CHM 130 - General Chemistry I

2.  Apply principles of the quantum theory to explain and describe the structures and properties of atoms and the behavior of energized atoms. (GELO 7)

3.  Describe and explain the periodic trends in the properties of elements in the periodic table.

4.  Apply the nomenclature rules to name chemical compounds.

5.  Describe the major classes of chemical reactions and distinguish between them by their fundamental chemistry and by counting. (GELO 3, GELO 7)

6.  Discern relevant information when predicting and explaining the shapes and polarities of molecules using chemical bonding theories. (GELO 3)

7.  Explain the relationships between atomic properties and macroscopic observations.

8.  Describe and explain the type of interactions within and between particles based on their atomic and molecular structures.

9.  Discern relevant information to predict and explain whether there is solution formation based on types of particle interactions. (GELO 3)

10.  Use calculation to solve chemical stoichiometry problems. (GELO 7)

11.  Explain the relationship between changes in matter and energy flow.

12.  Describe and explain factors that affect solubility and the (colligative) properties of solutions.

13.  Use chemical principles to make informed decisions about chemical products. (GELO 3)

14.  Identify quality sources for data and information pertinent to a problem or issue being examined. (GELO 7)

15.  Identify the best solution to a problem or issue. (GELO 3)

16.  Complete work accurately, with attention to detail.

II.  Atoms, Molecules, and Ions

        A. Law of Mass Conservation

        B. Law of Definite Proportions

        C. Dalton’s Atomic Theory

        D. Modern Atomic Theory

        E. Structure of the Atom: Electrons, Protons, and Neutrons

        F. Atomic Numbers, Mass Numbers, and Isotopes

        G. Atomic Mass

        H. Molecules and Ions

        I. Introduction to Chemical Bonding

        J. The Periodic Table

        K. Nomenclature

III.  Stoichiometry

        A. Balancing Chemical Equations

        B. Avogadro’s Number and the Mole

        C. Mole-mole, mole-mass, and mass-mass calculations

        D. Percent Yield

        E. Limiting Reactants

        F. Molar Concentration

        G. Diluting Concentrated Solution

        H. Stoichiometry of Reactions in Solution

        I.  Percent Composition and Empirical Formulas

        J. Determining Empirical Formulas

IV.  Major Types of Chemical Reactions

        A. Aqueous Reactions

        B. Electrolytes and Nonelectrolytes

        C. Molecular, Ionic, and Net Ionic Equations

        D. Precipitation Reactions and Solubility Rules

        E. Acid Base Reactions

        F. Oxidation-Reduction Reactions

        G. Classification of Reactions as Combination, Decomposition, Single Replacement, or Double Replacement Reactions

V.  Thermochemistry

        A. Energy and its Units

        B. Heat and Work

        C. System and Surroundings

        D. Energy Changes and Energy Conversion

        E. The First Law of Thermodynamics

        F. Energy and Enthalpy

        G. Standard State of Thermodynamics

        H. Enthalpies of Physical and Chemical Changes

        I.  Calorimetry and Heat Capacity

        J. Thermochemical Equations

        K. Hess’s Law

        L. Calculating Heats of Reaction from Bond Energies

        M. Standard Heats of Reaction and Heats of Formation

VI.  Quantum Theory and Atomic Structure

        A. Electromagnetic Spectrum and Electromagnetic Radiation

        B. The Wave Nature and Particle Nature of Light

        C. Atomic Spectra

        D. Bohr’s Model of the Hydrogen Atom

        E. Wave Nature of Electrons and Particle Nature of Photons

        F. Wave Picture of The Atom

        G. Quantum Numbers and Atomic Orbitals

        H. Shapes of Atomic Orbitals

        I.  Ways of Assigning Electron Addresses

        J. Electron Configurations

        K. Electron Configurations of Main Group Elements, Transition Elements, and Ions

VII.  Periodic Trends

        A. Atomic Radii

        B. Ionization Energy

        C. Electron Affinity

        D. Ionic Radii

        E. Metallic Behavior

        F. Electronegativity

        G. Reactivity

VIII.  Types of Chemical Bonds

           A. Ionic Bonds

           B. Covalent Bonds

                  1. Types of Covalents (in terms of # of electrons shared)

                  2. Bond Length, Bond Strength, and Bond Energy

                  3. Ionic Character of Bonds

           C. Metallic Bonds

IX.  Molecular Geometry and Bonding Theories

        A. Electron Dot Notation

        B. Lewis Structures

        C. Octet Rule

        D. Lewis Structures and Exceptions to the Octet Rule

        E. Resonance Structures

        F. Formal Charges

