Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

Username is available taken
show password


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.
Didn't know it?
click below
Knew it?
click below
Don't know
Remaining cards (0)
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

AP Chem Stack #2 tp

Atomic theory

Scientists involved in the development of the atomic theory Democritus, Dalton, Thomson, Millikan, Rutherford, Bohr
John Dalton Postulate 1 Matter is made up of tiny, indivisible particles called atoms which can't be created or destroyed.
John Dalton Postulate 2 Atoms of the same element are identical in mass and size and are different from other elements
John Dalton Postulate 3 Atoms combine in small whole-number ratios to form compounds.
John Dalton Postulate 4 In reactions, atoms are combined, separated, and rearranged.
J.J. Thomson Discovered ELECTRONS using the cathode ray tube. He concluded that they were negatively charged and there must be positively charged particles to balance out the charge.
Robert Millikan Performed the oil drop experiment and determined the charge to be negative by measuring the amount of current needed to keep oil drops suspended.
Ernest Rutherford Discovered atom's nucleus with alpha-particles and gold foil. Concluded that most of the atom is empty space and that the nucleus is very small.
1st Quantum number: Principal (n) main energy level: values range from 1 --> ?
2nd Quantum number: azimuthal (l) number of sub shells and orbital shape: values range from 0 --> n - 1 .... 0 = s 1 = p 2 = d 3 = f
3rd Quantum number: magnetic (ml) number of spacial orientations of orbital values range from -l --> +l
4th Quantum number: spin (ms) axial rotation of electrons: values are +1/2 or -1/2
Aufbau Principle An electron will occupy the lowest possible energy orbital that will receive it. Empty orbitals overlap in their energies at higher main energy levels and should be filled in order according to diagonal rule.
Hund's Rule When filling orbitals of equal energy electrons of the same spin will occupy each orbital as singles before pairing. Empty bus seat rule.
Pauli Exclusion Principle No two electrons of the same atom will have the same 4 quantum numbers.
Created by: tracypippins



Use these flashcards to help memorize information. Look at the large card and try to recall what is on the other side. Then click the card to flip it. If you knew the answer, click the green Know box. Otherwise, click the red Don't know box.

When you've placed seven or more cards in the Don't know box, click "retry" to try those cards again.

If you've accidentally put the card in the wrong box, just click on the card to take it out of the box.

You can also use your keyboard to move the cards as follows:

If you are logged in to your account, this website will remember which cards you know and don't know so that they are in the same box the next time you log in.

When you need a break, try one of the other activities listed below the flashcards like Matching, Snowman, or Hungry Bug. Although it may feel like you're playing a game, your brain is still making more connections with the information to help you out.

To see how well you know the information, try the Quiz or Test activity.

Pass complete!

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