The graph of temperature versus molar mass is given for the hydrides of oxygen, sulfur, selenium, and tellurium. The points given are the melting (Mp) and boiling (Bp) points of the hydrides. The melting and boiling points decrease from hydrogen telluride, H2Te, to hydrogen sulfide, H2S; however, we find an abrupt increase in the melting and boiling points for water. Water shows an abrupt increase in its melting and boiling points because the water molecule has stronger intermolecular forces than the hydrides of sulfur, selenium, and tellurium. Which of the following statements explain this anomalous behavior of water? Check all that apply. View Available Hint(s) Check all that apply. H20 HoTe Bp 25 Mp Molar mass (g/mol) Solution Options (b) and (c) explains the anomalous behaviour. Due to stronger intermolecular hydrogen bonding apart from weak London forces (e.g, Vander Waals forces) that exists in other compounds also there is an abrupt increase in melting and boiling point of water. London forces are weakest forces and therefore, it requires more energy to break hydrogen bonds than to break them. .

1. The graph of temperature versus molar mass is given for the hydrides of oxygen, sulfur,
selenium, and tellurium. The points given are the melting (Mp) and boiling (Bp) points of the
hydrides.
The melting and boiling points decrease from hydrogen telluride, H2Te, to hydrogen sulfide,
H2S; however, we find an abrupt increase in the melting and boiling points for water. Water
shows an abrupt increase in its melting and boiling points because the water molecule has
stronger intermolecular forces than the hydrides of sulfur, selenium, and tellurium.
Which of the following statements explain this anomalous behavior of water?
Check all that apply.
View Available Hint(s)
Check all that apply.
Molecules in ice are held together only by covalent bonds.
It requires more energy to break hydrogen bonds than to break only London forces.
Water exhibits intermolecular hydrogen bonding in addition to London forces.
Hydrides of sulfur, selenium, and tellurium show extensive hydrogen bonding.
H20 HoTe Bp 25 Mp Molar mass (g/mol)
Solution
Options (b) and (c) explains the anomalous behaviour.
Due to stronger intermolecular hydrogen bonding apart from weak London forces (e.g, Vander
Waals forces) that exists in other compounds also there is an abrupt increase in melting and
boiling point of water. London forces are weakest forces and therefore, it requires more energy
to break hydrogen bonds than to break them.