Why does PH3 have a lower boiling point than AsH3?
I am doing my Chemistry homework, and the question asks rank NH3, PH3 and AsH3 in the order of ascending boiling points. It is PH3
How does NH3 have a lower boiling point than PH3?
Because in NH3 due to high electro negativity and small size of nitrogen the NH bond is highly polar and leads to intermolecular H-bonding between NH3 molecules due to molecules are strongly associated and hence more energy needed for separating molecules.hence high temperature needed. So it has high m.pt.and b.pt.Whereas in PH3 P has low electro negativity and bigger in size and the polarity of PH is not much to form H - Bandelettes lårbånd intermolecular H bonding possible in PH3. So it has low m.pt.and b.pt.
Why does NH3 have a boiling point of -33 C while PH3 has a boiling point of -87 C?
Because the major contribution to the boiling point here is not so the molecular mass of the molecule you are thinking, but the relationship between the molecular mass and the interactions amongst molecules. In fact, despite the fact NH3 have a smaller mass than PH3 (phosphine) it has a stronger interaction, namely, hydrogen bonds (or hydrogen "bridges"), that are formed in the sequence of N ... H - N where the dots represents the hydrogen bond and the trace represents the covalent bond. That type of interaction does not occur in elements other than F, O and N when hydrogen is present. And this type of interaction is many times stronger than the equivalent ones in other situations where these elements does not occur.
Why does NH3 have more of a boiling point than PH3?
N and P both are Group 15 elements! NH3 have B.P = - 33°c which is greater than of PH3 i.e B. P = -83°C!Explanation : We know that in Periodic Table from going up to down electronegativity decreases! This is due to increase in the size of atomic radius.NH3 molecules makes strong intermolecular H bonding b/w themselves. But due to lesser electronegativity of larger PH3 molecules, they cannot form Hydrogen Bonding b/w themselves! Instead of this there is Weak London dispersion force b/w them.So due to greater attraction in NH3 molecules, they are tightly held. So the Boiling point of NH3 is greater than PH3.
Highest Boiling Point? NH3, PH3, AsH3?
NH3 Ammonia molecules can form hydrogen bonds between them, so more energy has to be supplied to the system to break the forces so molecules can enter the gas state. More energy means higher boiling point......
Why does NH3 have a higher boiling point than SbH3, AsH3, and PH3?
I know that a larger dipole-dipole and/or London force makes the boiling point greater. I also know the strength of a dipole-dipole force is based on the electronegativity difference. So the difference for Nitrogen is a lot greater than that of the next 3 in the group when finding the difference for Hydrogen. But why is it that Nitrogen is so much higher than the next 3 in the group/group 15?