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.
Don't know
remaining cards
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:
restart all cards
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

Chem Unit 2

elements pro/neu/elec, spectrum, valence electrons

how to find the atomic mass Average of protons and neutrons
how to find the atomic mass number add protons and neutrons together
why do electrons not count towards the atomic mass? electron's are so small their weight is insignificant
how to find the number of neutrons atomic mass (rounded) - the number of protons
define an ion atom with a net electric charge due to the gain or loss of electrons
how to find the number of electrons protons minus the charge (divided by -1)
define atomic mass the weighted average of all isotopes
how much is the atomic mass unit in comparison to the carbon-12 atom? atomic mass unit=1/12th the mass of a carbon 12 atom. (carbon has 6 protons and 6 neutrons)
how to determine the atomic mass %=abundance * isotope + %=abundance * isotope =atomic mass (abundance= % in regular number form)
how to determine which isotope is the most common out of a distribution go to the periodic table and look at the atomic mass, round it to the isotope that has the nearest number
what louis de broglie discover the slower an electron moves and the faster an electron moves, the more it acts like a particle and the more it acts like a wave (respectively)
what did Erwin schrodinger discover there are different sizes depending on their energy, and different types of orbitals depending on shape of wavelength
what are the different letters of the probability clouds s-clouds=sphere path, p-clouds=double pea in a pod shape (infinity symbol)
how is the letter of the probability cloud formed electron runs along the wavelength, then the nucleus in the middle of the wavelength pulls the electron back (- and + charge)
Heisenburg Uncertainty principle there is no way to find out the position AND velocity of an electron at the same time.
what does "v" represent in terms of light waves? frequency
define ㅅ wavelength
define c speed of light (3.0x10^8)
define e energy
define h planks constant (6.626x10^-34)
equation for frequency V=c/ㅅ
equation for energy (2) E=hv or E= hc/ㅅ
What causes the light's color to be seen? phosphorus absorbing UV light and remitting it as visible light.
What was Bohr's explanation or the atomic spectrum The energy of an electron depends on its distance from the nucleus.
ground state electron is closer to the nucleus; has less energy
excited state electron has absorbed energy and moved AWAY from nucleus.
Does the transition from ground to excited state cause any light to be emitted? No, it's just like charging a battery
What is ionization energy When there is too much energy in an electron , it will pop out of the atomic spectra (therefore meaning no color emitted)
how many energy rings does s, p, d, and f have? 1, 3, 5, 7
Define electron configuration The position of an atom's electrons around the nucleus
What is the Aufbau Principle Electrons fill orbitals with the lowest energy requirements. each ring=quantum.
Pauli Exclusion Principle An orbital will only hold 2 electrons
what causes the form of the orbitals? an electron is traveling in a wavelength form and the nucleus that is in the middle of the wavelength pulls the electron back, creating a mirrored path of the electron's original path.
inside the orbital, what are the two electrons doing? spinning in different directions, away from each other (opposite charges)
what causes the two electrons to be a little attracted? Electrons have opposite poles facing each other, so the poles connect, but that doesn't connect the negative charges.
Hund's Rule Each orbital in a sub-level is single occupied before any are doubly occupied.
millikan discovery discovered weight of electron and exact charge
Democritus discovery said that all thing are made up of their own atoms
define orbital area of probability where the electrons are found
Created by: allyson.lee