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In phosphorus pentachloride (PCl₅), the five P–Cl bonds are not equivalent due to the molecule's trigonal bipyramidal geometry. The three equatorial bonds are arranged in a plane at 120-degree angles to each other, while the two axial bonds are oriented perpendicular to this plane at 180 degrees. This difference in spatial arrangement leads to variations in bond lengths and angles, resulting in the bonds having slightly different characteristics. Consequently, the five P–Cl bonds exhibit different environments, making them non-equivalent.
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How many bonds in PCl5 are equivalent?
In phosphorus pentachloride (PCl5), there are five equivalent P-Cl bonds. This equivalence arises because the molecule has a trigonal bipyramidal geometry, where all P-Cl bonds experience the same environment due to the symmetrical arrangement of the chlorine atoms around the phosphorus atom. Thus, the bond lengths and strengths are uniform across all five bonds.
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How many bonds in PCl5 are equivalent?
In phosphorus pentachloride (PCl5), there are five equivalent P-Cl bonds. This equivalence arises because the molecule has a trigonal bipyramidal geometry, where all P-Cl bonds experience the same environment due to the symmetrical arrangement of the chlorine atoms around the phosphorus atom. Thus, the bond lengths and strengths are uniform across all five bonds.
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