Download Unit 2 – Electrons and Periodic Behavior Cartoon courtesy of

Chapter 4: Arrangement
of electrons in atoms
Unit 2 – Electrons and
Periodic Behavior
Cartoon courtesy of
NearingZero.net
Cartoon courtesy of NearingZero.net
4-1 Properties of Light
• Electromagnetic radiation-is a form of
energy that exhibits wavelike behavior as
it travel through space.
• Examples x-rays, UV, infrared light,
microwaves, radio waves
• Electromagnetic spectrum all
electromagnetic radiation, arranged
according to increasing wavelength.
• Spectroscopic analysis of the visible spectrum…
produces all of the colors in a continuous
spectrum
• Continuous spectrum- spectrum in which all
wavelengths within a given range are included.
Speed of Light
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C= v
C= speed of light
3.0 x 1010 cm/s
3.0 x 108 m/s
= wavelength (m)
v= frequency (Hz)
Crest
Trough
• Photoelectric
effect- is the
emission of e- by
certain metals
when light shines
on them
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E= h v
E= energy
h= Planck’s constant (6.626x10-34 J.S)
v= frequency
Quantum is a finite quantity of energy
that can be gained or lost by an atom.
• 1 quantum = 1 photon
• Ground state is the
state of lowest
energy (stable)
• Excited state has
higher potential
energy. Emits light.
• Example Neon
lights
Wave-Particle Duality
• JJ Thomson won the Nobel prize
for describing the electron as a
particle.
• His son, George Thomson won the
Nobel prize for describing the
wave-like nature of the electron.
4-2 The Quantum Model
of the Atom
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1.
2.
3.
4.
Quantum Numbers
Each electron in an atom has a unique set
of 4 quantum numbers which describe it.
Principal quantum number
Angular momentum (orbital) quantum
number
Magnetic quantum number
Spin quantum number
Principal Quantum
Number
• Generally
symbolized by n,
it denotes the
shell (energy
level/shell) in
which the electron
is located.
n=1
n=2
n=3
Angular Momentum
Quantum Number
• The angular momentum quantum number,
generally symbolized by l, denotes the
orbital (subshell) in which the electron is
located (s,p,d,f).
l =0
l =1
s
p
l =2
d
1s
Magnetic Quantum
Number
• The magnetic quantum number, generally
symbolized by m, denotes the
orientation of the electron’s orbital with
respect to the three axes in space
(x,y,z). Have to split up p, d, f orbitals.
Spin Quantum Number
• Spin quantum number denotes the
behavior (direction of spin) of an
electron within a magnetic field.
• Possibilities for electron spin: +1/2
or -1/2
4-3 Electron
Configurations
• Electron configuration is the
arrangement of electrons in
an atom.
• Aufbau Principle
states an electron
occupies the
lowest-energy
orbital that can
receive it.
Pauli Exclusion Principle
No 2 electrons in the same
atom can have the same 4
quantum #’s
Hund’s Rule
• States that orbital
of equal energy are
each occupied by 1
electron before
any orbital is
occupied by a 2nd
electron. Fill in all
the up arrows
first.
Lewis-Dot Notation
• A notation in which only
the valence shell
electrons of the atom
are represented.
Electron-Configuration
Notation
(O)=
Orbital Notation
x y z
x y z
x y z
Noble Gas Notation
• Is a shorthand configuration. Use
the noble gas before the element and
then continue with the electronconfiguration notation.
• Li= (He)2s1
• Al= (Ne) 3s23p1
Work Cited
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“Aufbau principle chart and electron-configuration of O”. Drawings. Aug. 7, 2006.
http://people.uis.edu/gtram1/organic/introduction/intro.htm
“Oxygen Lewis Dot”. Drawing. Aug. 7, 2006.
http://edweb.tusd.k12.az.us/Secrist/teachers/rjones/what_we_have_accomplished_i
n_the.htm
“Wavelength diagram and prism diagram” Pictures. Aug. 7, 2006.
http://eqseis.geosc.psu.edu/~cammon/HTML/Classes/PhysicalGeology/Notes/Chapter
02/P03.html
“Orbital Notations”. Drawings. Aug, 7, 2006. http://www.chemistry.ohiostate.edu/~grandinetti/teaching/Chem121/lectures/periodic%20trends/ionization_en
ergy.html
“xyz axis”. Drawing. Aug. 7, 2006.
http://wine1.sb.fsu.edu/chm1045/notes/Struct/QMech/Struct05.htm
“Electron shape chart”. Chart. Aug. 7, 2006.
http://wine1.sb.fsu.edu/chm1045/notes/Struct/QMech/Struct05.htm
“spd orbitals”. Drawing. Aug. 7, 2006.
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.html
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“Atom”. Drawing. Aug. 7, 2006.
http://bioweb.wku.edu/courses/Biol115/Wyatt/Exam1/Quiz1/quiz1.htm
“Periodic Table”. Drawing. Aug. 7,
2006.http://www.epcc.edu/faculty/victors/elconfig.htm
“Route 66 sign”. Photo. Aug. 7, 2006.
http://www.lightgod.com/led.asp?catid=865
“Neon Sign”. Photo. Aug. 7, 2006. http://www.neon-signage.com/
“Photo electric effect”. Picture. Aug. 7, 2006.
http://www.pa.msu.edu/courses/1997spring/PHY232/lectures/quantum/ph
otoelectric.html
“S,P,D,F blocks on periodic table”. Drawing. Aug. 8, 2006.
http://wine1.sb.fsu.edu/chm1045/notes/Struct/E
Period/Struct09.htm
• “Wolfgang Pauli”. Photo. Aug. 8, 2006.
http://www.homeoint.org/dynamis/synchro.htm
• “Na and Cl lewis dot struture”. Drawing. Aug 8,
2006.
http://www.d94.org/science/carrow/chemistry/in
teractions/calendar/notes/lewis.htm
• Information. Aug 6, 2006.
http://www.sciencegeek.net/Chemistry/Powerpoin
t/Unit2/Unit2_files/frame.htm
• Holt, Rinehart and Winston. Modern Chemistry.
Harcourt Brace & Company. 1999.