In covalent bonding, the two electrons shared by the atoms are attracted to the nucleus of both atoms. Neither atom completely loses or gains electrons.

POLARITY

 In covalent bonding, the two electrons shared

by the atoms are attracted to the nucleus of both atoms. Neither atom completely loses or gains electrons as in ionic bonding. It occurs between 2 nonmetals.

What is it?

 Non-polar bonding with an equal

sharing of electrons between identical non metals (exception carbon/hydrogen).

There are two types of covalent bonding:

Polar bonding with an unequal sharing of electrons between two different nonmetals. The number of shared electrons depends on the number of electrons needed to complete the octet.

Polarity results from the uneven

partial charge distribution between various atoms in a compound.

What does it mean?

Less electronegative More

electronegative

Water is polar.

Oxygen and hydrogen are bonded together by sharing electrons. The oxygen atom is “stronger” (more electronegative) and pulls the shared electrons closer to itself. This creates a positive and negative side to the molecule.

Water and Polarity

Atoms, such as nitrogen, oxygen, and halogens, that are more electronegative have a tendency to have partial negative

charges.

Halogen is more electronegative than carbon.

Atoms, such as carbon and hydrogen, have a tendency to be more neutral or

have partial positive charges.

Equal pull of electrons by hydrogen and carbon. Charge is equally distributed. No pole is formed.

. A polar molecule results when a molecule contains polar bonds in an unsymmetrical arrangement.

Electrons in a polar covalent bond are unequally shared between the two bonded atoms, which

results in partial positive and negative charges.

The separation of the partial charges creates a dipole.

The word dipole means two poles: the separated partial positive and negative charges.

+ region -region

A polar molecule results when a molecule contains polar bonds in an unsymmetrical

arrangement.

http://education-portal.com/academy/lesson/di

poles-dipole-moments-molecule-polarity.html

Crash course in chemistry polarityhttps://www.youtube.com/watch?v=PVL24HAesnc

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