If5 polarity11/13/2023 It used in iodometry for the manufacture of medicine. Iodates are used in treatment of thyroid gland disorder. IO3- LEWIS STRUCTURE HYBRIDIZATION Io3- Uses Due to sp3 hybridization iodate should have tetrahedral geometry but as because of presence of lone pair of electron the shape of io3- ion is pyramidal. In this compound I uses sp 3 hybrid orbital to make I-O bonds. ![]() There still 1 unpaired electron present on O atom which forms 2 I=O pi bonds. In the next step 3 O atom gave 3 unpaired electron to form 3 electron pair by which 3 I-O single bond is formed. In the excited state, I transfer 2 p electrons in 5d orbital and now a total of 5 unpaired electron is present. As we see from electronic configuration of I atom that there is only 1 unpaired electron and to form io3- ion 3 unpaired electron is required. The ground state outermost shell electronic configuration of I is 5s 25p 5. Hybridization is the process in which hybrid orbitals are formed by mixing of same energy atomic orbitals. There are 26 valance electrons in io3- ion. The total valance electrons that present on io3- ion will be equal to the (sum of the valance electron of I and O atom+1 negative charge) i.e. ![]() Also one negative charge is present on O atom. There is 6 electrons in the valance shell of O atom. The electronic configuration of O atom is 2s 22p 4. The electronic configuration of I is 4d 105s 25p 5 and as we see from electronic configuration that there are 7 electrons in valance shell of I atom. IO3- Valance Electronsįirstly to find out the total valance electron in io3- ion, it is important to know the electronic configuration of I and O atom. These lone pair of electrons is found In the lewis structure of io3- on the given atoms as electron dots. Lone pair present on single bonded O- ion= 8-2=6 i.e.3 lone pair. Lone pair present on each double bonded O atom=6-2=4 i.e. In io3- lone pair present on I atom= 7-5=2 i.e. No of lone pairs= Total no of valance electron of the atom-no of bonds formed by that atom. The basic formula with the help of which we can find the lone pair of electron on the given atom is given below: The valance shell electron that don’t take part in sigma as well as pi bonding is called lone pair of electron or nonbonding electrons pair. ![]() Hence according to octet rule iodate is a stable compound. It can increase their octet more than 8 electrons. In io3- ion I forms 2 I=O double bonds and 1 I-O single bond, also there exist 1 lone pair of electron that present on central I atom creating a total of 12 electrons around I atom. In the lewis structure of io3- we found that each O atom has 8 electrons in its outermost shell and fulfill their octet. To minimize this bond pair-lone pair repulsion O-I-O bond angle is reduced to 100 0 from 109 028’. But lp-lp repulsion is stronger in nature than bond pair-bond pair electronic repulsion. In this compound both lp-lp and bp-bp repulsion occurs. This is because of lone pair present on I atom. Io3- has distorted tetrahedral geometry hence normal tetrahedral bond angle 109 028 ’ does not arises here. Each double bond O atom has 0 and single bond O atom has -1 formal charge making the whole compound is negatively charged. Hence iodine atom has 0 formal charge on it. Hence formal charge on I atom in io3- = 7-10/2-2=0.įormal charge on each double bonded O atom in io3- =6-4/2-4=0.įormal charge on single bond O atom in io3- =6-2/2-6=-1. V= No of valance electrons, B= No of bonding electrons, N= No of nonbonding electrons. The formal charge on any atom or ion can be calculated by the formula given below: But as because lone pair is present the structure becomes is distorted and the correct geometry is pyramidal. As lone pair is absent on I atom the geometry of this compound is tetrahedral. ![]() Due to the presence of 1 lone pair on central I atom ideal tetrahedral geometry does not occur. IO3- LEWIS STRUCTURE RESONANCE IO3- Lewis Structure ShapeĪccording to VSEPR theory the shape of io3- is pyramidal in which iodine is tetrahedrally surround by 2 O atoms and 1 O- ion.
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