A) CH3CH2CH2CH2Br B) None have dipole-dipole forces C) H2O D) H2 E) All have dipole-dipole forces

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A) CH3CH2CH2CH2Br B) None have dipole-dipole forces C) H2O D) H2 E) All have dipole-dipole forces

Chemistry
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Dipole dipole interactions would be different from say like induced dipole, or instantaneous dipole moment. An instantaneous dipole moment is like at any movement electrons can be more concentrated in one region of the molecule than another, and this virtually happens in all molecules. But this is not dipole dipole interactions so it can't be all of them. I'm guessing for dipole dipole interaction the molecule would need to have some kind of dipole moment
In terms of intermolecular forces, H2O would primarily be hydrogen bonding, But I don't think two molecules of H2 can have a dipole dipole interactions. That long bromo-Alkane I think it would have dipole dipole interactions. I'm going to go with A,
H-Bonding, Dipole-Dipole interaction and London forces, all three are kind of \(\bf Van~der~waal's~interaction\). H-bonds form when a h atom is attached to highly electronegative element like F, O or N. Dipole interaction occurs when there is an electronegativity difference between the central atom and ligand atom eg. C-Cl bond will be polar and there will be dipole dipole interaction. Finally london dispersion forces arrise due to instantaneous polarity created due to directional nature of electron clouds. E.g. atoms of noble gases are held together by london forces in their solid state.

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Also note that strength of these are in order H-Bond > Dipole-Dipole > London forces.
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. @Photon336 I agree it should be A
they are not all Van der Waal's interaction

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