hydrogen bonding
Oxygen attracts electrons much more strongly than hydrogen, resulting in a net positive charge on the hydrogen atoms, and a net negative charge on the oxygen atom. The presence of a charge on each of these atoms gives each water molecule a net dipole moment,. Electrical attraction between water molecules due to this dipole pulls individual molecules closer together. This attraction is known as hydrogen bonding. The molecules of water are constantly moving in relation to each other, and the hydrogen bonds are continually breaking and reforming very very fast in nanoseconds..
WITHIN the molecule: covalent bonding.
OUTSIDE the molecule: hydrogen bonding, mainly.
Covalent Bonding
covalent bond
hydrogen bonds
Polar covalent bonds
A molecule with hydrogen bonded to O, N, or F (Apex)
Water is H2O, thus there are 2 hydrogen atoms present and one oxygen atom.
phosopholipid
A diatomic molecule for example oxygen gas (O2)
ionic
hydrogen bonding between H2O and covalent bonding within the H2O molecule
A molecule.
The atoms in an ammonia molecule are covalently bonded.
Covalent
Ionic bond is present in calcium phosphide.
A molecule with hydrogen bonded to O, N, or F (Apex)
Water is H2O, thus there are 2 hydrogen atoms present and one oxygen atom.
phosopholipid
Hydrogen bonding is usually formed between one lone pair of electrons of the oxygen atom of one water molecule and the hydrogen atom of another water molecule. Hydrogen bonding forms as a result of electro-negativity difference between oxygen atom and hydrogen, with oxygen being more electro-negative.
A diatomic molecule for example oxygen gas (O2)
A diatomic molecule for example oxygen gas (O2)
inorganic