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

Ch 4 section 11-14

The electronic structures of atoms

Electromagnetic radiation The wavelength of EM radiation has the symbol . Wavelength is the distance from the top (crest) of one wave to the top of the next wave. Measured in units of distance such as m, cm, Å. 1 Å = 1 x 10-10 m = 1 x 10-8 cm
Frequency symbol V Frequency is the number of crests or troughs that pass a given point per second Measured in units of 1/time – 1/s - s-1 lamda*v = speed of propagation of the wave or lamda*v = c (for light) c = speed of light (3.00 x 108m/s)
Wavelength and frequency are inversely proportional to each other, for the same wave, shorter wavelengths correspond to higher frequency
UV vs IR UV: shorter λ, higher ν IR: longer λ, low ν High Energy; High Frequency; Short λ or Low Energy; Low Frequency; Long λ
Electromagnetic Radiation Molecules interact with electromagnetic radiation. Molecules can absorb and emit light.
Once a molecule has absorbed light (energy), the molecule can Rotate Translate Vibrate Electronic transition
Planks constant E=hV or E=(hc)/lamda h=6.626e-34j*s energy is directly proportional to frequency
The Photoelectric Effect e- r ejected only if light is of sufficiently short wavelength/high energy no matter how long or bright when photon energy of light is high enough to start photoelectric effect the # of e- emitted per second (current) increases with brightness/intensity
Intensity of light The intensity of the light is the brightness of the light. In wave terms, it is related to the amplitude of the light waves. In photon terms, it is the # of photons hitting the target.
emission spectrum formed by an electric current passing through a gas in a vacuum tube (at very low pressure) which causes the gas to emit light. Sometimes called a bright line spectrum
absorption spectrum is formed by shining a beam of white light through a sample of gas. Absorption spectra indicate the wavelengths of light that have been absorbed.
Every element has a unique spectrum. Can use spectra to identify elements. Can serve as fingerprints that allow us to identify different elements present in a sample, even in trace amounts. Atomic and molecular spectra are important indicators of the underlying structure of the species.
Rydberg equation is an empirical equation that relates the wavelengths of the lines in the hydrogen spectrum. Derived from numerous observations, not from theory LOOK AT SLIDE
When an electron is excited from a lower energy level to a higher one it absorbs a definite (or quantized) amount of energy. When the electron falls back to the original energy level, it emits exactly the same amount of energy it absorbed in moving from the lower to the higher energy level
Orbits Orbits get farther apart as n increases, but their energies get closer together.
Postulates of Bohr’s theory Atom has a number of definite and discrete energy levels (orbits) in which an electron may exist without emitting or absorbing electromagnetic radiation. As the orbital radius increases so does the energy
Postulates of Bohr's theory The larger the value of n, the farther from the nucleus is the orbit being described and the radius of this orbit increases as the square of n increases.
Postulates of Bohr's theory e- may move from one energy level/orbit to another, but, in so doing, monochromatic radiation is emitted or absorbed in accordance with the following equation. Energy is absorbed when e- jump to higher orbits Energy is emitted when e- fall to lower orbi
Postulates of Bohr's theory e- moves in a circular orbit about nucleus & motion is governed by ordinary laws of mechanics & electrostatics, with the restriction that the angular momentum of the e- is quantized (can only have certain discrete values).angular momentum = mvr = nh/2pi
origin of emission spectra Light of a characteristic wavelength (and frequency) is emitted when electrons move from higher E (orbit, n = 4) to lower E (orbit, n = 1).
origin of absorption spectra Light of a characteristic wavelength (and frequency) is absorbed when electrons jump from lower E (orbit, n = 2) to higher E (orbit, n= 4)
Electron wavelength =h/(mv)
Created by: tilleryc