mccord ch301

exam 2

10/15


Where do I go for Exam 2 ?

Monday • 10/15 • 7:30 - 9pm


9:30 Class (49885)

Room Assignments:

last names A - Mi in BUR 106

last names Mo - Z in JES A121A

Please make SURE you go to the right room!

11:00 Class (49900)

Room Assignments:

last names A - Mi in UTC 2.112A

last names Mo - Z in UTC 2.102A

Please make SURE you go to the right room!

What we provide on Exams We will provide all students with:

  • copy of the exam
  • an answer sheet - aka: bubblesheet
  • a Periodic Table Handout sheet
  • scratch paper if needed

Note that the periodic table handout is available on the gchem site in the appendix under "Exam Preparation". Here is a direct link to the Periodic Table Handout for Exam 2.

Coverage: Exam 2 covers all the material that was covered on LE's 10-18 and HW's 04-07. The exam covers all of Chapter 3 (Atomic Theory) and a portion of Chapter 4 (Bonding) from the gchem site.

Questions: The exam will be have 20 multiple choice questions. The questions will have an equal weight of 5 points each. Point values are included with all questions. We will only grade you by what is bubbled in on the answer sheet. We will not look at your exam copy for answers, nor consider them in any way. Bubble carefully and correctly.

Bring the Following to the Exam

  • a pencil(s) - mechanical or wood
  • scanner only reads pencil - no ink!
  • bring eraser if you are prone to mistakes
  • bring a non-programmable, non-graphing, scientific calculator
  • we provide the rest - see top of page

DO NOT bring...

  • ink pens
  • graphing calculator
  • any type of programmable calculator
  • electronic devices - including earbuds, etc...
  • smart watches - put away that Apple Watch!
  • small creatures - or large... no creatures

Main Equations/Formulas for Exam 2

electromagnetic radiation: \[c = \lambda \cdot \nu \]

single photon energy: \[E = h \cdot \nu \]

work function: \[E_{\rm k} = {1\over 2} m v^2 = h\nu - \Phi \]

Rydberg formula: \[\Delta E = {\cal R}\left({1\over n_i^2} -{1\over n_f^2}\right) \]

H Energy Levels: \[E_n = -{\cal R}\left({1\over n^2}\right) \]

The Rydberg constant

(\({\cal R}\)) is clearly labeled and given on the Exam Periodic Table Handout which you will recieve with your exam. Actually, three values are given - use your favorite!

\({\cal R}= 2.18\times 10^{-18} \; \;{\rm J}\)
\({\cal R}= 1.097\times 10^{7} \; \;{\rm m^{-1}}\)
\({\cal R}= 3.29\times 10^{15} \; \;{\rm s^{-1}}\)

EM radiation

light : it's a wave! it's a particle!

Emission vs Absorption

emission: the electron drops down to lower level

absorption: the electron jumps up to higher level

Quantum Concepts

total nodes (nodal surfaces actually) in a given orbital    \(= (n-1)\)

angular nodes (cones and planes)    \(= \ell\)

spherical or radial nodes (spheres)    \(= n - \ell - 1\)

Electron Configurations

use the periodic table to follow the Aufbau order

when making cations from transition metals - remove the \(s\) electrons first

Learning Outcomes for Atomic Theory

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.

NOTE: Only learning outcomes 1-13 will be on Exam 2 for Chapter 4 (Bonding).

Learning Outcomes for Bonding

Students will be able to...

  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.
  5. Describe the distance dependence of the potential energy of a covalent bond.
  6. Predict and explain relative bond strength and lengths in a compound.
  7. Name and write formulas for covalent compounds.
  8. Interpret line drawings of chemical compounds with implicit hydrogens, carbons, and lone pairs.
  9. Rank the polarity of covalent bonds based on relative electronegativity.
  10. Define dipole moment and identify polar bonds.
  11. Draw the best Lewis structure (including any resonance structures) for a molecule or polyatomic ion.
  12. Apply formal charges to structures and use them to predict the most likely structure.
  13. Recognize and apply exceptions to the octet rule.
  14. Apply the VSEPR model to determine a molecule's electronic and molecular geometry based on its Lewis dot structure.
  15. Assess if a molecule is polar based on polar bonds and its molecular geometry.
  16. Identify the orbital hybridization for any atom in a given molecule using the VB model.
  17. Describe the type of bond (e.g. sigma, pi) and the atomic orbitals that are associated with the bond using the VB model.
  18. Differentiate between localized and delocalized electrons within a structure.
  19. Diagram orbital hybridization using orbital notation.
  20. Recognize that Molecular Orbital (MO) theory is used to determine the energy of the electron in a molecule as well as its geometry.
  21. Differentiate between constructive interference and destructive interference of atomic orbitals.
  22. Construct and fully interpret a MO diagram, including identifying the bond order, the lowest energy electronic excitation energy (HOMO-LUMO gap), and the magnetism (paramagnetic or diamagnetic) for a compound.