And as per VSEPR theory, these lone pairs try to repel each other, which distorts the molecule’s shape. However, there are two lone pairs of electrons on each Oxygen atom. Here two Oxygen atoms are forming bonds with Hydrogen atoms. VSEPR theory helps us determine the molecular geometry of any given molecule. There is one s orbital and three p hybrid orbitals to form to accommodate the lone pairs as well as the bonding pairs of electrons. The steric number of H2O2 also corresponds to 4, which means it is sp3 hybridized. You can also find the steric number for finding the hybridization this way, one can easily get the hybridization of any molecule. In short, it needs to form four hybrid orbitals. If you consider one Oxygen atom, for now, it forms a bond with the Hydrogen atom, neighbouring oxygen atom and has two lone pairs. Here both Oxygen atoms are forming bonds, and hence these two Oxygen atoms undergo hybridization. H2O2 Hybridizationĭetermining hybridization for any molecule becomes easy and quick once you know the central atom, the atoms forming bonds with it and the number of lone pairs of electrons. There are three single bonds formed in these molecules, and hence there are 3 bonding pairs and four lone pairs of electrons in H2O2. These pairs of electrons are called non-bonding or lone pairs of electrons.Īs a result, all the atoms have complete octets now as both Oxygen atoms have eight valence electrons in its outer shell and Hydrogen atoms have two valence electrons in its outer shell. Each Oxygen atom will have four valence electrons or two pairs of electrons that do not participate in any bond formation. Arrange the remaining eight electrons around the Oxygen atom. We used up six valence electrons out of 16 ( there are three single bonds in these molecules. As a result, four more valence electrons are used in total as both these Hydrogen atoms form a single bond with oxygen atoms. Now place two Hydrogen atoms next to these Oxygen atoms.Įach Hydrogen atom only requires one more valence electron to complete its octet, and hence it forms a bond with the neighbouring Oxygen atom. So now, for H2O2 Lewis Structure, we first put the central atoms and show their bond formation with other atoms.Īs there are two Oxygen atoms here, both of these oxygen atoms take the central position and share two valence electrons to form a bond.
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