Honors Chemistry
Worksheet 2.1
Name ________________________
Date _________ Class _________
12. What was Max Planck’s quantum hypothesis?
1.
Draw three waves with wavelengths of x, 2x, and 4x.
13. What happens to an electron as it absorbs a photon of
light?
2.
Order the wavelengths from question #2 from lowest to
highest frequency.
14. What is a “packet” of EM energy called?
3.
Order the wavelengths from lowest to highest energy and
explain your answer.
15. What is the range of frequencies for visible light?
16. What is the range of wavelengths of visible light?
4.
Microwaves are used to transmit information. What is the
wavelength of a microwave having a frequency of
3.44x109 Hz?
17. Define Electromagnetic radiation.
18. Is an electron a particle or a wave, explain?
5.
An X-Ray has a wavelength of 1.15x10-10m. What is it’s
frequency?
19. Describe the mathematical relationship between
wavelength and frequency.
6.
How much energy does a photon with a wavelength of
250nm have?
20. Give two examples of electromagnetic radiation with long
wavelengths.
7.
Why does ultraviolet light cause more damage to our skin
than visible light?
8.
As the frequency of light increases what happens to its
energy?
9.
What causes an atom to emit light?
10. What do we mean by the speed of EM radiation, how fast
is it?
11. Why do we say atomic spectra are like fingerprints of the
elements?
21. Which is the longer wavelength: blue light or red light?
Explain.
22. List the following types of electromagnetic radiation in
order of decreasing frequency:
(a)
X rays used for medical purposes
(b)
infrared from a heating lamp
(c)
TV signal from Channel 12
(d)
yellow traffic light
(e)
ultraviolet light that causes sunburn
23. Of the following regions of the electromagnetic spectrum,
which one has the shortest wavelength?
a. microwaves
b. infrared radiation
c. X-Ray
d. ultraviolet rays
e. radio waves
f. gamma rays
24. Complete the following table:
Energy
Number of
Sublevel letter(s)
Level (n)
sublevels
1st
2nd
3rd
4th
# of
electrons
25. What is an orbital? How many orbitals are possible at
each sublevel?
35. Describe the quantum mechanical model of the atom and
who described it?
36. Identify the atom based on the electron configuration
given:
a. [Kr]5s24d8
b. [Ar]4s23d104p4
c. [Xe]6s24f145d7
d. [He]2s2
e. [Rn]7s25f3
37. Describe the four quantum numbers: n, l, ml, ms
26. Write the electron configuration for the following
elements: Ba, P, I, Zr, Bi
38. What are the possible range of values for n, l, ml, ms ?
27. An atom’s electron configuration ends in 5s24d105p4.
Identify the element.
28. Draw the shape of an s and a p orbital.
39. Write all the quantum numbers for S.
29. Accurately explain the emission spectrum lines for a
hydrogen atom. In other words, exactly what produces
them?
30. Why are the energy levels in Bohr’s model of the atom
described like stair-steps rather than like a ramp?
40. Use the following quantum numbers to identify the
element: (1,0,0,+½) (1,0,0,-½) (2,0,0,+½) (2,0,0,-½)
(2,1,-1,+½) (2,1,0,+½).
41. Describe the Aufbau principle.
31. What are the differences between the 2s orbital and the
1s orbital of hydrogen? How are they similar?
32. The number of sublevels in an energy level
(increases/decreases) as the energy level number
increases?
42. Describe the Pauli Exclusion Principle.
43. Describe Hund’s Rule.
44. What are valence electrons
33. How do we know that the energy levels of the hydrogen
atom are not continuous, as physicists originally
assumed?
34. What does it mean to say that an atom is in an “excited
state”?
45. Draw the Lewis electron dot diagram for the following
elements:
a.
C
b.
P
c.
Ca
d.
Mn
e.
I