EXPLAIN HOW POLAR COVALENT BONDS ARE CREATED.

atoms within the bond do not have the same pull on the shared electron, and as a result the electron spends more time around one atom relative to the other atom within the bond.

To understand how polar covalent bonds are created, we need to first understand what a covalent bond is. A covalent bond forms when two or more atoms share electrons in order to achieve a stable electron configuration.

In a covalent bond, the shared electrons are attracted to the positively charged nuclei of both atoms involved. However, in some cases, the atoms within the bond have a different pull or electronegativity for the shared electrons. Electronegativity is a measure of an atom's ability to attract electrons towards itself.

When two atoms with different electronegativities form a covalent bond, the electron pair is not shared equally. The atom with higher electronegativity has a stronger pull on the shared electrons, causing the electrons to spend more time around that atom.

For example, let's consider a covalent bond between hydrogen (H) and oxygen (O) in a water molecule (H2O). Oxygen has a higher electronegativity than hydrogen, so oxygen attracts the shared electrons more strongly. As a result, the electrons spend more time around the oxygen atom, creating a partial negative charge (δ-) on oxygen and a partial positive charge (δ+) on the hydrogen atoms.

This uneven distribution of charges along the bond creates a polarity within the molecule, hence the name "polar covalent bond." In the case of water, the oxygen atom has a slightly negative charge, and the hydrogen atoms have slightly positive charges.

Overall, polar covalent bonds are formed when atoms with different electronegativities share electrons, resulting in an uneven distribution of electron density and creating partial charges within the molecule.