Choose the polar molecule from the following:
- \(CH_2=CH_2\)
- \(CHCl_3\)
\(CCl_4\)
\(CO_2\)
The Correct Option is B
Solution and Explanation
Among the given options, CHCl3 (chloroform) is polar due to the asymmetrical arrangement of chlorine and hydrogen atoms around the central carbon, resulting in a net dipole moment. In contrast:
- CCl4: Tetrahedral symmetry with four identical C-Cl bonds cancels out the dipole moments, making it non-polar.
- CO2: Linear molecule with symmetrical C=O bonds cancels out dipole moments, making it non-polar.
- CH2=CH2: Ethene has a planar structure with symmetrical bonds, making it non-polar.
Thus, CHCl3 is the only polar molecule.
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Concepts Used:
Polarity of bonds
Polarity, in chemical bonding, distribution of electrical charge over the atoms joined by the bond. Specifically, while bonds between identical atoms, as in H2, are electrically uniform in the sense that both hydrogen atoms are electrically neutral, bonds between atoms of different elements are electrically inequivalent.
Non-polar Covalent Bond:
A non-polar covalent bond is a type of chemical bond that is formed when electrons are shared equally between two atoms. Thus, in an atom, the number of electrons shared by the adjacent atoms will be the same.
The covalent bond is also termed as nonpolar because the difference in electronegativity is mostly negligible.
Polar Covalent Bond:
A polar covalent bond exists when atoms with different electronegativities share electrons in a covalent bond. Consider the hydrogen chloride (HCl) molecule. Each atom in HCl requires one more electron to form an inert gas electron configuration.
Dipole Moment
Dipole moment is defined as the product of the magnitude of charge and the distance of separation between the centres of positive and negative charge.
Dipole moment is a vector quantity and it is denoted by µ.
µ = charge (Q) * Distance of separation(r)
The dipole moment is expressed in Debye units (D).