Orbitals
Rules! and stuff
e- configs
EM Spectrum
Periodic Trends
100
a specific, quantized amount of energy that an electron can have within an atom or molecule; discrete levels are where electrons can exist
What is an Energy Level
100
what element? [He] 2s2 2p2
Carbon
100
1s2 2s2 2p6 3s1
Sodium
100
The longest wavelengths are seen as which color on the visible light spectrum?
Red
100
Which atom is bigger- Na or Mg?
Na
200
How many electrons can the d orbitals/sublevel hold?
10
200
What rule is this? Electrons occupy the orbitals of the lowest energy levels first
Aufbau
200
[Ar] 4s2
What is Calcium(Cl)
200
The shortest wavelengths are seen as which color on the visible spectrum?
Violet
200
which element has the highest ionization energy? Ge, Se, Cu, Br, Co
Br
300
What is the least energetic orbital?
s
300
What rule? Each atomic orbital can "hold" 2 electrons and in order to occupy the same orbital they must have different quantum numbers/spins
Pauli Exclusion Principle
300
1s2 2s2 2p6 3s2 3p6 4s1
K
300
What is the relationship between energy and wavelength?
as wavelength increases, energy decreases, and as wavelength decreases, energy increases. Inverse
300
Which element has the largest atomic size- He, F, Ar, or Na?
Na
400
How many orbitals make up the p orbitals/sublevel?
3
400
What rule? when electrons are assigned to equal orbitals, one electron goes in each orbital before being paired.
Hund's Rule
400
[Ar] 3d10 4s2 4p6
What is Krypton(Kr)
400
What terms are used to describe "a", "b", and "d"?
a is crest, b is trough, d is wavelength
400
Two elements belong to the same period. A is an alkali metal and B is an alkali-earth metal. Which has bigger radius?
A
500
Sulfur's valance electrons will be in what orbital? Be specific!
3p
500
What element? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4p14 5d10 6p2
Pb
500
1s2 2s2 2p6 3s2 3p6 4s2 3d10
Zn
500
What is emitted as an electron drops back to its ground state?
A photon
500
Highest ionization energy: Bismuth, Antimony, Phosphorus
P