In fact, each fluorine atom has a formal charge of 0 on it. This low bond energy of fluorine explains why it is reactive.Īnyway, back to the main topic of the article! The fluorine molecule is neutral, i.e., there is no charge on it. This is approximately half the energy required to break a carbon–carbon single bond. Both fluorine atoms share one pair of electrons and hence have a single covalent bond between them.ĭo you know how much energy it would take to break this bond? It is 157 KJ/mol. Now, let us construct a skeleton of the F2 molecule on the basis of the information presented in step 2. The three unshared pairs of electrons on each fluorine atom are called the lone pairs. There is no rocket science going into determining that both fluorine atoms can share one pair of electrons and be happy and satisfied with their individual octets achieved! The case of fluorine is really one of the simplest ones. To achieve the octet, each atom needs one more electron. Thus, each fluorine atom has 7 valence electrons. There are 2 electrons in its K shell and 7 electrons in its L shell. The atomic number of fluorine is 9 therefore, it possesses 9 electrons in its neutral atomic form. Start by calculating the number of valence electrons in each atom of F2 and see how many more electrons each fluorine atom needs to form an octet. Let us take a look at the chemical bonding represented by lewis structure in F2. This is exactly why they are called “noble.” Noble gases already have completely filled valance shells, so they do not need to bond/react with any other atoms/molecules. Hydrogen is an exception, though it seeks a duplet, not octet, because it has only one electron in its K shell, and thus needs only one more to achieve the maximum capacity of K shell. Several atoms tend to seek eight electrons in their valence shell through chemical bonding this is referred to as the octet rule and is reflected in the Lewis structure of a molecule. In a typical Lewis structure, each valence electron is represented as a dot, and a covalent bond between two atoms (formed as a result of sharing of two electrons) is represented as a line. It is to be noted though that this theory about the electronic structure is quite primitive and most limited. The valence electrons in each atom are the ones that participate in the bonding, and hence they are the only ones displayed in the Lewis structures. The Lewis theory of chemical bonding helps us visualize the arrangement of atoms-how they are attached or bonded-in molecules.
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