In this theory, we use certain notations to find out the exact molecular shape.Ī: central atom, here, Chlorine is the central atom. This is an image example of the VSEPR chart. Let us now find out the 3D molecular geometry of Chlorine Tetrafluoride with the help of the VSEPR model. Through VSEPR theory, we can visualize the electronic arrangement and structural configuration of a molecule in a far better manner.Īccording to this theory, since electrons are all negatively charged particles, like charges repel each other, and to minimize this repulsion the atoms are spread apart from each other.įor example, a diatomic molecule always usually has a linear molecular geometry having a 180-degree bond angle. It is an extension of the Lewis Structure concept which can only depict the 2-dimensional sketch but fail to go beyond that. This model is used to explain and predict the 3-dimensional molecular geometry of different molecules (usually covalent bonded). VSEPR stands for Valence Shell Electron Pair Repulsion theory. Therefore, the correct and suitable Lewis Structure diagram of ClF5 is: The formal charge value of Cl atom = 7 – 0.5*10 – 2 = 0.Ītoms of both the elements are present in their least possible formal charge values. In the case of all the five F atoms, the formal charge of each = 7 – 0.5*2 – 6 = 0. This is how we calculate the formal charge values of each atomic element. ClF5 cannot obey the octet fulfillment rule.īefore we can finalize our Lewis Structure diagram, we have to check another concept: Formal Charge.įormal charge deals with the charge assigned to atoms inside a molecule if we assume that electrons are always shared equally among them. This is an example of an exception to the general octet rule i.e. If we look at the five surrounding fluorine atoms, we can see that each one of them has eight electrons around them, six unbonded and two bonded.īut in the case of chlorine, it has 12 valence electrons around itself, with ten bonded and two unbonded. Here, Chlorine and fluorine both elements will tend to attain octet fulfillment of their valence shells. We have shown the bonds via straight lines indicating an electron pair each.Īccording to the octet rule, the elements present in the main groups (group 1-17) of the periodic table have a tendency to achieve the octet configuration of the outermost shell of noble gas elements. Since Chlorine is the central atom here, it will form bonds with all the five Fluorine atoms. Here, as we can see, we have put all the 42 electrons surrounding the six atoms in ClF5. Lewis Structure is also known as an electron-dot structure since it uses dot notations to represent the valence shell electrons in the skeletal diagram. Now, we will place the valence electrons around the atoms. We have placed the chlorine atom in the center and the fluorine atoms surrounding it. The element having the least electronegativity value is usually the central atom and thus chlorine here becomes the central atom. Among Cl and F, Cl is more electropositive than F. We will now find out which element will take the central position in the molecule. The total number of valence electrons ina ClF5 molecule = 7 + 7*5 = 7 + 35 = 42. Each one of the six atomic elements has 7 valence electrons. Both chlorine and fluorine belong to the group of halogens and therefore present in group 17. Valence electrons are the outermost shell electrons of an element that we can determine from the atomic number and Periodic table.Ī molecule of chlorine tetrafluoride has one atom of chlorine and five atoms of fluorine. Now, we will find out the suitable Lewis Structure diagram for our molecule, ClF5.Īt first, we will calculate the total number of valence electrons inside the molecule. It gives us a diagrammatic representation of the arrangement or distribution of electrons around the constituent atoms to help us have a simplified idea of bond formation. Lewis Structure is a step-by-step procedure to draw a two-dimensional sketch of a molecule or ionic structure. If we want to understand the science behind the chemical bonding of any given molecule, we have to first draw the Lewis Structure diagram. Let us now learn the chemical bonding inside a molecule of chlorine tetrafluoride in detail. We have several types of bonds – ionic, covalent, metallic, hydrogen, and so on. The study of atomic attraction that results in product formation is known as chemical bonding and the bond formed is called a chemical bond. ClF3 + F2 -> ClF5 (at high temperature and high pressure)Ītoms of similar or different elements come together and form a new molecular composition, which creates new chemical compounds.
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