A polar bond is a covalent bond in which electrons are shared unevenly due to differences in the electronegativities of the bonded atoms, usually resulting in one atom having a partial negative charge and the other a partial positive charge.
A polar molecule is a group of covalently bonded atoms that that has a partial negative at one end and a partial negative charge at the other because it contains at least one polar bond.
a polar molecule is a MOLECULE containing atoms of enough electronegativity difference to make the electrons to be more likely to be closer to the more electronegative atoms. A hydrogen bond is a type of BOND or interaction per se that results between polar molecules due to the electrical differences between a partial positive part and a partial negative part.
There are several types of covalent bonding and those are stated below along with an example.
Polar molecules with polar bonds - Hydrogen Chloride
Non-polar molecules with polar bonds - Sulfur Hexafluoride
Non-polar molecules with non-polar bonds - Ozone
Dipole is more of a general term for two point charges that are separated by a distance and have an electric field between them. Every polar bond creates a dipole, but a molecule containing polar bonds might not have a total dipole moment.
These occur in cases of symmetry where dipole vectors cancel each other out.* For example, all four bonds in carbon tetrachloride (CCl4) are polar because chlorine is very electronegative. This results in four dipoles where all four vectors point from the central carbon to one of the four chlorines. But because CCl4 is tetrahedral, the vectors point in "opposite" directions and cancel each other out because they have the same magnitude. (If you draw it out, you notice that the vectors aren't really in opposite directions, but their components in the x, y, and z are opposite).
* If the content about vectors is confusing, here's the short version: between two atoms such as carbon and chlorine where there is a significant electronegativity difference, a polar bond is created. Chlorine is so electronegative that it will pull electron density from carbon. This creates a difference in electric potential and an electric field between the positive carbon and negative chlorine. We represent this field by an arrow pointing from carbon to chlorine (this is the vector). You sum these vector contributions within a molecule to determine if the overall molecule has a dipole moment. If the vector are oriented symmetrically, they could cancel each other out and no molecular dipole is created.
polar bond.
When a polar and a non-polar molecule come close the attraction taking place between them due to partial charges isknown as dipole induced dipole interaction.
Every polar molecule has a permanent dipole.
Dipole-dipole forces play a significant role when a molecule is polar.
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
The shape of the molecule and The electronegativity differences of atoms in the molecule
Dipole-dipole is between two polar molecules, that would be polar anyway. Dipole-induced dipole is between a polar molecule and a non-polar molecule that is now polar due to the proximity of a polar molecule.
When a polar and a non-polar molecule come close the attraction taking place between them due to partial charges isknown as dipole induced dipole interaction.
Every polar molecule has a permanent dipole.
Ay molecule with a net dipole moment will have dipole -dipole interactions. These are molecules with polar bonds caused by a diference in electronegativity between the atoms being bonded.
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. They are much weaker than ionic and it happens when the two molecules are close together!
When the charge between molecules hasn't completely cancelled out. Br2 will cancel- vdw forces H2O will not- dipole-dipole bonds
a dipole in induced.
Dipole-dipole forces play a significant role when a molecule is polar.
This compound, called propane, is nonpolar.
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
The shape of the molecule and The electronegativity differences of atoms in the molecule
Intermolecular attraction