Electric field intensity is a vector field we assign the symbol E and has units of electrical potential per distance; in SI units, volts per meter (V/m).

Electric field intensity is a vector quantity because it has both magnitude and direction.

Secondly, electric field has a direction which is outward from positive charges and inward to negative charges. To be concluded, electric field has both magnitude and direction which are the standards to be defined as a vector quantity. Hence, an electric field is a vector quantity.

The space around an electric charge in which its influence can be felt is known as the electric field. The electric field intensity at a point is the force experienced by a unit positive charge placed at that point. Electric Field Intensity is a vector quantity. It is denoted by ‘E’.

As mentioned earlier, electric field strength is a vector quantity. Unlike a scalar quantity, a vector quantity is not fully described unless there is a direction associated with it.

unit. Electric dipole moment is defined as the product of charge and the distance between the charges, and is directed from negative to positive charge. The SI unit of electric dipole moment is coulomb metre (Cm).

An electric dipole is defined as a couple of opposite charges q and –q separated by a distance d. The simplest example of an electric dipole is a pair of electric charges of two opposite signs and equal magnitude separated by distance.

Electric dipole moment is a vector quantity and it is represented as →p=q×→d in vector form.

A dipole moment is the product of the magnitude of the charge and the distance between the centers of the positive and negative charges. It is denoted by the Greek letter ‘µ’. It is measured in Debye units denoted by ‘D’. 1 D = 3.33564 × 10-30 C.m, where C is Coulomb and m denotes a meter.

A dipole moment is simply the measure of net polarity in a molecule. Polar molecules exhibit a large difference in electrical charge (a positive end and a negative end), otherwise known as a dipole moment. For example, ammonia (NHsub3) is a polar molecule.

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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.

Dipole moment (μ) is the measure of net molecular polarity, which is the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges. Dipole moments tell us about the charge separation in a molecule. The symbol δ indicates the partial charge of an individual atom.

The dipole moment of two equal but opposite charges (q+, q−) is defined as the product of charges and the distance separating them; thus it is a vector quantity where the magnitude of the dipole moment vector is qr and the direction is from the negative charge to the positive.

The electric dipole moment, a vector, is directed along the line from negative charge toward positive charge. Dipole moments tend to point along the direction of the surrounding electric field.

It is a vector since it points in one direction (from one charge to the other), has an associated magnitude and so on. In a way, when you consider a multipole expansion it makes sense, the monopole momentum is just the net charge (a scalar), the dipole momentum a vector and from then on matrix quantities.

NH3 is a polar molecule because, in the NH3 molecule, it has three dipoles because of three bonds and these dipoles do not cancel out each other. They form a net dipole moment.

Although NH3 vigorously accepts hydrogen bonds in the gas phase, there is yet no example in which NH3 acts as a hydrogen-bond donor. The stereochemistry of the weak interactions of ammonia is dominated by its lone-pair orbital, which leads to the characterization of NH3 as a strong Lewis base.

The nitrogen atom, like the oxygen in water, is much more electronegative than the attached hydrogens. This causes an uneven distribution of electrons and makes ammonia a polar molecule. Because ammonia is a polar molecule, it can be dissolved by water.

Ammonia (NH3), shown in the middle, has a lone pair of electrons, and since nitrogen is more electronegative than hydrogen, the nitrogen atom has a partial negative charge (red color).

In the case of ammonia, the amount of hydrogen bonding is limited by the fact that each nitrogen only has one lone pair. That means that on average each ammonia molecule can form one hydrogen bond using its lone pair and one involving one of its δ+ hydrogens.

The electronegativity of Hydrogen and Sulfur is 2.20 and 2.58, respectively. Their electronegativity difference, 0.38, is less than 0.5. Thus, H2S is a non-polar bond. Due to Sulfur being more electronegative than Hydrogen, it is partially negative.

Hydrogen sulfide is non-polar on account of its nonpolar H–S bonds. The EN difference between hydrogen and sulfur is 0.4, so hydrogen and sulfur form non-polar bonds. Although it has an asymmetrical molecular geometry, the entire molecule is non-polar dues to the absence of any polar bonds.