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Transcript
CHM 50
Class Activity – Chapter 7
Name
Complete the table of wavelength, frequency and energy values.
Wavelength
Frequency
Energy per photon
Energy per mole of
photons
522 nm
2.86 x 1015 s-1
9.41 x 10-24 J
1.44 kJ
2.
The retina of a human eye can detect light when radiant energy incident on it is at least 4.0 x 10-17 J. For
light of 5.85 nm wavelength , how many photons does this energy correspond to?
3.
What wavelength is predicted by the Rydberg equation for the following electron transitions in the hydrogen
atom? . n = 7 to n = 3
4.
Using the Bohr equation, calculate is the change in energy when an electron transitions from n = 3 to
n= 2 in a hydrogen atom.
5. Give the orbital designations of electrons with the following quantum numbers:
a. n = 3, l = 0, ml =0
b. n = 4, l = 2, ml = 0
6. What does the first quantum number tell us about an electron?
7. What does the second quantum number tell us about an electron?
8. Which sublevels are contained within the second energy level?
9. Which sublevels are contained within the fourth energy level?
10. What is an orbital?
11. What is the shape of an “s” orbital?
12. What is the shape of an “p” orbital?
13. How many orbitals are in each type of sublevel (s, p, d, f)?