Water has London forces, dipole -dipole interactions and hydrogen bonding, why isn't it a solid? Because with all of these intermolecular forces shouldn't it be really hard for it to be in liquid form because you have to break some of the intermolecular forces at high energy because of how stable the molecule is together so the atoms are more moveable?
water is found in a liquid state. This is because of the tiny, weak hydrogen bonds which, in their billions, hold water molecules together for small fractions of a second. Water molecules are constantly on the move.
water is found in a liquid state. This is because of the tiny, weak hydrogen bonds which, in their billions, hold water molecules together for small fractions of a second. Water molecules are constantly on the move.
Then shouldn't everything be in liquid form because some things only have London forces (which are the weakest) but are still solid?
Water has London forces, dipole -dipole interactions and hydrogen bonding, why isn't it a solid? Because with all of these intermolecular forces shouldn't it be really hard for it to be in liquid form because you have to break some of the intermolecular forces at high energy because of how stable the molecule is together so the atoms are more moveable?
It may be to do with the strength of the intermolecular forces.
Then shouldn't everything be in liquid form because some things only have London forces (which are the weakest) but are still solid?
yh and those things that have London forces are liquid and they are only held for a fraction of a second so maybe for a moment they are solid but then change the molecules make new dipoles and so it they dont stay in that from??
yh and those things that have London forces are liquid and they are only held for a fraction of a second so maybe for a moment they are solid but then change the molecules make new dipoles and so it they dont stay in that from??
Graphite is in solid form and only has London forces (as far as I'm aware)
Graphite is in solid form and only has London forces (as far as I'm aware)
Graphite is a macromolecule. It has a large network of covalent bonds which have to be broke and hence it has a very high melting and boiling point. It does have Van der Waals forces between the hexagonal layers, however, this only causes the layers to slide past eachother. Energy is required to break most of the covalent bonds in graphite in order to break the lattice structure.