Covalent Bonds – Quantum Numbers

by Adam Le Gresley, PhD

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    00:01 each with a charge of 1–. So I talked earlier on about the importance of having a full outer shell in order to achieve stability. And this applies to all elements: not just those in the first three groups and the last two groups, but also those within the middle. And whereas I talked before about the formal transfer of electrons from one atom to another, now I'd just like to briefly introduce you to the idea of covalent bonds—that is, where you have electrons which are shared. So rather than formally transferred, they're shared in order for both species to obtain a full outer shell and the stability that comes with that. Let's take, for example, methane. This consists of two elements: one carbon and four hydrogen atoms. Let's consider those individual atoms in isolation. If we look at carbon (again, we're using the abbreviated form, so the helium nucleus followed by 2s2, 2p2) we can see that it needs, or requires, four additional electrons to complete its valence shell. If, on the other hand, we look at hydrogen (which, as you should recall, has the electron configuration 1s1), it needs to gain one additional valence electron in order to complete its outer shell. So if carbon shares all four of its valence electrons with four hydrogen atoms, such as this shown, this enables the completion of the outer shell for both atoms, or both sets of atoms. The hydrogen gains the electron it requires to create 1s2, and the carbon can share the four electrons from the hydrogen to create the 2s2, 2p6 outer shell. So hopefully, you can appreciate in this scenario, where the actual loss of individual electrons is not energetically preferable, sharing, or covalent bond formation (which is what I'm showing you here), is the preferred way in which atoms can achieve the energetic stability associated with a full outer shell. The bonds between the carbon and the hydrogen are covalent bonds. And I'll just want to briefly draw your attention to the shape of the molecule, as I've shown here. If you recall, if we look back at the anionic and ionic systems, I talked about the idea that they form these crystal lattices, or structures, where you have multiple ions all able to interact with each other electrostatically. However, in the case of covalent bonds—and this is very important for macroscopic properties—the bonds are directional. The carbon is bound to the hydrogen and nothing else. And so therefore, you don't have the same macroscopic interactions, which means that the methane exists as a gas rather than as a crystal structure.

    03:22 So due to their electron requirements, hydrogen will always form one covalent bond and is said, formally, to have a valency of 1. Carbon will always form four covalent bonds and therefore has a valency of 4. And as we will see when we actually start looking at things like hybridization, it'll make you realize the importance of the carbon in organic chemistry. Because whilst it's possible to form many thousand formula units, compounds, and molecules and so forth from other parts of the periodic table from different elements, carbon in itself is directly related to the millions and millions of different compounds which exist on this planet and is therefore one of the most—or the most—important compound because of its diversity.

    04:22 So, question for you now: • Ammonia is a molecule that contains a single nitrogen covalently bound to hydrogen atoms. So what will the molecular formula for ammonia be? • What, therefore, is the valency of nitrogen? • And a follow-up: Hydrazine, which is a related molecule, contains two nitrogen atoms and hydrogen atoms. The nitrogen atoms are joined by a covalent bond. What you should do as an exercise is draw the bonding and give the molecular formula for hydrazine.

    About the Lecture

    The lecture Covalent Bonds – Quantum Numbers by Adam Le Gresley, PhD is from the course Chemistry: Introduction.

    Included Quiz Questions

    1. …two atoms share the electrons between them.
    2. …two atoms formally exchange the electrons between them.
    3. …two atoms formally pick up the electrons from the lone pair present on the oxygen atom of water molecule.
    4. …two electrons share their protons and neutrons with each other.
    5. …two atoms formally gave up the electrons to a water molecule.
    1. 4
    2. 0
    3. 1
    4. 2
    5. 3
    1. …the loss of one or two electrons is energetically not preferable.
    2. …the atom is highly deficient in electrons.
    3. …the atom is already existing in a cationic form.
    4. …the incoming atom is existing in an anionic form.
    5. …the external source of energy is not available to produce ions.
    1. Because the atoms bonded to each other via covalent bonds have specific spatial orientations relative to each other.
    2. Because one atom pulls the shared pair of electrons more towards itself than the other.
    3. Because the lone pair present on an atom pushes away the shared pair of electron towards the other atom.
    4. Because of the higher atomic number of the participating atoms the shared pair of electrons gets attracted towards it.
    5. Because of the higher atomic mass of one of the participating atoms the covalent bond is slightly tilted towards it.

    Author of lecture Covalent Bonds – Quantum Numbers

     Adam Le Gresley, PhD

    Adam Le Gresley, PhD

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