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What type of intermolecular forces does HBr have?
Dipole
What type of intermolecular forces would you expect to find in a liquid sample of HBr?
Dipole-dipole.
What intermolecular forces are displayed by HBr?
HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
Is HBr an ion ion intermolecular force?
an ion
Why does hydrogen iodide have a higher boiling temperature than hydrogen bromide?
There is no hydrogen bonding in HBr and HI. The intermolecular forces are London dispersion forces- HI has more electrons, so more instantaneous induced dipole-dipole interaction- more intermolecular force- and therefore a higher boiling point.
What type of intermolecular forces does HBr have?
Dipole
What type of intermolecular forces would you expect to find in a liquid sample of HBr?
Dipole-dipole.
Does HBr have London dispersion forces as its only intermolecular force?
No, since its a polar compound its also considered to be polar. Therefore, it has dipole-dipole forces
What intermolecular forces are displayed by HBr?
HBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules. The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
Is HBr an ion ion intermolecular force?
an ion
Why does hydrogen iodide have a higher boiling temperature than hydrogen bromide?
There is no hydrogen bonding in HBr and HI. The intermolecular forces are London dispersion forces- HI has more electrons, so more instantaneous induced dipole-dipole interaction- more intermolecular force- and therefore a higher boiling point.
What is the intermolecular forces of CH3F?
These are polar forces, intermolecular forces of attraction between molecules.
What is the intermolecular force of Ch2Br2?
Dipole forces and London forces are present as intermolecular forces in these molecules.
Why is the boiling point of HI higher than HBr?
This is to do with the intermolecular forces in the two compounds. There are no hydrogen bonds between the molecules of either compound, since Br and I are not electronegative enough to polarise the molecules sufficiently. But since HI molecules contain more electrons than HBr, there are increased van der Waals forces in HI. For the same reason HBr has a higher boiling point than HCl, but HF has a higher boiling point than HCl, HBr or HI because of hydrogen bonding.
Which forces internal or intermolecular must be broken for methyl alcohol to evaporate?
These are intermolecular forces.
What interaction is not a type of intermolecular force?
Intramolecular forces are not intermolecular forces !
What can you say about the relative strength of the intermolecular forces in the two compounds?
The intermolecular forces in acetone are weaker.
