V= Number of Valence electrons of the central atom.Ĭ= Charge on cation or more electropositive atom.Ī= Charge on anion or more electropositive atom. The formula to find the Hybridization of any molecule is given below:. This is useful if you don’t remember the theory. Method 2: Next we come to the formula aspect of hybridization. So total value of H is 4, which makes the molecule Sp3 hybridized. It makes 4 sigma bonds with each O atom (double bonds/triple bonds are considered as one sigma bond) and it has no lone pairs present on it. The value of Hybridization (H) is determined by:. Method 1: The theory aspect- Hybridization of PO43- can be found by adding the number of bonds and the lone pair of the central atom. This can be understood through two methods:. Let us now take a look at the Hybridization of the molecule which will give us more information on the nature of their chemical bonds. Thus, we get the required best Lewis structure for PO43. We cannot induce more double bonds with O for the simple reason that P will acquire a -1 charge which will make the molecule highly unstable. The rest 3 O atoms will have a -1 charge, thus giving rise to the -3 charge on the molecule. So, if P makes a double bond with one of the oxygen atoms then P will have a charge of 0 and so will the doubly bonded O atom. In PO43-, P can hold more than 8 valence electrons (period 5). So the best Lewis structure should ideally have each atom with a charge of 0 on it. Now, this looks all fine.īut is this the lowest formal charge possible? Remember that the charges on each atom of a molecule make it more unstable. We see that P has a +1 charge and all the O atoms have a -1 charge. Now we check the formal charge of each atom of PO43. We observe that all 32 valence electrons are now used up.ĥ. Now we arrange the remaining 24 valence electrons around each atom so that it completes its octet. 8 valence electrons are used up for this.Ĥ.
Now we start arranging these electrons as lone pairs on each atom so that it resembles a chemical bond. Following this reasoning P is the central atom of PO43-.ģ. The atom which has the highest valence factor, as well as the highest bonding sites, is termed as the central atom. Hence, total number of valence electrons is 5+24+3= 32 valence electrons.Ģ. Now there is a charge of -3 on the whole atom which means there are 3 additional valence electrons present. O belongs to group 6, hence has 6×4= 24 valence electrons (4 atoms of O). P belongs to group 5, hence has 5 valence electrons. Let us count the total number of valence electrons for the molecule PO43. Steps of Drawing lewis structure of PO43-ġ. The formula for calculating formal charge is given below:. The best Lewis structure of any molecule will have 0 as the ideal formal charge for each atom. We also check the formal charge of each atom and make sure that it is the lowest possible. Converting potential lone pairs into double or triple bonds to make the molecule more stable. Arrangement of the remaining valence electrons so that each atom completes its octet.ĥ. Arranging the electrons as lone pairs to form bonds with each atom.Ĥ. Locating the central atom of the molecule.ģ. Counting the total number of valence electrons of the molecule.Ģ. Let us now look that steps required for drawing a Lewis structure:-ġ. In the Lewis structure of PO43-, P forms single bonds with 3 oxygen atoms and forms a double bond with one oxygen atom. The overall charge on the phosphate ion is -3 and the phosphorus atom is in an oxidation state of +5. To draw the Lewis structure of any compound, we always use the concept of valence electrons (number of electrons in the outer shell of each atom). (Credit: Jodi So Source: CK-12 Foundation License: CC BY-NC 3.Before we begin to draw the Lewis structure of PO43- step by step let us look at an overview of how the Lewis structure will look like. \): A nonpolar covalent bond is one in which the distribution of electron density between the two atoms is equal.
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