The structures of hydrogen peroxide $$\text{H}_2\text{O}_2$$ in the solid and gaseous states are given below. Liquid $$\text{H}_2\text{O}_2$$ is slightly more viscous than liquid $$\text{H}_2\text{O}$$. The correct options among the following are

Both O atoms are near enough to cause repulsion between the electron lone pairs thus making the O-O bond susceptible for cleavage

The strong intermolecular H-bonding along with restricted rotation present in the liquid state of $$\text{H}_2\text{O}_2$$ make it more viscous than liquid $$\text{H}_2\text{O}$$

The molecule gets twisted to minimize the repulsion between the lone pair and bond pair of electrons

The difference in the dihedral angles in the solid and gaseous states is a consequence of hydrogen bonding between the molecules