Question
What is dipole moment? Explain with example.
✓
Answer
The product of value of charge and distance between charges in polar molecule is called dipole moment.
Dipole moment $(\mu)=$ Charge $( Q ) \times( r )$ distance between charges
$
\text { or } \mu=Q \times \operatorname{r} \text { or } \mu=Q \times d
$
The unit of dipole moment is Debye (D) :
$
1 D=3.3 \times 10^{-30} Cm
$
C = Coulomb
$m =$ meter
It is a vector quantity.
The dipole moment of polyatomic molecules is the vector sum of bond moments of its various polar bonds.
Those molecules in which all the bonds are equal and whose geometry is symmetric and regular, such as linear, triangular planar and tetrahedral etc. then the resultant dipole moment of the molecule is absolutely zero. The dipole moment of $BF _3$ is zero because its geometry is triangular planar and all the bonds in it are equal which cancel each other's effect.
Due to the bent shape of $H _2 O$, its dipole moment is high.
Dipole moment $(\mu)=$ Charge $( Q ) \times( r )$ distance between charges
$
\text { or } \mu=Q \times \operatorname{r} \text { or } \mu=Q \times d
$
The unit of dipole moment is Debye (D) :
$
1 D=3.3 \times 10^{-30} Cm
$
C = Coulomb
$m =$ meter
It is a vector quantity.
The dipole moment of polyatomic molecules is the vector sum of bond moments of its various polar bonds.
Those molecules in which all the bonds are equal and whose geometry is symmetric and regular, such as linear, triangular planar and tetrahedral etc. then the resultant dipole moment of the molecule is absolutely zero. The dipole moment of $BF _3$ is zero because its geometry is triangular planar and all the bonds in it are equal which cancel each other's effect.
Due to the bent shape of $H _2 O$, its dipole moment is high.
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