Mixed Bag

3. Mixed Bag

4. Which element has the electron configuration 1s22s22p63s23p3?

5. If you add up the exponents, there are 15 electrons which corresponds to phosphorous.

6. What is the difference between the ground state and the excited state for an electron?

7. 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).

8. How many valence electrons does carbon have in it’s outer shell? (Hint: first write out the e- configuration)

9. 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.

10. How many unpaired electrons does germanium have in it’s valence shell? (Hint: draw the orbital diagram first!)

11. After drawing the orbital diagram, there are 2 unpaired electrons in the germanium atom.

12. How many unpaired electrons are in there in a bromine atom? How does this relate to the charge on a bromide ion?

13. 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).

14. Periodic Trends

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

16. 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)

17. Define the term “electron affinity”

18. The energy involved when an atom gains an electron. (The opposite of ionization energy)

19. Rank the following elements in order of increasing atomic radius: In, Al, B, Ga

20. B < Al < Ga < In

21. Rank the elements in order of increasing metallic character: N, Zr, Cs, Co

22. N < Co < Zr < Cs

23. Describe the comparative size of a cation compared to the atom from which it forms.

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

25. Electron Configuration

26. What is the electron configuration for cobalt?

27. Co = 1s22s22p63s23p64s23d7

28. What is the noble gas configuration for zirconium?

29. Zr = [Kr]5s24d2

30. What is the orbital configuration for sulfur?

31. 1s 2s 2p 3s 3p

32. What do the coefficient, letter, and exponent signify when writing electron configurations?

33. Coefficient = principal energy level Letter = sublevel Exponent = # of electrons in sublevel

34. What is the electron configuration for iridium?

35. Ir = 1s22s22p63s23p64s23d10 4p65s24d105p66s24f145d7

36. Quantum #’s

37. What is the maximum number of electrons that can be contained in an: s sublevel? p sublevel? d sublevel? f sublevel?

38. s sublevel – 2 e- p sublevel – 6 e- d sublevel – 10 e- f sublevel – 14 e-

39. Which sublevels (s, p, d, or f) are located in the fourth principal energy level?

40. The third energy level has s, p, d, and f sublevels present.

41. How many total electrons can fit into the third principal energy level? (Take into account all sublevels present in the 3rd energy level)

42. The third energy level contains s, p, and d sublevels so 2 + 6 + 10 = 18 total electrons!

43. How do you draw arrows in an orbital diagram and why are they drawn that way?

44. 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).

45. Define the Aufbau Principle and how it relates to the electrons in an atom.

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

47. Light

48. Describe the dual nature of light

49. Light behaves as both a particle and a wave.

50. What is the wavelength of a portion of light having a frequency of 4.73 x 1012Hz?