If we look up this notation in the VSEPR chart given below we find that HNO2 has a bent shape. Here, N=1 as there is a pair of lone pair on N atom. Now N here represents the non-bonding electrons i.e lone pairs on the central atom. So X=2 (2 Oxygen atoms bonded to Nitrogen). Next, we look at X which represents the number of atoms bonded to the central atom. This can be determined by using the AXN notation where A represents the central atom which is N in this case. The bond angles formed are close to 120°. The molecular geometry of HNO2 is Bent (a bent-shaped molecule). It gives us the shape and the bond angles between each atom. The next important step is to determine the molecular geometry of HNO2. Hence, the hybridization of HNO2 can be found using these two methods. H=3, indicating that HNO2 is Sp2 hybridized. Since HNO2 is a neural molecule (overall charge is 0), the charge of cation or anion will also be zero. The only monovalent atom is H of which there is only one atom. V = 5 (valence electrons of the central atom N) H= Hybridization, V= Number of Valence electrons, C= Charge on cation or more electropositive atom, and A= Charge on anion or more electropositive atom. The formula to find the Hybridization is as follows:. We also have a formula that is useful to determine the Hybridization of a molecule. Thus the total (H) is 2+1=3 making it sp2 hybridized.Ģ. It’s bonded to two oxygen atoms and has a lone pair. The value of Hybridization (H) goes like this, Hybridization is determined by adding the number of bonds and the lone pair of the central atom. We can find hybridization by understanding the theory behind it. There are two ways to understand Hybridisation:-ġ. Hybridization is the formation of new hybrid orbitals which help determine a molecule’s shape and properties. You can use the above-mentioned steps to find the Lewis structure of any molecule.Īfter understanding the Lewis structure we next come to the Hybridization of a molecule. Now the Lewis structure of HNO2 is complete and if we check the formal charge of each atom it turns out to be zero. Thus we turn one pair of valence electrons from O to form a double bond with N so that each atom achieves its octet. It should be the lowest possible and can be calculated by the formula given below.Īfter arranging all the 18 valence electrons around the molecule, we notice that N is short of 2 valence electrons for it to complete its octet. You can also check out the formal charge of each atom as a last step. After arranging these electrons if the atoms do not achieve their octet form then we turn the valence electrons into a double or a triple bond so that each atom has its complete octet. Now we start arranging the rest of the valence electrons so that each atom attains its octet or duplet (H). Now we put 2 valence electrons between each atom which resembles a chemical bond. Hence we see that N is the central atom as it has the highest bonding sites and is less electronegative than O. In the case of HNO2, we need to note that whenever H is attached to a polyatomic molecule (in this case NO2) the H will always be attached to one of the oxygen atoms. Now we come to the second step which is to determine the central atom of the compound (one which has the highest number of bonding sites). Thus, when we add it all up we get the total number of valence electrons which is 1+5+12 = 18 valence electrons. Looking at HNO2, we see that H has 1 valence electron, N has 5 valence electrons and O has 6 valence electrons and there are two atoms of O, so 6×2 = 12 valence electrons. We begin by counting the total number of valence electrons of the molecule. Now let us take a look at the steps of drawing a Lewis diagram:. Only hydrogen and helium are exceptions as they follow the duplet rule i.e 2 electrons in its outermost shell. This basically means each atom should have 8 electrons around it so that it can achieve its stability. These electrons are arranged in such a way that each atom completes its octet. The valence electrons are shown in the form of dots around the atom. Valence electrons of a particular group can be determined by looking at the number written on top of their column in a periodic table. The number of valence electrons of an atom is denoted by the Lewis structure. Now, before we proceed to make the Lewis structure for HNO2, there are a few things you need to note. Hence, whenever bonding is mentioned besides a molecule or a compound your mind should immediately jump to the Lewis structure of the given compound. Making a Lewis structure is the first and most crucial step for identifying various properties related to the bonding of the molecule.
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