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Chapter 4 electrons in atoms

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This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.

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Chapter 4: Electrons in Atoms ,[object Object],[object Object],[object Object],[object Object],[object Object]
Chapter 4 : Arrangement of Electrons in Atoms ,[object Object],[object Object],[object Object],[object Object]
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If + and – charges attract, why don’t e - collapse into the nucleus? ,[object Object],[object Object],[object Object]
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[object Object]
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],Metal Light Electrons
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],Metal Light Electrons
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],S’up.
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],The ground state of an electron, the energy level it normally occupies, is the state of lowest energy for that electron.                    There is also a maximum energy that each electron can have and still be part of its atom. Beyond that energy, the electron is no longer bound to the nucleus of the atom and it is considered to be ionized. When an electron temporarily occupies an energy state greater than its ground state, it is in an excited state . An electron can become excited if it is given extra energy, such as if it absorbs a photon , or packet of light , or collides with a nearby atom or particle.                                       
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],Electrons do not stay in excited states for very long – they soon return to their ground states, emitting a photon with the same energy as the one that was absorbed.
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[object Object],[object Object],Notice this!
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[object Object],[object Object]
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[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],    3d yz 3d xz 3d xy                                                                              3d z 2 3d x 2 -y 2                                  
“Rungs of a ladder” N Energy of e- increases as you travel further away from the nucleus. e- can jump from energy levels when they gain/lose energy Quantum = amount of energy req’d to move an e- from its present energy level to the next highest; “quantum leap” Unlike a ladder, levels are not evenly spaced; closer further away thus easier to move b/t or leave.
The Quantum Mechanical Model (QMM) ,[object Object],[object Object],[object Object],“ Chance”
[object Object],The > probability of finding an e- is within these areas surrounding the nucleus ( represent where the e- is 90% of the time ). N The “fatter” the area of the e- cloud, the greater the chance of finding an e- and vice versa.
Atomic Orbitals ,[object Object],[object Object],[object Object],n =1 n = 2 n = 3 n = 4 ↑ energy, ↑ distance from nucleus, ↓ spacing N
[object Object],[object Object],[object Object],3 sublevels n = 3 2 sublevels n = 2 1 sublevel n = 1 # of sublevels in that level Principal energy level (n) 7 orbitals 4 th = f 5 orbitals 3 rd = d 3 orbitals 2 nd = p 1 orbital 1 st = s # of orbitals within each sublevel Sublevels (lowest  highest energy)
Do Now: ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Basically… ,[object Object],[object Object],[object Object],[object Object],s orbital p orbital (x 3) d orbital (perpendicular orbital coming at you; x 5) Fig 13.4, 5 in book Low to High
 
Another representation of the atomic orbitals… Clouds/”bubbles” indicate where you’ll find e- most of the time!
[object Object],[object Object],[object Object],Does the probability of finding an e- vary with direction in 1s? Does the same hold true for p and d orbitals?
[object Object],N P P P P P Coming @ you Going away from you 3.) Spaces represent what? P S 2.) How many total orbitals are there? What are the max # of e- that can be held in n= 2? 1.) P orbitals stick out further therefore they have > ____?
[object Object],[object Object]
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Homework ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Electron Configurations ,[object Object],WHY? High energy systems are very unstable Atom works to attain the most stable e- configuration possible
[object Object],[object Object],[object Object],[object Object],1 s 2 s 2 p Long form vs. Short form? Electron Configurations/Aufbau Diagrams
[object Object],Aufbau Diagram
[object Object],[object Object]
[object Object],____ 5s ___ ___ ___ 4p ___ ___ ___ 4d ___ ___ Element
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[object Object]
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Homework ,[object Object],[object Object],[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Physics and the QMM ,[object Object],[object Object]
[object Object],[object Object],All waves travel in a vacuum at 3.0 x 10^10 cm/s (or 3.0 x 10^8 m/s)  = ? I’m smarter than he is? How’d he measure that?
Anatomy of a Wavelength origin amplitude Λ = “lambda” Frequency ( ν ) = “nu” = # of wave cycles that that pass through a point in a given time = Hertz (Hz) or s^-1 Wavelength and frequency are inversely related! Which leads us to…
Take 3 minutes only for quiz – hand in when finished. ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
ν “times” λ = speed of light ,[object Object],[object Object],Electromagnetic Spectrum = relative size?
Every element bends light in a specific way… Open book and complete sample 13.2 and practice problem 11
Another idea that came about through the study of light… ,[object Object],[object Object],[object Object],[object Object],[object Object]

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Chapter 4 electrons in atoms

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  • 27. “Rungs of a ladder” N Energy of e- increases as you travel further away from the nucleus. e- can jump from energy levels when they gain/lose energy Quantum = amount of energy req’d to move an e- from its present energy level to the next highest; “quantum leap” Unlike a ladder, levels are not evenly spaced; closer further away thus easier to move b/t or leave.
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  • 35. Another representation of the atomic orbitals… Clouds/”bubbles” indicate where you’ll find e- most of the time!
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  • 54. Anatomy of a Wavelength origin amplitude Λ = “lambda” Frequency ( ν ) = “nu” = # of wave cycles that that pass through a point in a given time = Hertz (Hz) or s^-1 Wavelength and frequency are inversely related! Which leads us to…
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  • 57. Every element bends light in a specific way… Open book and complete sample 13.2 and practice problem 11
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