Difluoromethane (CH2F2) is a colorless gas in ~ room temperature and atmospheric pressure. The is thermally stable and it has application in endothermic processes such together air conditioners, refrigerators, and fire extinguishers. However, difluoromethane can cause injury to the skin on contact (Frostbite) owing to its low boiling point (-52 °C) and also melting allude (-136 °C).

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So, is CH2F2 polar or nonpolar? Yes, difluoromethane (CH2F2) is polar regardless of its symmetrical form i.e., tetrahedral geometry. The polarity arises fan to the large difference in electronegativity that the C-F bond. The C-F link is polar in nature and hence, outcomes in the formation of the solid dipole. Therefore, the molecule will have a network dipole moment with a an unfavorable pole top top the fluorine atom. It leader to the polar nature of the CH2F2 molecule.

Let us discuss the polar nature that the CH2F2 molecule in detail.

First that all, we require to know the meaning of polar and also nonpolar molecules. Then, us will relocate towards determinants on i beg your pardon the polarity of the molecule depends. Afterward, us will study that just how CH2F2 is a polar molecule.

Let us start with the basics of chemical bonding i.e., Ionic and Covalent.

Ionic Bond and Covalent Bond

Generally, elements do not exist in your atomic kind except noble gases. Hence, the attraction in between two comparable or different atoms leads to the formation of the chemistry bond.

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The chemical bond is formed in between two atoms either by share electron pair (s) or delivering the electron(s) indigenous one atom to another atom. The electrons, i beg your pardon are supplied for the development of chemical bonds, room valence electrons.

The valence electron are current in the outermost shell or valence shell of an atom. The chemical bond in the molecule is classified together Ionic and Covalent Bond.

Ionic Bond: Ionic link is developed when one atom move its electron to another atom, which subsequently generates cation and also anion, respectively. Move of electron takes ar when there is a very big difference in electronegativity of two atoms and hence, they cannot share the electron pair.

In an ionic bond, two atoms are organized together by the electrostatic pressure of attraction.

Covalent Bond: A covalent shortcut is developed when two atoms re-superstructure the electron pair (s). The share of one, two, and three electron pairs in between two atoms an outcome in the development of single, double, and also triple bonds, respectively.

The covalent bond can be a polar or nonpolar covalent bond depending upon the distinction in electronegativity of 2 atoms.

Polar Covalent Bond: A polar covalent bond is created when over there is unequal sharing of electron pairs between two atoms owing to the difference in your electronegativity values. The electronegativity distinction should be higher than 0.4 together per the Pauling scale.Nonpolar Covalent Bond: The nonpolar covalent bond is developed when there is equal sharing the electron pair fan to the exact same electronegativity of 2 atoms or very small difference in their electronegativity, i beg your pardon are affiliated in the formation of the chemical bond.

The polar covalent binding may bring about the formation of the polar molecule or nonpolar molecule depending on other factors, i beg your pardon we will certainly study later on in this article.

Now, what are polar or nonpolar molecules?

Polar and Nonpolar Molecules

In Polar Molecules, over there is one appreciable distinction in the electronegativity worths of atoms. A polar molecule will have a net dipole moment.

In nonpolar molecules, there might be or might not it is in a significant difference in the electronegativity values of atoms. But the net dipole minute of the nonpolar molecule will be definitely zero.

Polar molecule dissolve in the polar solvent vice versa, nonpolar molecule dissolve in a nonpolar solvent.

As we said, the polar covalent link may an outcome in polar as well as nonpolar molecules. Then, exactly how will us decide even if it is the molecule is polar or nonpolar?

For that, we have actually to talk about other factors, which reason polarity in the molecule.

Factors influence Polarity in the Molecule

The polarity of the molecules counts upon 3 factors.

The shape of the molecule The net dipole moment in the molecule The circulation of charge approximately the central atom

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We will talk about these factors worrying the difluoromethane, CH2F2 molecule.