        G. VSEPR Theory and Shapes of Molecules

        H. Valence Bond Theory and Hybridization

        I.  Electronegativity and Bond Polarity

        J. Molecular Shape and Molecular Polarity

X.   Liquids, Solids, and Phase Changes

        A. Intermolecular Forces

        B. Surface Tension, Viscosity, Capillarity

        C. Evaporation, Vapor Pressure, and Boiling Point

        D. Properties of Water

        E. Phase Changes

        F. Kinds of Solids

        G. Phase Diagrams

XI.  Properties of Solutions

        A. Solutions

        B. Energy Changes and The Solution Process

        C. Dissolving Ionic Solids, Liquids, and Gases

        D. Solubility as an Equilibrium Process

        E. Factors Affecting the Solution Process

        F. Molarity, Molality, Mass Percent, Volume Percent, and Mole Fraction

        G. Colligative Properties

        H. Osmosis and Osmotic Pressure

        I. Some Applications of Colligative Properties

1.  Essential judgment skills include the ability to identify, assess, and comprehend situations for the purpose of problem solving and coming to appropriate conclusions and/or course of actions.  Specifically, students must be able to:

• Apply mathematical concepts to solve problems
• Discern relevant and irrelevant information when solving problems
• Express knowledge of the appropriate level of chemistry in written and/or  verbal formats
• Draw conclusions based on knowledge and experimental results

2.  Essential communication skills include the ability to communicate effectively with fellow students, faculty, and all members of the Physical Sciences department. Specifically, students must be able to:

• Understand written and verbal direction when completing tasks and assignments associated with the lecture portion of science courses
• Understand written and verbal directions when following all Departmental safety rules and procedures
• Use information technology skills consistent with effective communication.

3.  Essential emotional coping skills include the ability to demonstrate the mental health necessary to safely engage in the practice of scientific discovery.  Specifically, students must be able to:

• Engage in multitasking without becoming overly stressed
• Collaborate with classmates to complete a task in the classroom
• Cooperate with others and work in groups or alone as indicated by a particular course

4.  Essential intellectual/conceptual skills include the ability to measure, calculate, analyze, synthesize, and evaluate to engage competently in the safe practice of Chemistry. Specifically, students must be able to:

• Select appropriate methods to solve mathematical problems
• Use a calculator to complete calculations
• Use a computer to generate graphs and reports
• Analyze complex graphical data and/ or concepts
• Express an understanding of the concepts learned in chemistry in written form or verbally

5.  Other essential behavioral attributes include the ability to engage in activities consistent with safe practice without demonstrated behaviors of addiction to, abuse of, or dependence on alcohol or other drugs that may impair behavior or judgment. The student must demonstrate responsibility and accountability for actions as a student in the Physical Sciences Department and as a developing professional in the field of chemistry consistent with accepted standards of practice.

Grand Rapids Community College strives to be more than ADA compliant. We strive to be accessible and welcoming to all students of all abilities. After reviewing the Essential Abilities/Technical Standards for this program; your responsibilities as a student entail determining if you can complete all associated coursework either:

• With Accommodation. I am otherwise qualified to meet the same academic standards as any other student entering the program. However, based on a medically documented condition or diagnosis, I would qualify for reasonable accommodation under the Americans with Disabilities Act (1990). I will meet with Disability Support Services on campus to arrange those accommodations in an interactive process with the department of Physical Sciences.

• Without Accommodation. I am able to complete the program without need for reasonable accommodation or modification. In the event my medical documentation reveals otherwise or a condition manifests that would necessitate an accommodation; it is my responsibility to inform a responsible authority figure within the department of (field of study) and work with Disability Support Services to see if a reasonable accommodation or modification can be made.

If you have a medically documented condition or diagnosis, please contact the (field of study) office, or contact Disability Support Services (DSS) at disability@grcc.edu or by phone at 616.234.4140 to arrange accommodations through our interactive process.