CHM 140 - General Chemistry II

1. Use the scientific concepts to make decisions about current societal issues.
2. Perform and solve basic calculations in chemistry using a calculator, mathematical formulas, and elementary algebra.
3. Explain common observations using the basic concepts, theories, and principles of chemistry.
4. Explain gas phase behavior in qualitative and quantitative terms.
5. Describe the rates of chemical reactions and the factors that affect those rates.
6. Explain the concept of chemical equilibrium.
7. Describe acid-base behavior and interpret results of acid-base titrations.
8. Discuss the principles of equilibrium applied to aqueous ionic systems (acid-base buffers, slightly soluble ionic compounds, and complex ions).
9. Use the principles of thermodynamics to discuss why chemical and physical changes occur and the directions of those changes.
10. Describe the relationship between electricity and chemical reactions.
11. Discuss nuclear reactions including their applications, kinetics, and energetics.
12. Translate or explain what written information means and/or how it can be used. 
13. Create and/or organize data and information into meaningful patterns in order to interpret and draw inferences from it. 
14. Complete work accurately, with attention to detail. 

II.  GASES

       A. Characteristics of gases

       B. Gas pressure and its measurement

       C. The gas laws

       D. The ideal gas equation

       E. Solving gas laws problems

       F. Gas laws and reaction stoichiometry

       G. Density and molar masses of gases

       H. Gas mixtures: partial pressures and mole fractions; collecting gases over water

       I. The kinetic-molecular theory

       J. Behavior of real gases: the van der Waals equation

III. CHEMICAL KINETICS

       A. Reaction rates (average, instantaneous) in terms of concentrations

       B. Factors influencing reaction rates

       C. Reaction rates and stoichiometry

       D. Rate law and its components

       E. Integrated rate laws for 0, 1st, 2nd order reactions (no derivation)

       F. Graphical determination/recognition of 0, 1st, 2nd order reactions

       G. Temperature and reaction rate: the Arrhenius equation

       H. Energy profile (reaction energy) diagrams

       I. The activated complex (or transition state)

       J. Reaction mechanisms

       I. Catalysts: heterogeneous, homogeneous, and enzymes

IV.  CHEMICAL EQUILIBRIUM

       A. The concept of dynamic equilibrium

       B. The equilibrium constant (K) and reaction quotient (Q)

       C. The equilibrium constants Kc and Kp and their relation

       D. Determining and manipulating equilibrium constants

       E. Meaning of the equilibrium constant

       F. Comparing Q and K to predict reaction direction

       G. Calculating equilibrium concentrations from K and vice-versa

       H. Calculating equilibrium and initial concentrations using ICE tables

       I. Le Chatelier’s Principle  (changes in volume, concentration, temperature, and adding a catalyst)   

V.  ACIDS and BASES

       A. Arrhenius acids and bases

       B. Recognizing acids and bases

       C. Relative strengths of acids and bases based on their chemical formulas          

       D. Bronsted-Lowry acids and bases

       E. Conjugate acids and bases

       F. Autoionization of water

       G. pH and the pH scale

       H. Ionization (dissociation) constants of acids (Ka) and bases (Kb)

       I. Calculations of concentrations, pH, and pOH for strong acids and bases and for weak acids and bases using K’s and pH

       J. Polyprotic acids and bases

       K. Relationship between Ka and Kb

       L. Acid-base properties of salt solutions

       M. Molecular properties and acid strength

       N. Lewis acids and bases

VI.  AQUEOUS IONIC EQUILIBRIA

       A. Acid-Base buffer solutions and the Common Ion Effect

       B. Buffer capacity and range

       C. The Henderson-Hasselbalch equation

       D. Acid-base titrations and indicators

       E. Qualitative descriptions of features of acid-base titration curves

       F. Calculating Ka for a weak acid from a titration curve

       G. Qualitative and quantitative aspects of solubility equilibria

       H. Factors affecting solubility: common ion effect and pH

       I. Qualitative aspects of complex ions equilibria

VII. CHEMICAL THERMODYNAMICS

       A. Spontaneous (and nonspontaneous) reactions

       B. The second law of thermodynamics

       C. Entropy

       D. The third law of thermodynamics and molar entropies

       E. Qualitative rules for entropy

       F. Calculating entropy changes in the system and surroundings

       G. Calculating entropy changes in the universe

       H. Free energy change and process spontaneity

       I. Effect of temperature on process spontaneity

       J. Standard free energy change

       K. Calculations of free energy change using the Gibbs Equation

       L. Calculations of enthalpy change (delta H), entropy change (delta S), and Gibbs free energy change (delta G) using thermodynamic data tables

       M. Relationships between the standard and non-standard Gibbs free energy changes and equilibrium

VIII. ELECTROCHEMISTRY

       A. Simple redox reactions

       B. Oxidation numbers

       C. Oxidizing and reducing agents

       D. Balancing simple redox equations

       E. Voltaic (galvanic) cells

       F. Cell notation

       G. Cell potential (Ecell) or electromotive force (EMF)

       H. Relative strengths of oxidizing and reducing agents

       H. Standard reduction potentials

       I. The Nernst equation (non-standard conditions)

       J. Concentration cells

       K. Relationship of cell potential to free energy change and chemical equilibrium

       L. Some applications: batteries and corrosion

       M. Electrolytic cells

       N. Electrolysis of water, molten salts, and aqueous solutions

       O. Electroplating and quantitative aspects of electrolysis

IX.  NUCLEAR CHEMISTRY

       A. Nature of radioactivity

       B. Nuclear reactions

       C. Types of radioactive decay

       D. Kinetics of radioactive decay and radiocarbon dating

       E. Nuclear transmutations

       F. Biological effects of nuclear radiation

       G. Units of radioactivity

       H. Applications of radioisotopes

       I. The energy of nuclear reactions

       J. Fission

       K. Fusion
      
X.  COORDINATION CHEMISTRY (OPTIONAL)

       A. Structure and terminology

       B. Properties of transition metals

       B. Basic nomenclature

       C. Crystal Field Theory

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 completing laboratory tasks and assignments
• 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 or laboratory
• 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.