Pages 90-99 Electrons deBroglie—proved that particles with mass could have wave-like properties. A...
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Transcript of Pages 90-99 Electrons deBroglie—proved that particles with mass could have wave-like properties. A...
![Page 1: Pages 90-99 Electrons deBroglie—proved that particles with mass could have wave-like properties. A stream of e- could behave similar to a wave. He created.](https://reader035.fdocuments.net/reader035/viewer/2022070307/551b0789550346f70d8b59d1/html5/thumbnails/1.jpg)
Pages 90-99
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Electrons
• deBroglie—proved that particles with mass could have wave-like properties. A stream of e- could behave similar to a wave.
• He created the “wave-particle duality of nature” concept
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Quantum mechanics
• Two types of movement:
• A) Newtonian Mechanics—describes behavior of objects big enough to see with unaided eye and traveling at ordinary speeds ( cars, planes, space shuttle)
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Quantum mechanics
• B) Quantum Mechanics---describes behavior of objects too small to be seen with the unaided eye and traveling at a velocity near the speed of light (e-)
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Electrons
• Heisenberg Uncertainty Principle—the position of an e- cannot be determined with certainty, because in order to “see” the e- one must strike it with a photon of light and this will change the momentum and the position.
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Electrons
• Momentum---product of mass and velocity
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Electrons
• Electron Cloud Model-(Quantum Model)– The nucleus is positive---due to p+
– The nucleus has neutral no
– The mass of atom is in nucleus– The volume around the positive center in which
the electrons are most likely located is referred to as the “e- cloud”
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Electrons
• The e- cloud is the area of greatest probability in which the e- are most likely to be found at any given time.
•
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Electrons
• Erwin Schrodinger-----derived an equation that treated the e- of H atom as a wave. He applied to all atoms.
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Electrons
• Schrodinger’s quantum mechanical model of the atom describes each e- using 4 quantum numbers:
• “n” ---principal quantum number
• value of 1-7
• indicates the “size of e- cloud”
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Electrons
• “l” ----sublevel of energy
• value of 0 to n-1
• indicates the “shape of the cloud”
• “m” ----describes cloud orientation in space
• “s” ---describes the spin of the e-
• values: clockwise spin +1/2
• counterclockwise spin –1/2
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Electrons
• Greatest number of electrons in any energy level may be determined by :2n2
• Quantum level max e- number
• 1 2
• 2 8
• 3 18
• 4 32
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Electrons
• Sublevels of energy:
• “s”---spherical shape only 2e-
• “ p” ----3 in number ( 2e- each)
• dumbbell in shape
• located on 3 axis
• “d” -----5 in number ( 2e- each)
• “ f” -----7 in number ( 2e- each )
•
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Electrons
• Orbital ---space occupied by 2 e-
• Degenerate orbital---orbital with the same number of electrons and energy
• 3 p orbitals
• 5 d orbitals
• 7 f orbitals
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Electrons
• Pauli Exclusion Principle---no two e- in an atom have the same set of 4 quantum #. E- in the same orbital must have opposite spins
• Hund’s Rule—no orbital can have 2e- until all orbitals have at least 1 e-
• Aufbau Principle---e- fill lower energy orbital first ( demo on board)
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• Two exceptions to the filling rule:
• Cr----24
• Cu -----29
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• Simplified notation or noble gas notation
• Use chart to find previous “noble gas” and work the e-configuration from there
• Demo
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• Periodic chart divided into :
• Rows or periods-----( principal quantum #)
• Groups or families ( vertical columns)
• Group 1 alkali metalsGroup 2 alkaline earth metals
Group 17 halogens
Group 18 noble gas
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Electrons
• Demo:
• e-configuration p 99
• orbital diagrams---
• noble gas notation
• arrow diagram---
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Electron Dot Diagram
• Electrons in the outer most energy level are the e- most often involved in a chemical reaction.
• Valence e- ---- the e- in outer energy level
• Lewis Dot diagram:– Write the e-configuration for the element
– Write the chemical symbol
– Valence e- are placed in the 4 locations around the symbol –pairing them as necessary
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Electron dot diagrams
• Write the Lewis dot diagram for:
• Carbon
• Chlorine
• Nickel
• Sodium
• Neon
• Calcium
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Electron Dot Diagram
• Two exceptions to filling rule are:
• Copper
• Chromium
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• Wave-particle duality of nature Probability
• Electron cloud quantum mechanics
• Heisenberg Uncertainty principle
• Lewis e- dot diagram
• Momentum
• Newtonian mechanics
• Orbital principal quantum number
• Pauli exclusion principle
• Sublevel
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Work to do!!
• Page 126 # 12• Page 134 # 17• Page 141 #25,26,28• Page 145---vocab list• Page 146-149----#
38,39,44,46,49,52,53,55,59,61,64,78,79,80,81,82,84,86,87,91,93,101,102,103,104,
• Princeton review: 3,5,6,7,8,9,10