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How do you determine whether a molecule is polar? select all that apply. select all that apply. determine whether the polar bonds add together to form a net dipole moment. determine if the bonds are ionic or covalent. draw the lewis structure for the molecule and determine the molecular geometry. determine whether the molecule contains polar bonds?

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Answer:

The two basic steps to determine whether a molecule is polar are:

1)  determine whether the molecule contains polar bonds?

2) determine whether the polar bonds add together to form a net dipole moment.

Explanation:

The fundamental requirement is that there are polar bonds. Polar bonds are covalent bods with dipole moments. Dipole moments are the result of two atoms of different electronegativity sharing electrons. The more electroneative atom pulls the electrons with more strength than the other atom which is what generate the dipole moment.

If the molecule is symmetrical, and the dipole moments are place symmetrically they wil cancel each other and the molecule will not be polar. For example, the molecule of CCl4 has four C - Cl bonds each with dipole moment, but they are loacates symmetrically around the C atom, so they will cancel each other resulting in a zero net sum of dipole moments, being the molecule non-polar.

To be polar, a molecule must be asymmetric and the elecronegative difference of constituent atom is high. Explanation:

Polarity in molecules:

  • When atoms of molecules are bonded with ionic bond.
  • When elecronegative difference of constituent atom is high.
  • Symmetry of the molecule.

In symmetrical molecule dipole moment of canceled out. for example Carbon dioxide.

Hence to be polar molecule must be asymmetric and the elecronegative difference of constituent atom is high.

To know more about polar molecules, refer to the link:

https://brainly.com/question/15173422?referrer=searchResults

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