Which one of the following has the highest dipole moment

The correct Answer is A In p-dichlorobenzene, the two C − C l bond dipoles (equal in magnitude and opposite in direction) cancel each other. In o-dichlorobenzene, the vertical component of one C − C l bond dipole reinforces the bond dipole of other C − C l bond dipoles (equal in magnitude and opposite in direction) cancel each other. In o-dichlorobenzene, the vertical component of one C − C l bond dipole reinforces the bond dipole of other C − C l bond while in m-dichlorobenzene, the vertical component of one C − C l bond dipole opposes the bond dipole of another C − C l bond.

The explanation for the correct option: Option(3) N H 3 • Among nitrogen and hydrogen, nitrogen is more electronegative and so the hydrogen gives dipole toward nitrogen. • And nitrogen gives dipole toward lone pair. • The direction of the lone pair dipole moment and the bond pair dipole moment is the same. so there is a net dipole in one direction. • The molecular geometry is pyramidal. The explanation for the incorrect option: 1. C O 2 • ​ C O 2 has a linear structure, there is a bond dipole moment between the C − O bonds. • But, as the dipole moment of one bond is canceled by the other, hence the dipole moment is zero. 2. C H 4 • ​It has zero dipole moment because it is tetrahedral in shape and each bond pair are at an equal distance which means these are symmetrically arranged hence each dipole moment of bond balance each other 4. N F 3 • ​Among nitrogen and fluorine, fluorine is more electronegative, hence the dipole is towards the fluorine atom. • N-F bonds are in the opposite direction, so they partly cut the bond moment of the lone pair. Hence, Option(3) N H 3 is the molecule with a higher dipole moment.

The three dimensional structures of the three compounds along with the direction of dipole moment in each of their bonds are given below : C l 4 being symmetrical has zero dipole moment . ln C H C l 3, the resultant of two C-Cl dipole moments is opposed by the resultant of C - H and C - Cl bonds . Since the dipole moment of latter resultant is expected to be smaller than the former, C H C l 3 has a finite dipole (1.03 D) moment. ln C H 2 C l 2, the resultant of two C - Cl dipole moments is reinforced by resultant of two C - H dipoles, therefore , C H 2 C l 2 (1.62 D) has a dipole moment higher than that of C H C l 3. Thus , C H 2 C l 2 has highest dipole moment.

https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FRiverland_Community_College%2FCHEM_1000_-_Introduction_to_Chemistry_(Riverland)%2F14%253A_Liquids_Solids_and_Intermolecular_Forces%2F14.07%253A_Intermolecular_Forces-_Dispersion_DipoleDipole_Hydrogen_Bonding_and_Ion-Dipole Expand/collapse global hierarchy • Home • Campus Bookshelves • Riverland Community College • CHEM 1000 - Introduction to Chemistry (Riverland) • 14: Liquids, Solids, and Intermolecular Forces • 14.7: Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole Expand/collapse global location \( \newcommand\) • • • • • • • • • • • • • • • • • • • • • • • • • Learning Objectives • To describe the intermolecular forces in liquids. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. In contrast to intramolecular forces, such as the covalent bonds that hold atoms together in molecules and polyatomic ions, intermolecular forces hold molecules together in a liquid or solid. Intermolecular forces are generally much weaker than covalent bonds. For example, it requires 927 kJ to overcome the intramolecular forces and break both O–H bonds in 1 mol of water, but it takes only about 41 kJ to overcome the intermolecular attractions and convert 1 mol of liquid water to water vapor at 100°C. (Despite this seemingly low value, the intermolecular forces in liquid water are among the strongest s...

