(i) Phosphine (PH3) is a molecule that consists of one phosphorus atom and three hydrogen atoms. The Lewis structure of phosphine is drawn by first writing the symbols for phosphorus (P) and hydrogen (H) with phosphorus in the center. Phosphorus has 5 valence electrons and each hydrogen atom has 1 valence electron. Three of the phosphorus's valence electrons are shared with the three hydrogen atoms, forming three single bonds. The remaining two valence electrons of phosphorus remain as a lone pair. So, the Lewis structure of phosphine is:

H
|
H - P - H
:
:

(ii) The hybridization of the phosphorus atom in phosphine is sp3. This is because phosphorus forms three sigma bonds with the hydrogen atoms and has one lone pair of electrons, making a total of four electron groups. According to VSEPR theory, four electron groups around a central atom lead to sp3 hybridization.

(iii) Phosphine would act as a Lewis base. This is because it has a lone pair of electrons on the phosphorus atom that can be donated to an electron-deficient species (Lewis acid).

(iv) The bonds in phosphine are polar. This is because phosphorus is more electronegative than hydrogen, creating a dipole along each P-H bond. However, due to the symmetry of the molecule, these bond dipoles cancel each other out, making the overall molecule non-polar.

(v) Despite having a greater molar mass, phosphine has a significantly lower boiling point than ammonia because of the difference in their intermolecular forces. Ammonia molecules can form hydrogen bonds, which are much stronger than the van der Waals forces present in phosphine. This means more energy is required to break the intermolecular forces in ammonia, leading to a higher boiling point.

Question

(i) Phosphine (PH3) is a molecule that consists of one phosphorus atom and three hydrogen atoms. The Lewis structure of phosphine is drawn by first writing the symbols for phosphorus (P) and hydrogen (H) with phosphorus in the center. Phosphorus has 5 valence electrons and each hydrogen atom has 1 valence electron. Three of the phosphorus's valence electrons are shared with the three hydrogen atoms, forming three single bonds. The remaining two valence electrons of phosphorus remain as a lone pair. So, the Lewis structure of phosphine is:

H
       |
   H - P - H
       :
       :

(ii) The hybridization of the phosphorus atom in phosphine is sp3. This is because phosphorus forms three sigma bonds with the hydrogen atoms and has one lone pair of electrons, making a total of four electron groups. According to VSEPR theory, four electron groups around a central atom lead to sp3 hybridization.

(iii) Phosphine would act as a Lewis base. This is because it has a lone pair of electrons on the phosphorus atom that can be donated to an electron-deficient species (Lewis acid).

(iv) The bonds in phosphine are polar. This is because phosphorus is more electronegative than hydrogen, creating a dipole along each P-H bond. However, due to the symmetry of the molecule, these bond dipoles cancel each other out, making the overall molecule non-polar.

(v) Despite having a greater molar mass, phosphine has a significantly lower boiling point than ammonia because of the difference in their intermolecular forces. Ammonia molecules can form hydrogen bonds, which are much stronger than the van der Waals forces present in phosphine. This means more energy is required to break the intermolecular forces in ammonia, leading to a higher boiling point.

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(i) Phosphine (PH3) is a molecule that consists of one phosphorus atom and three hydrogen atoms. The Lewis structure of phosphine is drawn by first writing the symbols for phosphorus (P) and hydrogen (H) with phosphorus in the center. Phosphorus has 5 valence electrons and each hydrogen atom has 1 valence electron. Three of the phosphorus's valence electrons are shared with the three hydrogen atoms, forming three single bonds. The remaining two valence electrons of phosphorus remain as a lone pair. So, the Lewis structure of phosphine is:

H
       |
   H - P - H
       :
       :

(ii) The hybridization of the phosphorus atom in phosphine is sp3. This is because phosphorus forms three sigma bonds with the hydrogen atoms and has one lone pair of electrons, making a total of four electron groups. According to VSEPR theory, four electron groups around a central atom lead to sp3 hybridization.

(iii) Phosphine would act as a Lewis base. This is because it has a lone pair of electrons on the phosphorus atom that can be donated to an electron-deficient species (Lewis acid).

(iv) The bonds in phosphine are polar. This is because phosphorus is more electronegative than hydrogen, creating a dipole along each P-H bond. However, due to the symmetry of the molecule, these bond dipoles cancel each other out, making the overall molecule non-polar.

(v) Despite having a greater molar mass, phosphine has a significantly lower boiling point than ammonia because of the difference in their intermolecular forces. Ammonia molecules can form hydrogen bonds, which are much stronger than the van der Waals forces present in phosphine. This means more energy is required to break the intermolecular forces in ammonia, leading to a higher boiling point.

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