Quick Hydrogen Bonding Question

I understand how the relatively strong hydrogen bonds between water molecules result in water having a relatively high melting point. However if when water (s) melts and these hydrogen bonds collapse, how is water still able to have such a relatively high boiling point as said in the textbook (since surely there would be no hydrogen bonds between the water molecules in its liquid state)?

There are still hydrogen bonds in the liquid state ...

Oh okay that'd make sense; it's just the textbook says that 'when ice melts, the rigid hydrogen bonds collapse, allowing the H"2"O molecules to move closer together' which suggested to me that the only intermollecular from then on were vdw / pd forces.

Thank you.