The most stable hydride isa)NH₃b)PH₃c)AsH₃d)SbH₃Correct answer is option 'A'. Can you explain this answer?

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is the most stable hydride among the hydrides of group 15 elements because the strength of E-H (Here E = N, P, As, Sb, or Br) bond decreases down the group due to increase in size of the central atom

es NH3 is more basic than PH3 as NH3 has more density of electron. Owing it to the small size of nitrogen and small P orbitals it has the ability to form stronger bonds due to effective overlap. In PH3 however, the large size of P results in the P orbitals becoming diffused preventing effective

Answer

The bond length of NH3 is more shorter than other 3 .

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Most stable hydride is NH3
As stability down the group decrease due to decrease in bond dissociation. enthalpy

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NH3​ is the most stable hydride among the hydrides of group 15 elements because the strength of E-H (Here E = N, P, As, Sb, or Br) bond decreases down the group due to increase in size of the central atom. so op A.

Answer

Answer:
Introduction:
In this question, we need to determine the most stable hydride from the given options: NH₃, PH₃, AsH₃, and SbH₃. Stability of hydrides can be explained by considering the size and electronegativity of the central atom, as well as the electron density around it.

Explanation:
To determine the most stable hydride, we need to analyze the properties of each of the given hydrides.

1. NH₃ (Ammonia):
- Nitrogen (N) is a small atom, and it is highly electronegative.
- Ammonia has a pyramidal structure with a lone pair of electrons on nitrogen.
- The presence of a lone pair of electrons makes the molecule polar.
- The lone pair of electrons also contributes to the hydrogen bonding in ammonia.
- Hydrogen bonding increases the stability of ammonia, making it the most stable hydride among the given options.

2. PH₃ (Phosphine):
- Phosphorus (P) is larger than nitrogen but still electronegative.
- Phosphine has a pyramidal structure similar to ammonia.
- However, the lone pair of electrons on phosphorus is less available for hydrogen bonding compared to ammonia.
- Therefore, phosphine has weaker intermolecular forces and is less stable than ammonia.

3. AsH₃ (Arsine):
- Arsenic (As) is larger than phosphorus but less electronegative.
- Arsenine also has a pyramidal structure similar to ammonia and phosphine.
- The larger size of arsenic leads to weaker intermolecular forces.
- Additionally, the lower electronegativity of arsenic further weakens the hydrogen bonding.
- As a result, arsine is less stable than both ammonia and phosphine.

4. SbH₃ (Stibine):
- Antimony (Sb) is larger and less electronegative than arsenic.
- Stibine also has a pyramidal structure similar to the other hydrides.
- The larger size and lower electronegativity of antimony weaken the intermolecular forces and hydrogen bonding.
- Therefore, stibine is the least stable among the given hydrides.

Conclusion:
Based on the analysis, NH₃ (ammonia) is the most stable hydride among the given options. Its smaller size, higher electronegativity, and the presence of a lone pair of electrons contribute to stronger intermolecular forces and hydrogen bonding, making it more stable compared to the other hydrides.

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