dipole moments
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Re: dipole moments
Yes. The larger the difference in electronegativity, the larger the dipole moment.
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Re: dipole moments
Larger differences in electronegativity lead to larger dipole moments (the electrons are pulled towards the atom with higher electronegativity).
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Re: dipole moments
Yes, larger differences in electronegativity cause polar covalent bonding. However, certain molecular shapes, such as tetrahedral, tend to not have a dipole moment because the dipole moment is actually a vector sum between all polar bonds in the molecule.
Re: dipole moments
Yes a greater difference in electronegativity typically results in a greater bond dipole moment.
Re: dipole moments
Yes, the larger the difference in electronegativity the stronger the dipole moments of the molecule are.
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Re: dipole moments
Yes, electronegativity is how much an atom can attract electrons. A dipole moment is when one atom is strongly attracting the electrons more than the other. Thus, the dipole moment is centered from electronegativity.
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Re: dipole moments
If you visualize the electron cloud surrounding a molecule, it would make sense that the more electronegative atom(s) would pull the shared electrons closer to itself, forming a negative dipole moment on that region of the molecule and a positive dipole moment on the opposite end.
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