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
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
