The Development of A New Atomic Model
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Transcript of The Development of A New Atomic Model
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CH. 4 .1
The Development of A New Atomic Model
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Properties of Light
Acts like a wave Electromagnetic radiation-wavelike energy traveling
through space X-Rays, ultraviolet light, infrared light, radio waves, etc
Electromagnetic Spectrum- organized list of all forms of electromagnetic radiation All forms travel 3.00 x 108 m/s in a vacuum
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Wavelength Frequency
λDistance from crest
to crest(or tough to trough) of corresponding waves
SI Unit: m, cm, or nm
ν# of waves that
pass a given point in a specific time
SI Unit: Hz
Properties of Light
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Photoelectric Effect
Emission of electrons from a metal when light shines on the metal
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Light as a Particle
Quanta Quantum of energy is
the minimum amount of energy that can be lost or gained by an atom
E- energy, J h- Plancks Constant
6.626 x 10-34 Js v- frequency, s-1
Photon Particle of
electromagnetic radiation having zero mass and carrying a quantum energy
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Ground State Excited State
Lowest energy state of an atom
Atom has a higher potential energy than it does in ground state
Gives off light Moving from excited
back to ground state
The Hydrogen-Atom Line Emission Spectrum
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Line-Emission Spectrum Continuous Spectrum
Narrow beam of light, when passing through a prism
Emission of a continuous range of frequencies of electromagnetic radiation
The Hydrogen-Atom Line Emission Spectrum
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Bohr’s Model of the Hydrogen Atom
Emission Electron falls to a
lower energy level Photon is emitted
Absorption Electron jumps from
lower to higher energy level
Energy must be added
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CH 4 .2
The Quantum Model of the Atom
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Diffraction Interference
Bending of a wave as it passes through a small object
Waves overlapDifferent areas have
Reduced energy Increased energy
Electrons as Waves
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Heisenberg Principle
It is impossible to determine simultaneously both the position and the velocity of an electron of any other particle
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Schrodinger Wave Equation
Quantum Theory Describes mathematically the wave properties of
electrons and other very small particles
Gives the probability of finding an electron in a given orbital 3 dimensional region around the nucleus
that indicates the probable location of an electron
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Atomic Orbital's and Quantum Numbers
Quantum Number Specifies the properties of atomic orbital's and the
properties of electrons in orbital's
1st 3 Numbers Indicate main energy level, shape and orientation of
orbital4th Number
“Spin” number describes the fundamental state of the electron that occupies the orbital
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Principle Quantum Number
Symbol- nIndicates main
energy level occupied by electron
Positive integers only 1,2,3, etc
As n increases, distance from nucleus increases
Electrons can have the same value Same shell
Total orbital's in a shell(main energy level n2
Atomic Orbital's and Quantum Numbers
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Angular Momentum Quantum Number
Sublevels Orbital's of different
shapes exist for a given value of n
Symbol- l Indicates the shape of
the orbitalValue
n-1; can be zero or positive integers
Atomic Orbital's and Quantum Numbers
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Angular Momentum Quantum Number
s orbital Spherical
p orbital Dumbbell shape
d & f orbital's More complex
n=1 S orbital
n=2 s & p orbitals
n=3 s, p, & d orbitals
n=4 s, p, d & f orbitals
Atomic Orbital's and Quantum Numbers
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Magnetic Quantum Number
Symbol- mIndicates the
orientation of an orbital around the nucleus
Value Whole numbers,
including zero; -l to +l
Atomic Orbital's and Quantum Numbers
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Spin Quantum Number
Only 2 Values +1/2 and -1/2
Indicates the 2 spin states of an electron in an orbital
Single Orbit Max of 2 electrons Must have opposite
spin states
Atomic Orbital's and Quantum Numbers
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CH 4 .3
Electron Configuration
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Electron Configuration
Arrangement of electrons in an atom
Unique for each element
Ground State Electron Configuration Lowest energy arrangement of electrons for each
element
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Aufbau Principle
Electrons occupy the lowest energy orbital that can receive it
Rules for Electron Configuration
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Pauli Exclusion Principle
No two electrons in the same atom can have the same set of four quantum numbers
Arrows represent different spin states
Rules for Electron Configuration
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Hund’s Rule
Orbital's of equal energy are each occupies by one electron before any orbital is occupied by a second electrons
All electrons in singly occupied orbital's must have the same spin state
Rules for Electron Configuration
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Orbital NotationElectron Configuration Notation
Unoccupied orbital ___
Orbital with 1 electron ___
Orbital with 2 electrons ___
Quantum # and Sublevel underneath
Eliminates lines and arrows
Uses superscripts
1s22s22p6
Representing Electron Configurations
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Practice pg 113
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2nd Period Elements
Highest Occupied Energy Level Electron contained main energy level with the highest
principle quantum number
Inner Shell Electrons Electrons no in the highest occupied energy level
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3rd Period Elements
Shorthand Notation 1st 10 electrons in an atom have the same
configuration as NeonNoble Gas Configuration
Outer main energy level occupied by 8 electrons (most cases)
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4th & 5th Period Elements
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Practice pg 120
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Practice pg 121
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Practice pg 122