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?
M/N Trans Ionic Polar e- transfer,
N/N Shared Covalent Polar Sharing of e-
Covalent and Nonpolar
M Shared Alloys Sharing of e-
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,
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.
1s2 2s2 2p6 3s2 3p6 4s2
Ion: 1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p3
Ion: 1s2 2s2 2p6
c. Hg (ion: 2+)
[Xe] 6s2 4f14 5d10
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
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
No Yes moderate
V. Write formulas for the
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
VI. Write names for the 8. PCl3 Phosphorus trichloride
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
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
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.