Which of the following is a non-polar solvent | vedclass

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(B) molecule is non-polar if its net dipole moment is zero. Carbon tetrachloride $(CCl_4)$ has a tetrahedral geometry where the four $C-Cl$ bond dipol

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Carbon tetrachloride

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(B) molecule is non-polar if its net dipole moment is zero. Carbon tetrachloride $(CCl_4)$ has a tetrahedral geometry where the four $C-Cl$ bond dipoles cancel each other out due to symmetry,resulting in a net dipole moment of $0$. Therefore,$CCl_4$ is a non-polar solvent. In contrast,$Dimethyl 	ext{ } sulphoxide$,$Ammonia$,and $Ethyl 	ext{ } alcohol$ are all polar molecules due to the presence of lone pairs or electronegativity differences that do not cancel out.

Which of the following is a non-polar solvent?

Similar Questions

The correct set of species with zero dipole moment is:
$(i) \, CO_2, \, (ii) \, COCl_2, \, (iii) \, CH_2Cl_2, \, (iv) \, BCl_3$

Which of the following bonds is the most polar?

For which molecules among the following,the resultant dipole moment $(\mu) \neq 0?$

Which set contains molecules with $\mu = 0$?

What is the unit of dipole moment? Also,write the formula for dipole moment.

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