Which of the following statements concerning polar molecules is false? Group of answer choices There must be an odd number of polar bonds so that their polarities not cancel. A molecule with symmetrically arranged polar bonds can be polar if the central atom is bonded to atoms of different elements. There must be at least one polar bond or one unshared pair of electrons on the central atom. If there are more than one polar bond, they must not be symmetrically arranged so that their polarities cancel. If there are more than one unshared pair of electrons on the central atom, they must not be symmetrically arranged so that their polarities cancel.

The polarity of a molecule depends not only on the presence of polar bonds but on the orientation of the polar bonds. However, the polarity of a molecule does not depend on the presence of odd or even polar bonds but on the spatial arrangement of these polar bonds which eventually decide the dipole moment and polarity of a molecule.

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luisvaschetto luisvaschetto · Answer 2 · 2021-11-18T18:36:30+01:00

The statement 'there must be an odd number of polar bonds so that their polarities not cancel' regarding polar molecules is FALSE.

A polar bond is a type of chemical bond between two or more atoms that occurs when pairs of electrons are not shared symmetrically.

A polar molecule contains polar bonds in an unsymmetrical arrangement, thereby the polarity of a molecule depends on how polar bonds are geometrically arranged.

If polar bonds of a given molecule are geometrically (symmetrically) arranged, then bond dipoles can cancel partial charges and therefore they do not generate a molecular dipole.

In conclusion, the statement 'there must be an odd number of polar bonds so that their polarities not cancel' regarding polar molecules is FALSE.

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