Quantum notes
What is the full electron configuration for copper (Cu)?
1s22s22p63s23p64s13d10
Is this the proper electron configuration for molybdenum (Mo)? If not, correct it. 1s22s22p63s23p64s23d4
1s22s22p63s23p64s13d5
How does the 1st ionization energy change from left to right across the Light and Quantum Review Answers Periodic Table?
Increases
What is the trend for electronegativity from left to right across the Periodic Table?
Increases
What is the Noble gas electron configuration for bromine (Br)?
[Ar] 4s23d104p5
What is the abbreviated electron configuration for xenon (Xe)?
[Xe]
Write the full electron configuration for lead (Pb)
1s22s22p63s23p64s23d104p65s24d105p66s24f14 5d106p2
What is the full electron configuration for titanium (Ti)?
1s22s22p63s23p64s23d2
What is the final entry configuration for the element sulfur (S)?
3p4
What is the final entry electron configuration for silver (Ag)?
5s14d10
Convert 620. nm to meters.
6.20x10-7 m
How does the atomic radius change from left to right across the Periodic Table?
Decreases
What happens to the ionic radius from left to right on the Periodic Table?
Decreases to Group 3, then increases, then decreases
What do each of the variables in E=hν represent, and what units are associated with each?
E = energy in J h = Planck's constant in J/Hz or J·s ν = frequency 1/s or Hz
List the electromagnetic spectrum in order from low frequency to high frequency
Radio Microwave Infrared Visible Ultraviolet X-Ray Gamma
Why do Cr, Mo, Cu, and Ag have exceptions for filling the orbitals (electron configurations)?
Those elements take one electron from the s orbital to make the d orbital half or completely filled
What do each of the variables in c=λν represent, and what units are associated with each?
c = speed of light in m/s λ = wavelength in m or nm v = frequency in 1/s or Hz
What is the trend for electronegativity down a group on the Periodic Table?
decreases
What happens when an electron falls from an excited state back down to its ground state?
emits light
A valence electron goes from energy level n=1 to n=4. At this point, the electron configuration or state of the atom is called the _____ state.
excited
What is the trend for atomic radius down a group on the Periodic Table?
increases
What is the trend for ionic radius down a group on the Periodic Table?
increases
List the final orbital type and electron quantity for the halogens
p5
Which color in the visible spectrum has the longest wavelength?
red
What is the orbital type and electron quantity for elements in the alkaline earth metals?
s2
How many orbitals are possible for n=2 (Period 2)?
s=1, p=3 for a total of 4
Give the maximum number of orbitals than can exist per energy level for each of the following: s, p, d, f
s=1, p=3, d=5, f=7
How many electrons can inhabit all of the n=5 orbitals?
s=2, p=6, d=10, f=14 total = 32
What is the hybridization for carbon in CO2?
sp
What is the hybridization for the central atom of NH3?
sp3
What is the hybridization for sulfur in SF6?
sp3d2
Which color in the visible spectrum has the highest frequency?
violet
List the visible spectrum from high energy to low energy.
violet, indigo, blue, green, yellow, orange, red
What is the frequency of a photon with a wavelength of 730 nm?
ν = 4.1x1014 Hz
What is the energy of a photon with wavelength 600 nm?
ν = 5x1014 Hz E = 3x10-19 J
What is the frequency of a photon with energy of 4.3 x 10-19J
ν = 6.5x1014 Hz
What is the energy of a photon of light with a wavelength of 4.5x10-7m?
ν = 6.7x1014 Hz E = 4.4x10-19 J
What is the wavelength of a photon with energy of 5.5x10-19J
ν = 8.3x1014 Hz λ = 3.6x10-7 m
What is the energy of a photon with wavelength 6.2x10-7m?
ν=4.8x10-7 Hz E = 3.2x10-19J
What is the frequency of a photon with energy of 6.22x10-19J?
ν=9.35x1014 Hz
