Answer
See the explanation
Work Step by Step
a. $OCl_{2},KrF_{2},BeH_{2},SO_{2}$
$OCl_{2}$ (Dichlorine Monoxide):
Lewis Structure: O=Cl-Cl
Molecular Structure: Bent (Trigonal Planar)
This molecule is polar due to the unequal sharing of electrons between the oxygen and chlorine atoms, resulting in a dipole moment.
$KrF_{2}$ (Krypton Difluoride):
Lewis Structure: F-Kr-F
Molecular Structure: Linear
This molecule is nonpolar because the two Kr-F bond dipoles cancel each other.
$BeH_{2}$ (Beryllium Hydride):
Lewis Structure: H-Be-H
Molecular Structure: Linear
This molecule is non-polar because the two hydrogen atoms are equally shared with the beryllium atom, resulting in a symmetric distribution of electrons.
$SO_{2}$ (Sulfur Dioxide):
Lewis Structure: O=S=O
Molecular Structure: Bent (Trigonal Planar)
This molecule is polar due to the unequal sharing of electrons between the sulfur and oxygen atoms, resulting in a dipole moment.
b. $SO_{3},NF_{3},IF_{3}$
$SO_{3}$ (Sulfur Trioxide):
Lewis Structure: O=S=O
Molecular Structure: Trigonal Planar
This molecule is nonpolar because bond dipoles cancel
$NF_{3}$ (Nitrogen Trifluoride):
Lewis Structure: F-N-F
Molecular Structure: Trigonal Pyramidal
This molecule is polar due to the unequal sharing of electrons between the nitrogen and fluorine atoms, resulting in a dipole moment.
$IF_{3}$ (Iodine Trifluoride):
Lewis Structure: F-I-F
Molecular Structure: T-shaped
This molecule is polar due to the unequal sharing of electrons between the iodine and fluorine atoms, resulting in a dipole moment.
c. $CF_{4},SeF_{4},KrF_{4}$
$CF_{4}$ (Carbon Tetrafluoride):
Lewis Structure: F-C-F
Molecular Structure: Tetrahedral
This molecule is non-polar because the four fluorine atoms are equally shared with the carbon atom, resulting in a symmetric distribution of electrons.
$SeF_{4}$ (Selenium Tetrafluoride):
Lewis Structure: F-Se-F
Molecular Structure: Square Planar
This molecule is polar due to the unequal sharing of electrons between the selenium and fluorine atoms, resulting in a dipole moment.
$KrF_{4}$ (Krypton Tetrafluoride):
Lewis Structure: F-Kr-F
Molecular Structure: Square Planar
This molecule is polar due to the unequal sharing of electrons between the krypton and fluorine atoms, resulting in a dipole moment.
d. $IF_{5},AsF_{5}$
$IF_{5}$ (Iodine Pentafluoride):
Lewis Structure: F-I-F
Molecular Structure: Trigonal Bipyramidal
This molecule is polar due to the unequal sharing of electrons between the iodine and fluorine atoms, resulting in a dipole moment.
$AsF_{5}$ (Arsenic Pentafluoride):
Lewis Structure: F-As-F
Molecular Structure: Trigonal Bipyramidal
This molecule is nonpolar as bond dipoles cancel.
Polar Compounds:
$OCl_{2}$, $SO_{2}$, $NF_{3}$, $SeF_{4}$,
$IF_{3}$,
$IF_{5}$,
Non-Polar Compounds:
$KrF_{2}$,
$SO_{3}$,
$BeH_{2}$,
$KrF_{4}$,
$CF_{4}$
$AsF_{5}$
