3.3 Review
Name________________________________
Quantum Theory & The Atom
Period_______Date_____________________
Part I: True and False - If the statement is true write “true.” If it is false, change the underline word to
make it correct.
____________________1. Planck proposed that the energy emitted or absorbed by any object is restricted
to quanta of particular sizes.
____________________ 2. We are not aware of quantum effects in the world around us because quanta
of energy are very large.
____________________ 3. Light consists of protons, which are quanta of energy behaves like tiny
particles.
____________________ 4. We are constantly surrounded by low frequency X-rays.
____________________ 5. Planck’s theory relates the frequency of radiation to its energy.
____________________ 6. The dual nature of light means that light has the properties of a charge and a
wave.
Part II: Completion – Complete the following sentences.
7. Every element has a uniquely characteristic atomic ____________________ spectrum.
8. An electron that absorbs a quantum of energy can jump to a level of _______________ energy, called
an excited state of the atom.
9. _________________is emitted when an electron jumps from a higher energy level to a lower energy
level.
10. The Bohr model is an inaccurate model of the atom because there is no way to measure the exact
_________________ of an electron in an atom.
11. When radiation is absorbed by a hydrogen electron, the hydrogen atom changes its ground state to an
____________________ state.
Part III: Matching – On the line at the left, write the first letter of the scientist’s name who made the
contribution to the quantum theory listed below. Each name may be used more than once.
Planck
Bohr
Heisenberg
______ 12. Stated that energy is emitted or absorbed in discrete pieces called quanta.
______ 13. Used Planck’s idea of quantization to explain the line spectrum of hydrogen.
______ 14. Stated that the position and momentum of a moving object cannot be simultaneously
measured and known exactly.
______ 15. Labeled each energy level in his atomic model with the principal quantum number, n.
______ 16. Wrote the equation E=h.
______ 17. The constant, h, is named for this scientist.
______ 18. Stated that you cannot observe or measure the “orbit” of an electron.
Part IV: Drawing
19. Label the energy levels n=1,n=2, and n=3 on the Bohr atom.
20. Label the ground state in this atom.
21. Label an excited state of this atom.
22. Draw an arrow to show the direction an electron moves when it absorbs energy.
Part V: Short Answer
23. Use an analogy to explain the difference between a continuous change and a quantized change.
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24. Describe the difference between a continuous spectrum and a line spectrum, and name a source of each.
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