chapter 10 quantum numbers and shapes. chpt 10 – quantum numbers an orbital is an orientation in...
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Chapter 10
Quantum Numbers and Shapes
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Chpt 10 – Quantum Numbers
An orbital is an orientation in space, so a series of steps (quantum numbers) are used to describe various properties of the orbital. The steps are:
1. principal energy level2. sublevels3. orbital's4. electron spin
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Chpt 10 – Quantum Numbers
1. principal energy level Has whole numbers (1, 2, 3,…) that relate to
the size and energy of the orbital. The orbital becomes larger with an increase in
the principle energy level number, thus the electron spends more time away from the nucleus.
The energy is higher because the electron is not as tightly bound by the nucleus.
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Chpt 10 – Quantum Numbers
2. sublevel’s “s” sublevels *contains 1 orbital “p” sublevels *contains 3 orbitals “d” sublevels *contains 5 orbitals “f” sublevels *contains 7 orbitals
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Chpt 10 – Quantum Numbers
3. orbital’s Relates to the orientation of the orbital in
space. (Example: (p-sublevel) x, y, z) An orbital is the area that there is a 90%
chance of finding the electron in that area. The orbital’s of different sublevels have
different shapes based upon mathematical models.
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nodes
90% boundary:Inside this lies90% of the probability
S orbitals are spherical in shape
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P-orbitals
Node at nucleus
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The Boundary Surface Representations of All Three 2p Orbitals
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The Boundary Surfaces of All of the 3d Orbitals
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Representation of the 4f Orbitals in Terms of Their Boundary Surfaces
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1
s
E
2
s
2p3
s
3p
3d4
s
4p5
s
4d
Remember the energies are < 0
THE MULTI-ELECTRON ATOM ENERGY LEVEL DIAGRAM
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Sublevels and orbitals based on the Periodic Table
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Alternative Periodic Table
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THE BUILDING-UP PRINCIPLE.
assign electrons to orbitals one at a time
lowest energy electronic configuration
Electrons go into the available orbital of lowest energy.At least one electron is in each orbital of a sublevel before a second electron is added to the orbital.
A maximum of two electrons per orbital.
ELECTRONIC CONFIGURATIONS
GROUND STATE
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Order of Filling Orbitals
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THE AUFBAU (BUILDING-UP) PRINCIPLE:
The electron configuration of any atom or
ion…....
electrons are added to hydrogen-like atomic orbitals in order of increasing energy
can be represented by an orbital diagram
1
s
E
2
s
2p3
s
3p
3d4
s
4p5
s
4d
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1s 2s 2p
He:
Hydrogen has its one electron in the 1s
orbital: 1s 2s 2p
H:
1s 2s 2p
He:
1s1
ORBITAL DIAGRAM
with opposite spins:
both occupy the 1s orbitalPauli principle
Helium has two electrons:
1s2
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Hydrogen has its one electron in the 1s
orbital: 1s 2s 2p
H:
1s 2s 2p
He:
1s 2s 2p
He:
helium ground
state
Helium has two electrons:
1s1
1s12s1
1s2
ORBITAL DIAGRAM
Now onto the next atoms
Helium can also exist in an excited state such as:
with opposite spins:
both occupy the 1s orbitalPauli principle
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Lithium has three electrons, so it must use the
2s orbital:
Beryllium has four electrons, which fill both the
1s and 2s orbitals:
Boron’s five electrons fill the 1s and 2s orbitals,
and begin to fill the 2p orbitals. Since all three
are degenerate, the order in which they are
filled does not matter.
1s 2s 2p
Li: 1s22s1
1s 2s 2p
Be: 1s2 2s2
1s 2s 2p
B: 1s22s22p1
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1s 2s 2p
C: 1s22s22p2
1s 2s 2p
C: 1s22s22p2
How can we decide?????
A CHOICE
OR
CARBON Z=6
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HUND’S RULEFOR THE GROUND STATE
ELECTRONS OCCUPY DEGENERATE ORBITALS SEPARATELY
THE SPINS ARE PARALLEL
SO FOR CARBON THE GROUND STATE IS
1s 2s 2p
C: 1s22s22p2
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1
s
E
2
s
2p3
s
3p
3d4
s
4p5
s
4d
ENERGY LEVEL DIAGRAM FOR A MULTI-ELECTRON ATOM
BROMINE ELECTRONIC CONFIGURATION
[Ar] 4s23d104p5
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The valence electron configuration of the
elements in the periodic table repeat
periodically! H He1s1 1s2
Li Be B C N O F Ne2s1 2s2 2p1 2p2 2p3 2p4 2p5
2p6
Na Mg Al Si P S Cl Ar3s1 3s2 3p1 3p2 3p3 3p4 3p5
3p6
Every element in a group
hasthe same valence electron configuration!
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Chpt 10 – Quantum Numbers Electron Spin
4. electron spin The concept of electron spin was developed
to account for a magnetic moment. Classical physics indicates that a moving
(spinning) charge produces a magnetic moment (field).
Opposite spins produce opposite magnetic fields.
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Electron Spin
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In silver (and many other atoms) there is one more “spin up” electron than“spin down” or vice versa. This means that an atom of silver can interact with a magnetic field and be deflected up or down, depending on which type of spinis in excess.
This 2-valued electron spin can be shown in an experiment
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Transition Metal Demonstration
dsArZnelectrons
dsArZnelectrons
dsArFeelectrons
dsArFeelectrons
dsArMnelectrons
dsArMnelectrons
dsArCrelectrons
dsArCrelectrons
34_28
34_30
34_23
34_26
34_23
34_25
34_21
34_24
2
2
2
3
The chromium, manganese, and iron ions will exhibit magnetic character because of the high number of unpaired electrons in the 3d orbitals.Will zinc show any magnetic character?