In the resonance hybrid on the right, one of the electrons from the P=O double bond has accumulated around the O atom, giving it a negative charge and leaving the P atom with a positive charge. These charges are important in noncova-lent interactions.

▲ FIGURE 2-3 The dipole nature of a water molecule. The symbol 8 represents a partial charge (a weaker charge than the one on an electron or a proton). Because of the difference in the electronegativities of H and O, each of the polar H—O bonds in water has a dipole moment. The sizes and directions of the dipole moments of each of the bonds determine the net dipole moment of the molecule.

10 Ways To Fight Off Cancer

10 Ways To Fight Off Cancer

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