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Rutherford. Quantum Mechanics. Through the Looking Glass. This is how the model of the atom has developed so far:. Bohr-Planetary Model. Correcting Bohr’s Planetary Model. …using the Photoelectric Effect. then why can’t particles have a wavelike nature?. Louis DeBroglie’s insight:. - PowerPoint PPT Presentation
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Quantum MechanicsThrough the Looking Glass
Rutherford Bohr-Planetary Model
This is how the model of the atom has developed so far:
Louis DeBroglie’s insight:If light radiation can have a particle nature
then why can’t particles have a wavelike nature?
If electrons are particles
Electrons must have a wavelike nature
= h mv
Werner Heisenberg (1901-1976)
There is an uncertainty in either the position or the momentum of an electron that cannot be reduced beyond a certain minimum level
Heisenberg’s Uncertainty Principle
Is Shrodinger’s cat dead or alive?
The Quantum Mechanical Model
Describes the wave properties of electrons
and regions of space surrounding the nucleus
Called orbitals
Where there is a high probability offinding electrons
Describing an electron’s address
Bohr’s model places the electron ina quantum energy level (n)
Bohr-Planetary Model
Describing an electron’s addressusing the Quantum Mechanical Model
Electrons exist in orbitals
A collection of orbitals with the same energyis called an electron shell designated (n)
1st quantum #-principle quantum number (n) n = (1,2,3,…, ) describes shell or energy level
Describing an electron’s addressusing the Quantum Mechanical Model
2nd quantum # - azimuthal number (l), value 0 to n-1 describes sublevel
3rd quantum # - magnetic number (ml), value = l to 0 to-l The orientation of the orbital in space
4th Quatum # - Spin (ms), value is + or – ½, describes the spin
The first energy level (n = 1) is constructed from a single orbital (l = 0), also designated ‘1s’,
which is spherical ( ml = 0)
The second energy level (n = 2) is constructed from a single orbital (l = 0) also designated ‘2s’
which is spherical ( ml = 0)
The third energy level (n = 3) is constructed from a single orbital (l = 0) also designated ‘3s’
which is spherical ( ml = 0)
Energy level ‘n = 2’ is more complex than energy level ‘n =1’ and is constructed from
two kinds of orbitals
The innermost part of ‘n =2’ consists of asingle spherical orbital designated ‘2s’
The outermost part of ‘n = 2’ consists of three orbitals which are not spherical, (l = 1)
Each dumbbell-shaped orbital (l = 1), also designated ‘2px, 2py,2pz’is oriented along
the x, y, and z axes ( ml = -1, 0, 1)
Like the ‘s’ orbital, the ‘p’ orbitals also repeat in subsequent energy levels
Energy level ‘n = 3’ is more complex than energy level ‘n =1’ or ‘n = 2’ and consists of an
innermost spherical orbital designated ‘3s’
The middle part of ‘n = 3’ consists of three dumbbell-shaped orbitals , (l = 1)
The outermost part of ‘n = 3’ consists of five orbitals which are also not spherical, (l = 2)
Each four-lobed orbital (l = 2), also designated ‘3 d orbital ’is oriented along different
planes ( ml = -2, -1, 0, 1, 2)
Like the ‘s’ and ‘p’ orbitals, the ‘d’ orbitals also repeat in subsequent energy levels
Energy level ‘n = 4’ is more complex than energy level ‘n =1, 2, or 3’ and consists of an
innermost spherical orbital designated ‘4s’
The lower middle part of ‘n = 4’ consists of three dumbbell-shaped orbitals , (l = 1)
The upper middle part of ‘n = 4’ consists of five orbitals which are also not spherical, (l = 2)
The outermost part of ‘n = 4’ consists of seven orbitals, also designated ‘f ’ orbitals, which are also not spherical, (l = 3)
In fact, they are a real
nightmarenightmare ( ml = -3, -2, -1, 0, 1, 2, 3)
Quantum Mechanics: Where ever you go...there you are!
Schwartzchild’s Radical
which of the following is not an allowable quantum number1. 4,4,3,1/22. 3,2,2,13. 5,2,-1,-1/2
What are the maximum number of electrons allowed that have the quantum
numbers designated?1. n=32. n=3, l=23. n= 3, l=2, ml = 1
4. n= 3, l=2, ml = 1, ms = 1/2
Which of the following are in an excited state and what element do they represent?
1. 1s22s22p63p64s23d104p65s24d105p6