List of Exam 1 Topics (Quarter 2; 2016)

  • Identify a standard enthalpy of formation reaction from a set of reactions
  • Understand what the signs of G, H, S, q, and w mean
  • Understand how the size of K is related to the sign of G
  • Know which combinations of H and S are temp independent and which are temp-dependent and be able to solve for temp at which just becomes spontaneous
  • Identify sign of S upon examination of a chemical equation that includes phase descriptors
  • From this set, know which terms are state functions and which terms are extensive: G, H, S, q and w
  • Know what information is conveyed when using either a bomb or a coffee cup calorimeter
  • Know what the magnitude of specific heat says about the usefulness of a substance as a heat sink
  • Be able to calculate final temp when two objects come into contact and exchange heat
  • Know how to calc Ssurroundings from H
  • Be able to state the sign of G and Suniverse for all spont reactions
  • Be able to calc the temperature of a phase transition given enthalpy and entropy data
  • Have a working definition (in addition to a mathematical formula) for each of these terms: Gibbs free energy, enthalpy, entropy
  • Understand what higher bond energy means in terms of stability of a bond
  • Calculate heat flow when given specific heat (including that for a calorimeter if a bomb is used), mass and temperature change
  • Given a set of word problems, decide which change is exothermic or endothermic (especially for transitions involving change of phase)
  • Know all 9 phase transition names (e.g., gas to solid = deposition)
  • Be able to state each of the three laws of thermodynamics
  • Calculate entropy given reversible heat flow and temperature
  • Know how G and the speed of a reaction are related (hint: they’re not!)
  • Know the value of G at equilibrium
  • Know how to calculate Suniverse given entropy and enthalpy data
  • Be able to calculate G using the Gibbs Helmholtz equation
  • Know the limitations of Bohr’s model of the atom
  • Be able to rationalize all periodic trends (radius, IE, EA and EN) for both period [row] family [column] comparisons
  • Understand why ionization energies successively increase and why larger jumps are seen once an ion is isoelectronic with a noble gas
  • Become fluent with the notion of ‘penetration’ as it pertains to order of electron filling we know as the Aufbau order; i.e., which has greater penetration, 3s or 3p?
  • Be able to calculate the maximum number of electrons per energy level (remember: you add one new type of orbital for each successively higher energy level; Some People Do Fine; how many electrons can each of these hold: s, p, d, f?)
  • Be able to quickly generate an electron configuration (in either the numerical or suborbital format) for the first 36 elements; don’t forget exceptions to the Aufbau rule seen in the Cr and Cu families
  • Be able to generate a formula for an ionic compound by knowing the valence electron configurations for a given family of metal and non-metal

**There will be 34 multiple choice problems, 19 of which are “no calculator allowed”. Not every “calculator allowed” problem will require a calculator, however.

All problems are worth the same number of points.