Mixed Bag

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.

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).

7. How many valence electrons does carbon have in it’s outer shell?

8. 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.

9. 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

11. 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).

13. Periodic Trends

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

15. 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)

16. Define the term “electron affinity”

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

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

19. B < Al < Ga < In

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

21. N < Co < Zr < Cs

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.

24. Electron Configuration

25. What is the electron configuration for cobalt?

26. Co = 1s22s22p63s23p64s23d7

27. What is the noble gas configuration for zirconium?

28. Zr = [Kr]5s24d2

29. What is the orbital configuration for sulfur? (i.e. Draw an orbital diagram)

30. 1s 2s 2p 3s 3p

31. What is the electron configuration for iridium?

32. Ir = 1s22s22p63s23p64s23d10 4p65s24d105p66s24f145d7 or [Xe]6s24f145d7

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

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

35. Electronic Structure

36. 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

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.

40. 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!

42. How many orbitals are found in the 4f?

43. 7 orbitals in an f sublevel

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.

46. Light

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

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

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

50. Use c = λν… λ = 6.34 x 10-5 m