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Chapter 10• Chapter 10 Topics
– Electromagnetic (Light) Spectrum
– Spectroscope– Bohr Model– Quantum Model
(Schrödinger)• Principle• Orbital Shape• Exclusion• Electron
Configuration• Noble Gas Cores
– Periodic Table Trends– Valence Electrons
• What we’ll do:– Light & Spectrometer
Demonstration– Bohr Model Animation– Quantum Model –
Beginning– Computerized Orbitals
(breath)
– Quantum Model Extension– Periodic Trends– Valence Electrons (ns2np5)
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Electromagnetic Spectrum (Light)
• Visible Light (400 – 700 nm)
Red700 nm
Yellow585 nm
Blue491 nm
Orange647 nm
Green575 nm
Violet400 nm
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Bohr Model of the Atom
• View Animations Online
• View UV/Visible Spectrum of:– Hydrogen Lamp– Neon Lamp– Mercury Lamps (overhead lights)– Projector Lamp (Incandescent / W)– Fire works.
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Quantum Model
• Bohr Model works perfectly for Hydrogen
• Doesn’t work well for rest of the periodic table.
• Refined with the Schrodinger Equation– Still have Bohr Energy Levels– Add “sublevels” – shape of the orbital– Multiple orbitals per sublevel.– 2 Electrons per orbital
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Quantum Model - n
• Principle Quantum Number (n)– n can be {1, 2, 3, 4, 5, 6, 7}– Corresponds to the ROWS on the
periodic table
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Quantum Model - Sublevels
• Sublevels = Shape• Show Web Site with shapes.
http://www.chem.purdue.edu/gchelp/aos/1s.html
• Possible Sublevels:– s, p, d, f– # of possible sublevels is same as value of n:
• n = 1: s sublevel only• n = 2: s & p• n = 3: s, p & d• n = 4: s, p, d & f• We never need more than f – there aren’t enough
stable elements.
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Quantum Model – the One s Orbitals
• “s” sublevels are “spherical” (round)
• These are the Alkali Metal & Alkaline Earth Metals!
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Quantum Model – the Three p Orbitals
• “p” orbitals are sketched as pear-shapes (middle).• There is one along each axis – x, y, z for a total of 3.• These are the {Al, C, N, O} families, halogens, noble
gases.
Left: true shape Middle: sketch Right: All at once.
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Quantum Model – the Five d Orbitals
• 4 of the “d” are 4-petal flowers. The 5th is weird! These are the transition elements!
• These are thetransition metals.
B: True Shape
C & D: Sketch
E: The funny one.
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Summary
n Sublevels# of
Orbitals# of
ElectronsTotal
Electrons
1 s only 1 2 2
2 s 1 2 8
p 3 32=6
3s 1 2 18
p 3 6
d 5 52=10
4 s,p,d,f 1, 3, 5, 7 32
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Team Exercise• This chapter is mainly qualitative
– We will use the team activity to actively review the topics.
– Discuss what you don’t fully understand.– Note topics that you want me to go over.
• Review your chapter notes. – Update them with good ideas from
teammates.
• GOAL / ASSIGNMENT: Spend time actively reviewing the material.
• Complete your active learning log.
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Orbitals / Energy Levels
• Bigger orbitals have higher energy, electrons want to fill in the bottom levels first.
• Filling Order:1s 1s 2s 2p 2s 2p 3s 3p 3d 3s 3p 3d 4s 4p 4d 4f 4s 4p 4d 4f 5s 5p 5d 5f 5g 5s 5p 5d 5f 5g 6s 6p 6d 6f 6h 6i 6s 6p 6d 6f 6h 6i 7s 7p 7d 7f 7h 7i 7j 7s 7p 7d 7f 7h 7i 7j
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Electron Configuration
• On Chalkboard:– Energy Level Diagrams– Shorthand #1: 1s22s23p6…– Shorthand #2: Noble Gas Core
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Team Exercise Time• This chapter is mainly qualitative
– We will use the team activity to actively review the topics.
– Discuss what you don’t fully understand.– Note topics that you want me to go over.
• Review your cheatsheets – Update them with good ideas from
teammates.
• GOAL / ASSIGNMENT: Spend time actively reviewing the material.
• Complete your active learning log.
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