Home
Class 12
CHEMISTRY
The measure of net molecular polarity is...

The measure of net molecular polarity is a quantity called dipole moment which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance 'r' between the charge :
`mu=Qxxr`
Molecular polarities give rise to some of the forces that occur between molecules.Such forces are termed as intermolecular forces.These molecular forces are of several different types including dipole-dipole forces, London dispersion forces, hydrogen bonds and ion-dipole forces (operate between ions and molecules).These intermolecular forces are electrical in origin and results from the mutual attraction of unlike charges or the mutual repulsion of like charges.
A formal positive charge on the central atom affect the size of orbitals.A formal positive charge on central atom will pull in all electrons towards the nucleus and this will leads to the contraction in size of orbitals.
Which of the following molecule does not have dipole moment ?

A

`Trans - N_2F_2`

B

`NF_3`

C

`CIO_2-`

D

`CH_2Cl_2`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given molecules does not have a dipole moment, we will analyze each option step by step. ### Step 1: Analyze Trans-N2F2 1. **Structure**: The molecule has a trans configuration with nitrogen (N) atoms double bonded to each other and each nitrogen bonded to a fluorine (F) atom. 2. **Dipole Moment**: The dipole moments from the N-F bonds will point towards the fluorine atoms. However, because the molecule is symmetric (trans), the dipole moments will cancel each other out. 3. **Conclusion**: The dipole moment for trans-N2F2 is **zero**. ### Step 2: Analyze NF3 1. **Structure**: The nitrogen atom is bonded to three fluorine atoms and has one lone pair of electrons. 2. **Dipole Moment**: The dipole moments from the N-F bonds will point towards the fluorine atoms, and the lone pair will also contribute to the dipole moment. The overall dipole moment will point downwards due to the presence of the lone pair and the three fluorine atoms. 3. **Conclusion**: The dipole moment for NF3 is **not zero**. ### Step 3: Analyze ClO2- 1. **Structure**: Chlorine (Cl) is bonded to two oxygen (O) atoms and has a negative charge. The molecule has a bent shape due to lone pairs on chlorine. 2. **Dipole Moment**: The dipole moments from the Cl-O bonds will not cancel out due to the bent shape. The electronegativity of oxygen is higher than that of chlorine, creating a net dipole moment. 3. **Conclusion**: The dipole moment for ClO2- is **not zero**. ### Step 4: Analyze CH2Cl2 1. **Structure**: The molecule has a tetrahedral geometry with two hydrogen (H) atoms and two chlorine (Cl) atoms. 2. **Dipole Moment**: The dipole moments from the C-Cl bonds will not cancel out due to the asymmetrical arrangement of the chlorine and hydrogen atoms. The electronegativity difference between C and Cl creates a net dipole moment. 3. **Conclusion**: The dipole moment for CH2Cl2 is **not zero**. ### Final Conclusion Among the options provided: - **Trans-N2F2** has a dipole moment of **zero**. - **NF3**, **ClO2-**, and **CH2Cl2** all have non-zero dipole moments. Thus, the molecule that does not have a dipole moment is **Trans-N2F2**. ---
To determine which of the given molecules does not have a dipole moment, we will analyze each option step by step. ### Step 1: Analyze Trans-N2F2 1. **Structure**: The molecule has a trans configuration with nitrogen (N) atoms double bonded to each other and each nitrogen bonded to a fluorine (F) atom. 2. **Dipole Moment**: The dipole moments from the N-F bonds will point towards the fluorine atoms. However, because the molecule is symmetric (trans), the dipole moments will cancel each other out. 3. **Conclusion**: The dipole moment for trans-N2F2 is **zero**. ### Step 2: Analyze NF3 ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • QUALITATIVE ANALYSIS PART 1

    RESONANCE ENGLISH|Exercise A.L.P|39 Videos

  • SOLID STATE

    RESONANCE ENGLISH|Exercise PHYSICAL CHEMITRY (SOLID STATE)|45 Videos

Similar Questions

Explore conceptually related problems

The measure of net molecular polarity is a quantity called dipole moment which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance 'r' between the charge : mu=Qxxr Molecular polarities give rise to some of the forces that occur between molecules.Such forces are termed as intermolecular forces.These molecular forces are of several different types including dipole-dipole forces, London dispersion forces, hydrogen bonds and ion-dipole forces (operate between ions and molecules).These intermolecular forces are electrical in origin and results from the mutual attraction of unlike charges or the mutual repulsion of like charges. A formal positive charge on the central atom affect the size of orbitals.A formal positive charge on central atom will pull in all electrons towards the nucleus and this will leads to the contraction in size of orbitals. Select the correct statement.

Between ionic and covalent bonds, there are large majority of bonds, in which the bonding electrons are shared unequally between two atoms but are not completely transferred.Such bonds are said to be polar covalent bonds and the bond polarity is due to difference in electronegativity, the ability of an atom in a molecule to attract the shared electrons in a covalent bond. The measure of net polarity is a quantity called the dipole moment, mu , which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges : mu=Qxxr .Molecular polarities give rise to some of the forces that occur between molecules and these forces are of several different types including dipole-dipole forces, London dispersion forces, and hydrogen bonds. All these intermolecular forces are electrical in origin and result from the mutual attraction of unlike charges or the mutual repulsion of like charges. Which of the following statements is incorrect ?

Knowledge Check

  • The molecule which does not exhibit net dipole moment is

    A
    `NH_3`
    B
    `CHCl_3`
    C
    `H_2 O`
    D
    `C Cl_4`

    • Similar Questions

    Explore conceptually related problems

    Between ionic and covalent bonds, there are large majority of bonds, in which the bonding electrons are shared unequally between two atoms but are not completely transferred.Such bonds are said to be polar covalent bonds and the bond polarity is due to difference in electronegativity, the ability of an atom in a molecule to attract the shared electrons in a covalent bond. The measure of net polarity is a quantity called the dipole moment, mu , which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges : mu=Qxxr .Molecular polarities give rise to some of the forces that occur between molecules and these forces are of several different types including dipole-dipole forces, London dispersion forces, and hydrogen bonds. All these intermolecular forces are electrical in origin and result from the mutual attraction of unlike charges or the mutual repulsion of like charges. Which of the following statement is true ?

    All molecules with polar bonds have dipole moment.

    All molecules with polar bonds have dipole moment.

    Which of the following molecules will have polar bonds but zero dipole moment?

    Which of the following molecules will have polar bonds but zero dipole moment ?

    What is the difference between London dispersion forces and dipole-dipole forces ?

    Point out the difference between London dispersion forces and dipole-dipole forces.

    Home
    Profile