Chemistry 111, Fall 2012

Study Problems for Midterm 2 Oct. 26

Solutions

1. define the terms solvent, solute, solution, aqueous solution, and molarity

2. define and distinguish among the following terms: - concentrated and dilute - soluble, slightly soluble, and insoluble - saturated, unsaturated, and supersaturated

3. perform dilution calculations and mixing two different solutions calculations.

4. Limiting reactant problems in solutions.

Atomic Structure I

1) Relate the wavelength, frequency, amplitude, and velocity of electromagnetic radiation

1) relate the frequency of light to the energy of a photon, and understand the relationship between the continuous wave and quantized particle descriptions of light

2) define and distinguish between the terms ground and excited state, excitation and relaxation, absorption and emission, line and continuous spectra, and absorption and emission spectra

3) calculate the energy/wavelengths of lines in the absorption and emission spectra of the hydrogen atom, and relate these spectra to the electron energy levels of the atom

5) understand the concept of wave-particle duality, and relate the DeBroglie wavelength of a wave or particle to its momentum

Atomic Structure II (Quantum Numbers handout)

2) understand the nature and relationship of the principal (n), azimuthal (l), and magnetic (ml) quantum numbers and identify which orbital properties are determined by each of these numbers
4) understand how the different quantum numbers give rise to shells and subshells of orbitals
5) name an orbital given its quantum numbers, or provide quantum numbers for a given orbital
6) provide a simple sketch indicating the relative shapes, sizes, and spatial orientations of s, p, and d orbitals
7) define the Pauli Exclusion Principle, and its relationship to the electron spin quantum number (ms) and the population of orbitals by electrons
8) explain the difference in orbital energies when comparing one-electron to multielecton systems
9) define Hund’s Rule, and provide a physical rationale for this rule
10) define and distinguish between core and valence electrons and orbitals
11) list the qualitative order of orbital energies in a multielectron atom, as predicted by the Aufbau principle, from 1s to 6s
12) understand the relationship between electronic configuration of an atom and its position in the Periodic Table
13) Understand paramagnetic and diamagnetic properties and how they relate to the number of unpaired electrons in an atom.
14) provide the Aufbau-predicted ground state electronic configuration, using either an orbital diagram or spdf notation, of Main Group atoms.
15) identify elements as alkali metals, alkaline earth metals, halogens, noble gases, main group elements, transitions metals,
16) Periodic Properties: atomic and ionic sizes, ionization energies, electronegativity. (Memorize the trends in the Periodic Table and understand the reasons for these trends)

You may use some old final exams for additional practice.

Old Midterm 2 may be helpful, but there will be more multiple choice questions on the midterm. You will be allowed the formula sheet and the Periodic table identical to the one in Midterms in Vista.