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What is the direction of the dipole moment expected for hydrogen bromide?
Wiki User
∙ 16y ago
The HBr molecule is linear (obviously, since it contains only two atoms). The dipole moment is a vector, parallel to the bond, pointing toward the partially positively charged atom, which is, in this case, the hydrogen. The magnitude of the dipole moment is the difference in the partial electrical charges on each atom times the spatial separation of the atoms in the bond. In a molcule with more than two atoms (more than one bond), the dipole moment of each bond must be added vectorially and the resultant vector will determine the dipole moment of the molecule. For instance, carbon dioxide has two carbon-oxygen double bonds of high polarity, but because the molecule is linear, and the individual dipoles oppose each other, the carbon dioxide molecule has no net dipole moment.
Wiki User
∙ 16y ago
Wiki User
∙ 11y agono, although the c - cl bond is a polar bond due to the difference in pauling's electronegativity values the actual molecule is not a polar molecule due to the symmetry of the chlorine atoms surrounding the central carbon atom. therefor there is no dipole (Difference in charge) present in the molecule. however, there is induced dipole interactions due to the constant movement of electrons around the molecule giving temporary dipole moments which in turn induces neighboring molecules to also exibit these dipole moments. (Van der Walls forces)
Wiki User
∙ 16y agoIt has no net dipole moment, therefore, it is non polar.
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Who has the stronger dipole-dipole hydrogen chloride or hydrogen flouride?
Hydrogen fluoride as it is a hydrogen bond.
Is SO2 dipole in nature?
Yes it is a dipole but i do not know the direction of movement of the dipole.
What are examples of The main interactions between molecules of hydrogen chloride?
dipole-dipole
Is Nitrogen TriFluoride a hydrogen bond?
No, Nitrogen TriFluoride has dipole-dipole forces
What type of bond is hydrogen?
A hydrogen bond is a very strong dipole-dipole bond. A hydrogen bond can only form between hydrogen and a strong electromagnetic atom; fluorine, oxygen or chlorine.
Does Hydrogen Bromide exhibit dipole-dipole interactions?
Yes. Hydrogen bromide shows dipole-dipole interactions.
What is the direction of the dipole moment expected for methanol?
It should be pointed towards the oxygen.
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.
Who has the stronger dipole-dipole hydrogen chloride or hydrogen flouride?
Hydrogen fluoride as it is a hydrogen bond.
Which is stronger dipole-dipole interactions or hydrogen bonds?
hydrogen bonding is stronger.
Is a hydrogen a very strong dipole-dipole force?
The hydrogen bond is not strong.
Is HBr dipole?
There are two different atoms.So it is polar.
Does water have permanent dipole?
Yes, water shows all three types of common intermolecular forces, namely dispersion forces, dipole-dipole forces and hydrogen bonds. Dispersion forces are present at any species which consists of movable charges that can be shifted with respect to one another. Thus a dipole emerges which on his part can induce dipoles in close-by molecules. The permanent dipole of water molecules leads to dipole-dipole forces. They can be distinguished from hydrogen bonds as they are present even at angles where no significant hydrogen bonds are expected any more.
How do hydrogen bonds compare with other intermolecular forces?
Hydrogen bonds are stronger than dipole-dipole and Van der Waals forces.
What is the strongest dipole-dipole force?
a hydrogen bond
What is the direction of the dipole for H-F?
1 D (Debye) ~ 3.34 x 10^-30 C m (Coulomb meters), therefore the dipole moment of HF =1.91 x 3.34 x 10^-30 = 6.38 x 10^-30 C m
What type(s) of intermolecular forces are expected between CH3CH2CONHCH3 molecules?
Amides have some hydrogen bonding, between the lone pair on the nitrogen and the hydrogen on the nitrogen in the next molecule. There will also be van der Waals forces and a little dipole-dipole attraction.
