Respuesta :
[tex]{\mathbf{BeC}}{{\mathbf{l}}_{\mathbf{2}}}[/tex] molecule is [tex]\boxed{{\text{non polar}}}[/tex] in nature but the bonds present in [tex]{\mathbf{BeC}}{{\mathbf{l}}_{\mathbf{2}}}[/tex] is [tex]\boxed{{\text{polar}}}[/tex].
[tex]{{\mathbf{O}}_{\mathbf{3}}[/tex] molecule is [tex]\boxed{{\text{polar}}}[/tex] in nature and the bonds present in [tex]{{\mathbf{O}}_{\mathbf{3}}}[/tex] are also [tex]\boxed{{\text{polar}}}[/tex].
Further Explanation:
The polarity of the overall molecule is determined by the net dipole moment and the bond polarity can be determined by the electronegativity difference [tex]\left( {\Delta {\text{EN}}} \right)[/tex].
The dipole moment is a vector quantity that predicts the polarity of the overall molecule. It is produced due to the separation of charges of two atoms and ions. The magnitude of dipole moment is the product of the charges and the distance between the separation of charges and the direction of the dipole moment vector is from electropositive atom to the more electronegative atom.
Net dipole moment is the sum of the total individual dipole moment present in the molecule.
The value of net dipole moment is zero in polar molecules and the value of net dipole moment is non zero in nonpolar molecules.The polarity of a bond can be predicted by [tex]{\mathbf{\Delta EN}}[/tex].
[tex]\Delta {\text{EN}}[/tex] is the electronegativity difference between the two atoms that are bonded to each other. The formula to calculate [tex]\Delta {\text{EN}}[/tex] in XY bond is as follows:
[tex]\Delta {\text{EN}} = \left( {{\text{electronegativity of Y}}} \right) - \left( {{\text{electronegativity of X}}} \right)[/tex]
Here, X is the electropositive atom and Y is the electronegative atom.
If there is electronegativity difference between the atoms then the bond is polar and if there is no electronegativity difference between the atoms then the bond is nonpolar.
The shape of [tex]{\text{BeC}}{{\text{l}}_{\text{2}}}[/tex] is linear. The individual dipole moment in [tex]{\text{BeC}}{{\text{l}}_{\text{2}}}[/tex] cancel each other so the value of net dipole moment is zero and therefore [tex]{\text{BeC}}{{\text{l}}_{\text{2}}}[/tex] is nonpolar in nature.
Chlorine is more electronegative than beryllium so [tex]{\left( {\Delta {\text{EN}}} \right)_{{\text{Be}} - {\text{Cl}}}}[/tex] is non zero and therefore the bonds present in [tex]{\text{BeC}}{{\text{l}}_{\text{2}}}[/tex] are polar.
In ozone [tex]\left( {{{\text{O}}_3}} \right)[/tex], the central oxygen atom has to share the electrons with both of the side oxygen atoms while the side oxygen atoms have to share electrons with only the middle oxygen atom. Therefore the distribution of electrons in [tex]{{\text{O}}_3}[/tex] is uneven so the individual dipole moment will not cancel each other. Hence, [tex]{{\text{O}}_3}[/tex] is polar in nature.
The [tex]s{p^2}[/tex] hybridized oxygen atom is more electronegative as compared to [tex]s{p^3}[/tex] hybridized oxygen atom and therefore the bonds present in [tex]{{\text{O}}_3}[/tex] are polar.
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Covalent bonding and molecular structure
Keywords: Dipole moment, electronegativity difference, polarity, bond polarity, polar, nonpolar, BeCl2 and O3.
The [tex]\rm BeCl_3[/tex] molecule is polar, and the [tex]\rm O_3[/tex] molecule is non polar.
The polarity can be defined as the charge leading to the dipole of the molecule. In [tex]\rm BeCl_3[/tex], the Be-Cl bonds are polar, as there is a difference in between the electronegativities of the two atoms.
The outer electrons on Be indicate the linear geometry of the molecule. The bonds are equal with opposite charges thus have zero dipoles.
In [tex]\rm O_3[/tex], the O-O bond and O=O bond are nonpolar due to the same electronegativity of the atom. The molecule is nonpolar due to the 0 overall polarity of oxygen bonds.
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https://brainly.com/question/11405437
