Review Unit 6 – Bonding
I. Bond Types: Fill in the table to show the basics of bond types.
Type of
Electrons
Type of
What holds
Bond
atoms
transferred
Compound
the bond
involved
or shared?
formed
together?
M/N
Trans
Ionic Polar
e- transfer,
Ionic
electrostatic
forces
N/N
Shared
Covalent
Sharing of eCovalent
Polar and
Nonpolar
M
Shared
Alloys
Sharing of eMetallic
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
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
Yes
Ionic
Covalent
Only with like
molecules
No
Conductivity
In aqueous and
little in molten
No
Melting Point
Relatively high
Yes
moderate
Relatively low
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
VI. Write names for the
following compounds.
8. PCl3 Phosphorus trichloride
9. (NH4)2CO3 Ammonium
1. BaCl2 Barium Chloride
Carbonate
2. K2CO3 Potassium Carbonate
10. NO2 Nitrogen Dioxide
3. HgI2 Mecury (II) Iodide
11. AuBr Gold(I) Bromide
4. HNO3 Nitrous Acid
12. H3PO3 Phosphorus acid
5. Ca(NO3)2 Calcium Nitrate
13. Na2O Sodium Oxide
6. CuO Copper (II) Oxide
14. NBr Sodium Bromide
7. HI Hydroiodic acid
15. CaO Calcium oxide
Vocabulary
Chapter 8
chemical bond
cation
anion
ionic bond
electrolyte
lattice energy
delocalized electrons
alloy
1.
2.
3.
4.
5.
6.
6.
7.
8.
formula unit
monatomic ion
oxidation number
polyatomic ion
oxyanion
electron sea model
metallic bond
Chapter 9
covalent bond
molecule
Lewis structure
endothermic
exothermic
structural formula
Given a name for a compound, be able to give the chemical formula. (ionic, covalent or acid)
Give the chemical formula for a compound, be able to name it. (ionic, covalent or acid)
Be able to explain why two elements will form an ionic bond.
Be able to explain properties of metals, based on their bonding.
Be able to explain why water is a polar molecule.
Be able to explain what an electrolyte is.
Be able to draw Lewis Structures of ionic compounds or molecules.
Be able to determine if a bond is polar, nonpolar covalent or polar covalent.
Know properties of ionic and covalent compounds and metals.