Review Unit 6 – Bonding
I. Bond Types: Fill in the table to show the basics of bond types.
                Type of atoms  ...
Ion: [Xe] 4f14 5d10 *** Remember the valence shell is the highest quantum
           number. That is why 6s left.

III. Le...
VI. Write names for the                                           8.   PCl3 Phosphorus trichloride
    following compounds...
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Review unit 6 key

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Review unit 6 key

  1. 1. Review Unit 6 – Bonding I. Bond Types: Fill in the table to show the basics of bond types. Type of atoms Electrons Type of What holds the Bond involved transferred or Compound bond together? shared? formed M/N Trans Ionic Polar e- transfer, Ionic electrostatic forces N/N Shared Covalent Polar Sharing of e- Covalent and Nonpolar M Shared Alloys Sharing of e- Metallic II. Short Answer: 1. Why are some covalent bonds polar? Higher electronegative atoms unequally share the electrons in the bond. 2. Which of the following compounds express polarity? To which element are the compounds polar too? a. H2O Yes O b. HF Yes F c. CCl4 No d. CO2 Yes O 3. What are Binary Acids? List 4 and include the formula for each. Binary acids consist of H and another element. HF HCl HI HBr 4. What are Tertiary Acids? List 4 and include the formula for each. Tertiary Acids include H and a polyatomic ion in most cases. HNO3, HClO3, HPO4, and H2SO3 5. How does electronegativity relate to the strength of an acid? The higher the electronegativity the greater the strength of the acid. 6. Is it possible for a bond to be partially ionic? Explain. No, only whole electrons are transferred in an ionic bond resulting in a definite charge. 7. What is an ion? How does it form? An ion is a charged atom that forms from the gain or loss of electrons. 8. What is a polyatomic ion? What kind of bond holds the atoms in a polyatomic ion together? A polyatomic ion is a charged, covalently bonded molecule that combines with a metal to form an ionic compound. 9. Show the electron configuration for each of the atoms below and the configuration for the ion as well. a. Ca 1s2 2s2 2p6 3s2 3p6 4s2 Ion: 1s2 2s2 2p6 3s2 3p6 b. N 1s2 2s2 2p3 Ion: 1s2 2s2 2p6 c. Hg (ion: 2+) [Xe] 6s2 4f14 5d10
  2. 2. Ion: [Xe] 4f14 5d10 *** Remember the valence shell is the highest quantum number. That is why 6s left. III. Lewis Dot Structures: Show the bonding that would occur in the following compounds. 1. Carbon tetrachloride 4. Barium oxide 2. Potassium chloride 5. Nitrogen trihydride 3. Copper (II) fluoride 6. Hydrosulfuric acid IV. Ionic, Molecular and Metallic Compounds: Complete the chart below. Type of Bond Solubility Conductivity Melting Point Yes In aqueous and Relatively high Ionic little in molten Only with like No Relatively low Covalent molecules No Yes moderate Metallic V. Write formulas for the following compounds. 1. magnesium oxide MgO 2. Potassium hydroxide KOH 3. copper (II) carbonate CuCO3 4. acetic acid CH3COOH 5. lead (II) nitrate Pb (NO3)2 6. carbon disulfide CS2 7. iron (III) chloride FeCl3 8. ammonium phosphate (NH4)3PO4 9. nitrogen tribromide NH3 10. potassium tungstate K2WO4 11. nitrous acid HNO2 12. hydrosulfuric acid H2SO4 13. sulfur dioxide SO2 14. sodium chlorate NaClO3 15. copper (I) sulfite Cu2SO3
  3. 3. VI. Write names for the 8. PCl3 Phosphorus trichloride following compounds. 9. (NH4)2CO3 Ammonium Carbonate 1. BaCl2 Barium Chloride 10. NO2 Nitrogen Dioxide 2. K2CO3 Potassium Carbonate 11. AuBr Gold(I) Bromide 3. HgI2 Mecury (II) Iodide 12. H3PO3 Phosphorus acid 4. HNO3 Nitrous Acid 13. Na2O Sodium Oxide 5. Ca(NO3)2 Calcium Nitrate 14. NBr Sodium Bromide 6. CuO Copper (II) Oxide 15. CaO Calcium oxide 7. HI Hydroiodic acid Vocabulary Chapter 8 Chapter 9 chemical bond formula unit covalent bond cation monatomic ion molecule anion oxidation number Lewis structure ionic bond polyatomic ion endothermic electrolyte oxyanion exothermic lattice energy electron sea model structural formula delocalized electrons metallic bond alloy 1. Given a name for a compound, be able to give the chemical formula. (ionic, covalent or acid) 2. Give the chemical formula for a compound, be able to name it. (ionic, covalent or acid) 3. Be able to explain why two elements will form an ionic bond. 4. Be able to explain properties of metals, based on their bonding. 5. Be able to explain why water is a polar molecule. 6. Be able to explain what an electrolyte is. 6. Be able to draw Lewis Structures of ionic compounds or molecules. 7. Be able to determine if a bond is polar, nonpolar covalent or polar covalent. 8. Know properties of ionic and covalent compounds and metals.

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