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Chapter 6 - Quantum Mechanics
Chapter 7 - Periodic Table
Chapter 6
Atomic Orbitals …
Number
n
l
ml
ms
Name
Principle
Quantum
Number
Angular
Momentum
Quantum
Number
Magnetic
Quantum
Number
Spin
Quantum
Number
Description
energy level
(i.e.; Bohr’s
Theory)
general
(number) shape
of the orbitals
3-D orientation
of the orbital
spin of the
electron
Legal Quantum Numbers …
(4 , 1 , 0 , +1/2)
(5 , 3 , 3 , -1/2)
(2 , 2 , 1 , +1/2)
legal
legal
illegal
Meaning
n=
1,2,3,4,5,6,7
Mathematics
n= 1,2,3,4,…
l = s, p, d, f
l = n-1
(s =0, p =1
d =2, f =3)
s=1, p=3, d=5,
f=7
clockwise or
counterclockwise
ml = 2l + 1
ms = +1/2
or –1/2
Meaning … ___________________
Meaning … ___________________
Filling Order of the Orbitals … use the diagonal rule (some exceptions do occur).
1s
2s
2p
Start with 1s and follow the arrows.
3s
3p 3d
Maximums: s = 2, p = 6, d = 10, f = 14
4s
4p 4d 4f
5s
5p 5d 5f
6s
6p 6d
7s
7p
Example: Bromine has 35 e-‘s
1s22s22p63s23p64s23d104p5
or … [Ar]4s23d104p5
This is known as electron configuration.
Orbital Notation and Hund’s Rule …
Hund’s Rule … Each sub-orbital may hold 2 electrons with opposite spins.
1s
Phosphorus (17 e-‘s)
2s
2p
3s
3p
Three unpaired electrons in the valence shell.
Diamagnetism and Paramagnetism …
Paramagnetic, attracted by a magnet.
Diamagnetism, repelled by a magnet.
General rule: Any element with an odd-electron number must be paramagnetic.
Shielding … describes why some orbitals are at higher or lower energy levels than others.
Example: A 2s electron spends more of its time (on average) around the nucleus than a 2p electron due to
the size of the orbitals. The 2s is said to be more “penetrating” than the 2p, and is less shielded
by the 1s electrons. See attachment.
Lanthanide Contraction … The atomic radius does not follow the trend established in previous periods.
Chapter 7
Periodic Table Trends
Physical Properties …
Atomic Radius
Ionic Radius
Ionization Energy
Electron Affinity
Chemical Properties …
Hydrogen
Group 1A
Group 2A
Group 3A
Group 4A
Group 5A
Group 6A
Group 7A
Group 8A
Increases as you move LEFT or DOWN
Increases as you move DOWN, Small in full or ½ full orbitals
Decreases as you move DOWN, High in full or ½ full orbitals
Decreases as you move DOWN, High in almost full orbitals, low in full
orbitals
Metal or a non-metal (ox. no. of +1 and –1)
Metal w/ox. no. of +1, increase reactivity down table, Rx with water
To form H2, forms oxides or peroxides when Rx with O2
Metal w/ox. no. of +2, react with acid to form H2, may Rx with O2
Metal w/ox. no. of +3, reacts with Acid and O2, heavier elements
somewhat inert
Metalloids w/ox. no. of +4 or –4, will not react with H2O, may react
with acid
First 2 are nonmetals, later are metalloids. Wide variation with ox. no.
First 3 are nonmetals, later are metalloids. Commonly –2 ox. no.
Very reactive with numerous compounds possible.
Most reactive non-metals. Commonly, -1 ox. no.. React with H to form
hydrogen halides.
Noble gases. Reactive only in extreme situations. NOT INERT.
Oxide Properties Across a Period …
Na2O Ionic, Basic
MgO
Ionic, Basic
Al2O3 Ionic, Amphoteric
SiO2
Molecular, Acidic
P4O10 Molecular, Acidic
SO3
Molecular, Acidic
Cl2O7 Molecular, Acidic