Chem 167 SI:
Exam 2 Material
Supplemental Instruction
Iowa State University / Leader: / Max
Course: / Chem 167
Instructor: / Burnett
Date: / Oct 13

Note: This is NOT an exhaustive list of the material you are expected to know for the exam, however, these are some of the highlights in chapters 4,5,6, and part of 7.

Compound / Formula
Methane / CH4
Ethane / C2H6
Propane / C3H8
Butane / C4H10
Pentane / C5H12
Hexane / C6H14
Heptane / C7H16
Octane / C8H18
Nonane / C9H20
Decane / C10H22

A helpful acronym for the first four is Mom Eats Peanut Butter (Methane, Ethane Propane, Butane)

Don’t forget limiting reactant problems!

Gas / # moles present
N2 / 31.929
O2 / 8.567
Ar / 0.382
CO2 / 0.013
Other trace gases / 0.002
Total / 40.893

(from this, other gas laws are derived (Boyle’s, Charles, Avogadros, etc)

Also note that from this we can say:

Mole fraction:

STPconditions: 273 K, 1 atm, and 22.4 L

Kinetic Molecular Theory:

  1. A gas is made up of vast particles in constant motion
  2. Particles in a gas are infinitely small and can be said to occupy no volume
  3. Particles in gas move in straight lines except when colliding with other molecules or the confinements of the container. Collisions are said to be elastic—kinetic energy is conserved
  4. Particles in gas interact with each other only when collisions occur
  5. Average kinetic energy of particles depends on their absolute temperature

Also be aware of the instances when the kinetic theory breaks down (there are two) and how the van-der waals equation corrects for these

Gas sensors:

Know how the Capacitance Manometer, Thermocouple gauge, and Ionization Gauge work, along with what is unique about the Mass Spectrometer.

Wave-particle Duality- some situations light behaves as a wave, and in others, it behaves as a particle.

Be able to describe situations where light behaves as a wave and a particle

whereh = Planck’s constant (6.626*10-34Js) and v = frequency

where c = speed of light (3.00*108 m/s), = wavelength

1. Principal (shell) quantum number -n

  • Describes the energy level in the atom (1 through 7)
  • The maximum number of electrons innis2n2

2. Angular (subshell) quantum number -l

  • Describes the sublevel inn
  • Each energy level hasnsublevels

3. Magnetic quantum number -m

  • Describes the orbital withinl
  • s has 1 orbital
  • p has 3 orbitals
  • d has 5 orbitals
  • f has 7 orbitals

4. Spin quantum number -s

  • Describes the spin of the electrons in an orbital.
  • Electrons in the same orbital must have oppisite spins.
  • Possible spins are clockwise or counterclockwise.

Also, be familiar with:

Hund’s Rule:

Pauli Exclusion Principle:

Aufbau Principle:

Heisenberg Uncertainty Principle:

Be able to apply periodic trends Ionization energy, atomic size, and electron affinity (electronegativity).

Good luck!