Question

A diatomic molecule has a dipole moment of 1.2 d. If its bond length is 1.0 , what fraction of an electronic charge, exist on each atom?

Answer 1

Electronic charge ′e′=Dipole momentBond length′e′=Dipole momentBond length

=1.2×10−18esucm1.0×10−8cm=1.2×10−18esucm1.0×10−8cm

=1.2×10−10esu=1.2×10−10esu

Thus, fraction of electronic charge on each end

=1.2×10−104.8×10−10=1.2×10−104.8×10−10=0.25=0.25

=25%=25%of ′e′

Answer 2

Answer:

Explanation:

Dipole Moment:

In any system where the charges are separated, a dipole moment develops. Both covalent and ionic bonding have the potential to produce a dipole moment. Due to the difference in electronegativity, the dipole moments develop. Between these two atoms that are connected chemically is electronegativity.

A molecule's polarity between two atoms is gauged by a bond dipole moment. Electric dipole moment is a notion that is related to bond dipole. It gauges how well positive and negative charges are separated in a system. Being a vector quantity, the bond dipole moment has both magnitude and direction.

The formula for Dipole Moment:

Dipole Moment = Charge (Q) $*$Distance of separation (r)

Let the electronic charge on each atom be x.

Given : The dipole moment is 1.2D

The dipole moment in esu units is $1.2 *$$10^{-18}$esu.cm

The dipole moment is the product of its charge and the inter atomic distance.

It would be x × 100 × 10–10 = $1.2 * 10^{18}$

X = 1.2 ×$10^{-10}$esu

But the electronic charge e = $4.8 * 10 ^{-10}$esu

Partial electronic charge on each atom =  $1.2*10^{-10} esu / 4.8*10^{10} esu *100$

where

X = 25% of e (0.25)

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