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tales to tell.

March 25, 2009

Atomic Structure lessons.

I wasn't prepared for the first lesson, but I was able to follow Mr Tan quite well. The first lesson was pretty much about recalling the basic concepts from my O-levels. I know about isotopes, the sub-atomic particles (mass and charge of protons, neutrons and electrons) but when he came to the s, p, f, d, I got more attentive.

To be able to keep up with the lesson, I went back and did some research, but I was unable to understand anything.

So for the second lesson I was quite confused most of the time. Thanks to the new student Cindy, I somehow managed to keep up with the lesson. This reminds me about the post we did on our strength and weakness in Chemistry. I'm going to add in: strength - I'm a fast and quick learner. A sudden newfound talent.

Using the website (http://www.chemguide.co.uk/atoms/propsmenu.html#top) on the last page of the IT Activity worksheet that was given out today, I went to do more research on this topic...

(Half an hour later)

I think Cindy's explaination is easier to understand than all those research notes. Maybe I should 'interview' her on this topic to compile my notes. Haha.

- - -
Update (27/3/09).

I used my most trusted research website Wikipedia to collate my notes. And I finally understood the topic. Cheers.

Important terms related to this topic:

The orbital names (s, p, d, f) are derived from the characteristics of their spectroscopic lines: sharp, principal, diffuse and fundamental.
(Source - http://en.wikipedia.org/wiki/Atomic_orbital)

The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. It is also referred to as the screening effect or atomic shielding.
(Source - http://en.wikipedia.org/wiki/Screening_effect)

Elaboration:
Electrons that are nearer to the nucleus has higher energy compared to the electrons further away from the nucleus. This is because the electrons nearer to the nucleus intercept the energy to reach the electrons further away from the nucleus. Thus we can conclude that as the number of inner electrons increase, the shielding effect increases.
(Source - borrowed lecture notes collated by teacher from a student of Raffles Junior College)

Quantum chemistry is a branch of theoretical chemistry, which applies quantum mechanics and quantum field theory to address issues and problems in chemistry. The description of the electronic behavior of atoms and molecules as pertaining to their reactivity is one of the applications of quantum chemistry. Quantum chemistry lies on the border between chemistry and physics, and significant contributions have been made by scientists from both fields. It has a strong and active overlap with the field of atomic physics and molecular physics, as well as physical chemistry.

Quantum chemistry mathematically describes the fundamental behavior of matter at the molecular scale. It is, in principle, possible to describe all chemical systems using this theory. In practice, only the simplest chemical systems may realistically be investigated in purely quantum mechanical terms, and approximations must be made for most practical purposes (e.g., Hartree-Fock, post Hartree-Fock or Density functional theory, see computational chemistry for more details). Hence a detailed understanding of quantum mechanics is not necessary for most chemistry, as the important implications of the theory (principally the orbital approximation) can be understood and applied in simpler terms.
(Source - http://en.wikipedia.org/wiki/Quantum_chemistry)

Bohr model is a primitive model of the hydrogen atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics, and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems, the Bohr model is still commonly taught to introduce students to quantum mechanics, before moving on to the more accurate but more complex valence shell atom.
(Source - http://en.wikipedia.org/wiki/Bohr_Model)

Diagram on s, p, d, f:




Note: this topic is very closely related to quantum physics.
by ツバサ at 11:40:00 PM
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