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Sagot :
NH3, PH3, and AsH3 are all covalent compounds. SbH3 is a metallic compound.
The boiling point of a substance is a measure of the strength of the forces that hold the molecules together in the liquid state. In general, the stronger the forces between the molecules, the higher the boiling point will be.
The boiling points of NH3, PH3, AsH3 and SbH3 show a significant variation, which can be explained in terms of the different types of intermolecular forces that are present in these substances.
NH3, PH3, and AsH3 are all covalent compounds, which means that they are composed of molecules that are held together by covalent bonds. These bonds involve the sharing of electrons between the atoms in the molecule, and they are generally quite strong.
However, the strength of the intermolecular forces in these substances can vary depending on the types of atoms that are present and the way that they are bonded together. For example, NH3 has a relatively low boiling point (-33.4 oC) because the N-H bonds in the molecule are fairly weak. This allows the molecules to move more easily and escape from the liquid state at a lower temperature.
On the other hand, PH3 and AsH3 have much higher boiling points (-87.5 oC and -62.4 oC, respectively) because the P-H and As-H bonds are stronger. This makes it more difficult for the molecules to escape from the liquid state, so they need to be heated to higher temperatures in order to boil.
SbH3, on the other hand, has a much lower boiling point (-18.4 oC) because it is a metallic compound. In metallic compounds, the atoms are held together by a network of delocalized electrons, which are not as tightly bound as the electrons in covalent bonds. This means that the intermolecular forces in metallic compounds are generally weaker, which leads to lower boiling points.
Overall, the variation in the boiling points of NH3, PH3, AsH3 and SbH3 can be explained by the different types and strengths of the intermolecular forces that are present in these substances.
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