The carbon atom is the main atom in the CH2F2 molecule and also other atoms i.e., Hydrogen and also fluorine atoms, will surround it.

For this, you must refer to the article on the CH2F2 lewis structure.

The an initial step would certainly be to inspect whether the C-H and C-F bonds space polar covalent bond or nonpolar covalent bonds.

Hence, we must see the electronegativity difference between these bonds.

According come the Pauling Scale,

Electronegativity that the Carbon atom = 2.55

Electronegativity that the hydrogen atom = 2.20

Electronegativity the the fluorine atom = 3.98

Electronegativity difference of the C-H shortcut in the CH2F2 molecule = 2.55 – 2.20 = 0.35

Electronegativity distinction of the C-F link in the CH2F2 molecule = 3.98 – 2.55 = 1.40

For a covalent bond to be a polar covalent bond, the electronegativity difference should it is in at the very least 0.4. Hence, the C-H bond and the C-F link in the CH2F2 molecule are nonpolar (or we deserve to say contempt polar) and also polar covalent bonds, respectively.

The polar C-F link acts together a dipole v a partial optimistic charge and also a partial an adverse charge on the carbon atom and the fluorine atom in the CH2F2 molecule, respectively. Hence, the C-F link will have a dipole moment.

The dipole minute is characterized as

Dipole minute = fee on atoms * Distance between atoms

It is a vector quantity, which means dipole will have actually direction from optimistic pole to negative pole of it. The dipole moment of the C-F bond is 1.51 Debye (D) pointing in the direction of the fluorine atom.

The dipole moment measures the polarity of the covalent bond. The larger the dipole moment of the covalent bond, it will certainly be an ext polar bond.

According come the Valence shell electron pair repulsion concept (VSEPR) and Valence bond theory (VBT), the CH2F2 molecule well matches with the AX4 geometry, and hence, the geometry the CH2F2i s tetrahedral, which is a symmetry shape.

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The symmetry shape way that if there would be every C-H binding or C-F binding in a molecule, the net dipole moment will it is in zero as the dipole will certainly cancel the effect of each other.

The weak dipole the the C-H bond cannot cancel the result of the strong dipole the the C-F bond. Hence, the difluoromethane molecule will have actually a network dipole moment in spite of its symmetrical tetrahedral geometry.

The network dipole minute of the difluoromethane molecule can be calculate by the vector enhancement of dipole moment of two polar covalent binding i.e., the C-F bonds.

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The net dipole moment of the difluoromethane molecule is 1.97 D and hence, confirming the polar nature the the difluoromethane molecule. The direction the the net dipole minute in the difluoromethane molecule will be indigenous the carbon atom to an are between 2 C-F bonds, as it has actually been approximated from the vector enhancement of 2 C-F bonds.

All the above-mentioned factors indicate that difluoromethane is a polar molecule. Hence, there will certainly be dipole-dipole intermolecular forces in between difluoromethane molecules.

Conclusion

The difluoromethane is a colorless gas and vital haloalkane v applications in refrigerators, air conditioners, and also fire extinguishers.

Here, we have studied the polar nature that the difluoromethane molecule.

In brief, the difluoromethane molecule has actually symmetrical geometry i.e., tetrahedral geometry, which indicates the symmetric fee distribution around the main atom, the carbon atom. The electronegativity distinction of the C-F bond is really large, representing the polar nature that the C-F bond. Hence, the C-F bond will be a dipole through the optimistic pole top top the carbon atom and the an adverse pole ~ above the fluorine atom.

There room two C-F bonds and also hence, the network dipole moment have the right to be approximated by the vector enhancement of two C-F bonds, which comes out to it is in 1.97 D.

The net dipole moment and also the large electronegativity difference of the C-F bond in the molecule indicate the polar nature of the difluoromethane molecule.

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I hope you have taken the principle of polarity in the difluoromethane molecule. If you have still any type of doubt, feel free to ask.