- official UT ID card (with your picture and name on it)
- a simple scientific calculator (not a graphing calculator)
- a pencil(s) and eraser
- memorized formulas in your head - not on paper or anything else
- nothing else is allowed

- A printed copy of the exam (every exam has a unique version number on it).
- An answer sheet for the exam. This is a bubblesheet for your answers.
- An exam cover page that has ALL needed conversion factors and data. No formulas will be given.
- A periodic table of the elements with symbols, atomic number, and atomic weights.

**reduction** = the gain of electrons (ox# decreases)

**oxidation** = the loss of electrons (ox# increases)

**cathode** = the electrode where reduction occurs red cat

**anode** = the electrode where oxidation occurs an ox

shorthand cell notation

anode \(\bigl|\) anodic solution \(\bigl|\bigl|\) cathodic solution \(\bigl|\) cathode

\(E^\circ_{\rm cell} = E^\circ_{\rm cathode} - E^\circ_{\rm anode} \)

\(\Delta G^\circ = -nFE^\circ\)

\(\Delta G^\circ = -RT\ln K\)

\(nFE^\circ = RT \ln K\)

\(E = E^\circ - {RT\over nF}\ln Q\)

\(E = E^\circ - {0.05916\over n}\log Q\)

\(\displaystyle{I\cdot t\over n\cdot F} = {\rm moles} \)

Periodic Table

- Constants (such as...)
*F*= 96485 C/mol e^{–}*R*= 8.314 J/mol K*R*= 0.08206 L atm/mol K

- Table of Standard Potentials
- Conversion factors

Students will be able to...

- Identify an oxidation – reduction (redox) reaction based on changes in oxidation numbers across the chemical change.
- Identify oxidizing/reducing agents in chemical reaction.
- Completely balance a redox reaction in acidic or basic solution.
- Recognize degrees of reactivity based on an activity series or a standard potential table.
- Apply standard potential data to determine the relative strength of oxidizing and reducing agents.
- Construct an electrochemical cell diagram or drawing which includes the identification of the anode, cathode, and salt bridge from either a redox reaction or from the short hand cell notation.
- Show the direction of electron flow, the sign of the electrodes, the direction of ion flow in the salt bridge, on a given cell diagram or drawing.
- Describe the standard hydrogen electrode (SHE) and state its function.
- Apply standard potential data (\(E^\circ\)) to calculate the standard cell potential (\(E^\circ_{\rm cell}\)) for an electrochemical cell and from the sign of the potential predict if the cell is voltaic or electrolytic.
- Calculate the cell potential for a nonstandard cell.
- Describe fully the relationship between the standard free energy (\(\Delta G^\circ\)) and the standard cell potential (\(E^\circ\)).
- Describe fully the relationship between standard cell potential (\(E^\circ\)) and the equilibrium constant (\(K\)).
- Explain thermodynamically the operation of a concentration cell, and be able to predict the concentration in the cell based on the measured cell potential.
- Understand the relationship between the quantity of charge delivered or produced (coulombs) and the amount of reactant used or product formed (moles) for both voltaic and electrolytic cells.
- Describe the basic principles of battery design and function.
- Identify the differences and similarities of the three fundamental types of batteries: primary cells, secondary cells, and fuel cells.
- Know the details of the chemical reactions used in a lead-acid battery.