What is dipole moment in chemistry?
Dipole moment in chemistry expressed the polar character or polarity of the molecules. The product of charge and distance of separation of atoms in chemical bond defines the term dipole moment. If +q amount positive charge separated by -q amount of negative charge by the bond distance l, then dipole moment (μ) of polar molecule = q × l. Perfectly non-polar molecules like hydrogen, oxygen, and nitrogen have zero dipole moment and the polar molecules like water, ammonia, and methane have positive values. It is a tool used to calculate the percentage ionic character, electric polarization, and residual charge on the atoms of the molecules
What are polar molecules?
When the center of gravity of the positive charge does not coincide with the center of gravity of the negative charge, polarity arises in the molecules. These molecules are called polar molecules. Hydrogen chloride, water, methyl chloride, and benzyl chloride are examples of polar molecules.
Unit of dipole moment
In the CGS system, the charge is expressed in esu and bond length in cm. Therefore, the unit of dipole moment is esu cm. The charge is of the order of 10-10 esu and the distance of separation is the order of 10-8 cm. Hence the order of μ is 10-18 esu cm. This magnitude is called 1 Debye. Therefore, 1 Debye = 10-18 esu cm.
In the SI system, the charge is expressed in coulomb and the length is meter. Hence the unit of dipole moment in the SI system is the coulomb meter.
Debye to coulomb meter
In the CGS system, μ = 4.8 × 10-10 × 10-8 esu cm = 4.8 Debye. In the SI system, μ = 1.6 × 10-19 × 10-10 coulomb m = 16 × 10-30 coulomb m. Therefore, 4.8 Debye = 16 × 10-30 coulomb m. Form the above formula, 1 Debye = 3.336 × 10-30 coulomb m.
Application of dipole moment
It is used for the calculation of the percentage ionic character, bond angle, electric polarization, and residual charge on the atoms in the molecules. It also helps to determine the size or shape of molecules and the arrangements of chemical bonds in the molecules.
Percentage ionic character
Dipole moment data used to calculate the percentage ionic character of covalent or ionic heteronuclear diatomic molecules. Let us consider a molecule AB having the observed dipole moment = μobs and the bond length l cm. If the shared pair lies at the midpoint of the atoms, the bond would be a purely covalent bond, and the percentage ionic character is zero. But if the bond is 100 percent ionic and B is more electronegative than A. Therefore, A carries a unit positive charge, and B carries a unit negative charge.
Percentage ionic character formula
In that case, the μ of AB would be, μionic = e × l = 4.8 × 10-18 esu cm. But the μ of AB is neither zero nor μionic.
Percentage ionic character of HCl
If we consider HCl as a purely ionic compound the charge on hydrogen and chlorine = 4.8 × 10-10 esu and bond length = 1.27 × 10-8 cm. Therefore, the dipole moment of HCl, μionic = e × l = 4.8 × 10-10 × 1.27 × 10-8 esu cm. The calculated or observed dipole moment = 1.03 Debye = 1.03 × 10-18 esu cm. Hence the percentage ionic character of HCl = (µobs/µionic) × 100 = (1.03 × 10-18/4.8 × 10-10 × 1.27 × 10-8) × 100 = 16.89.
Electric polarization formula
In learning chemistry, the induced electric polarization formula is used to calculate the radius of the molecules. The induced electric polarization formula of the molecules is,
At NTP, M/ρ = molar volume or density = 22400cc/mole and for spherical molecule, αi= r3. Therefore, r3 = (22400/4πN0)(D0 -1) = 2.94 × 10-21 (D0 -1). Therefore, with the known value of capacitance, we can easily determine the radius of the molecule.
Dipole moment examples
It is used to define the structure, bond angle, bond energy, and polarity of different molecules in chemistry. Mono-atomic noble gases and benzene are non-polar because the charge of the constituent atom is distributed symmetrically.
Homonuclear diatomic molecules examples
Homonuclear diatomic molecules like nitrogen, oxygen, and chlorine have zero dipole moment due to the symmetrical charge distributions and similar electronegativity and ionization energy.
Heteronuclear diatomic molecules examples
Hydrogen bromide and hydrogen iodide have non-zero dipole moments indicate the unsymmetrical charge distribution between two bonding atoms in the molecules. Due to the difference in electronegativity of the constituent atoms in heteronuclear diatomic molecules always polar. Hence the electron pair is not equally shared in hydridized orbital and shifted to the more electronegative atom. Therefore, μHCl = 1.03 Debye, μHBr = 0.79 Debye, μHI = 0.38 Debye, μHF = 2.00 Debye.
Dipole moment of CO
The electronegativity difference between carbon and oxygen in CO is very large but the dipole moment of carbon monoxide very low. This suggested that the charge density in the oxygen atom somehow back-donated to the carbon atom. Hence CO formed a coordinate covalent bond directing towards carbon atom to decreases polarity.
How to calculate dipole moment?
