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The bond between water molecules is known as a hydrogen bond.
The intermolecular bonds between water molecules are hydrogen bonds.
The forces between ions in crystals are ionic bonds. These bonds are stronger and are a much more extreme version of electron sharing between metal atoms and nonmetal atoms. London forces and dipole-dipole forces are attractive forces that occur between covalently bonded nonmetal atoms.
Ionic bonds
ionic bonds
Hydrogen bonds.
Ionic bonds are stronger.
extra strong intermolecular attractions between polar molecules -apex
extra strong intermolecular attractions between polar molecules -apex
Hydrogen bonds
d.polarWater molecules are polar covalent and therefore form attractions between the molecules called hydrogen bonds. Much of the heat that goes into raising the temperature of water to its boiling point goes to breaking the hydrogen bonds first.
strong polar attractions between molecules involving h, f, o, and n
Adjacent water molecules are connected by the electrical attraction between the oxygen of one water molecule and the hydrogen of another water molecule. This type of bonding is called hydrogen bonding.
There are no bonds between hexane molecules. There are intermolecular forces, called London Dispersion Forces which attract other hexane molecules.
Within the molecule, covalent bonds hold them together. Between the molecules there can be several different forces. There are dipole-dipole attractions, hydrogen bonds and van der Waals forces. Which of them apply in a particular substance depends on the structure of the molecules.
There are a few types of hydrogen bonds. Fluorine, oxygen, and nitrogen are the elements that typically form bonds with hydrogen.
Hydrogen Bonds.(Hydrogen bonding is another term for the dipole-dipole attractions between H2O molecules.) A Hydrogen bond is between a H atom in one molecule and either a O, N, or F atom in another.