Since we know that the steric number of ClO 3 – is 4 (1 lone pair and three bonded pairs), we can determine that the Molecular geometry of ClO 3 – is Trigonal Pyramidal.įrom the Lewis structure above, we know that its electronic shape is tetrahedral. According to the VSEPR theory (Valence Shell Electron Pair Repulsion), the lone pair on Chlorine and the electron clouds on the surrounding oxygen atoms repel each other. ClO 3 – Molecular Geometry and ShapeĬhlorine forms the central atom in the ClO 3 – ion with oxygen atoms surrounding it. ClO 3 – Bond Anglesĭue to the repulsion of electrons on the surrounding oxygen atoms and the lone pair on Chlorine, the atoms get pushed apart and form bond angels of 109.5°. Therefore, the hybridization of ClO 3 – is sp 3. The rest of the electrons from the sigma bonds are filled into the 3p orbital. Now, we insert the two pi bonds into the first two 3d orbital spaces. In ClO2- lewis dot structure, the total number of 7 lone pairs and 3 bond pairs are present. The bond angle in ClO2- is slightly less than 109°. The overall formal charge in ClO2- is -1. Therefore, the two lone pairs fill in the 3s orbital and the three sigma bonds present fill-up the 3p orbital. ClO2- is a polar molecule due to the asymmetrical distribution of charges caused by the presence of lone pair electrons. Its electronic configuration is given by 3s 2 3p 5. Since Chlorine is in the third row in the periodic table, it is capable of expanding its orbitals in an excited state. To calculate ClO 3 – hybridization state, we need to determine the number of lone pairs and the number of sigma bonds present in the ion. The central atom, Chlorine (Cl), forms covalent bonds of double and single nature with the surrounding atoms of Oxygen. Therefore, it becomes a conductor for more electron bonds than Oxygen hence taking up the center stage as shown in the figure. The Chlorine atom takes up a central position in the structure due to its ability to share a higher number of electrons. The total number of electron pairs in a chlorate ion is given by: The Lewis dot structures of an element represent a schematic arrangement of its constituent molecules, atoms and their electron bonds. Therefore, the total valence electrons in the chlorate ion is 7 + 18 +1 = 26 Lewis Structure of ClO 3 – The anionic charge of -1 and contributes one valence electron. Therefore, given 3 oxygen atoms contribute 6 x 3 =18 electrons. Oxygen’s electronic configuration is 1s 22s 22p 4. Therefore, the single Chlorine atom contributes 7 x 1 = 7 electrons.īeing in group 6 of the periodic table, Oxygen has six valence electrons and has a valency of -2. The possibility of electrons in its d shell makes it hypervalent. Chlorine’s electronic configuration is given by 3s 23p 5. There also exists a negative ionic charge of -1 in the ion.īeing in group 7 of the periodic table, Chlorine has seven valence electrons with a valency of -1. Now, a lot of people ask why it is necessary to know the Lewis structure of any given molecule or compound. To understand the hybridization, polarity and molecular geometry of the Ozone molecule it is crucial to know the Lewis structure of the same. It is written as O3 in the core chemistry equations. ClO3– Molecular Geometry and Shape ClO 3 – Valence ElectronsĪ Chlorate ion consists of one chlorine atom and three oxygen atoms. The molecule of Ozone has three oxygen atoms.\), you can see that the fluorine atoms possess extra lone pairs that they can use to make additional bonds with boron, and you might think that all you have to do is make one lone pair into a bond and the structure will be correct.
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