Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
42 Cards in this Set
- Front
- Back
|
electromagnetic radiation: |
transmission of energy through space in the form of oscillating waves |
|
|
wavelength: |
distance between identical points of successive waves |
|
|
frequency, v: |
# of times per second a wavelength moves past a point |
|
|
v= |
1/sec (Hertz of Hz) |
|
|
(m) * (1/sec) = |
m/sec velocity!!! |
|
|
Speed of light, or c? |
c = 3.00 x 10^8 m/sec = 180,000 m/sec |
|
|
c= wavelength * v is _________ proportional. |
inversely |
|
|
Question: 443 nm? |
(1) c= wavelength * velocity (2) 3.00 x 10^8 m/sec = (443nm)(v) (3) (CONVERT) 1m = 1 x 10^9 nm (4) 443nm x 1m / (1 x 10^9 nm) = 4.43 x 10^-7m (5) 3.00 x 10^8 m/sec = (4.43 x 10^-7m) v (6) 3,00 x 10^8 m/sec / 4.43 x 10^-7 = v (7) 6.77 x 10^14 1/sec = v |
|
|
The photoelectric effect: |
ability of light to knock e- out of a metal (the # of electrons ejected are indeed dependent on the intensity of light wave) |
|
|
quantum:
|
the smallest amount of energy an atom can absorb or release |
|
|
quantized: |
only certain, fixed energies are allowed |
|
|
continuous: |
any energy is allowed |
|
|
photon: |
the smallest particle of electromagnetic radiation possible. |
|
|
E= |
energy of photon |
|
|
h= |
planks constant = 6.626 x 10^-34 J*sec |
|
|
wave-particle duality theory: |
sometimes light exhibits properties of a wave, and at other times it exhibits properties of a particle |
|
|
continuous spectrum: |
all colors in the visible spectrum where one color bleeds into the next with no discontinuity |
|
|
emission spectrum: |
light emitted from an excited species |
|
|
line spectrum: |
light of only certain wavelengths or colors are observed |
|
|
Niels Bohr said that electrons are found at ______ or ________ distances from the nucleus. |
fixed or quantized |
|
|
the energy the electron possesses is defined by the ___________ |
distance |
|
|
electron close to the nucleus |
low energy |
|
|
electron farther from the nucleus: |
more energy |
|
|
n=1 |
GROUND STATE |
|
|
when electrons gain energy they move ______ from the ________ |
further, nucleus |
|
|
excited state: |
e- in atom are promoted to higher energy states (further from nucleus) |
|
|
excitation: |
going from ground to excited state or getting charged/heated |
|
|
emission= |
photon is released, brings e- back to ground state |
|
|
Quantum #'s |
values which describe the energy shape, orientation, and spin of the electron in an atom |
|
|
Principle Quantum number: |
n, determines the distance & thus the energy of an e- from nucleus possible integer values |
|
|
energy of electron increases as ___ increases? |
n |
|
|
angular momentum quantum # |
l, determines the shape of the orbital *for a given call of n, l has possible values of 0 up to n-1 and all integers in between ex. n=3 l=0, l=1, l=2 |
|
|
magnetic quantum number, m(l): |
describes the orientation of orbitals in space relative to each other. m(l) values depend on l possible m(l) values= -l to +l |
|
|
electron spin quantum #, M(s) |
comes directly from experiment electrons can spin only one way quantized M(s) values = = +1/2 or - 1/2 |
|
|
electrons always arrange themselves in the _____ energy possible |
lowest |
|
|
degenerate: |
electrons that have the same energy |
|
|
each orbital subtle can contain a maximum of ____ electrons |
2 |
|
|
Pauli Exclusion Principle: |
no two electrons in the same atom can have the same 4 quantum #'s |
|
|
Hund's Rule |
electrons fill unpaired in degenerate orbitals as long as possible |
|
|
pairing energy |
the cost of energy in the same space |
|
|
paramagnetic: |
atom contain one or more unpaired electrons |
|
|
diamagnetic: |
all electrons in the atom are paired |
