Predicting Acidity of PH3: Comparison to NH3 Dipole Moments

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SUMMARY

The discussion focuses on the acidity of phosphine (PH3) in comparison to ammonia (NH3), highlighting their respective dipole moments of 0.58D and 1.47D. It concludes that while NH3 is a basic molecule due to its higher dipole moment, PH3 is considered basic on its own, but can be viewed as relatively acidic when compared to NH3. The relationship between dipole moment and acidity is emphasized, with a suggestion to explore how electronegativity (EN) of the central atom influences bond strength.

PREREQUISITES
  • Understanding of molecular polarity and dipole moments
  • Basic knowledge of acid-base chemistry
  • Familiarity with electronegativity concepts
  • Knowledge of bond strength and its relation to molecular structure
NEXT STEPS
  • Research the relationship between dipole moments and acidity in organic compounds
  • Learn about the electronegativity of elements and its impact on molecular properties
  • Explore the concept of bond strength and its correlation with molecular polarity
  • Investigate the hydrolysis of aluminum phosphide and its implications in chemistry
USEFUL FOR

Chemistry students, educators, and researchers interested in molecular polarity, acid-base behavior, and the properties of phosphine and ammonia.

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Homework Statement


Aluminum phosphide is hydrolysed by water to generate the highly toxic gas phosphine. NH3 is a polar molecule with a dipole moment of 1.47D while PH3 has a dipole moment of 0.58D. Predict whether PH3 is acidic neutral or basic.

Homework Equations

The Attempt at a Solution


If NH3 has a higher dipole moment than PH3 and is basic does it mean PH3 is acidic? How does polarity affect the acidity of a molecule?
 
PH₃ on its own is basic, i hope you Know that..So i don't understand how you could say it's acidic. It definitely not. But relative to NH₃, you could say its acidic, though its not.
other than that, could you relate dipole moment( the EN of the central atom) with the bond strength?
 

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