[AngelShare]

I have to, again, take notes but the link I was provided with won't work for one part so...help? :roll: (I absolutely love the smilies on this site. :daisy:)

Take notes on information that relates to the location and structure of the electron in the atom, electron energy levels, and electron configuration within the atom.

[AngelShare]

Aha, two hours later and I think I've got it!:Lighten:

The electrons in an atom circle the nucleus in orbitals. The s orbital can hold 2 electrons, the p orbital can hold 6 electrons, and the d orbital can hold 10. As for f, I don't think I'll be needing it but if someone wants to reply and just mention how many it holds, it might be helpful later.:clap2:

As for the energy levels, the closer to the nucleus the orbital is, the weaker it is so 1s is weaker than 4s for instance, right? Would that be because of the protons in the nucleus?

Then, where they are...hm...it would go, out from the nucleus, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc. right? If not, could someone help? Why does it go from 4s to 3d? Why 3?

Hm, I think that's all I have to ask/say right now...:biggrin2:

EDIT: Ah, wait, one more...I can't find this last one for the life of me.

According to the Bohr model, what determines the color of light emitted when an electron moves from one energy level to another?

[Donaldson Tan]

The electrons in an atom circle the nucleus in orbitals.

An orbital is a region of space whereby there is at least 95% probability of finding an electron. An orbital is not a path but a volume of space. In fact, the path of the electron is found inside the orbital.

The s orbital can hold 2 electrons, the p orbital can hold 6 electrons, and the d orbital can hold 10. As for f, I don't think I'll be needing it but if someone wants to reply and just mention how many it holds, it might be helpful later.

You quoted the energy levels correctly. There is 1 orbital in the s energy level, 3 orbitals in the p energy level, 5 orbitals in the d energy level, 7 orbitals in f energy level, etc. Each orbital holds a maximum of 2 electrons. Therefore, the 1s subshell holds up to 2 electrons, the 2p subshell holds up to 6 electrons..

As for the energy levels, the closer to the nucleus the orbital is, the weaker it is so 1s is weaker than 4s for instance, right? Would that be because of the protons in the nucleus?

Lower energy level does not translate to weaker energy level. Lower energy level = higher stability, ie. an electron is the 1s energy level is more likely to remain in its original energy level than an electron in the 4s energy level. This is due to stronger attraction between the electron and nucleus (because the lower energy level electrons are closer to the nucleus) and electrons furthur away from the nucleus experience repulsion from inner-core electrons, thus they are easier to be removed.

[Donaldson Tan]

According to the Bohr model, what determines the color of light emitted when an electron moves from one energy level to another?

energy levels are quantised, so the energy of the photon will correspond to transition of the energy levels. given that E = hf, therefore the frequency of the photon will be of a particular frequency that corresponds to the energy of the photon. The frequency dictates the colour of the photon.