Polarity

Question 1

Polarity Of Bonds:

Answer 1

Purely Covalent - forms between two identical atoms; electrons are shared equally.
Polar Covalent - two different atoms; the electrons are not shared equally; the electron pair spends more time near the nucleus of the more electronegative atom
Ionic- Atoms which vary greatly in terms of electronegativity, the electrons are completely transferred to the more electronegative atom (Non-metal).

Question 2

Bond Dipole:

Answer 2

Polar Covalent Bonds - between atoms of differing electronegativity have a bond dipole(Electric Dipole).
A bond Dipole means the more electronegative atom has a small negative charge, and the less electronegative atom has a small positive charge.
Net Dipole: The overall movement of electrons.

Question 3

Shape and Polarities of Molecules:

Answer 3

The Polarity of a molecule is predicted by drawing its molecular shape and indicating all of its bond dipole.
Polar Molecules have an uneven charge distribution(overall net dipole).
Non-Polar Molecules have an even distribution of charge throughout (net dipole of zero).
Non-symmetrical molecules with polar bonds will have a net molecular dipole.
In symmetrical molecules the net dipole is zero.

Question 4

Polar Bond and Polar Molecule:

Answer 4

A polar bond is between two different atoms where the electrons are not shared equally and the electron pair spends more time near the nucleus of the more electronegative atom.

A polar Molecule has an overall uneven charge distribution or a net dipole, due to unsymmetrical bond dipoles.