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Introduction to Quantum Mechanics Graded A+
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Introduction to Quantum Mechanics Graded A+ Back to Bohr: Bohr gave us Quantization Quantization means electrons can only exist in certain discrete energy levels (like a staircase, they can only completely be on the first or second stair but never in between stairs different distances from ...

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  • October 11, 2024
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  • 2024/2025
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Introduction to Quantum Mechanics Graded A+

Back to Bohr: Bohr gave us ✅Quantization



Quantization means ✅electrons can only exist in certain discrete energy levels

(like a staircase, they can only completely be on the first or second stair but never in between stairs -
different distances from ground)



If you recall rings= ✅orbits



e- must be in a _______ and e- are different distances(or E) from ________ ✅orbit; nucleus



Bohr was Bad: Bohr model of the atom could predict the ____________ ____________ of
_____________ ✅Emission Spectrum of Hydrogen



Bohr's model failed because the model needed to know the position, **Cant locate the _______
_______ (Model failed except for hydrogen) ✅electrons precisely



Electron is somewhere, we don't know location for sure but we know it is in a __________ _______,
detecting where probably is ✅certain orbital



It failed because the electrons are the same distance from the nucleus. Model needed to know -> ✅the
position and momentum of electron, you cant know this



Heisenberg Uncertainty Principle (Bohr=orbit, Quantum m= orbitals): It is impossible to know ✅the
position(location) and momentum(speed) of the electron at the same time



Orbitals: a region of space where ✅you are most likely (90%) to find the electron you are looking for

, -Most likely to find electron at center (dark blue bit), this is called the ___ ________, the "_" tells us the
shape is spherical ✅1st Orbital; s



Principle Energy Levels-> Quantization gives us Principle Energy Levels(Bohr)

-Denoted by whole #s (ex. 1,2,3,4, etc,)

-Each of these levels is divided into ________ ✅Sublevels



Look at notes to compare Bohr and Quantum Mechanics Model ✅(Bohr is normal method with rings
and "Xs" for electrons, with quantum it is EX. 1s2)



1s^2 (1-1st layer, s=orbital, 2 electrons) this is the _______ _________ _______. ✅Principle Quantum
Number



An s orbital can only hold 2 electrons soooo in addition to s orbitals there are __________ ✅p-orbitals



P-orbitals: __ options, each hold __ e-, total-> 6e- ✅3 options, 2e-



D-orbitals__ options, each hold __ e-, total-> 10e- ✅5 options, 2e-



Boron has 5 e-, sooooooo it would be ✅1s2 2s2 2p1



This leads to a filling order of ✅1s2 2s2 2p6 3s2 3p6 4s2



Examples: Mg-> 12 e- -> ✅1s2 2s2 2p6 3s2



Ca -. 20 e- -> ✅1s2 2s2 2p6 3s2 3p6 4s2



What about the D-orbitals? After 4s2, elements can start to have e- in d-orbitals, elements in ___
___________ __ ____ ✅row 4 and below

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