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Date:
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ACADEMIC Chapter 4 Review Sheet
Vocabulary
Define the following words:
electromagnetic radiation
amplitude
wavelength
frequency
speed of light
visible spectrum
quantum
Planck’s constant
photoelectric effect
photon
line spectrum
quantum number
ground state
excited state
matter wave
uncertainty principle
quantum-mechanical model
electron density
orbital
principal energy level
sublevel
electron configuration
orbital diagram
Section 4-1
1. Calculate the wavelength, in nm, of light that has a frequency of 1.23 ´ 1012 Hz. Show your work.
2. Calculate the frequency, in Hz, of light that has a wavelength of 625 nm. Show your work.
3. What are the four characteristics of a wave?
4. What is the speed of light in meters/second? You must memorize this.
5. What happens to the frequency of light if you decrease the wavelength? (i.e. Does the frequency increase or decrease?)
Section 4-2
6. What is Planck’s constant? You must memorize this.
7. Why don’t we notice quantized energy in the world around us?
8. What particle shoots out of the sheet of Na metal in the photoelectric effect?
9. How did Einstein explain why violet light, no matter how dim, initiates the release of electrons from Na metal?
10. Why don’t radio waves, no matter how intense, hurt us?
11. Use an analogy to explain the difference between a continuous change and a quantized change.
Section 4-3
12. How did Bohr explain the line spectra from elements when they are energized (either by heat or electricity)? I.e. Where do the lines from an atomic line spectrum come from with respect to electrons?
13. Explain what Louis de Broglie meant by matter waves?
14. Why can’t photons be used to find the location of electrons?
15. How do we know what elements are in Jupiter’s atmosphere if we have never been there?
16. Why can’t an electron’s position and momentum be known at the same time?
Section 4-4
17. Sketch the shape of an s-orbital. Sketch the shape of a p-orbital. Sketch the shapes of the two kinds of d-orbitals.
18. Complete the following table:
Energy Level / Names of the Sublevel(s) / Total number of orbitals this energy level represents / Maximum number of electrons this energy level can holdn=1
n=2
n=3
19. What is the difference between an orbit and an orbital?
20. What is Pauli’s exclusion principle?
Section 4-5
21. What part of the atom comes into contact when two atoms interact?
22. How many electrons does Na have? How about Na+?
23. How many electrons does Se have? How about Se-2?
24. Chromium does not strictly follow the Aufbau Principle. What is the actual electron configuration for Cr?
25. Copper does not strictly follow the Aufbau Principle. What is the actual electron configuration for Cu?
26. Identify the element with the following electron configuration: 1s22s22p2.
27. Identify the element with the following electron configuration: 1s22s22p63s23p64s23d3.
28. Write the electron configuration for oxygen. How many unpaired electrons does this element possess?
29. Write the electron configuration for nickel. How many unpaired electrons does this element possess?
30. Write the electron configuration for selenium. How many unpaired electrons does this element possess?
Name:
Date:
Period:
ACADEMIC Chapter 4 Review Sheet
Vocabulary
Define the following words:
electromagnetic radiation
amplitude
wavelength
frequency
speed of light
visible spectrum
quantum
Planck’s constant
photoelectric effect
photon
line spectrum
quantum number
ground state
excited state
matter wave
uncertainty principle
quantum-mechanical model
electron density
orbital
principal energy level
sublevel
electron configuration
orbital diagram
Section 4-1
1. Calculate the wavelength, in nm, of light that has a frequency of 1.23 ´ 1012 Hz. Show your work.
(ANS: 2.44 ´ 105 nm)
2. Calculate the frequency, in Hz, of light that has a wavelength of 625 nm. Show your work.
(ANS: 4.80 ´ 1014 Hz)
3. What are the four characteristics of a wave?
(ANS: amplitude, wavelength, frequency, and speed)
4. What is the speed of light in meters/second? You must memorize this.
(ANS: 3.00 ´ 108 m/s)
5. What happens to the frequency of light if you decrease the wavelength? (i.e. Does the frequency increase or decrease?)
