Exam 2 - Atomic Theory / Bonding

Wed 10/5 7-9pm

What the Student Brings to Exams

• 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

What we provide for the Exams

• 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.

What Formulas the Student Should Memorize

Electromagnetic Radiation

$$c = \lambda \cdot \nu$$

$$E = h \cdot \nu$$

Work Function (Φ) Equation

$$E_{\rm k} = {1\over 2} m v^2 = h\nu - \Phi$$

$E_n = -{{\cal R}\over n^2}$

$\Delta E = {\cal R} \left({1 \over n_f^2} - {1 \over n_i^2}\right)$

$\lambda = {h\over mv}$

$\Delta x \cdot m\Delta v \geq { h \over 4 \pi }$

More to Memorize...

Nomenclature: Know the formula and names of the first 10 alkanes. Know how to name ionic compounds (salts) and simple covalent compounds.

Metric Prefixes: Do you know the differences in pm, nm, μm, mm, cm, km ? How about Hz, kHz, MHz, GHz, THz ?

What we provide on the exam cover page

c = 3.00 × 10⁸ m/s

h = 6.626 × 10^-34 J·s

R = 8.314 J/mol K

${\cal R} = 2.18\times 10^{-18}\;{\rm J}$

N_A = 6.022 × 10²³ mol^-1

$m_{\rm electron} = 9.11 \times 10^{-31}$ kg

$m_{\rm proton} = 1.673 \times 10^{-27}$ kg

$m_{\rm neutron} = 1.675 \times 10^{-27}$ kg

$e^- = 1.602 \times 10^{-19}$ C

1 W = 1 J/s    (power in watts, W)

1 eV = $1.602 \times 10^{-19}$ J

Learning Outcomes for Atomic Theory

All sections are covered for this chapter.

Students will be able to...

1. Perform quantitative calculations based on the relationship between wavelength, energy, and the speed of light.
2. Identify and rank the different types of radiation which comprise the electromagnetic spectrum.
3. Explain why classical mechanics doesn't describe electromagnetic radiation.
4. Describe the photoelectric effect and relate the energy and/or intensity of the photons to the work function and kinetic energy of the ejected electrons.
5. Explain the origin of atomic and emission spectra and relate these spectra to discrete energy levels.
6. Apply the Rydberg formula to predict the energy of transitions between fixed energy levels in the hydrogen atom.
7. Explain that quantum mechanics is a mathematical model, the solutions of which yield wave functions and energies.*
8. List the possible combinations of quantum numbers that are allowed.
9. State the atomic orbital names based on quantum numbers.
10. Explain that a wave function can be used to calculate a radial distribution function that describes the probability of an electron as a function of distance away from the nucleus
11. Distinguish between one-electron systems and multi-electron systems.
12. Apply the Aufbau principle to determine the configuration for any atom or ion.
13. Relate the electronic configuration of an element to its position on the periodic table.
14. Recognize that there are exceptions to the Aufbau principle and predict where on the periodic table these are likely to occur.
15. Apply Hund's Rule and the Pauli Exclusion Principle to determine electron configuration using an orbital diagram (electrons in individual orbitals with spins).
16. Fill an electron atomic orbital diagram and determine whether the element is paramagnetic or diamagnetic.
17. Apply the shell model of multi-electron atoms to describe the concept of core vs. valence electrons.
18. Describe the organization of the periodic table and the characteristics of elements in different regions of the table.
19. Describe the concept of electronic shielding and effective nuclear charge (Zeff) and their relationship to trends in ionization energy, atomic radii, and ionic radii.

* McCord Students: this includes the one-dimensional model of particle in a box

Learning Outcomes for Bonding (Exam 2 only)

Only the first two sections are on Exam 2, the rest will be on Exam 3. This means you stop at the green line on the gchem site for Exam 2.

Students will be able too...

1. Identify metals and non-metals, and predict the types of compounds (ionic/covalent) that will form from different elements.
2. Distinguish between molecules, ions, and atoms.
3. Predict the anion or cation that a main-group element is likely to form.
4. Relate Coulomb’s law to ionic radii, ionic charge, and lattice energy.

Learning Outcomes from Fundamentals (Exam 2 only)

Three sub-sections from the Nomenclature section: Ionic Nomenclature, Polyatomic Ions, and Hydrocarbons

Students will be able too...

1. Identify the name, formula, and charge of various cations and anions.
2. Provide the name for a given ionic compound.
3. Provide the formula for a given polyatomic ion name or ionic compound name.
4. Provide chemical formulas for the first 10 normal alkanes.
5. Provide the name of any of the first 10 alkane formulas.