Polarity of PCl3: PCl3 (phosphorus trichloride) is a polar molecule.
Molecular Geometry: PCl3 has a trigonal pyramidal geometry. The central phosphorus atom is bonded to three chlorine atoms and has one lone pair of electrons. This lone pair significantly influences the molecular shape and, consequently, its polarity. https://www.wikiwhat.page/kavramlar/Molecular%20Geometry
Bond Polarity: The P-Cl bond is polar because chlorine is more electronegative than phosphorus. This means that chlorine pulls the electron density towards itself, creating a dipole moment in each P-Cl bond. https://www.wikiwhat.page/kavramlar/Bond%20Polarity
Net Dipole Moment: Due to the trigonal pyramidal geometry, the bond dipoles do not cancel each other out. Instead, they add up to create a net dipole moment for the molecule, making PCl3 polar overall. The lone pair of electrons on the phosphorus atom contributes to the overall dipole moment. https://www.wikiwhat.page/kavramlar/Net%20Dipole%20Moment
Asymmetry: The asymmetry of the molecule, caused by the lone pair, is a key factor in determining its polarity. Symmetrical molecules with polar bonds can be nonpolar if the bond dipoles cancel out (e.g., CO2), but PCl3 lacks this symmetry. https://www.wikiwhat.page/kavramlar/Asymmetry
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