enow.com Web Search

Search results

  1. Results from the WOW.Com Content Network
  2. Chemical polarity - Wikipedia

    en.wikipedia.org/wiki/Chemical_polarity

    Note that the dipole moments drawn in this diagram represent the shift of the valence electrons as the origin of the charge, which is opposite the direction of the actual electric dipole moment. The bond dipole moment [5] uses the idea of electric dipole moment to measure the polarity of a chemical bond within a molecule. It occurs whenever ...

  3. Polarizability - Wikipedia

    en.wikipedia.org/wiki/Polarizability

    The polarizability of an atom or molecule is defined as the ratio of its induced dipole moment to the local electric field; in a crystalline solid, one considers the dipole moment per unit cell. [1] Note that the local electric field seen by a molecule is generally different from the macroscopic electric field that would be measured externally.

  4. Carbon–nitrogen bond - Wikipedia

    en.wikipedia.org/wiki/Carbon–nitrogen_bond

    A CN bond is strongly polarized towards nitrogen (the electronegativities of C and N are 2.55 and 3.04, respectively) and subsequently molecular dipole moments can be high: cyanamide 4.27 D, diazomethane 1.5 D, methyl azide 2.17, pyridine 2.19. For this reason many compounds containing CN bonds are water-soluble.

  5. 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 ...

  6. Electric dipole moment - Wikipedia

    en.wikipedia.org/wiki/Electric_dipole_moment

    The electric dipole moment is a measure of the separation of positive and negative electrical charges within a system: that is, a measure of the system's overall polarity. The SI unit for electric dipole moment is the coulomb-metre (C⋅m). The debye (D) is another unit of measurement used in atomic physics and chemistry.

  7. Debye - Wikipedia

    en.wikipedia.org/wiki/Debye

    Typical dipole moments for simple diatomic molecules are in the range of 0 to 11 D. Molecules with symmetry point groups or containing inversion symmetry will not have a permanent dipole moment, while highly ionic molecular species have a very large dipole moment, e.g. gas-phase potassium bromide, KBr, with a dipole moment of 10.41 D. [3] A proton and an electron 1 Å apart have a dipole ...

  8. Symmetry of diatomic molecules - Wikipedia

    en.wikipedia.org/wiki/Symmetry_of_diatomic_molecules

    Molecular symmetry in physics and chemistry describes the symmetry present in molecules and the classification of molecules according to their symmetry. Molecular symmetry is a fundamental concept in the application of Quantum Mechanics in physics and chemistry, for example it can be used to predict or explain many of a molecule's properties, such as its dipole moment and its allowed ...

  9. Inductive effect - Wikipedia

    en.wikipedia.org/wiki/Inductive_effect

    The vector addition of the individual bond dipole moments results in a net dipole moment for the molecule. A polar bond is a covalent bond in which there is a separation of charge between one end and the other - in other words in which one end is slightly positive and the other slightly negative. Examples include most covalent bonds.