The higher the difference in the electronegativities of the bonding atoms, the greater the bond polarity. This is because O is more electronegative than N which is more electronegative than carbon. The C-O bond is more polar than the C-N bond which is more polar than the C-C bond.

Water

The molecule with the polar bond that has the greatest difference in electronegativity is the most polar. For example a carbon-oxygen bond is more polar than an oxygen-fluorine bond because the difference in electronegativity for oxygen and carbon is greater than the difference between fluorine and oxygen.

The terms “polar” and “nonpolar” usually refer to covalent bonds. To determine the polarity of a covalent bond using numerical means, find the difference between the electronegativity of the atoms; if the result is between 0.4 and 1.7, then, generally, the bond is polar covalent.

It contains two polar bonds that are arranged symmetrically. Carbon forms a double bond with each oxygen atom. But the geometry of CO2 is linear so that the two bond dipole moments cancel and there is no net molecular dipole moment. Thus, the molecule is non-polar.

Individual bond dipole moments are indicated in red. Due to their different three-dimensional structures, some molecules with polar bonds have a net dipole moment (HCl, CH2O, NH3, and CHCl3), indicated in blue, whereas others do not because the bond dipole moments cancel (BCl3, CCl4, PF5, and SF6).

Molecules with only two atoms contain only one (single or multiple) bond, so the bond dipole moment is the molecular dipole moment. They range in value from 0 to 11 D. At one extreme, a symmetrical molecule such as chlorine, Cl2, has 0 dipole moment. This is the case when both atoms’ electronegativity is the same.

CO2 has the structure as O=C=O. in which there is bond dipole moment (C-O bond). But, as the dipole moment of one bond is cancelled by other, the structure of CO2 is a linear. So, CO2 has zero dipole moment because it is a linear molecule.

A dipole moment is a measurement of the separation of two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to the charge multiplied by the distance between the charges and the direction is from negative charge to positive charge: μ = q · r.

The applications of dipole moment are. (i) The dipole moment helps to predict whether a molecule is polar or non-polar. As µ = q X d, greater is the magnitude of dipole moment, higher will be the polarity of the bond. For non-polar molecules, the dipole moment is zero.

(i) Ionic character can be calculated using the value of dipole moment. (ii) Geometry of the molecule can be predicted using the dipole moment. (iii) Dipole moment is helpful in predicting nature of the molecule.

Dipole moment is the product of electric charge and distance between the positive and negative species present in the molecule. Answer verified by Toppr.

Applications : 1) Dipolemoment is useful in calculating the percent ionic character of polar covalent bonds. 2) Dippolemoment is useful in predicting the shapes of molecules.

1a : a pair of equal and opposite electric charges or magnetic poles of opposite sign separated especially by a small distance. b : a body or system (such as a molecule) having such charges or poles.

A dipole is any molecule with a positive end and a negative end, resulting from unequal distribution of electron density throughout the molecule.