Study Guide for CHEM 101 Test 2
Chapters 7, 8 & 9

  1. For each of the compounds below, draw the Lewis structure.

    1. PBr3
    2. CCl4
    3. CO2
    4. BF3
    5. PF5
    6. SF4
    7. SeCl6
    8. I3-
    9. XeF4
    10. ICl3
    11. ClO3-

  2. Properly name the following compounds.

    1. MnSO4
    2. AlPO4
    3. P2O3
    4. K3PO4
    5. KClO3
    6. Sc2S3
    7. N2O5
    8. Ca(NO3)2
    9. CoNO3
    10. FeSO4

  3. Draw Lewis structures for these more complex molecules:

    1. hydrazine H2N-NH2
    2. ethylene H2C=CH2
    3. propylene (CH3)CH=CH2

  4. Define:

    1. valence electrons
    2. bonding pair of electrons
    3. lone pair or non-bonding pair (electrons)
    4. electronegativity
    5. first ionization energy
    6. electronegativity
    7. quantum number
    8. n
    9. l
    10. ml
    11. ms
    12. Pauli exculsion priciple
    13. Hund's rule
    14. periodicity
    15. period
    16. group or family
    17. isoelectronic
    18. paramagnetic
    19. diamagnetic

  5. Predict the products for the reaction between the paired elements below.

    1. O and Li
    2. P and S
    3. S and F
    4. Al and F
    5. Mg and N

  6. What are the electron configurations for the elments below? Follow the Aufbau (building-up) principle.

    1. Mn

    2. Se

    3. Pr

    4. Pb

    5. As

    6. Sr

    7. In

    8. He

    9. Mg

    10. Sc

  7. Provide the quantum numbers for the last electron placed in each of the elements in problem above.

  8. Tell if each element in the problem two problems above is diamagnetic or paramagnetic.

  9. Rationalize your way to the proper electron configurations for these exceptions to the Aufbau (building-up) principle

    1. Cr

    2. Gd

    3. Au

    4. Pd

    5. Mo

  10. What is the trend for electronegativity?

  11. What is the trend for first ionization energy?

  12. What is the trend for electron affinity?

  13. Given the formula for the compound below in each example, predict the formula for the compound asked for

    1. If the formula for the oxide of aluminum is Al2O3, what would the formula for the oxide of indium, In, be?

    2. If the formula for the sulfide of beryllium is BeS, what would the formula for the sulfide of strontium, Sr, be?

    3. If the formula for the nitride of sodium is Na3N, what would the formula for the phosphide (P3-) of sodium be?

    4. If the formula for the fluoride of of zinc is ZnF2, what would the formula for the fluoride of cadmium, Cd, be?

    6. If the formula for the oxide of titanium is TiO2, what would the formula for the oxide of zirconium, Zr, be?

  14. Are the compounds below ionic or covalent?

    1. CH4

    2. Na2S

    3. SO3

    4. Na2SO3

    5. MgH2

    6. P2S3

    7. BF3

    8. AlBr3

    9. SeO2

    10. CO2

  15. Determine the formal oxidation state of the underlined element in the compounds and ions below:

    1. ClO4-

    2. P2O3

    3. Fe2(SO4)3

    4. PPF5

    5. ClO2-

    6. SnS2

    7. PO43-

    8. ClO-

    9. Li3N

    10. CO32-

  16. Label all the columns and parts of the periodic table on the blank periodic table below: