Bond dipole momentFrom Wikipedia, the free encyclopedia

The bond dipole moment uses the idea of electric dipole moment to measure the polarity of a chemical bond

within a molecule. It occurs anytime there is a separation of positive and negative charges. The bond dipole µ is

given by:

.

The bond dipole is modeled as +δ — δ- with a distance d between the partial charges +δ and δ-. It is a vector,

parallel to the bond axis, pointing from minus to plus, as is conventional[1] for electric dipole moment vectors.

(Some chemists draw the vector the other way around, pointing from plus to minus, but only in situations where

the direction doesn't matter.)[1] This vector can be physically interpreted as the movement undergone by

electrons when the two atoms are placed a distance d apart and allowed to interact, the electrons will move from

their free state positions to be localised more around the more electronegative atom.

The SI unit for electric dipole moment is the coulomb-meter, but that is much too large to be practical on the

molecular scale. Bond dipole moments are commonly measured in debyes, represented by the symbol D, which

is what you get if you measure the charge δ in units of 10-10 statcoulomb and measure the distance d in

Angstroms. Note that 10-10

statcoulomb is 0.48 units of elementary charge. Another useful conversion factor is

1 C m = 2.9979 × 1029 D.

Typical dipole moments for simple diatomic molecules are in the range of 0 to 11D. At one extreme, a

symmetrical molecule such as chlorine, Cl2, has zero dipole moment, while near the other extreme, gas phase

potassium bromide, KBr, which is highly ionic, has a dipole moment of 10.5D.[2]

For a complete molecule the total molecular dipole moment may be approximated as the vector sum of

individual bond dipole moments. Often bond dipoles are obtained by the reverse process: a known total dipole

of a molecule can be decomposed into bond dipoles. The reason for doing this is the transfer of bond dipole

moments to molecules that have the same bonds, but for which the total dipole moment is not yet known. The

vector sum of the transferred bond dipoles gives an estimate for the total (unknown) dipole of the molecule.

The Bond Dipole is two atoms in a bond, such that the electronegativity of one atom causes electrons to be

drawn towards the other, in turn causing a partial negative charge. There is therefore a difference in polarity

across the bond, which causes a dipole moment.

See also

Chemical polarity

Electric dipole moment

References

^ a b The Electric Dipole Moment Vector : Direction,Magnitude, Meaning, Etc. (http://www.av8n.com/physics

/electric-dipole.htm)

1.

^ Physical chemistry 2d Edition (1966) G.M. Barrow McGraw Hill2.

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Categories: Chemical bond properties

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