Friday, November 30, 2007
Fri-Day 1
Bio- we illustrated some diagrams of the cross-section of a leaf noting the structure and function of each part or layer.
Yes, the diagrams did not exactly match the illustrations that I posted BUT you must develop the skill of recognizing features contained in various drawings of a given structure. It's best to practice this in class when you are not being penalized for a wrong answer and when you can correct your mistakes by asking questions.
For those who are still unsure about today's handouts, I am posting answers to those handouts on Blackboard. Check them out this weekend.
We then finished our "Factors That Affect Photosynthesis" Lab noting the effect of increasing light intensity and increasing carbon dioxide concentration on the photosynthetic rate in Elodea (by measuring the oxygen production rate).
Next week, we will finish Cellular Respiration and then we will compare and contrast Photosynthesis and Cellular Respiration.
On Monday, the outline of text section 9.2 is due.
Chem 7- we discussed the quantum mechanical model of the atom, which takes into account the wave nature AND the particle nature of the electron as well as the electron-electron repulsion interactions. The end result is the calculation of all possible electron energies and of all possible electron transitions from any excited state to the ground state in atoms of any element. Thus, all spectral line for each element are predicted and associated with specific electron transitions (jumps) between two energy SUBLEVELS. We also learned that a given electron that has a specific sublevel of energy can be found in a specific shaped region of probability called an ORBITAL (which is NOT an orbit- electrons do not move in "orbits"; electrons are WAVES and thus do not have a specific location like a planet in orbit!). The trick is to remember that the "s" sublevel of energy only has one orbital, the "p" sublevel of energy has THREE equal-electron energy orbital regions, the "d" sublevel has FIVE equal-electron energy orbitals, and the "f" sublevel has SEVEN equal-electron energy orbitals. You must also know that the number of sublevels OF a principal energy level is EQUAL to the principal energy level number e.g. the n=3 (third) Principal Energy Level has THREE sublevels of electron-energy, the "s", the "p", and the "d", in increasing order of energy.
We also saw how to figure the relative energies of the various sublevels by drawing diagonal lines through the various horizontally-listed sublevels (see notes). These relative energies are calculated via the Schroedinger Equation (which is far too difficult for us to even look at).
We then practiced writing, for several elements:
ORBITAL DIAGRAMS (with the boxes, representing orbitals, and the arrows, representing electrons).
Quantum Mechanical ELECTRON CONFIGURATIONS, which show the number of electrons (using a superscript) in each OCCUPIED sublevel in an atom.
You MUST practice both of these notations this weekend and you are responsible for any hw question that involves these.
The homework packet is due on Monday and the only hw questions that are optional (won't be graded) are those that we did not cover yet in class, i.e. Lewis Dot Diagrams.
Our Atomic Concepts Unit Exam is on Wednesday.
Chem 8/9- we discussed the quantum mechanical model of the atom, which takes into account the wave nature AND the particle nature of the electron as well as the electron-electron repulsion interactions. In an astonishing experiment, JJ Thomson's son, showed that electrons have a "wave nature" in addition to their particle nature. Thus, any model that treats the electron solely as a particle is incomplete and not as accurate as it could be.
These problems led to a mathematical solution to finding all of the allowed specific energies of each electron in each element; the mathematical solutions resulted in the development of the quantum/wave mechanical model of the atom. The end result is the calculation of all possible electron energies and of all possible electron transitions from any excited state to the ground state in atoms of any element. Thus, all spectral line for each element are predicted and associated with specific electron transitions (jumps) between two energy SUBLEVELS. We also learned that a given electron that has a specific sublevel of energy can be found in a specific shaped region of probability called an ORBITAL (which is NOT an orbit- electrons do not move in "orbits"; electrons are WAVES and thus do not have a specific location like a planet in orbit!). The trick is to remember that the "s" sublevel of energy only has one orbital, the "p" sublevel of energy has THREE equal-electron energy orbital regions, the "d" sublevel has FIVE equal-electron energy orbitals, and the "f" sublevel has SEVEN equal-electron energy orbitals. You must also know that the number of sublevels OF a principal energy level is EQUAL to the principal energy level number e.g. the n=3 (third) Principal Energy Level has THREE sublevels of electron-energy, the "s", the "p", and the "d", in increasing order of energy.
We also saw how to figure the relative energies of the various sublevels by drawing diagonal lines through the various horizontally-listed sublevels (see notes). These relative energies are calculated via the Schroedinger Equation (which is far too difficult for us to even look at).
We then practiced writing, for several elements:
ORBITAL DIAGRAMS (with the boxes, representing orbitals, and the arrows, representing electrons).
Quantum Mechanical ELECTRON CONFIGURATIONS, which show the number of electrons (using a superscript) in each OCCUPIED sublevel in an atom.
Lewis Dot Diagrams, which show the number of VALENCE ELECTRONS (ONLY the HIGHEST number PRINCIPAL energy level electrons!) in an atom of a given element.
You MUST practice these this weekend and you are responsible for any hw question that involves today's material.
