Dipole means that there's an uneven distribution of electrons in a molecule; this usually occurs when you've a molecule with atoms of very different electronegativities.
Covalent describes bonds that have electrons shared between atoms. The opposite of this would be ionic, where one atom takes electrons from another atom.
covalent bond.
Dipole dipole forces
'''''Increasing strength''''' 1.London dispersion 2. dipole-dipole 3. ionic 4. covalent
polar covalent compound, although the difference in electronegativity is not enough to form dipole, the assymetry of the compound structure causes it to gain polarity.
Polar covalent- due to the difference in electronegativity between H and Br.
covalent bond.
Dipole dipole forces
'''''Increasing strength''''' 1.London dispersion 2. dipole-dipole 3. ionic 4. covalent
polar covalent compound, although the difference in electronegativity is not enough to form dipole, the assymetry of the compound structure causes it to gain polarity.
intramolecular: covalent bond intermolecular: dipole-dipole interaction (smaller version of ionic bond)
Covalent, specifically polar covalent with no dipole moment.
Polar covalent- due to the difference in electronegativity between H and Br.
interaction with water, dipole dipole interaction, within the phospholipid itself covalent
Since the covalent bond between sulfur and oxygen is polar, dipole dipole attractions are present as intermolecular forces.
A bond between two or more polar covalent molecules is called a Dipole-Dipole attraction (or interaction).
There are two kinds of chemical bonding in elements. They are ionic bonds and covalent bonds. Both are very important.
No, dissolving does not break covalent bonds. The molecules separate because intermolecular forces such as dipole-dipole attractions are disrupted.