What is the strongest intermolecular force in BCl3?

London forces
BCl3 is a non-polar molecule; its strongest intermolecular forces are London forces; it has the lowest melting point.

Is there dipole dipole in BCl3?

B-Cl has a dipole due to the difference in the electronegativity of boron and chlorine atom. The overall dipole of a molecule also depends on the geometry. The geometry of BCl3 is planar with a bond angle of 120 degree. The resultant dipole of two B-Cl bonds cancels the third one, resulting in net zero dipole.

What is the strongest type of intermolecular force present in SO2?

SO2 is a polar molecule. Generally dipole-dipole forces are stronger than LDF forces.

Which substance has dipole dipole forces as its strongest intermolecular force?

hydrogen bonding
The strongest intermolecular force is hydrogen bonding, which is a particular subset of dipole-dipole interactions that occur when a hydrogen is in close proximity (bound to) a highly electronegative element (namely oxygen, nitrogen, or fluorine).

Does SO2 have dipole dipole forces?

Yes, sulfur dioxide (SO2) is a polar molecule that feature dipole dipole interactions in its intermolecular forces.

What is the dipole moment of bcl3?

Now BCl3 is a planar molecule in which the three B – Cl bonds are inclined at an angle of 120°. Therefore, the resultant of two B – Cl bonds in cancelled by equal and opposite dipole moment of the bond B – Cl bond as shown. Hence overall dipole moment of BCl3 is zero.

What is the dipole moment of BCl3?

Is SO2 a dipole dipole force?

Is SO2 a dipole?

SO2 (on the right) has an asymmetric charge distribution, resulting in a net dipole moment (yellow arrow) compared to CO2 (on the left). Polarity determines many physical and chemical properties of molecules, and how molecules interact with other molecules.

Which of the following will have the strongest dipole-dipole attractions?

Hydrogen bonds are the strongest dipole-dipole attraction and are therefore considered to be the strongest type of van der Waals force.

Why does SiO2 have a higher melting point than SO2?

Where SiO2 has strong covalent bonds between molecules, SO3 only has weak van der waals intermolecular forces holding its molecules together. Since covalent bonds require more energy to overcome than van der waals, SiO2 requires a higher temperature than SO3 to melt, thus SiO2 has a higher melting point.