![]() ![]() 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. It is due to VSEPR theory that both structures are different. The number of bond pairs and lone pairs combine to give a shape, while the ratio of both determine any varience from the regular geometry.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. Sb is in group 5, so it has 5 electrons in its outer shell. There are 4 Sb-F bonds, and also a negative charge on the central antinomy atom, so there are in total (5+4+1=) 10 electrons. Therefore there are 5 pairs. This suggests it is a trigonal bipyramedal shape, (seesaw) typically with bond angles of 120 and 90 degrees. However as there are 4 bond pairs, and 1 lone pair, then the lone pair will distort this perfect geometry, forming angles between Sb-F bonds to be less than 90 and 120 degrees. The lone pair forms on the axial part of the molecule as there is minimum repulsion. Therefore it has 8 electrons in its outer shell. Fluorine atoms have 7 electrons, yet one is an unpaired electron, so this is the electron in fluorine that gets involved in bonding. There are 4 of these, so around the xenon atom, there are (8+4=) 12 electrons, so 6 electron pairs and as there are 4 fluorine atoms bonding, there are 4 bond pairs, and 2 lone pairs of electrons. Therefore this is an octahedral shape, with 90 degree angles between each bond and lone pair of electrons. Due to VSEPR (valence shell electron pair repulsion) theory, the most energetically stable form of XeF4 will form, with the lone pairs as far away from each other as possible, hence forming the shape seen. ![]()
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