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1.44 - 1.46 Covalent bonding - "sharing nicely"

 1.44 Sharing electrons

Covalent bonds are formed when electrons are shared between atoms

In the previous topic you will have seen how ionic compounds are formed when the atoms of metals transfer electrons to the atoms of non-metals. The electron transfer enables the atoms to fill their outer electron shells and become stable. 

Here we consider what happens when atoms of non-metals bond with other atoms of non-metals.  

Non-metal atoms tend to hold on to electrons and tend not to form positive ions. By sharing electrons the atoms' outer electron shells become full and therefore stable.

Assumed background knowledge:

 1.44 - 1.45 Activity 1. Opposites attract

 Students should:

  • 1.44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons
  • 1.45 understand covalent bonds in terms of electrostatic attractions

Play the video to see an animation showing the way in which electrons shared between two nuclei will create an electrostatic attraction between them. This attractive force is known as a covalent bond.

Notice that as the bond forms, energy is released.

It follows then that to break a bond, energy needs to be supplied

 1.46 Activity 2. Crossing and dotting

 Students should:

  • 1.46 understand how to use dot-and-cross diagrams to represent covalent bonds in molecules.

​Dot and cross diagrams are a useful way of representing how atoms share electrons to form molecules. 

Watch the video and notice that:

  1. Only the outer electrons need to be shown.
  2. The electrons on one of the atoms are shown as dots.
  3. The electrons on the other atom involved are shown as crosses.
  4. Normally  a "dot" and a "cross" pair up to form an ordinary single covalent bond.

 1.46 Activity 3. Four simple molecules

  • Study the animation carefully.
  • What can you say about the number of electrons in the outer shell of the carbon atom in methane, the nitrogen atom in the ammonia molecule and the oxygen atom in the water molecule?
  • Make a copy of  each of the images below and add dots and crosses to them to show the complete electron configurations

In the dot and cross diagrams the central atom ( carbon in methane, nitrogen in ammonia and oxygen in water) has 8 ( a full outer shell) electrons and is therefore stable. The hydrogen atoms have 2 electrons and therefore also have a full outer shell.

 1.46 Activity 4. Multiple Bonds

Some non-metal atoms can form more than one bond with another non-metal atomOxygen is one example. The element oxygen is represented by the formula O2. 

This is because oxygen atoms pair up with one another form diatomic molecules.​ The atoms in O2 are held together by a double bond. 

Select "oxygen" in the animation but before looking at the dot and cross diagram,  try to work out and draw how the electrons are arranged in an oxygen molecule. Check your answer against the animation. Repeat this for carbon dioxide and nitrogen.
  • What is unusual about one of the bonds in carbon monoxide? Open or Close

    The dot and cross diagram shows that a triple bond forms in the carbon monoxide molecule. It also shows that in one of the triple bonds, both electrons come from the  oxygen atom. 

    This type of bond is still an ordinary covalent bond but is is known as a dative covalent bond. Such bonds are sometimes represented by an arrow.

Study the dot and cross diagrams for each of the three molecules shown in the animation. 

Notice that for ethane and ethene two different colours of cross have been used to distinguish the electrons associated with one of the carbon atoms from the electrons on the other. The same method is used to distinguish Chlorine's electrons from the carbon's electrons in the chloromethane.

Think about the formula, shape, structure and name of each of the molecules shown. 

Predicting an unknown molecule

  • Try to draw a 3d representation of chloroethene  
  • Try to draw a dot and cross diagram to show the electron arrangement in chloroethene

Check your answers here:

 Activity 6. Complete the matching exercise below