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21 Cards in this Set
- Front
- Back
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Isotopes of hydrogen names
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protium, deuterium, tritium
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Bohr model
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electrons travel in specific orbits at specific energy levels around dense, positive nucleus
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Quantum
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Energy difference between energy levels
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Quantum Mechanical Model
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electrons move in complex patterns called orbitals, defined by areas where you are most likely to find the electron
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Heisenberg uncertainty principle states...
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impossible to know both an electron's position and momentum at same time
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Hund's rule states...
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electrons prefer to be unpaired with parallel spins.
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Energy value of a quantum (J) = ?
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= Planck's constant (J·s) * frequency of radiation (1/s)
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Planck's constant (h)
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6.626 x 10^-34 J•s
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mol
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6.02 · 10^23
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Energy of an electron (J)=
(related to permitted angular momentum values) |
- Rydberg constant (J) /
n^2 (dimensionless) as n increases, E increases (due to negative sign) |
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Rydberg constant (R subscript H)
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2.18 · 10^-18 J/electron
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Electromagnetic Energy of excited photon (J) =
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(Plank's constant (J·s) * speed of light (m/s)) /
wavelength of radiation (m) |
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speed of light (c)
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3.00 * 10^8 m/s
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Energy of frequency of light emitted by an electron (J) =
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- Rydberg constant (J) ( (1 / initial n^2) - ( 1 / final n^2) )
The energy of the emitted photon corresponds to the precise difference in E b/w the higher E initial state and the lower E final state. |
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n (principal quantum number) =
n, l, m(l), m(s) |
any positive integer
larger value = higher energy & larger radius of orbital 2n^2 = electron capacity |
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l (azimuthal / angular momentum quantum number) =
n l m(l) m(s) |
0 to (n-1)
l = 0 = s subshell l = 1 = p subshell l = 2 = d subshell l = 3 = f subshell etc. refers to shape and number of subshells w/in given principal E level |
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m subscript l (magnetic quantum number) =
n l m(l) m(s) |
-l to +l including 0
specifies particular orbital w/in a subshell (orbital can hold max 2 e), # of possible values = # of orbitals |
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m subscript s (spin quantum number) =
n l m(l) m(s) |
-1/2 or +1/2
Denotes one of two spin orientations. In same orbital, must have opposite (parallel) spins. |
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Electron Subshell Flow Diagram
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1s
2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f etc. Draw out at beginning of Phys. Sci. Section |
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paramagnetic
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atoms made up of unpaired electrons so that a magnetic field will cause parallel spins in unpaired e's ∴ causing an attraction
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diamagnetic
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materials consisting of atoms with all paired e's, meaning they will be slightly repelled by a magnetic field
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