrons and that the two electrons in an orbital must have
opposite spins.
C. Indicate the proper placement of electrons in an atom using electron configuration and orbital diagrams.
D. Predict the trends in atomic size, electronegativity, ionization energy, and electron affinity down a group or across a period
of the periodic table.
13. Understand fundamental concepts of bonding and molecular structure.
A. Determine the number of valence electrons for a given element from the periodic table.
B. Define the difference between ionic and covalent bonding.
C. Predict whether two elements will form an ionic or covalent bond based on their positions on the periodic table or the
difference in their electronegativity.
D. Describe the importance of lattice energy in the formation of ionic bonds.
E. Draw Lewis Electron Dot Structures for compounds, including compounds that do not obey the octet role.
F. Understand the difference between oxidation numbers and formal charges.
G. Assign a formal charge to each atom in a Lewis Electron Dot Structure and use the charges to determine the best structure
from several possibilities.
H. Draw and explain resonance structures and resonance hybrids for Lewis Electron Dot Structures.
I. Define and predict trends in bond order, bond length, and bond dissociation energy.
J. Predict the formation of polar bonds and polar molecules based on electronegativity.
K. Describe the 5 basic molecular shapes and predict the shape or geometry of a molecule or ion using the Valence Shell
Electron Pair Repulsion Theory.
L. Understand the main components of valence bond theory and molecular orbital theory.
M. Describe and identify and bonds in a molecule.
N. Use the concept of orbital hybridization to describe bonding in a molecule.
14. Demonstrate an understanding of the behavior of gases.
A. Understand the variables P, V, n, and T and their relationships in the behavior of gases.
B. Understand the concept of and know the conditions of standard temperature and pressure.
C. Understand the Kinetic Molecular Theory and how it explains the gas laws.
D. Understand the individual and combined gas laws and how to apply them.
E. Understand and use Dalton’s Law of Partial Pressure in calculations.
F. Understand the ideal gas law and how to apply it.
G. Understand the phenomena of effusion and diffusion and how to use Graham’s Law.
H. Understand that gases do not usually behave as ideal gases and know when to apply the Van der Waal Equation of State
for Real Gases.
15. Demonstrate an understanding of the behavior of liquids and solids.
A. Use the kinetic molecular theory to distinguish between liquids, solids, and gases.
B. Describe the different intermolecular interactions in liquids and solids and predict which will occur based on molecular
structure.
C. Explain the processes of evaporation and condensation of a liquid or its vapor and use the enthalpy of vaporization in
calculations.
D. Explain the process of melting and freezing of a solid or its liquid and use the enthalpy of fusion in calculations.
E. Define and use the concept of equilibrium vapor pressure and dynamic equilibrium.
F. Understand the concept of normal boiling point, normal freezing point, critical temperature,
critical pressure, and the triple point and identify all of these areas on a phase diagram.
G. Understand and describe how the intermolecular forces affect the physical properties of a
substance.
H. Understand and describe the different types of solids and their properties.
I. Understand the concept of crystal lattices and be aware that different types of crystal
lattices exist.
16. Practice intellectual curiosity and apply it in independent ways to deepen their understanding of course material.
A. Complete at least one significant project, either individually or as a group depending on the instructor’s discretion, and work
with the instructor to assure that the project demonstrates intellectual curiosity and academic rigor.
B. Actively engage with their peers in conversations, seminars, or in other formats at the instructor’s discretion to enhance
the depth of knowledge of the relevant material
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