Tuesday, November 14, 2006
Tuesday
Honors: Today, we covered the simple formulas for determining , for a principal energy level, "n", the number of sublevels within that PEL = n, the number of orbitals within that PEL = n^2, and the maximum number of electrons of that PEL = n^2 * 2.
We defined "degenerate" orbitals. We also discussed "isoelectronic" particles such as Ne, F- , and Mg 2+ .
We then reviewed the physical significance of the terms: Principal Energy Level, Sublevel, and Orbital.
We viewed the electron density vs. distance from the nucleus video as well as the orbital/energy diagram video.
We then launched into the intro to the Periodic Table unit discussing the Law of Triads and the "Law of Eights or Octaves" as developed by Newlands and Mendeleev.
The Periodic Table info will not be on Thursday's exam BUT the above info about electron configurations, orbitals, isoelectronic particles, etc. will be.
E: we explained the periodic trends in atomic volume/size/radius and ionization energy. We also explained why all cations are smaller than their respective atoms and why all anions are larger than their respective atoms.
AP: we finished electron configurations and orbital diagrams of transition elements (valence electrons" first in, first out). Then we delicately discussed electron shielding and penetration within a given principal energy level: s electrons shield p,d,and f electrons, p electrons shield d and f electrons, and d electrons shield f electrons from some of the nuclear charge. "s" electrons are the most penetrating followed by p,d, and f electrons of a given principal energy level.
We began to explain the first of five or six major periodic trends. Of course, we will explain any and all exceptions in a perfectly normal, perfectly logical manner. Good times.
We defined "degenerate" orbitals. We also discussed "isoelectronic" particles such as Ne, F- , and Mg 2+ .
We then reviewed the physical significance of the terms: Principal Energy Level, Sublevel, and Orbital.
We viewed the electron density vs. distance from the nucleus video as well as the orbital/energy diagram video.
We then launched into the intro to the Periodic Table unit discussing the Law of Triads and the "Law of Eights or Octaves" as developed by Newlands and Mendeleev.
The Periodic Table info will not be on Thursday's exam BUT the above info about electron configurations, orbitals, isoelectronic particles, etc. will be.
E: we explained the periodic trends in atomic volume/size/radius and ionization energy. We also explained why all cations are smaller than their respective atoms and why all anions are larger than their respective atoms.
AP: we finished electron configurations and orbital diagrams of transition elements (valence electrons" first in, first out). Then we delicately discussed electron shielding and penetration within a given principal energy level: s electrons shield p,d,and f electrons, p electrons shield d and f electrons, and d electrons shield f electrons from some of the nuclear charge. "s" electrons are the most penetrating followed by p,d, and f electrons of a given principal energy level.
We began to explain the first of five or six major periodic trends. Of course, we will explain any and all exceptions in a perfectly normal, perfectly logical manner. Good times.