Bond Type

Book Activity

Name ______

Directions: Use the World of Chemistry books that are in the cabinet. You can find the definitions in the glossary at the back of the book or in Chapter 12. The questions will be answered as you read sections 12.1-12.3 (pgs. 359-365).

Define the Key Terms

  1. Bond
  2. Bond energy
  3. Ionic bonding
  4. Covalent bonding
  5. Polar covalent bonding
  6. Electronegativity
  7. Dipole moment
  8. Lewis structure
  9. Duet rule
  10. Octet rule
  11. Bonding pair
  12. Lone (unshared) pair
  13. Single bond
  14. Double bond
  15. Triple bond
  16. Resonance

Answer the Following Questions

  1. A force that holds groups of two or more atoms together and makes them function as a group is called a ______.
  1. You can obtain information about the strength of a bond by measuring ______

______.

  1. Atoms can interact with one another in several ways to form ______.
  1. What fact convinces chemists that sodium chloride is composed of Na+ and Cl- ions?
  1. What happens to the electrons when solid sodium chloride is formed?
  1. How is an ionic substance formed?
  1. An ionic compound is formed when a ______reacts with a ______.
  1. What happens to the electrons when two hydrogen atoms are brought close together?
  1. Electrons are shared in a ______bond.
  1. A covalent compound is formed when a ______reacts with a ______.
  1. What happens to the participating atoms in an ionic bond?
  1. What happens to the participating atoms in a covalent bond?
  1. Between these extremes are intermediate cases in which the atoms are not so different that electrons are completely transferred but are different enough so that unequal sharing of electrons results, forming what is called a ______.
  1. Diagram the hydrogen fluoride (HF) molecule. Make sure to indicate the partial charge.
  1. What is the most logical explanation for the development of bond polarity?
  1. When two identical atoms react, a bond forms in which electrons are shared ______.
  1. When different nonmetals react, a bond forms in which electrons are shared ______.
  1. The unequal sharing of electrons between two atoms is described by a property called ______: the relative ability of an atom in a molecule to attract shared electrons to itself.
  1. How do chemists determine electronegativity values for the elements?
  1. What happens to the electronegativity values as you move from the left to the right across a period?
  1. What happens to the electronegativity values as you move down a group?
  1. Remember, the higher the atom’s electronegativity values, the ______the shared electrons tend to be to that atom when it forms a bond.
  1. The polarity of a bond depends on the ______between the electronegativity values of the atoms forming the bond.
  1. When are the electrons shared almost equally, which causes the bond to show very little polarity?
  1. When is a very polar bond formed?
  1. For each of the following pairs of bonds, write the difference in electronegativity and the bond type (ionic bond, covalent bond, or polar covalent bond).

EXAMPLEH-P 2.1-2.1=0 Covalent Bond

  1. Na-Cl
  2. H-C
  3. H-H
  4. O-I
  5. N-O
  6. S-O
  7. K-Br
  8. O-F
  9. Cl-Cl
  10. C-Cl
  1. Describe the relationship between electronegativity and bond type described in table 12.1 on page 362.
  1. A molecule such as HF that has a center of positive charge and a center of negative charge is said to have a ______.
  1. Explain how the dipolar character of a molecule is often represented by an arrow.
  1. What type of molecule has a dipole moment?
  1. In a water molecule the oxygen atom has a greater electronegativity than the hydrogen atoms. This causes the electrons to not be shared equally. What is the result in this relationship?
  1. A water molecule is polar (has a dipole moment). What effect does that have on the properties of the water molecule?
  1. What would happen if water was nonpolar?