1. Electron Configuration
Light
Periodic Trends
Electronic Structure
Electron Configuration
Mixed Bag
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2. Mixed Bag

3. Which element has the electron configuration 1s22s22p63s23p3?

4. If you add up the exponents, there are 15 electrons which corresponds to phosphorous.
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5. What is the difference between the ground state and the excited state for an electron?

6. The ground state is the lowest energy level for an electron; the excited state is when an electron is at an energy level above its normal state (the excited state is temporary).
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7. How many valence electrons does carbon have in it’s outer shell?

8. The second energy level is the outside shell in this case. There are
C = 1s22s22p2
The second energy level is the outside shell in this case. There are
4 electrons in the second energy level (valence shell) for carbon.
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9. What is wrong with the following orbital diagrams
What is wrong with the following orbital diagrams? Which rules/principles do they violate? 1) 2)

10. ***Violates Hund’s Rule – electrons won’t pair up within a sublevel until they have to!
**Violates Hund’s Rule & Aufbau Principle: electrons must completely fill lower energy sublevels before filling higher energy sublevels
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11. How does this relate to the charge on a bromide ion?
How many unpaired electrons are in a bromine atom?
How does this relate to the charge on a bromide ion?

12. Bromine has 1 unpaired electron in it’s orbital diagram which makes sense since bromide ions have a charge of -1 (they have gained 1 e- to complete their valence shell).
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13. Periodic Trends

14. Which atom would have the largest ionization energy –
Mg or Cl?

15. (e- are held closer so it will be harder to rip the e- off)
Chlorine would have the largest I.E. because it is farther right on the periodic table
(e- are held closer so it will be harder to rip the e- off)
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16. Define the term “electron affinity”

17. The energy involved when an atom gains an electron.
(The opposite of ionization energy)
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18. Rank the following elements in order of increasing atomic radius:
In, Al, B, Ga

19. B < Al < Ga < In
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20. Rank the elements in order of increasing metallic character:
N, Zr, Cs, Co

21. N < Co < Zr < Cs
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22. Describe the comparative size of a cation compared to the atom from which it forms.

23. Cations are smaller than the atoms from which they form due to the increasing proton/electron attraction due to the loss of electrons.
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24. Electron Configuration

25. What is the electron configuration for cobalt?

26. Co =
1s22s22p63s23p64s23d7
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27. What is the noble gas configuration for zirconium?

28. Zr =
[Kr]5s24d2
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29. What is the orbital configuration for sulfur?
(i.e. Draw an orbital diagram)

30. 1s s p
3s p
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31. What is the electron configuration for iridium?

32. Ir = 1s22s22p63s23p64s23d10 4p65s24d105p66s24f145d7 or [Xe]6s24f145d7
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33. (Not just the relation to the periodic table!)
What do the coefficient, letter, and exponent signify when writing electron configurations?
(Not just the relation to the periodic table!)

34. Coefficient = principal energy level Letter = sublevel
Exponent = # of electrons in sublevel
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35. Electronic Structure

36. (Think about what the letters stand for)
What are the 3-D shapes of the atomic orbitals comprising the s, p, d, and f sublevels?
(Think about what the letters stand for)

37. s = sphere p = peanut d = dumbell (clover) f = flower
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38. Which sublevels (s, p, d, or f) are located in the fifth principal energy level?

39. The fifth energy level has s, p, d, and f sublevels present.
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40. How many total electrons can fit into the third principal energy level
How many total electrons can fit into the third principal energy level? (Taking into account all sublevels present)

41. The third energy level contains s, p, and d sublevels so 2 + 6 + 10 =
18 total electrons!
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42. How do you draw arrows in an orbital diagram and why are they drawn that way?

43. Arrows are drawn with the first pointing up and the second pointing down due to the Pauli Exclusion Principal (electrons must have opposite spins in the same orbital).
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44. Define the Aufbau Principle and how it relates to the electrons in an atom.

45. The Aufbau Principle says that electrons completely fill from the lowest energy level to the highest energy level.
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46. Light

47. What is meant by the statement: “Light has a dual nature”

48. Light behaves as both a particle and a wave.
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49. What is the wavelength of a portion of light having a frequency of 4
What is the wavelength of a portion of light having a frequency of 4.73 x 1012 Hz?

50. Use c = λν…
λ = 6.34 x 10-5 m
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51. Calculate the energy of a photon of light having a frequency of
3.11 x 1013 kHz.

52. Use E = hv…
E = 2.06 x J
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53. What is the wavelength (in nanometers
What is the wavelength (in nanometers!) of a portion of light having an energy of 1.44 x J?

54. Use both light equations or First calculate the frequency…
E = hc/λ!
First calculate the frequency…
v = 2.17 x 1021 Hz
Then use v to find λ…
λ = 1.38 x m =
1.38 x 10-4 nm
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55. Describe why you saw colors in the flame during the flame test lab (think about what is going on with the electrons)

56. As the element samples are placed in the flame, the electrons are given energy so they jump from the ground state to the excited state. When the electrons go back down to the ground state, they emit this extra energy which we see as light (the color depends on the λ and v).
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57. What is the electron configuration for a chloride ion?
Final Jeopardy
What is the electron configuration for a chloride ion?

58. Final Jeopardy Cl-1 = 1s22s22p63s23p6
Chloride would be isoelectronic with argon after gaining one electron to form the Cl- ion (they have the same number of electrons although they have different numbers of protons).
Cl-1 = 1s22s22p63s23p6