Ch.5 Electrons

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Last updated 7:22 PM on 5/25/26
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10 Terms

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Atomic Orbitals

A region in space where there is a high probability of finding an electron

Orbitals are found in principal energy levels. Electrons are placed into different energy levels depending on the amount of energy they have.

<p>A region in space where there is a high probability of finding an electron</p><p>Orbitals are found in principal energy levels. Electrons are placed into different energy levels depending on the amount of energy they have.</p>
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Different types of Atomic Orbitals

"S" Orbital - spherical shape

Electron(s) would be moving somewhere along that sphere

Only 1 "s" orbital occurs at one time

"P" Orbital - dumbbell shape

3 "p" orbitals occur together

Could have empty orbitals

"D" orbitals - more complex

5 "d" orbitals occur together

"F" orbitals - even more complex

7 "f" orbitals occur together

<p>"S" Orbital - spherical shape</p><p>Electron(s) would be moving somewhere along that sphere</p><p>Only 1 "s" orbital occurs at one time</p><p>"P" Orbital - dumbbell shape</p><p>3 "p" orbitals occur together</p><p>Could have empty orbitals</p><p>"D" orbitals - more complex</p><p>5 "d" orbitals occur together</p><p>"F" orbitals - even more complex</p><p>7 "f" orbitals occur together</p>
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Electron configurations

Electron Configuration - how electrons are arranged around the nucleus of atoms

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Aufbau principle

electrons enter orbitals of lowest energy first

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Pauli Exclusion Principle

an atomic orbital may contain two electrons at the most. Paired electrons must have opposite spins.

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Hund's Rule

when electrons occupy orbitals of equal energy, each electron first enters the orbitals unpaired and with the same spin

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Electron Configuration ex.

Ex: write the electron configuration of phosphorus

Determine the number of electrons to be placed in the orbitals

Follow the rules to place the electron and use a diagonal diagram

P has 15 electrons, 1s and can hold 2 electrons (13 electrons left), 2s can hold 2 electrons (11 electrons left), 2p can hold 6 (3 orbitals each hold 2 electrons = 6, so 5 electrons left), 3s -2 (3 electrons left), 3p (so all 3 electrons are being used)

Electron Configuration: 1s22s22p63s23p3

<p></p>
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<p>EMR/visible light spectrum Spectrum (ROYGBIV)</p>

EMR/visible light spectrum Spectrum (ROYGBIV)

red=700 nanometers

green=550 meters

violet=350 meters

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structure of a wave

(lambda) = wavelength, a= amplitude

Crest- peak on the wave

Trough - the lowest point on a wave

Amplitude - the heigh tof the wave from the origin tothd crest

Wavelength ( (lambda) - is the distance between crests

Wave cycle - when you reach the original position which you started at

<p>(lambda) = wavelength, a= amplitude</p><p>Crest- peak on the wave</p><p>Trough - the lowest point on a wave</p><p>Amplitude - the heigh tof the wave from the origin tothd crest</p><p>Wavelength ( (lambda) - is the distance between crests</p><p>Wave cycle - when you reach the original position which you started at</p>
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Equation for Electromagnetic Waves (EM)

Note: if the speed of light remains constant, then: if increases decreases, if decreases, increases

Note: Wavelength and frequency are inversely proportional

Ex. Find the wavelength of yellow light emitted by a sodium lamp.

C(speed of light) = 3.00 x 10^8 m/s

C = Lambda x nu

<p>C(speed of light) = 3.00 x 10^8 m/s </p><p>C = Lambda x nu </p>