question_answer 1)

Compare the structures of \[{{H}_{2}}O\] and\[{{H}_{2}}{{O}_{2}}\].

Answer:

In\[{{H}_{2}}O\], oxygen atom is \[\text{s}{{\text{p}}^{\text{3}}}-\text{hybridized}\], i.e., tetrahedral configuration. Two hybrid orbitals form two sigma bonds with two hydrogen atoms and two lone pairs of electrons are present, i.e., the shape of the water molecule is bent. The expected bond angle is reduced from \[{{109}^{{}^\circ }}{{28}^{'}}\]to \[\text{1}0\text{4}.\text{5}{}^\circ \]due to repulsions between lone pairs. \[{{H}_{2}}{{O}_{2}}\] has a non-planar structure. The two oxygen atoms are linked to each other by a single covalent bond and each oxygen is further linked to a hydrogen atom by a covalent bond. The two OH bonds are present in different planes. The dihedral angle between two planes is \[\text{111}.\text{5}{}^\circ \]in gaseous phase. The structure of \[{{H}_{2}}{{O}_{2}}\] is like that of an open book.