Name: ______Date: ______Period: ______

Atomic Structure Unit Review – GT

Organization of the Periodic Table:

  1. The periodic table is arranged in order of increasing ______
  2. State the periodic law: ______

______

  1. Metals are on the (left, right) side of the metalloid line.
  2. Nonmetals are on the (left, right) side of the metalloid line.
  3. Alkaline earth metals are in group ______
  4. Alkali metals are in group ______
  5. Representative/Transition metals are in group ______
  6. Noble gases are in group ______
  7. Halogens are in group ______

Theories of Atomic Models:

  1. What part of Dalton’s atomic theory is incorrect? Why?

______

  1. Describe Thomson’s model of the atom. What part is still in effect today?

______

  1. Describe Rutherford’s model of the atom. How did he come up with this model?

______

  1. Describe Bohr’s model of the atom.

______

  1. How is the Cloud model different from Bohr’s model of the atom?

______

  1. What is the most probable location for an electron? ______
  2. Where are protons and neutrons found? ______
  3. The majority of the atom is: ______

Structure of the Atom

Complete the following table:

Element/Ion / Atomic # / Mass # / Protons / Neutrons / Electrons / Charge
20. /
21. / 17 / 35 / 18
22. / 32 / 20 / 0
23. /

24.  Atoms in questions 20 & 23 are an example of a/an ______.

25.  The relative average of all mass numbers for each isotope of an element equals the element’s ______.

26.  Calculate Calcium’s atomic mass: Show all work

Ca-40 96.941%

Ca-42 0.647%

Ca-43 0.135%

Ca-44 2.086%

Ca-46 0.004%

Ca-48 0.187% ______

Natural samples of copper contain two isotopes. 63Cu has a mass of 62.930 amu and 65Cu has a mass of 64.928 amu. The percent abundance of 63Cu is 69.09%. Calculate the atomic mass of copper.

27.  Identify the element/ion with 15 protons and 18 electrons: ______

28.  Identify the element/ion with 38 protons and 36 electrons: ______

29.  Identify the element/ion with 53 protons and 54 electrons: ______

30.  Identify the element/ion with 19 protons and 18 electrons: ______

Electron Configurations

31.  1s22s22p63s23p5

This element is in period ______. This element is in group ______and has ______valence electron(s) and ______unpaired electron(s). This element is ______. The letters indicate the ______of the orbital.

Write the electron configurations for the following atoms:

32.  S ______

33.  S2- ______

34.  U ______

35.  Au ______

Identify each neutral atom based on the following electron configurations:

36.  1s22s22p63s1 ______

37.  1s22s22p63s23p64s23d8 ______

38.  1s22s22p63s23p6423d104p5 ______

39.  Draw a violation of Pauli’s Exclusion Principle ______

40.  Draw a violation of Hund’s Rule ____________

41.  Draw a violation of Aufbau’s Principle ______

42.  Energy level 4 can have ____ sublevels: ______

43.  The “s” sublevel can hold ______electrons

44.  The “p” sublevel can hold ______electrons

45.  What is true of electron configurations of all noble gases? ______

Periodic Trends:

1 / 18
2 / 13 / 14 / 15 / 16 / 17
X / Z / K
3 / 4 / 5 / 6 / 7 / 8 / 9 / 10 / 11 / 12 / D / E / G
Q / T
J
A

46.  Which element has the highest electronegativity? ______

47.  Which halogen has the smallest atomic radius? ______

48.  Which element will hold its outer shell electron(s) the tightest? ______

49.  Which element does not form compounds? ______

50.  What is ionization energy? ______

______

**Make sure you are able to EXPLAIN periodic trends

51.  What are the quantum numbers for:

Cr: ______K:______

As: ______

52.  Identify the following with the quantum numbers:

4, 0, 0, -½ ______5, 2, 0, ½ ______

4, 3, 3, ½ ______

53.  Draw the orbital diagram for Sulfur

54.  Explain how you were able to see color during the flame test lab.