Busy. Please wait.
or

show password
Forgot Password?

Don't have an account?  Sign up 
or

Username is available taken
show password

why


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.


Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.

Remove ads
Don't know
Know
remaining cards
Save
0:01
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
Retries:
restart all cards




share
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

Atomic Theory Chem

TermDefinition
Planck's Hypothesis Energy is quantized, and energy of a wavelength is related to its frequency
the higher the frequency... ... the higher the energy
wavelength and frequency are _____ proportional inversely
matter has wavelike properties called wave-particle duality of nature
quantum mechanics very small pieces of matter moving very quickly
Newtonian mechanics matter under usual conditions
Heisenburg Uncertainty Principle Its impossible to know both the location and direction of an atom (RIP Bohr model)
Scroedinger's Equations modern atomic theory; describes with 90% probability where electrons are likely to be found
Aufbau Principle electrons occupy the lowest energy orbitals first
Pauli Exclusion Principle an atomic orbital can only hold two electrons, each with a different spin
Hund's Rule with orbitals of the same energy, single electrons occupy each orbital before they pair up
Principle Quantum Number (n) tells the principle energy level of the electron and distance from nucleus
the greatest number of electrons that can be found is each energy level can be calculated with the equation: 2n^2
Second Quantum Number (l) tells you the sublevels of the electron (s, p, d, f)
S holds 2 electrons and is shaped like a sphere
P holds 6 electrons and is shaped like a dumbell
D holds 10 electrons
F holds 14 electrons
Third Quantum Number (m): the space occupied by one pair of electrons is called an orbital (each sublevel has half the number of orbitals as it does electrons)
Fourth Quantum Number (s) Spin (in a given orbital, each electron must *probably* spin in a different direction)
Created by: msullyart