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CHEM ch 5.2 - Flashcards

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Class:CHEM 1010 - Introduction to Chemistry
Subject:Chemistry
University:Southern Utah University
Term:Fall Semester 2013
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Continuous spectrum when white light is passed through a prism this is produced

there are no breaks between the colors (ex- rainbow)
atomic spectra consists of different colors separated by dark areas (opposite of continuous spectrum)

when light emitted from heated elements is passed through a prism it doesnt produce a continuous spectrum
energy levels electrons in lower energy levels are closer to nucleus

are assigned quantum numbers (n-1,2,3 etc)
line spectra when lines appear from light shined through a prism
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ground state when an electron is at the lowest energy level
excited state when energy is added added and the electron jumps to the next level.
energy sublevel (s,p,d,f) energy levels inside an energy level
photons the light emitted when atoms are heated (stream of particles)
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quantum each photon is a packet of energy also known as a quantam
photon frequency (high and low) high frequency photons have high energy and short wavelengths

low frequency photons have low energy and long wavelengths.
principle quantum numbers in an atom eache electorn has a specific energy level which is assigned values called principle quantum numbers (n=1, n=2, etc) electrons in lower energy levels are closer to the nucleus.

1>2>3>4>5>6>7
changes in energy levels electron can move up only if it absorbs the energy equal to the difference in energy levels. when it moves down it emits energy equal to the difference between the 2 energy levels. if the energy emitted is in the visible range we see one of the colors of visible light.
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orbitals a 3-dimensional space around a nucleus where an electron has the highest probability of being found.

has a shape that represents its electron density, (not a path the electron follows)

2=1 box(2 electrons)
how many orbitals are in the p and s sublevels? 3 p orbitals

1 s orbital
4 d sublevel? 5 orbitals
n=4? 16 orbitals
1s, 3p, 5d, 7f
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configuration examples 2He 10 Ne 18AR 2He- 1s2

10Ne- 1s2, 2s2, 2p6

1s2, 2s2, 2p6, 3s2, 3p6
abbreviated orbital diagram F Al F=[He} 2s2, 2p5

Al= [Ne] 3s2, 3p1
electronic configurations & the periodic table Cd Fe Cd= 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10

Fe=1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d6
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 Continuous spectrumwhen white light is passed through a prism this is produced

there are no breaks between the colors (ex- rainbow)
 atomic spectraconsists of different colors separated by dark areas (opposite of continuous spectrum)

when light emitted from heated elements is passed through a prism it doesnt produce a continuous spectrum
 energy levelselectrons in lower energy levels are closer to nucleus

are assigned quantum numbers (n-1,2,3 etc)
 line spectrawhen lines appear from light shined through a prism
 ground statewhen an electron is at the lowest energy level
 excited statewhen energy is added added and the electron jumps to the next level.
 energy sublevel(s,p,d,f) energy levels inside an energy level
 photonsthe light emitted when atoms are heated (stream of particles)
 quantumeach photon is a packet of energy also known as a quantam
 photon frequency (high and low)high frequency photons have high energy and short wavelengths

low frequency photons have low energy and long wavelengths.
 principle quantum numbersin an atom eache electorn has a specific energy level which is assigned values called principle quantum numbers (n=1, n=2, etc) electrons in lower energy levels are closer to the nucleus.

1>2>3>4>5>6>7
 changes in energy levelselectron can move up only if it absorbs the energy equal to the difference in energy levels. when it moves down it emits energy equal to the difference between the 2 energy levels. if the energy emitted is in the visible range we see one of the colors of visible light.
 orbitalsa 3-dimensional space around a nucleus where an electron has the highest probability of being found.

has a shape that represents its electron density, (not a path the electron follows)

2=1 box(2 electrons)
 how many orbitals are in the p and s sublevels?3 p orbitals

1 s orbital
 4 d sublevel?5 orbitals
 n=4?16 orbitals
1s, 3p, 5d, 7f
 configuration examples 2He 10 Ne 18AR2He- 1s2

10Ne- 1s2, 2s2, 2p6

1s2, 2s2, 2p6, 3s2, 3p6
 abbreviated orbital diagram F AlF=[He} 2s2, 2p5

Al= [Ne] 3s2, 3p1
 electronic configurations & the periodic table Cd FeCd= 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10

Fe=1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d6
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