the quantum model energy as wave and particle. quantum mechanics explains how small particles move...
TRANSCRIPT
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The Quantum Model
Energy as wave and particle
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Quantum Mechanics Explains how ‘small’ particles move
Sorry Mr. Smith
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What is light? Wave
Particle
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Photoelectric Effect
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The Electromagnetic Spectrum
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c =
If energy is constant then: (wavelength), in meters, is inversely proportional to (frequency), measured in hertz or 1/s
OR
As wavelength increases frequency decreases
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E = h
If energy is constant then: h is Planck’s constant, (J x s) (frequency), measured in hertz or 1/s E is energy in Joules (J)
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Red Light
Violet Light
• Low frequency
• Long wavelength
• High frequency
•Short wavelength
Wave Comparisonnm = 1 x 10-9 m
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Example Problem Refer to #1 on your Worksheet. On page 7 of
hw packet.
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Bohr Model
Electrons are a HUGE deal in chemistry
Responsible for chem rxns
Today: How many are there Where do they reside
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Periodic Table
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Electron Configurations Electron configurations are...
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Electron Configuration Vocab Principle Energy Level
correlates to the period (1-7), periods go from left to right across the periodic table
Sublevel are located in the principle energy level. There are 4 that we
will talk about s, p, d and f.
Orbital located in the sublevel. Where electrons are most likely to be
found 1 ORBITAL HOLDS 2 ELECTRONS
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Writing Electron Configurations Principle Energy Level[sublevel]number of electrons
OR a[b]c
Get your periodic table! Start from left to right!
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Orbital Diagrams Tool for creating electron
configurations
2 dimensional representation of where electrons are in an atom
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Aufbau Principle electrons are added to the lowest available
energy level. Hydrogen as an example:
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Pauli Exclusion Principle each orbital can hold two electrons those electrons must have opposite spins
spin is represented by the arrow facing up or down.
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Hund’s Rule Orbitals of equal energy are occupied by one
electron before 2 electrons occupy 1 orbital. The second electron is added after all orbitals have one electron
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Aufbau Diagram
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The Periodic Table1s 1s
2s 2p
3s 3p
4s 3d 4p
5s 4d 5p
6s 5d 6p
7s 6d 7p
4f
5f
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Noble Gas Configuration – Short cut Locate the element on the PT
Trace backward to the nearest noble gas
Put that noble gas in [] (brackets)
Fill in remaining electrons
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P orbitals in more detail p sublevel
3 orbitals x, y & z
Work like a coordinate plane Atoms are 3-D
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Valence Electrons Electrons in the HIGHEST energy level (n)
Electrons that interact during chem rxns
Always in the s & p sublevels
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Finding Valence Electrons Locate the highest
energy level Count the electrons
present Orbital diagrams
SUPER helpful
Example: Sulfur How many valence e’s?
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Stability – Hund’s Rule Exceptions to e configs
In the d-block (yo) Almost ½ filled d-block Almost full d-block
It is more stable for atoms to have 2 half filled sublevels Compared to 1 full and 1
partially filled Example: Chromium