UNIT 4 REVIEW - 2016

Vocabulary:

  • Groups
  • Periods
  • Transition/inner transition elements
  • Alkali metals
  • Alkaline earth metals
  • halogens
  • noble gases
  • octet rule
  • valence electrons
  • electronegativity (and the trend on the P/T)
  • cation/anion
  • ionic bond/covalent bond
  • monatomic/polyatomic ions
  • metallic bonding
  • molecule
  • rules for naming acids
  • rules for naming molecules
  • rules for naming ionic compounds
  • roman numbers
  • characteristics of ionic & covalent compounds (melting point and conductivity)
  • Energy diagram of bond strength and length
  • Coulomb’s law (how it helps bond strength)
  • prefixes (mono, di, tri, etc)
  • metals vs. nonmetals vs. metalloids on the periodic table
  • polar bond/molecule

Answer questions 1 – 7 on a separate sheet of paper.

  1. Describe how to make a cation vs. an anion.
  2. What is the octet rule?
  3. List all the rules for naming molecules, then name/give the formula for the following:

◦CO

◦H2O

◦N2F6

◦Carbon tetrafluoride

◦sulfur trioxide

◦dinitrogen tetrachloride

  1. Name the following compounds and then after the name, identify if they are covalent molecules, ionic compounds, or acids

  1. AgNO3
  2. HClO2
  3. CuOH
  4. H2CO3
  5. (NH4)2Cr2O7
  6. Pb(CrO4)2
  7. H2CO3
  8. BCl3
  9. C2H6

  1. Write the formulas for the following and identify if they are covalent molecules, acids, or ionic compounds.

  1. Nitrous Acid
  2. copper (II) nitrate
  3. phosphorus tetrasulfide
  4. Hydroselenic Acid
  5. carbon monoxide
  6. Phosphoric Acid
  7. magnesium sulfate
  8. Acetic Acid
  9. dihydrogen monoxide
  10. sodium nitride

  1. Fill in the following table

Sulfide Ion / Hydroxide Ion / Phosphate Ion / Sulfate Ion / Oxide ion / Fluoride ion
Calcium Ion
Ammonium Ion
Aluminum Ion
Lead IV Ion
  1. On the diagram below, label the two arrows as either “bond length” or “bond energy.”

  1. At which position above (A, B, or C) would the repulsion be the strongest? ______
  2. At which position above (A, B, or C) would the attractive forces be the strongest? ______
  3. Which type of bonding forms a molecule?
  4. Which type of bond has a higher melting point?
  5. Under what conditions will the compounds conduct electricity?
  6. What is the trend in electronegativity on the periodic table? Atomic size? Ionization energy?
  7. How is atomic size connected to electronegativity and ionization energy?
  8. Describe, very specifically, what electronegativity is.
  9. Describe, with the use of a picture what the electrons in a metallic bond are doing. How does this contribute to 2 specific characteristics of metals?
  10. Explain, very completely, why if an atom gains an electron it becomes a negative ion.
  11. Explain the difference between ionic bonding and covalent bonding.
  12. Is there an easy way to decide if to atoms will bond ionic or covalently? Describe the process to determine how two atoms bond based on their electronegativity values. Pick 2 examples of your own.
  13. Draw an atomic model for the following compounds:
  14. Calcium nitrate
  15. sodium carbonate
  16. lead (II) Phosphite
  17. Iron (III) sulfate
  18. Which of the following depicts a chemical reaction? Physical change?