[tex]\boxed{\left( 2 \right){\text{ CC}}{{\text{l}}_4}}[/tex] represents a nonpolar molecule containing polar covalent bonds.
Further Explanation:
The chemical bond is the attraction between atoms, molecules or ions that is responsible for the formation of chemical compounds. It is formed either due to electrostatic forces or by the sharing of electrons.
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A covalent bond is a bond formed by the mutual sharing of electrons between the bonded atoms. It is also known as a molecular bond. Such bonds usually exist between two or more non-metals.
Types of covalent bonds:
1. Polar covalent bond
This bond results from the presence of electronegativity difference between the bonded atoms. For example, the bond between hydrogen and chlorine in HCl is a polar covalent bond. In this molecule, Cl is more electronegative than H.
2. Non-polar covalent bond
When there is no or very small electronegativity difference between the bonded atoms, non-polar covalent bond is formed. Here, the net dipole moment of the molecule comes out to be zero. For example, bond between carbon and hydrogen in [tex]{\text{C}}{{\text{H}}_{\text{4}}}[/tex] is a non-polar covalent bond.
3. Coordinate covalent bond
When both the shared electrons are provided by the same atom, coordinate covalent bond is formed. This usually exists when metals are bonded with ligands. For example, the bond formed between cobalt and ammonia in case of hexamminecobalt (III) chloride is a coordinate covalent bond.
(1) [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex]
Oxygen is more electronegative than carbon so the bond between O and H is polar covalent bond. But this molecule has some net dipole moment due to its asymmetry so water molecule is a polar molecule. Therefore this option is incorrect. (For structure, refer to the attached image).
(2) [tex]{\text{CC}}{{\text{l}}_{\text{4}}}[/tex]
Chlorine is more electronegative than carbon so the bond between C and Cl is a polar bond. But the net dipole moment of this molecule comes out to be zero. So [tex]{\text{CC}}{{\text{l}}_{\text{4}}}[/tex] is a nonpolar molecule with polar covalent bonds and therefore this option is correct. (For structure, refer to the attached image).
(3) [tex]{\text{N}}{{\text{H}}_{\text{3}}}[/tex]
Nitrogen is more electronegative than hydrogen so the bond between N and H is polar covalent bond. But this molecule has some net dipole moment due to its asymmetry so ammonia molecule is a polar molecule. Therefore this option is incorrect. (For structure, refer to the attached image).
(4) [tex]{\text{N}}{{\text{H}}_{\text{3}}}[/tex]
It contains two hydrogen atoms in it. There is no electronegativity difference between both atoms and therefore this molecule is nonpolar in nature. Moreover the bond between two hydrogen atoms is also non-polar. Therefore this option is incorrect. (For structure, refer to the attached image).
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Answer details:
Grade: High School
Subject: Chemistry
Chapter: Ionic and covalent compounds
Keywords: polar, nonpolar, correct, incorrect, H2, CCl4, H2O, NH3, electronegativity difference, hydrogen atoms, asymmetry, dipole moment.
