Electromagnetic Spectrum
Bohr Model
Quantum Model
Quantum Principles
Electron configuration
100
What is the range of 750nm-380nm called?
The visible light spectrum
100
How is the Bohr model typically described?
The solar system/ planet model. Electrons orbiting the nucleus.
100
How is the quantum model different than the bohr model?
electrons are actually found in regions that can be determined mathematically rather than a fixed point around the nucleus.
100
What is the Pauli Exclusion Principle?
Means that there can be no 2 electrons that occupy the same space so they must have opposite spins.
100
What is the electron configuration for Nitrogen?
1s22s22p3
200
Which color has a shorter wavelength? Red or Blue?
Blue
200
According to the Bohr model how many electrons can be in n=1; n=2; n=3?
2, 8, 8
200
What are the 4 Quantum numbers?
Principle quantum number, azimuthal quantum number, magnetic quantum number, and spin projection.
200
What is the Aufbau principle?
Electrons must occupy all the lower energy shells before moving up to the next energy shell.
200
What is the noble gas configuration for Ne
(Ne)
300
How are wavelength and frequency related?
As wavelength increases, frequency decreases and vice versa.
300
Which shell has a higher energy level? n=2 or n=4?
n=4
300
How is the integer designation of the azimuthal quantum number found? Ex. What is the azimuthal quantum number for n=3? What is its letter designation?
l=n-1 so l=2 which is d.
300
What is hunds rule?
One electron in each sub orbital before filling up the rest.
300
What is the electron configuration for Nickel?
1s22s22p63s23p64s23d8
400
Light exists in what form?
Both waves and particles
400
Describe what happens when a photon hits an electron in a particular element.
The electron is excited and moves up an energy shell. However, the electron doesn't stay excited for long and ends up moving back down to its ground state. This emits a particular wavelength of light.
400
What does the magnetic quantum number tell us about the electron?
The shape and orientation of the electron within its subshell.
400
What element is this orbital diagram for? 
Sulfur
400
What is the electron configuration for Chromium?
1s22s22p63s23p64s13d10
500
What is the equation that relates photons with wavelength? What is it called?
E=hf ; plancks relation
500
Define Spectroscopy
the science of identifying elements based on their particular spectrum of light that is emitted after photons excite electrons in that element.
500
If I am referring to n=3, what are the subshell names within this energy shell? Ex. n=1 is 1s
3d, 3p, 3s
500
Why is there an exception to the Aufbau principle with some elements in the d orbital?
Because in some elements it is more energetically favorable for the electrons in the d orbital to be filled, so it steals an extra electron from the s orbital.
500
Why are noble gases considered perfectly stable elements and the reason we use them for condensed electron configurations?
Because they have all of their shells filled with electrons. Energetically stable.