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Explain the relationship between the polarity of a molecule, its dipole moment, and intermolecular bonding.

Answer and Step-by-step explanation:

First, let's define these terms. Polarity is a phenomenon caused by an unequal distribution of electrons that results in one part of the molecule to be more or less negatively-charged than the other part. Dipole moment is essentially a moment in time when one side of the molecule is positively charged and the other side is negatively charged. And finally, intermolecular bonding refers to the bonds between molecules and how molecules interact with each other.

Now for the relationships. Polarity is usually caused when the electronegativity values of the atoms that make up the molecule are very far apart. Electronegativity is the inclining of a molecule to attract electrons to itself. The more electronegative the molecule, the more polar it is. And, because we're relating to electrons here, higher polarity will also mean bigger dipole moments. In addition, because the molecule is so polar (with one end negative and the other end positive), the attractive forces between the molecules increases and become stronger. This, in turn, means that the intermolecular forces or bonds are stronger.

step-by-step explanation:

we are given

since, we have to isolate x on anyone side

so, we can move all x terms on one side

subtract both sides by 2x

add both sides by 9

divide both sides by 4

we get

answer

false

explanation

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