Objectives After completing this section, you should be able to • explain how dipole moments depend on both molecular shape and bond polarity. • predict whether a molecule will possess a dipole moment, given only its molecular formula or Kekulé structure. • use the presence or absence of a dipole moment as an aid to deducing the structure of a given compound. Study Notes You must be able to combine your knowledge of molecular shapes and bond polarities to determine whether or not a given compound will have a dipole moment. Conversely, the presence or absence of a dipole moment may also give an important clue to a compound’s structure. BCl 3, for example, has no dipole moment, while NH 3 does. This suggests that in BCl 3 the chlorines around boron are in a trigonal planar arrangement, while the hydrogens around nitrogen in NH 3 would have a less symmetrical arrangement (e.g., trigonal pyramidal, T-shaped). Remember that the $\ce$ bond can usually be assumed to be nonpolar. Molecular Dipole Moments You previously learned how to calculate the dipole moments of simple diatomic molecules. In more complex molecules with polar covalent bonds, the three-dimensional geometry and the compound’s symmetry determine whether there is a net dipole moment. Mathematically, dipole moments are vectors; they possess both a magnitude and a direction. The dipole moment of a molecule is therefore the vector sum of the dipole moments of the individual bonds in the molecule. If the individual bond...

1) Dichlormethane (CH 2Cl 2) μ = 1.60D 2) Chloroform (CHCl 3) μ = 1.08D 3) Carbon tetrachloride (CCl 4) μ = 0D CCl 4is a symmetrical molecule. Therefore, the dipole moments of all four C−Cl bonds cancel each other. Hence, its resultant dipole moment is zero. As shown in the above figure, in CHCl 3, the resultant of dipole moments of two C−Cl bonds is opposed by the resultant of dipole moments of one C−H bond and one C−Cl bond. Since the resultant of one C−H bond and one C−Cl bond dipole moments is smaller than two C−Cl bonds, the opposition is to a small extent. As a result, CHCl 3has a small dipole moment of 1.08 D. On the other hand, in case of CH 2Cl 2, the resultant of the dipole moments of two C−Cl bonds is strengthened by the resultant of the dipole moments of two C−H bonds. As a result, CH 2Cl 2has a higher dipole moment of 1.60 D than CHCl 3i.e., CH 2Cl 2has the highest dipole moment. Hence, the given compounds can be arranged in the increasing order of their dipole moments as: CCl 4< CHCl 3< CH 2Cl 2 The three dimensional structures of the three compounds along with the direction of dipole moment in each of their bonds are given below: CCl 4being symmetrical has zero dipole moment. In CHCl 3, the resultant of two C – Cl dipole moments is opposed by the resultant of C – H and C – Cl bonds. Since the dipole moment of latter resultant is expected to be smaller than the former, CHCl 3has a finite dipole (1.03 D) moment. In CH 2CI 2, the resultant of two C – Cl dipole ...

Hint: Dipole moment is the product of the charge and the distance between the centers of positive and negative charges. Determine whether each molecule is symmetrical or not and also determine if the atoms have significant electronegativity difference. Complete answer: > If a bond is present between two atoms having same electronegativity, then the bond is nonpolar. A bond is polar if the atoms have an electronegativity difference. If a molecule contains only nonpolar bonds, then it is non-polar with zero dipole moment. If one or more polar bonds are present in the molecule, then the polar or nonpolar nature of the molecule depends on its molecular symmetry. > If an asymmetrical molecule contains polar bonds, then the molecule has a dipole moment. In this molecule, the individual bond dipoles do not cancel each other. Due to this, the net (resultant) dipole moment of the molecule is non zero. The structures of sulphur dioxide, carbon dioxide, boron trifluoride and trans-2-butene are as shown below: > Sulphur dioxide contains two elements, sulphur and oxygen. The electronegativity value of sulphur is significantly different from the electronegativity value of oxygen. Hence, the bond between sulphur and oxygen is polar. The central sulphur atom has two bonding domains and one lone pair of electrons. \[s\] hybridisation results in electron pair geometry of trigonal planar and molecular geometry of bent or V shaped. Sulphur dioxide molecule is an asymmetrical molecule containi...