Chemistry Regents Practice Test 2025 – Complete Prep Resource

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What is a polar molecule?

A molecule that has no net dipole moment

A molecule with equal distribution of electrical charge

A molecule that has a net dipole moment due to polar bonds

A polar molecule is characterized by having a net dipole moment as a result of polar bonds within its structure. This occurs when there is an uneven distribution of electron density between atoms, usually due to differences in electronegativity. For instance, in a water molecule (H₂O), the oxygen atom is more electronegative than the hydrogen atoms, causing the electrons to spend more time closer to the oxygen. This results in a partial negative charge on the oxygen and a partial positive charge on the hydrogens, creating a dipole moment.

The presence of polar bonds means that, despite the overall shape of the molecule, the differing charges do not cancel each other out, leading to a molecule that can interact with other polar substances, including water. Hence, the net dipole moment is what defines a molecule as polar.

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A molecule that repels water

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