Net dipole
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
bond polarity is the polarity particular bond within a molecule, while molecular polarity is the polarity of the whole molecule. take for example water (H20): you could find the bond polarity of each H-0 bond (polar covalent), or the polarity of the whole molecule together (polar, because the electronegativity of oxygen is higher than the hydrogen atoms)
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
Polar covalent bonds. Not that due to the symmetry of the molecule (tetrahedral) the bond dipoles cancel each other out and overall the molecule is non-polar.
A polar molecule. or perhaps a polar covalent bond.
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
bond polarity is the polarity particular bond within a molecule, while molecular polarity is the polarity of the whole molecule. take for example water (H20): you could find the bond polarity of each H-0 bond (polar covalent), or the polarity of the whole molecule together (polar, because the electronegativity of oxygen is higher than the hydrogen atoms)
Polar covalent bonds. Not that due to the symmetry of the molecule (tetrahedral) the bond dipoles cancel each other out and overall the molecule is non-polar.
A polar molecule. or perhaps a polar covalent bond.
A molecule with polar bonds can be overall non-polar if the bond dipoles cancel each other out. For example the following all have polar bonds but the bond dipoles cancel each other out (vector addition) to make the molecule non-polar. Linear - CO2 trigonal planar - BF3 tetrahedral molecules, CF4 trigonal bipyramidal PF5 octahedral SF6
A dipole refers to two electrostatic charges which are separated by distance. In chemical compounds a dipole refers to unequal distribution of charge across a molecule that leads to an effective dipole often due to vector sum of bond dipoles.
It's positive in the direction of the greater one, and negative in the direction of the smaller one.
The reason why the overall charge of a water molecule is zero is because the number of positive hydrogen ions and the number of negative hydroxide ions are equal, so they cancel each other out.
An ion is a charged molecule. It is either positively or negatively charged due to the amount of electrons it is missing (+) or has extra (-). A charged molecule is said to be Ionized.
Generally if a molecule contains polar bonds and the bond dipole moments do not cancel each other out then that molecule will have an overall dipole moment. Bond dipoles arise when there is a significant difference in electronegativity between the atoms in the bond. There some cases such as phosphine PH3 where the lone pair can make a significant contribution to the molecular dipole moment.
The molecule can have an overall neutral charge, but one end is more negative and the other end is more positive. The negative end is the Polar head.