Water is a polar molecule with slight positive charge on its Hydrogen atoms, and a negative charge on the oxygen. The intermolecular attraction that makes water a liquid at room temperatures is an example of:
Hydrogen Bonding
Dipole-dipole forces
Loundon dispersion forces
Ionic compounds have strong electrical attraction acting on all sides between anions and cations in a crystal lattice. This is a
much stronger attraction than for hydrogen bonding or molecular dipole interaction.
Please explain in a few sentences why ice can melt in your hand, but it takes a furnace at 1,474°F (801"C) to melt dry salt.
оос
You need not, but certainly could, look up the structure of the following organic chemicals:
n-Heptane, n-C, H16 n-Heptanal, n-C, H2,0
These two molecules are similar EXCEPT for the fact that Heptane is nonpolar, and Heptanal has a slightly polar double bond
Oxygen in place of two Hydrogen atoms at the end of the molecule. One of them boils at 98.4°C, and the other at 150°C.
The higher boiling material is... n-Heptane, n-C, H16
n-Heptanal, n-C, H,O,
...because it has the strength of Loundon Dispersion forces.
Dipole-dipole interaction.