Expalin Dipole moment.
A dipole moment is a measurement of the separation of two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to the charge multiplied by the distance between the charges and the direction is from negative charge to positive charge:
μ = q · r
where μ is the dipole moment, q is the magnitude of the separated charge, and r is the distance between the charges.
Dipole moments are measured in the SI units of coulomb·meters (C m), but because the charges tend to be very small in magnitude, the historical unit for a dipole moment is the Debye. One Debye is approximately 3.33 x 10-30 C·m. A typical dipole moment for a molecule is about 1 D.
In chemistry a dipole moment is simply the measure of net polarity in a molecule. Dipole moments are applied to the distribution of electrons between two bonded atoms. The existence of a dipole moment is the difference between polar and nonpolar bonds. If a molecule contains polar bonds that are unevenly distributed about the center, there will be an uneven charge distribution across the entire molecule, making it a polar molecule. Polar molecules exhibit a large difference in electrical charge (a positive end and a negative end), otherwise known as a dipole moment. Molecules with a net dipole moment are polar molecules. If the net dipole moment is zero or very, very small, the bond and molecule are considered to be nonpolar. Atoms that have similar electronegativity values tend to form chemical bonds with a very small dipole moment.
A dipole moment is a measurement of the separation of two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to the charge multiplied by the distance between the charges and the direction is from negative charge to positive charge:
μ = q · r
where μ is the dipole moment, q is the magnitude of the separated charge, and r is the distance between the charges.
Dipole moments are measured in the SI units of coulomb·meters (C m), but because the charges tend to be very small in magnitude, the historical unit for a dipole moment is the Debye. One Debye is approximately 3.33 x 10-30 C·m. A typical dipole moment for a molecule is about 1 D.
In chemistry a dipole moment is simply the measure of net polarity in a molecule. Dipole moments are applied to the distribution of electrons between two bonded atoms. The existence of a dipole moment is the difference between polar and nonpolar bonds. If a molecule contains polar bonds that are unevenly distributed about the center, there will be an uneven charge distribution across the entire molecule, making it a polar molecule. Polar molecules exhibit a large difference in electrical charge (a positive end and a negative end), otherwise known as a dipole moment. Molecules with a net dipole moment are polar molecules. If the net dipole moment is zero or very, very small, the bond and molecule are considered to be nonpolar. Atoms that have similar electronegativity values tend to form chemical bonds with a very small dipole moment.
