Polar molecules

Polar molecules

Overview:

• Polar molecules are a type of molecule that exhibits a separation of electric charge, creating a positive and a negative end.
• The polarity of a molecule is influenced by the presence of polar covalent bonds and its overall molecular shape.

Polar Covalent Bonds:

• Polar molecules often contain polar covalent bonds.
• Polar covalent bonds occur when atoms with different electronegativities share electrons unevenly.
• This results in one atom having a partial negative charge (δ⁻) and the other a partial positive charge (δ⁺).

Influence of Molecular Shape:

• Whether a molecule is overall polar or non-polar depends on its molecular shape.
• The shape determines whether the partial charges are distributed symmetrically or asymmetrically within the molecule.

Examples:

Water (H₂O):

• Water is a polar molecule because it contains polar covalent bonds.
• Its bent shape (non-symmetrical) results in an overall polarity.
• The oxygen end is δ⁻, while the hydrogen ends are δ⁺.

Water (H₂O):

• Polar molecules have an uneven distribution of electron density, leading to partial charges within the molecule.
• The overall polarity of a molecule depends on its shape, with non-symmetrical shapes resulting in polarity and symmetrical shapes resulting in non-polarity.
• Understanding polar molecules helps explain various chemical properties and interactions in chemistry.