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Electron Location: Part III. Electron Configuration. 4f 4d 4p 4s. 14 (7). 10 (5). = sub-level = max. # of electrons = # of electrons = number of orbitals. 6 (3). 32. 2 (1). 3d 3p 3s. 10 (5). 6 (3). 2 (1). 18. 2p 2s. 6 (3). 2 (1). 8. 1s. 2 (1). 2. - PowerPoint PPT Presentation
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Electron Location: Part III
Electron Configuration
Principle Quantum # (n)LEVEL/SIZE 1 2 3 4
Angular Quantum # (l)
ORBITAL SHAPE or
SUBLEVEL
s s p s p d s p d f
Magnetic Quantum #
(m)AXIS/
ORIENTATION
or ORBITALS
1
only 1 orbital
1 3
4 totalorbitals
1 3 5
9 total orbitals
1 3 5 7
16 total orbitals
Spin Quantum # (s)
DIRECTION OF
ELECTRON SPIN
2 e- 8 e- 18 e- 32 e-
Table 3-6b Orbitals and Electron Capacity of the First Four Principle Energy Levels
Principle energy level (n)
Type of sublevel
Number of orbitals per type
Number of orbitals
per level(n2)
Maximum number of electrons
(2n2)
1 s 1 1 2
2s 1
4 8p 3
3
s 1
9 18p 3
d 5
4
s 1
16 32p 3
d 5
f 7
1s
2p
2s
3d
3p
3s
4f
4d
4p
4s
2 (1)
2 (1)
2 (1)
6 (3)
6 (3)
2 (1)
6 (3)
10 (5)
14 (7)
10 (5)
2
32
18
8
= sub-level= max. # of electrons= # of electrons= number of orbitals
Principal Energy LevelsPrincipal Energy LevelsPrincipal energy level
Number of sublevels
Type of sublevel and (# of orbitals)
n = 1 1 1s
n = 2 2 2s (1) 2p (3)
n = 3 3 3s (1) 3p (3) 3d (5)
n = 4 4 4s (1) 4p(3) 4d(5)
4f (7)
“Rules” for Writing Electron Configurations a method of writing where electrons are
found in various orbitals around the nulcei of atoms. three rules in order to determine this:
1. aufbau principle
2. Pauli exclusion principle
3. Hund’s rule
Aufbau Principle electrons occupy the orbitals of the
lowest energy first each written represents an atomic
orbital (such as or or or ….) electrons in the same sublevel have equal
energy ( ) principle energy levels (1,2,3,4..) can
overlap one anotherex: 4s orbital has less energy than a 3d orbital
“know” these two exceptions to the Aufbau principle! (There are many others at the bottom of the table that we won't memorize)
Cr we would predict: 1s2 2s2 2p6 3s2 3p6 4s2 3d4
but it is actually:1s2 2s2 2p6 3s2 3p6 4s13d5
Cu we would predict: 1s2 2s2 2p6 3s2 3p6 4s2 3d9
but it is actually:1s2 2s2 2p6 3s2 3p6 4s1 3d10
Pauli Exclusion Priciple
only two electrons in an orbitalmust have opposite spins represents one electron represents two electrons in an orbital
Hund’s Rules every orbital in a subshell must have one
electron before any one orbital has two electrons
all electrons in singly occupied orbitals have the same spin.
Order of ElectronsOrder of Electrons
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
Writing Electron Configurations To write out the electron configuration of an
atom:use the principal quantum number/energy
level (1,2,3, or 4…) use the letter term for each sub-level (s,p,d, or f); use a superscript number indicates how many
electrons are present in each sub-level hydrogen =1s1. Lithium =1s22s1.
don’t write anything for spin (yet)
Orbital Energy DiagramsOrbital Energy Diagrams
http://colossus.chem.umass.edu/genchem/whelan/class_images/Orbital_Energies.jpg
Carbon Carbon
Atomic # - 6 Atomic # - 6
Orbital Energy DiagramsOrbital Energy Diagrams
http://colossus.chem.umass.edu/genchem/whelan/class_images/Orbital_Energies.jpg
NeonNeon
Atomic # - 10 Atomic # - 10
Orbital Energy DiagramsOrbital Energy Diagrams
http://colossus.chem.umass.edu/genchem/whelan/class_images/Orbital_Energies.jpg
ScandiumScandium
Atomic # - 21Atomic # - 21
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