To be a polar molecule means that the molecule has an uneven distribution of electric charge across its structure, resulting in one side having a partial positive charge and the other side having a partial negative charge. This creates a dipole, where the molecule has two poles with opposite charges. This polarity arises because of differences in electronegativity between atoms in the molecule, causing electrons to be shared unevenly. The molecule's shape also affects polarity; if the shape is asymmetrical, the charges do not cancel out, making the molecule polar. Polar molecules typically have polar covalent or ionic bonds and exhibit properties like attracting other polar molecules, dissolving in polar solvents, and having higher boiling points than nonpolar molecules. Examples include water (H2O), where the bent shape and electronegativity difference between oxygen and hydrogen cause polarity, and hydrogen fluoride (HF) which also has a large electronegativity difference making it polar.