- 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.

Know how to balance a nuclear reaction.

Know the definitions and differences in the various types of nuclear decay/radiation types: fusion, fission, alpha decay, beta decay, positron emission, gamma rays/emission.

Know the definition of binding energy and how that relates to \(E = mc^2\).

\(a {\rm A} + b {\rm B} \rightarrow c {\rm C} + d {\rm D}\)

\({\rm reaction \; rate} =\) \(-{\Delta[{\rm A}]\over a\Delta t} = -{\Delta[{\rm B}]\over b\Delta t} = {\Delta[{\rm C}]\over c\Delta t} = {\Delta[{\rm D}]\over d\Delta t}\)

\({\rm rate} = k[{\rm A}]^x[{\rm B}]^y\cdots\)

\([{\rm A}]_0 - [{\rm A}] = kt \hskip24pt t_{1/2}={[{\rm A}]_0\over 2k}\)

\(\ln\left({[{\rm A}]_0 \over [{\rm A}]}\right) = kt \hskip24pt t_{1/2}={\ln2\over k}\)

\({1\over[{\rm A}]} - {1\over[{\rm A}]_0} = k t\hskip24pt t_{1/2}={1\over k[{\rm A}]_0}\)

\(k = A\,e^{-E_{\rm a}/RT}\)

\(\ln k = {-E_{\rm a}\over R}\left({1\over T}\right) + \ln A\)

\(\ln\left({k_2\over k_1}\right) = {E_{\rm a}\over R}\left({1\over T_1} - {1\over T_2}\right)\)

A Lewis base donates an electron pair (the ligand). A Lewis acid accepts an electron pair (the metal atom or cation). This is a dative bond in general although with metals and ligands the name coordinate covalent bond is more common.

monodentate charged: the halides, hydroxide, cyanide

monodentate neutral: ammonia, water, pyridine (py), carbon monoxide

bidentate charged: oxalate (ox)

bidentate neutral: ethylenediamine (en), bipyridine (bpy), phenanthroline (phen)

PLUS - if given in a formula, you should be able to recognize other ligands and their denticities.

Remember that the ligands provide a core set of electrons. For example, in a octahedral complex, the ligands provide 12 electrons. The metals then add to the ligand number via their *d*-orbital electrons and possibly their *s*-orbital electrons depending on the charge.

Periodic Table

Conversion factors

(like masses of protons, neutrons, etc...)

- Constants
*R*= 8.314 J/mol K*R*= 0.08206 L atm/mol K

- Data
- most "data" will be in the question itself

Students will be able to…..

- Explain the macroscopic observables associated with nuclear change and the microscopic or chemists view of nuclear change.
- Identify and define various types of nuclear transmutation including fission, fusion and decay reactions.
- Use proper isotopic notation to write down and balance a nuclear reaction.
- State and compare the differences and similarities between a nuclear change and a chemical change.
- Recall and properly use Einstein’s theory of relativity equation,
*E*=*mc*^{2}, to calculate the amount of energy released upon a nuclear change. - Define binding energy and mass defect and be able to calculate each for a given nucleus.
- Understand and explain the concept of ionizing radiation and distinguish between the three different types of radiation.
- Understand and explain the concept of isotopic stability including the band of stability.
- Be familiar with the units used to quantify nuclear decay
- Understand the concept of rate of change and half life in the context of nuclear decay.
- Understand the basics of nuclear chemistry applications: nuclear power, medical treatment, isotopic labeling, and carbon dating.

Students will be able to…..

- Understand the concept of rate of change associated with a given chemical reaction and how it can be measured.
- Determine rate law of chemical change based on experimental data.
- Be able to identify the reaction order for a chemical change.
- Understand the concept of pseudo-first order kinetics and when they apply.
- Apply integrated rate equations to solve for the concentration of chemical species during a reaction of different orders.
- Understand the concept of mechanism and using rate law data predict whether or not a proposed mechanism is viable or not.
- Recall and explain why certain factors such as concentration, temperature, medium and the presence of a catalyst will affect the speed of a chemical change.
- Interpret a reaction coordinate diagram and determine if such a diagram supports a given single or multistep mechanism, including the concept and depiction of any transition states and reaction intermediates.
- Understand the concept of an activation energy in the context of the transition state and be able to calculate the activation energy given some experimental data.
- Recall, manipulate and properly employ the Arrhenius Law.
- Explain the function and purpose of a catalyst.

Students will be able to…..

- Understand the fundamental differences between ionic, covalent and coordination bonds.
- Recall from CH301 general trends in reactivity and bonding and how these trends help organize elements in the periodic table.
- Understand trends in hydration energies and oxidation states of the transition metals.
- Be able to identify common organic ligands used to construct coordination complexes, and learn how certain ligands interact with transition metal ions.
- Understand basic substitution reactions involving ligands and transition metal ions.
- Be able to identify different coordination geometries in transition metal complexes, and use coordination geometry to predict the reactivity of coordination complexes.
- Understand the basics of crystal field theory and crystal field stabilization energy, and use these to predict the electronic configurations of transition metal coordination complexes.
- Relate electronic configurations to the basic spectroscopic properties of coordination complexes.
- Relate electronic configurations to the basic magnetic properties of coordination complexes.
- Calculate the "spin-only" magnetic moment of simple coordination complexes.