Carbon dioxide (CO2), beryllium chloride (BeCl2), stannous chloride (SnCl2) have zero dipole moment indicating that the molecules have symmetrical linear structures. In CO2, one carbon-oxygen bond cancels the bond moment of the other carbon-oxygen bond.
What is bond moment?
The electric moment associated with the bond arising from the difference of electronegativity is called bond moment (m). In a molecule, the vectorial addition of the bond moments used for the calculation of the μ. Therefore, μ2 = m12 + m22 + 2m1m2Cosθ, where m1 and m2 are the bond moments projecting at the angle of θ.
Bond moment and dipole moment calculation help to finding the bond angle of CO2, H2O, H2S, and SO2, etc. For CO2, µ = 0 and m1 = m2 = m. Therefore, 0 = 2m2(1 + cosθ) or θ = 180°. For H2O, H2S, and SO2 molecules, θ < 180° Therefore, these molecules are non-polar because they have non-linear structures.
|Molecule||Dipole moment (Debye)||Bond angle|
Dipole moment of water molecule
For water (H2O), dipole moment (μwater) = 1.84 Debye and bond moment (mOH) = 1.60 Debye. Therefore, (1.84)2 = 2(1.60)2(1 + cosθ). Form the above formula θ = 105°. Therefore, the contribution of non-bonding electrons toward the total dipole moment is included within the bond moment of water.
Dipole moment of BF3 and BCl3
Boron trichloride (BCl3), boron trifluoride (BF3) are the tetratomic compound having dipole moment zero, indicating that they have a regular planar structure.
From the above picture, three halogen atoms are on a plane at the corner of the equilateral triangle and a boron atom at the intersection of the medians. Therefore, the μnet of the BCl3 and BF3 is zero.
Dipole moment of NH3 and PH3
Other types of the molecule such as ammonia (NH3) and phosphine (PH3) are polar, where μ≠0 indicated that the molecule has a pyramidal structure. Hence three hydrogen atoms are on the plane and nitrogen or phosphorus atom at the apex of the pyramid in NH3 or PH3 molecule.
Dipole moment of NF3
NF3 shows a very small bond moment although there is a great difference in electronegativity and electron affinity between nitrogen and fluorine atoms and a similar structure of NH3. This low value of µ in NF3 is explained by the fact that the resultant bond moment of the three nitrogen – fluorine bonds are acting in the opposite direction to that of the lone pair placed at the nitrogen atom. But in NH3, the resultant bond moment is acting in the same direction as that of the lone pair electrons.
Penta atomic molecule
Methane (CH4), carbon tetrachloride (CCl4), platinum chloride (PtCl4) are examples of penta atomic molecules having zero dipole moment. This suggests that they are either regular tetrahedral or square planer structures. But the polar molecules of this type have pyramidal structures.
Dipole moment of methane
For the calculation of the dipole moment of methane, let us discuss the structure of methane. In methane molecule, the valence shell electronic configuration of central carbon atom 2s2 2p2. Hence the carbon atom in methane sp3 hybridized to form a regular tetrahedral structure with the angle of each H-C-H = 109°28ˊ. The electric moment associated with a group is called group moment. It depends on the arrangement of the bonds in the groups. The difference of the electronegativity of the constituent atoms forming the bonds in the group.
It can be shown that the group moment of the methyl group (mCH3) identical to the bond moment of a carbon hydrogen bonding (mCH). From the structure and bond moment, mCH3 = 3 mCH × Cos(180° -109°28՛) = 3 mCH Cos 70°32՛ = 3 mCH × (1/3) = mCH. Therefore, two bond moments cancel each other to show zero dipole moment in the CH4 molecule. It can be also calculate by another methods, µmethane = mCH (1 + 3 Cos 109°28՛) = 0.
Dipole moment measurement
Dipole moment of CCl4
By similar calculation, it can be shown that mCCl3 = mCCl = m in chloroform (CCl4). Therefore, the net dipole moment for CCl4 molecule (μchloroform) = 2m2(1 + Cosθ) = 0, where Cosθ = Cos180° = -1.
Dipole moment of chloromethane (CH3Cl)
We know, μ2 = m12 + m22 + 2 m1m2 Cosθ. But for dichloromethane (CH3Cl), θ = 0° hence Cosθ = 1. Therefore, μchlorometane = (m1 + m2) = (1.5 D + 0.4 D) = 1.9 D
Dipole moment of CHCl3
Similarly, for trichloromethane (CHCl3), θ = 0° hence Cosθ = 1. Therefore, μCHCl3 = (m1 + m2) = (1.5 D + 0.4 D) = 1.9 D.
Dipole moment of hydrocarbons
A similar calculation is done for μ of hydrocarbon like ethylene, propylene, butylene, etc, and alcohol in organic chemistry. The bond moment of mOH = 1.6, mC-O = 0.7, mCH3 = mCH = 0.4 Debye. Therefore, the resultant dipole moment of methyl alcohol = 1.56 while the observed value = 1.65 debye.