This is “Multiple Covalent Bonds”, section 4.3 from the book Introduction to Chemistry: General, Organic, and Biological (v. 1.0). For details on it (including licensing), click here.

For more information on the source of this book, or why it is available for free, please see the project's home page. You can browse or download additional books there. You may also download a PDF copy of this book (72 MB) or just this chapter (2 MB), suitable for printing or most e-readers, or a .zip file containing this book's HTML files (for use in a web browser offline).

Has this book helped you? Consider passing it on:
Creative Commons supports free culture from music to education. Their licenses helped make this book available to you.
DonorsChoose.org helps people like you help teachers fund their classroom projects, from art supplies to books to calculators.

4.3 Multiple Covalent Bonds

Learning Objective

  1. Recognize molecules that are likely to have multiple covalent bonds.

In many molecules, the octet rule would not be satisfied if each pair of bonded atoms shares two electrons. Consider carbon dioxide (CO2). If each oxygen atom shares one electron with the carbon atom, we get the following:

This does not give the carbon atom a complete octet; you will find only six electrons in its valence shell. In addition, each oxygen atom has only seven electrons in its valence shell. Finally, no atom makes the number of bonds it typically forms (Figure 4.2 "How Many Covalent Bonds Are Formed?"). This arrangement of shared electrons is far from satisfactory.

Sometimes more than one pair of electrons must be shared between two atoms for both atoms to have an octet. In carbon dioxide, a second electron from each oxygen atom is also shared with the central carbon atom, and the carbon atom shares one more electron with each oxygen atom:

In this arrangement, the carbon atom shares four electrons (two pairs) with the oxygen atom on the left and four electrons with the oxygen atom on the right. There are now eight electrons around each atom. Two pairs of electrons shared between two atoms make a double bondTwo pairs of electrons being shared by two atoms in a molecule. between the atoms, which is represented by a double dash:

Some molecules contain triple bondsThree pairs of electrons being shared by two atoms in a molecule., covalent bonds in which three pairs of electrons are shared by two atoms. A simple compound that has a triple bond is acetylene (C2H2), whose Lewis diagram is as follows:

Example 5

Draw the Lewis diagram for each molecule.

  1. N2
  2. CH2O (The carbon atom is the central atom.)

Solution

  1. The bond between the two nitrogen atoms is a triple bond. The Lewis diagram for N2 is as follows:

  2. In CH2O, the central atom is surrounded by two different types of atoms. The Lewis diagram that fills each atom’s valence electron shell is as follows:

Note

One application of CH2O, also called formaldehyde, is the preservation of biological specimens. Aqueous solutions of CH2O are called formalin and have a sharp, characteristic (pungent) odor.

Skill-Building Exercise

    Draw the Lewis diagram for each molecule.

  1. O2

  2. C2H4

Concept Review Exercise

  1. What is one clue that a molecule has a multiple bond?

Answer

  1. If single bonds between all atoms do not give all atoms (except hydrogen) an octet, multiple covalent bonds may be present.

Key Takeaway

  • Some molecules must have multiple covalent bonds between atoms to satisfy the octet rule.

Exercises

  1. Each molecule contains multiple bonds. Draw the Lewis diagram for each. The first element is the central atom.

    1. CS2
    2. C2F4
    3. COCl2
  2. Each molecule contains double bonds. Draw the Lewis diagram for each. Assume that the first element is the central atom, unless otherwise noted.

    1. N2
    2. HCN (The carbon atom is the central atom.)
    3. POCl (The phosphorus atom is the central atom.)
  3. Explain why hydrogen atoms do not form double bonds.

  4. Why is it incorrect to draw a double bond in the Lewis diagram for MgO?

Answers

  1. Hydrogen can accept only one more electron; multiple bonds require more than one electron pair to be shared.