Gemini Plamoottil 12/9/13

12/9/13- IN CLASS NOTES

• We checked in our hw worksheet. 
• We taped in 6 handouts, which all can be found on moodle in the handouts section 

We took some notes (WE ALSO ADDED A FEW NOTES TO THE NOTES THAT WE TOOK ON FRIDAY: 

•  Just some of the ADDITIONAL NOTES (Mrs. Friedman posted a cleaner version of her original notes on moodle and they are more detailed as well, so be sure to check that out).

A QUANTUM IS A SPECIFIC AMOUNT... AS IN A SPECIFIC AMOUNT OF ENERGY LIKE A STEP. SINCE THE ELECTRONS JUMP AND FALL IN SPECIFIC QUANTUM THEY RELEASE THE LINE SPECTRA THAT BOHR STUDIED.

1. Electrons like to be as low in energy as possible- the closer to the nucleus the lower the energy and this is called GROUND STATE 
2. Electrons absorbs energy (from an electric current for example) and that pushes it to a higher energy level which is called EXCITED STATE
3. Electron prefers to be at a low energy state, so it falls back down to the ground state. 
4. The electron releases the energy it absorbed as a wavelength of light. Then it falls a specific number of "energy levels", it always releases the same wavelength (energy) of light. 

Todays Notes: BOHR MODEL AND BEYOND CONTINUED..........

       To Summarize---- Electrons jump to higher energy levels when you put more energy in them (like electricity), then they release the extra energy as light when they fall back to GROUND STATE. 

"WAVELENGTH" of light released depends on how many levels the electron jumps and falls. 

~DeBroglie and Shroedinger 

• GO back to Einstein: A wave can act like a particle. What if an electron can act like a wave? 
• This one is n=3 (which is number of crests) ------>THIS WAVELENGTH WORKS!!!

• This one is n=5 (which is number of crests) ---------> THIS WAVELENGTH WORKS!! 

IF One has n= 3.5 then the wavelength does not work because the numbers can only be whole #'s. 

• These wave functions are called orbitals: Areas where you will probably find an electron. 

HEISENBERG- His contribution was "uncertainty principle" - ( You can't know an electron's position and momentum at the exact same time. ( All you can know is the orbital) 

• Orbitals: Areas of probability where you are likely to find an electron (However they have different shapes) 

This is an "S" orbital: 

It remains the same shape except the "bubble" gets bigger and bigger 

Also, electrons exist on the surface of the "bubble"

Three out of four of these are "P" orbitals

So here are just some of the different orbital we talked about in class. 

• WE MUST KNOW WHERE THE ELECTRONS ARE FOR EACH ELEMENT - there are two ways to map electrons

1. Electron Configuration 
2. Orbital diagram 

Quantum #'s allow us to "address electrons". 

N= energy level (1,2,3)

How far or close to the nucleus 

The closer to the nucleus the lower the "N" is. 

• This is the symbol that represents orbital shape/type of orbital (S,P,D,or F)     

• An m with the a subscript of the symbol above = Orbital orientation ( what direction it's going in PX,PY, PV)

When N=1 ----->zero=1S orbital---->An there is one possible type of orbital

When N=2 ----> zero=2S and 1=2P----> Zero is 2S---->-1,0,+1 (Px,Py,Pz)---> 4 possible orbitals 

We did not finish all the notes in class today, so whoever the blogger is tomorrow will finish the rest of the notes. 

Today's Hw is:

Finish the 2 webassigns by 11:59 pm today( the ones that we attempted over the weekend) 

Also 2 wksh: Quantum numbers and the continuation sheet

Also, continue to do the study guide packet because it's due on the 11th I believe. 

NOW FOR SOME JOKES!!!

This  I just thought was pretty clever!!

HAHA LOL

and it's pretty sweet, AWWW

The NEXT Blogger will be Kate M ( unless someone still hasn't blogged for second quarter then it will be them :)