Chem 120 Midterm 2 Study Guide – Fall 2010: Chapters 5, 6, and 7
Note for all questions numerical problems count more for those with simple facts,
definitions or qualitative relationships.
Chapter 5: Electronic structure of Atoms, Energy, Quantum theory and light
(20-25 questions, 25-35% of test)
1.) Be able to relate portions of the electromagnetic spectrum to their ranges of
wavelengths or frequencies: eg. radio, visible, xray…
2.) Be able to calculate interchangeably the energy, wavelength and frequency of a
photon given one of those quantities.
3.) What contributions were made to quantum theory by: Bohr, Balmer, Einstein,
Planck, Heisenberg and Schroedinger and who got nobel prizes and for what?
4.) Be able to calculate limiting photon energies for the photoelectric effect.
5.) What is meant by ionizing radiation and how energetic must this be?
6.) Be able to relate energy level transitions to the energy of emitted or absorbed
photons according to the Rydberg-Balmer equation.
7.) What are emission spectra and emission lines? How do these relate to element
specific absorption lines used in spectroscopic analysis?
8.) What is the de Broglie wavelength and how is this related to sub-atomic particles
like electrons.
9.) Be able to state and discuss Heisenberg’s uncertainty principle in terms of what
can and cannot be known.
10.)
What are the relationships between orbitals (for s, p, d, f) and quantum
numbers for electrons in atoms of various sizes?
11.)
What does each quantum number determine?
12.)
Which quantum number does not result from solutions to Schroedinger’s
equation and where does it come from?
13.)
What are the shapes of s, p, d and f orbitals for atoms of a given period
and be able to draw these upon request?
14.)
What are permissible versus impossible sets of quantum numbers (n, l, ml ,
ms ) for a particular electron eg. a p electron in Nitrogen.
15.)
Be able to give shorthand or box notation electron configurations for
common elements in their ground states (or an excited state).
Chapter 6 Periodic Properties of the elements
Approximately 20 questions and 25-35% of test
1.) How does the periodic table relate to the atomic numbers of elements and to their
electronic configurations?
2.) Relate position in the periodic table to atomic and ionic radii and give the
controlling effects?
3.) Be able to arrange sequences of atoms or ions in terms of increasing radius.
4.) Be able to arrange sequences of atoms or ions in terms 1st ionization energies.
5.) Be able to arrange sequences of atoms or ions in terms 2nd ionization energies.
6.) What is electron affinity and write an equation to express this for a given element.
7.) How does metallic character vary across the periodic table?
8.) How do the acid/base properties vary between metal and non metal oxides?
9.) How do properties like density, conductivity and melting point vary down
groups?
10.)
Which elements can form peroxides and superoxides?
11.)
Know the valence of the common ion(s) for each group and how this
relates to position in the periodic table and orbitals. Hint how do the electron
structures of common ions relate to noble gases?
12.)
Review the chemical properties by group for alkali metals, alkaline earth
metals, chalcogens, halogens and noble gases.
13.)
Be able to write electron configurations for common ions.
14.)
How does lattice energy in ionic bonds relate to ionic radius and charge?
15.)
How do bond polarities relate to unlike elements from their position in the
periodic table. Given 2 elements which one pulls the most electrons in a covalent
bond?
16.)
What is dynamite and who invented it?
Chapter 7 Chemical Bonding Concepts
Approximately 20 questions and 25-35% of test
1.) Be able to write lewis symbols for neutral atoms and ions, including the order of
filling orbitals and order of emptying orbitals upon ionization.
2.) What is the isoelectronic series for electronic structures equivalent to Ar?
3.) What are the general properties of ionic solids and how does this relate to the
nature of ionic bonds and structure of solids?
4.) What are the different components of energy in ionic bonds?
5.) Which compound would have a higher melting point, greater hardness and lower
solubility in water: a) BeO b) RaSe ?
6.) What is Coulomb’s Law and what is its relevance to ionic bond strengths.
7.) What determines the lengths of ionic bonds?
8.) How can you apply the concept and values for electronegativities to predict bond
character?
9.) What is the difference between polar and non polar covalent bonds?
10.)
Calculate the dipole moment in Debyes for a diatomic molecule given
mu= qr, bonding radii and charges for both atoms involved.
11.)
Explain the trend in decreasing dipole moments for the hydrogen halides
from HF to HI.
12.)
Which molecule is more polar: a) PH3
b) NH3
c) AsH3?
13.)
How does covalent bond length and strength vary between single, double
and triple bonds?
14.)
Be able to apply the method of formal charges to predict the most stable,
gound state Lewis structure for simple molecules.
15.)
What are resonance structures, give examples of molecules which posess
these and explain their relevance as greenhouse gases.
16.)
What is the octet rule and what are its exceptions?
17.)
What kind of a compound is SiCl4 and what would you expect its
chemical and physical properties to be?