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Electronic Structure
Electron Configuration
•A description of the electrons in
an atom
Orbital•The space in which the electrons (e-) are likely to be found
•Max 2 e- per orbital
Rule of Electron configuration
• Number: energy level (row #)
• Letter: energy sublevel (area)
• Superscript: # of e- in sublevel
• d electrons: 1 level < row #
• f electrons: 2 levels < row #
• Show all filled sublevels
Energy Levels•Corresponds to row #
•1 - 7
•Related to size
Energy Sublevels•Corresponds to an area on the periodic table
•= nodes in orbitals
•s, p, d, f
s - electrons•Columns 1A & 2A
•Spherical orbitals
p - electrons•Col. 3A - 8A or 13 - 18
•Dumbbell shaped orbital
•3 orbitals per sublevel
•1 node
d - electrons•Cols 3B - 2B or 3 - 12
•Transition area (2 nodes)
•Double dumbbell shaped
•5 orbitals in sublevel
f - electrons•Lower removed area
•Triple dumbbell shaped
•7 orbitals per sublevel
•3 nodes
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
5s -4s -3s -2s -1s -
5p - - -4p - - -3p - - -2p - - -
4d - - - - -3d - - - - -
Ground State•All electrons are in their lowest possible energy state
Excited State•One or more electrons are not in their lowest possible energy state
Degenerate Orbitals
•Orbitals at the same energy level
List, describe, & identify the area of the Periodic Table
for each type of orbital.
Write the ECs for:•Ne
•Rb
•Tc
•As
Write the ECs for:•Si
•Ag
•Br-1
•Fe+2
Write the ECs for:•Zn
•Au
•Al+3
•Fe+3
Electron Dot Diagram•Represents the valence electrons in an atom
•Maximum 4 pairs drawn on an imaginary square around the symbol
Valence Electrons
•Electrons in the outer most energy level
•Electrons involved in chemical reactions
Draw the electron
configuration for Uranium
Octet Rule•8 electrons in the outer level is stable
•elements attempt to get eight electrons in their outer level
Column 1A•1s1, 2s1, 3s1, etc
• Na
Column 2A•1s2, 2s2, 3s2, etc
• Mg
Column 3A• 2s22p1 ,3s23p1, etc
• Al
Column 4A• 2s22p2, 3s23p2, etc
• C
Column 5A• 2s22p3, 3s23p3, etc
• N
Column 6A• 2s22p43s23p4, etc
• O
Column 7A• 2s22p53s23p5, etc
• Cl
Column 8A• 2s22p63s23p6, etc
• Ne
EC for Transition El.•4s23d1 4s23d6
•4s23d2 4s23d7
•4s23d3 4s23d8
•4s13d5 4s13d10
•4s23d5 4s23d10
Chromium & Copper Are
Kinky
Transition Dot Diagrams
•Kinky ones have a single
•All the rest have a pair
Inner Transition Dot Diagrams
•All have a pair
HW: Problems 53 – 56 on page 171
Write ECs & EDDs for:
S -16 Cu -29
Sb -51Ca+2 -20
Quantum Numbers
•A more complete description of the electrons in an atom
Quantum Numbersn : Energy level(Row)
l : Energy Sublevel
m or ml : Orientation
s or ms : Spin
Quantum Numbersn : Size
l : Shape or nodes
m or ml : Orientation
s or ms : Spin
Quantum Numbersn : 1 ---> 7
l : 0 ---> (n - 1)
m : - l ---> + l
s : + 1/2 or -1/2
Quantum Numbers•Go from the lowest to highest possibilities:
•Start n with 1, start l with 0, etc.
Quantum Numbers
H: (1,0,0,1/2)
n = 1, l = 0, m = 0, s = 1/2
He: (1,0,0,-1/2)
etc
Drill: Predict EC, QN & EDD for:
•Pb-82
•Gd-64
Give QN, & EDD:Te-52 I-53Fe-26 V-23Pu-94 Al-13Sb-51 Au-79
Oxidation State•The charge or apparent charge of an element
•Oxidation numbers
Negative Ox #• Always = column # - 8
• Exceptions: only in apparent charges: peroxides, hydrocarbons
Positive Ox #• = column #
• = unpaired electrons
• = s e- ---> s + d e-
• Apparent: singles & pairs
Drill:Determine EC, EDD, QN, Ox # of:
Ba-56 Pt-78
Cl-17 Tb-65
Wave Formula•v or c = f •c = speed of light
= wavelength
or f = frequency
Calculate the wavelength of your
favorite radio stationFM in MHzAM in kHz
Plank’s Formula•E = hf = hc/•E = energy
•h = Plank’s Constant
Calculate the energy of a photon from your favorite
radio station:
Calculate the energy of uv
light at 221 nm:
DeBroglie’s Formula
= h/mv
Calculate the wavelength of a 221 g baseball
thrown at 15 m/s:
Calculate the energy and mass of a photon of IR light at 1.326 m:
Spectrum•The unique set of waves absorbed or emitted by a substance
Absorption Spectrum•The unique set of wavelengths absorbed by a substance
•Atomic Absorption Sp
Emission Spectrum•The unique set of wavelengths emitted by a substance
•Atomic Emission Sp
Atomic Absorption Spectrum
•Dark-line Spectrum
Atomic Emission Spectrum
•Bright-line Spectrum
Spectroscopy
•The study of a substance under continuous excitation energy
Determine the electron
configuration (EC) for each of the
following: Mg, Sn, P, K, Cl, & V
Determine the EC for each of the
following: Zr, He, Eu, Cr, U
Determine the EC for each of the
following: Br-1, Kr, & Sr+2
Determine the electron dot diagram (EDD) for each of the following: Mg, Sn, P, K, Cl, & V
Determine the EC & EDD for each of the following: He, Mn,
Eu, Cr, U
Determine the quantum numbers
(QN) for each of the following: He, Mn,
Eu, Cr, U
Determine the EC, EDD, & QN for
each of the following: Mg, Sn,
P, K, Cl, & V
Determine the oxidation state (OS)
for each of the following: Mg, Sn, N,
K, Cl, & V
Determine the EC, EDD, QN, & OS for
elements: 21, 14, 29, & 64
With a UV,visible,IR spectrophotometer waves at 221 nm, 663 nm, & 2.21 m were detected when element X was excited. Calculate the
energy differences among levels 1, 2, 3, & 4.
Excited sodium emits red light at 663 nm.
Determine EC, EDD, QN, OS, & the energy
of the light wave.
Chapter 3 General
•Define all the Key Terms on page 168
Wave Energies
•Work problems:
1 - 10
on page 169
EC
•Work problems:
39 -42
on page 170
Quantum Numbers
•Work problems:
21 - 32
on page 170