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  2. Hydrogen bond - Wikipedia

    en.wikipedia.org/wiki/Hydrogen_bond

    Consequently, hydrogen bonds between or within solute molecules dissolved in water are almost always unfavorable relative to hydrogen bonds between water and the donors and acceptors for hydrogen bonds on those solutes. [44] Hydrogen bonds between water molecules have an average lifetime of 10 −11 seconds, or 10 picoseconds. [45]

  3. Chemical polarity - Wikipedia

    en.wikipedia.org/wiki/Chemical_polarity

    The bond dipole moments do not cancel, so that the molecule forms a molecular dipole with its negative pole at the oxygen and its positive pole midway between the two hydrogen atoms. In the figure each bond joins the central O atom with a negative charge (red) to an H atom with a positive charge (blue).

  4. Intermolecular force - Wikipedia

    en.wikipedia.org/wiki/Intermolecular_force

    A hydrogen bond is an extreme form of dipole-dipole bonding, referring to the attraction between a hydrogen atom that is bonded to an element with high electronegativity, usually nitrogen, oxygen, or fluorine. [4] The hydrogen bond is often described as a strong electrostatic dipoledipole interaction.

  5. Dipolar compound - Wikipedia

    en.wikipedia.org/wiki/Dipolar_compound

    In organic chemistry, a dipolar compound or simply dipole is an electrically neutral molecule carrying a positive and a negative charge in at least one canonical description. In most dipolar compounds the charges are delocalized . [ 1 ]

  6. Dipole - Wikipedia

    en.wikipedia.org/wiki/Dipole

    For example, the zero dipole of CO 2 implies that the two C=O bond dipole moments cancel so that the molecule must be linear. For H 2 O the O−H bond moments do not cancel because the molecule is bent. For ozone (O 3) which is also a bent molecule, the bond dipole moments are not zero even though the O−O bonds are between similar atoms. This ...

  7. Non-covalent interaction - Wikipedia

    en.wikipedia.org/wiki/Non-covalent_interaction

    A hydrogen bond (H-bond), is a specific type of interaction that involves dipoledipole attraction between a partially positive hydrogen atom and a highly electronegative, partially negative oxygen, nitrogen, sulfur, or fluorine atom (not covalently bound to said hydrogen atom). It is not a covalent bond, but instead is classified as a strong ...

  8. Molecular orbital diagram - Wikipedia

    en.wikipedia.org/wiki/Molecular_orbital_diagram

    The σ from the 2p is more non-bonding due to mixing, and same with the 2s σ. This also causes a large jump in energy in the 2p σ* orbital. The bond order of diatomic nitrogen is three, and it is a diamagnetic molecule. [12] The bond order for dinitrogen (1σ g 2 1σ u 2 2σ g 2 2σ u 2 1π u 4 3σ g 2) is three because two electrons are now ...

  9. Properties of water - Wikipedia

    en.wikipedia.org/wiki/Properties_of_water

    Although hydrogen bonding is a relatively weak attraction compared to the covalent bonds within the water molecule itself, it is responsible for several of the water's physical properties. These properties include its relatively high melting and boiling point temperatures: more energy is required to break the hydrogen bonds between water molecules.