could someone explain to me dispersion forces, dipole dipole forces and hydrogen bonding, and possibly?

Question

give me examples of some. thanks.

Answer 1

London dispersion forces are weak intermolecular forces in which there is a temporary dipole that exists between the molecules of a compound. These forces occur in nonpolar molecules, and are the weakest bonds, and some example of compounds that have London dispersion forces are Cl2 Br2 CH4

http://www.teachmetuition.co.uk/Chemistry/Intermolecular/van_der_waals_forces.htm

Dipole-dipole forces occur between polar molecules, and it is when the more electronegative element in a compound has a partial negative charge and the less electronegative element has a partial positive, and example of this is HCl.

http://www.teachmetuition.co.uk/Chemistry/Intermolecular/dipole.htm

Hydrogen bonding occurs between hydrogen and either oxygen, nitrogen or fluorine, the 3 most electronegative elements. They exist in polar molecules, and are strong bonds.

http://www.teachmetuition.co.uk/Chemistry/Intermolecular/hydrogen_bonding.htm

Hope this helps!

Answer 2

London dispersion forces, sometimes called Heitler-London forces, are invoked to explain why one can liquefy helium, when that atom has no opposite charges and is too light for van der Waals forces to explain. There is a minute probability that all the electron distribution of a helium atom may rush suddenly to one "side." That means that side is negatively charged for a moment,and the other side positively charged by default. The negative charge lon on side distorts the electron cloud on a neighboring helium atom, repelling it. The positive side distorts the charge distribution of a third helium atom. As a result, there is a slight attraction that builds up among all the helium atoms in a sample.

Dipole forces create attraction among molecules when one "side" is permanently slightly positive and the other slightly negative. An example is CHCl3, chloroform. The molecule loiks like a tripod standing on three C-Cl "legs." The H sticks "in the air." The greater electronegativity of Cl makes the "bottom" of the molecule minus and the H positive by default.

Hydrogen bonding is the attraction of H in covalent bonds with atoms of high electronegativity for other atoms of high electronegativuity in other molecules. For example H2O. The H of one H2O is attracted to the O of another. Or an H of H2O may be attracted to N of ammonia, NH3.