Name: ______Date: ______Period: ______

Covalent Bonding and Mixed Nomenclature Review KEY

Bonding:

  1. What type of elements (metal, nonmetal, or metalloid) are found in each of the following compounds or bonds
  2. AcidsHydrogen + nonmental(s) or a poly atomic ion
  3. Covalent compounds2 nonmentals
  4. Ionic compound metal + nonmetal (s)or a poly atomic ion
  5. Molecular compounds2 nonmetals (molecular = covalent))
  6. Polar compound2 nonmetals with electronegativity difference in between 0.5 to 1.9
  7. Nonpolar compounds2 nonmetals with electronegativity difference 0.5
  8. What type of bond (single, double, or triple) holds each of the following diatomic molecules together? {HINT DRAW the compound using Lewis structures}
  9. Oxygen O2DBc. Fluorine F2SBe. Chlorine Cl2 SBg. water SB
  10. Nitrogen N2TBd. Hydrogen H2 SBf. SO2DBh. NH3 SB
  11. How many lone pairs surround each element in the following diatomic molecules? {HINT DRAW the compound using Lewis structures}
  12. Oxygen O22LPc. Fluorine F23LPe. Chlorine Cl23LPg. oxygen in water2LP
  13. Nitrogen N21LPd. Hydrogen H20LPf. SO21 for Sh. nitrogen in NH3 1LP
  14. Classify each of the following compound as Ionic, Covalent or an Acid
  15. CS2covalent – Carbon disulfided. CaSO4ionic-Calcium sulfate g. N2O4covalent
  16. BaI2Ionic -Barium iodide e. PCl3covalent – Phosphorus trichlorideh. VO3ionic
  17. H3Pacid -Hydro phosphoric acidf. H3PO3acid - phosphorus acidi. PCl5covalent

g. Dinitrogen teroxide h. Vanadium (VI) oxide i. Phosphorus pentachloride

  1. Classify each of the following as polar or nonpolar covalent bonds. Use electronegativity values in book on page 177.
  2. O2nonpolar [EN difference: 3.5-3.5= 0].
  3. HClPolar [EN difference: 3.0-2.1 = 0.9]
  4. H2OPolar (very) [EN difference: 3.5-2.1 = 1.4]
  5. SO2Polar [EN difference: 3.5-2.5 =1.0]
  6. FClPolar [EN difference: 4.0-3.0 = 1.0]
  7. SCl2slightly polar [EN difference: 3.0-2.5 = 0.5

Naming

  1. What covalent prefix corresponds to each of the following numbers
  2. Onemonod. Fourtetrag. Sevenheptaj. Tendeca
  3. Twodiee. Fivepentah. Eightocta
  4. Three trif. Sixhexai. Ninenona
  5. When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a roman number.
  6. In naming a binary covalent compound, the number of atoms of each element present in the molecule is indicated by prefixes
  7. Compare and contrast the properties of Covalent and Ionic bonds

Ionic / Covalent
  1. Formed by
/ Metal and nonmetal or a poly atomic ion / 2 nonmetal
  1. Electrons
/ Transferred / Shared
  1. Melting point
/ Very high melting point / Low melting points
  1. Most common phase
/ Solid / Liquid or gas
  1. Conductors
/ Conduct in aqueous or molten solutions. / Do not conduct electricity.
  1. For the following items if given the name write the chemical formula and if given the formula write the name. Make sure you follow the correct naming rules.

  1. Phosphorous acid H3PO3
  2. Phosphorous pentachloride PCl5
  3. Aluminum oxide Al2O3
  4. Fe2(SO4)3 iron (III) sulfate
  5. Iron (III) chloride FeCl3
  6. SO3 sulfur trioxide
  7. AlPO4 aluminum phosphate
  8. H2SO3 sulfurous acid
/
  1. S2F6 disulfur hexafluoride
  2. Vanadium (IV) sulfide VS2
  3. HBr hydrobromic acid
  4. Calcium sulfate CaSO4
  5. Hydrosulfuricacid H2S
  6. Sulfuric acid H2SO4
  7. KCl potassium chloride
  8. CoO2 cobalt (IV) oxide

Properties

  1. Ionic bonds form by transferingelectrons,covalent bonds form bysharing electrons.
  2. Ionic compound have high melting and boiling points while covalent compounds have low.

Lewis Structures

  1. Draw the Lewis Structure for CS2, and complete the table below showing number and types of bonds or lone pairs that each element has. [HONORS describe the molecular geometry]

Linear

  1. Draw the Lewis Structure for CH3I, and complete the table below showing number and types of bonds or lone pairs that each element has. [HONORS describe the molecular geometry]

tetrahedral

  1. Draw the Lewis Structure for HCN, and complete the table below showing number and types of bonds or lone pairs that each element has. [HONORS describe the molecular geometry]

linear