Reminder, the homework packet is due on Monday. Our Atomic Concepts unit exam is on Wednesday.
Yes, the diagrams did not exactly match the illustrations that I posted BUT you must develop the skill of recognizing features contained in various drawings of a given structure. It's best to practice this in class when you are not being penalized for a wrong answer and when you can correct your mistakes by asking questions.
For those who are still unsure about today's handouts, I am posting answers to those handouts on Blackboard. Check them out this weekend.
We then finished our "Factors That Affect Photosynthesis" Lab noting the effect of increasing light intensity and increasing carbon dioxide concentration on the photosynthetic rate in Elodea (by measuring the oxygen production rate).
Next week, we will finish Cellular Respiration and then we will compare and contrast Photosynthesis and Cellular Respiration.
On Monday, the outline of text section 9.2 is due.
Chem 7- we discussed the quantum mechanical model of the atom, which takes into account the wave nature AND the particle nature of the electron as well as the electron-electron repulsion interactions. The end result is the calculation of all possible electron energies and of all possible electron transitions from any excited state to the ground state in atoms of any element. Thus, all spectral line for each element are predicted and associated with specific electron transitions (jumps) between two energy SUBLEVELS. We also learned that a given electron that has a specific sublevel of energy can be found in a specific shaped region of probability called an ORBITAL (which is NOT an orbit- electrons do not move in "orbits"; electrons are WAVES and thus do not have a specific location like a planet in orbit!). The trick is to remember that the "s" sublevel of energy only has one orbital, the "p" sublevel of energy has THREE equal-electron energy orbital regions, the "d" sublevel has FIVE equal-electron energy orbitals, and the "f" sublevel has SEVEN equal-electron energy orbitals. You must also know that the number of sublevels OF a principal energy level is EQUAL to the principal energy level number e.g. the n=3 (third) Principal Energy Level has THREE sublevels of electron-energy, the "s", the "p", and the "d", in increasing order of energy.
We also saw how to figure the relative energies of the various sublevels by drawing diagonal lines through the various horizontally-listed sublevels (see notes). These relative energies are calculated via the Schroedinger Equation (which is far too difficult for us to even look at).
We then practiced writing, for several elements:
ORBITAL DIAGRAMS (with the boxes, representing orbitals, and the arrows, representing electrons).
Quantum Mechanical ELECTRON CONFIGURATIONS, which show the number of electrons (using a superscript) in each OCCUPIED sublevel in an atom.
You MUST practice both of these notations this weekend and you are responsible for any hw question that involves these.
The homework packet is due on Monday and the only hw questions that are optional (won't be graded) are those that we did not cover yet in class, i.e. Lewis Dot Diagrams.
Our Atomic Concepts Unit Exam is on Wednesday.
Chem 8/9- we discussed the quantum mechanical model of the atom, which takes into account the wave nature AND the particle nature of the electron as well as the electron-electron repulsion interactions. In an astonishing experiment, JJ Thomson's son, showed that electrons have a "wave nature" in addition to their particle nature. Thus, any model that treats the electron solely as a particle is incomplete and not as accurate as it could be.
These problems led to a mathematical solution to finding all of the allowed specific energies of each electron in each element; the mathematical solutions resulted in the development of the quantum/wave mechanical model of the atom. The end result is the calculation of all possible electron energies and of all possible electron transitions from any excited state to the ground state in atoms of any element. Thus, all spectral line for each element are predicted and associated with specific electron transitions (jumps) between two energy SUBLEVELS. We also learned that a given electron that has a specific sublevel of energy can be found in a specific shaped region of probability called an ORBITAL (which is NOT an orbit- electrons do not move in "orbits"; electrons are WAVES and thus do not have a specific location like a planet in orbit!). The trick is to remember that the "s" sublevel of energy only has one orbital, the "p" sublevel of energy has THREE equal-electron energy orbital regions, the "d" sublevel has FIVE equal-electron energy orbitals, and the "f" sublevel has SEVEN equal-electron energy orbitals. You must also know that the number of sublevels OF a principal energy level is EQUAL to the principal energy level number e.g. the n=3 (third) Principal Energy Level has THREE sublevels of electron-energy, the "s", the "p", and the "d", in increasing order of energy.
We also saw how to figure the relative energies of the various sublevels by drawing diagonal lines through the various horizontally-listed sublevels (see notes). These relative energies are calculated via the Schroedinger Equation (which is far too difficult for us to even look at).
We then practiced writing, for several elements:
ORBITAL DIAGRAMS (with the boxes, representing orbitals, and the arrows, representing electrons).
Quantum Mechanical ELECTRON CONFIGURATIONS, which show the number of electrons (using a superscript) in each OCCUPIED sublevel in an atom.
Lewis Dot Diagrams, which show the number of VALENCE ELECTRONS (ONLY the HIGHEST number PRINCIPAL energy level electrons!) in an atom of a given element.
You MUST practice these this weekend and you are responsible for any hw question that involves today's material.
Reminder, the homework packet is due on Monday. Our Atomic Concepts unit exam is on Wednesday.
# posted by C @ 6:58 PM 
