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UNIT 6: ELECTRON/ATOM STRUCTURE (6.6-6.9: More electron configurations…
UNIT 6: ELECTRON/ATOM STRUCTURE
6.1-6.4: The nature of everything
BUT all matter and particles also behave as waves/have a wavelength, according to De Broglie.
λ = h/(m*v)
Meaning that large objects have almost no wave behavior but electrons do extremely.
By extension, it is impossible to know both momentum and location of an electron.
EM radiation, or anything emitted/absorbed by matter, is quantized into photons (particles).
Energy of each photon: E = h * ν
All EM radiation travels at 2.998 * 10^8 m/s
Therefore, c = λ * ν
Energy is emitted when an electron is excited and jumps back down (from n levels.)
This new particle theory explained emission spectra, PE effect, blackbody.
6.5 Electron configurations
Quantum numbers:
n is the principal. Determines distance from nucleus and more and therefore energy level.
n = 1, 7
l is the subshell designation; determines the type of orbital.
l = 0, (n-1); s, p, d, f
m(l) is the magnetic number, or the orientation of the orbital... each subsequent type of orbital has 2 more orientations.
m(l) = -l, +l
m(s) is the spin number, and each 2 electron in an orbital spins opposite directions.
m(s) = +1/2, -1/2
Complexity of orbital AND distance from nucleus mean how much energy it possess
"A big counting problem"; n is dependent on electron #, l on n, m(l) on l, and m(s) on m(l)
Each orbital in a subshell is the same energy, a.k.a. degenerate.
each electron in an atom has a unique set of quantum numbers.
Notes: Any configurations of electrons is because it took the least energy to do/was the most stable configuration.
6.6-6.9: More electron configurations
Each energy level DOES possess associated s, p, d, f, orbitals... but due to complexity, d and f orbitals transcend their "n" designations.
d subshell associated with each n is higher energy than the s orbital in n + 1.
f orbital for a given n (where it exists) is higher energy than the s orbital in n + 2. (BUT ALWAYS STARTS W/d^1 because of per. table)
Configuration notation!
Ex. 1s^2
Coefficient: n level
letter: subshell/orbital type
Exponent: # of electrons in subsell
For higher degrees: use last noble gas's notation plus whatever other electrons. Ex. [Ar]4s^2
Orbital shapes: s is spherical, p is dumbbells, d is crosses, f is weird. For each higher n, the size gets bigger.
Valence electrons are electrons in the highest n for the atom. Core electrons are everything else (inner n electrons.)
Will fill low--> high energy. Will fill each orbital 1 first (megabus.) Will spin opposite. Orbitals fit 2 electrons.
PARAMAGNETIC: many unpaired electrons. DIAMAGNETIC: all electrons are paired.