(ANS: the frequency increases)
Section 4-2
6. What is Planck’s constant? You must memorize this.
(ANS: 6.6262 ´ 10-34 J s)
7. Why don’t we notice quantized energy in the world around us?
(ANS: The quantum size is too small to notice.)
8. What particle shoots out of the sheet of Na metal in the photoelectric effect?
(ANS: electrons)
9. How did Einstein explain why violet light, no matter how dim, initiates the release of electrons from Na metal?
(ANS: light is made of photons or particles of light. When a photon of violet light, which has a lot of energy, hits an electron, it transfers enough energy for the electron to escape)
10. Why don’t radio waves, no matter how intense, hurt us?
(ANS: a photon of radio waves don’t have enough energy to displace our electrons)
11. Use an analogy to explain the difference between a continuous change and a quantized change.
(ANS: a ramp is like a continuous gradient and stairs are like a quantum gradient; you can be at any point on a ramp but you can’t be on step 1.5; you are either on step one or step two if you have enough energy)
Section 4-3
12. How did Bohr explain the line spectra from elements when they are energized (either by heat or electricity)? I.e. Where do the lines from an atomic line spectrum come from with respect to electrons?
(ANS: each line on the atomic line spectra represents a jump from an excited state to a lower energy or ground state)
13. Explain what Louis de Broglie meant by matter waves?
(ANS: all matter has a wavelength)
14. Why can’t photons be used to find the location of electrons?
(ANS: photons of light used as a probe move the electron as its measuring its location)
15. How do we know what elements are in Jupiter’s atmosphere if we have never been there?
(ANS: The elements in Jupiter emits light. When the light reaches earth, we can send that light through a prism to see what atomic line spectra it contains and therefore elucidate the elements present)
16. Why can’t an electron’s position and momentum be known at the same time?
(ANS: because of Heisenberg’s uncertainty principle, the photon of light itself moves the electron; the tool used to measure the position of the electron itself moves the electron).
Section 4-4
17. Sketch the shape of an s-orbital. Sketch the shape of a p-orbital. Sketch the shapes of the two kinds of d-orbitals.
(ANS: see page 144 and 145 in the textbook)
18. Complete the following table:
Energy Level / Names of the Sublevel(s) / Total number of orbitals this energy level represents / Maximum number of electrons this energy level can holdn=1
n=2
n=3
First line: s, 1 orbital, 2 electrons
Second line: s and p, 4 orbital, 8 electrons
Third line: s and p and d, 9 orbitals, 18 electrons
19. What is the difference between an orbit and an orbital?
(ANS: an orbit has a fixed path; an orbital deals with probability)
20. What is Pauli’s exclusion principle?
(ANS: each orbital holds two electrons max and if the orbital hold two electrons, the two must have different spin)
Section 4-5
21. What part of the atom comes into contact when two atoms interact?
(ANS: the electrons)
22. How many electrons does Na have? How about Na+?
(ANS: 11 electrons, 10 electrons)
23. How many electrons does Se have? How about Se-2?
(ANS: 34 electrons, 36 electrons)
24. Chromium does not strictly follow the Aufbau Principle. What is the actual electron configuration for Cr?
(ANS: 1s22s22p63s23p64s13d5)
25. Copper does not strictly follow the Aufbau Principle. What is the actual electron configuration for Cu?
(ANS: 1s22s22p63s23p64s13d10)
26. Identify the element with the following electron configuration: 1s22s22p2.
(ANS: carbon)
27. Identify the element with the following electron configuration: 1s22s22p63s23p64s23d3.
(ANS: vanadium)
28. Write the electron configuration for oxygen. How many unpaired electrons does this element possess?
(ANS: 1s22s22p4)
29. Write the electron configuration for nickel. How many unpaired electrons does this element possess?
(ANS: 1s22s22p63s23p64s23d8)
30. Write the electron configuration for selenium. How many unpaired electrons does this element possess?
(ANS: 1s22s22p63s23p64s23d104p4)