Table of Contents
- 1 What is the strongest intermolecular force that HBr has?
- 2 Why does AsH3 have a higher boiling point than PH3?
- 3 Does HBr have stronger dipole-dipole forces than HCl?
- 4 What intermolecular forces does HBr have?
- 5 Why does HBr have higher boiling point?
- 6 Why boiling point of HCl is less than HBr?
- 7 Why does Br2 have a higher boiling point than HBR?
- 8 Why is the London force in AsH3 greater than in PH3?
What is the strongest intermolecular force that HBr has?
dipole-dipole force
The development of charge on hydrogen and bromine atoms makes it a polar molecule which results in dipole-dipole interaction. Therefore, dipole-dipole force is the major type of intermolecular force that occurs between particles of HBr.
Why does AsH3 have a higher boiling point than PH3?
Arsenic, being farther down on the Periodic Table than Phosphorus, has more electrons that may group together and form instantaneous dipoles. We can say that AsH3 has a higher boiling point than PH3 because arsenic has a higher polarizability than phosphorus.
Does HBr have stronger dipole-dipole forces than HCl?
F is small and very electronegative atom. Cl and Br are not as electronegative as F: the dispersion forces in HCl and HBr are more significant than the dipole-dipole forces as can be evidenced by the order of boiling points HF > HBr > HCl.
Why does boiling point increase from HCl to HBr to HI?
Explanation. The boiling point of covalent compounds(HF, HCl, HBr, HI) increases with an increase in their molecular weight due to an increase in Van Der Waal’s forces of attraction among molecules.
What is the boiling point of HBr?
-86.8°F (-66°C)
Hydrogen bromide/Boiling point
What intermolecular forces does HBr have?
HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules.
Why does HBr have higher boiling point?
HBr is a larger, more polarizable molecule than HCl . There should be a greater degree of dispersion forces, forces between molecules, operating in the HBr molecule, and thus the higher boiling point is observed.
Why boiling point of HCl is less than HBr?
Bromine is a larger ion than chlorine and thus has stronger Van der Waals forces. Larger amounts of energy (a higher temperature) are required to break these interactions and so the boiling point of HBr is higher than HCl.
Why is the boiling point of PH3 lower than AsH3?
Explain why the boiling point of PH3 is lower than the boiling point of AsH3 AsH3 is a larger molecule than PH 3 as As is lower down the periodic table, so has a higher atomic number so more electrons. Therefore AsH 3 has more electrons than PH 3 meaning that the instantaneous dipole produced by AsH 3 is greater.
What is the boiling point of NH3 at different temperatures?
Bp of NH3: -33°C, PH3: -87°C, AsH3: -62.4°C, SbH3: -18°C So the increasing order of boiling point is PH3 The regular trend for boiling point is that it increases down the group due to increase in size and van der waal forces between atoms.But the B.p of ammonia (NH3) is more than Ph3 and Ash3
Why does Br2 have a higher boiling point than HBR?
HBr’s weak bonds aren’t enough to offset the loss in entropy. As such Br2 actually has a higher liquid entropy than HBr. A higher gap between the gas and liquid entropy tends to drop the boiling temperature. Edit: So I was actually curious how much energy vs entropy matters for this particular species.
Why is the London force in AsH3 greater than in PH3?
Therefore AsH 3 has more electrons than PH 3 meaning that the instantaneous dipole produced by AsH 3 is greater. Therefore the induced dipoles on neighbouring molecules are greater, so the London forces are stronger than in PH 3.