The strength of chemical bonds can vary, and it's important to note that the values can depend on the specific compounds involved and the conditions under which the measurements are made. However, in general, here is a list of chemical bonds in order of increasing strength:

Covalent Bonds: These are also considered intramolecular bonds formed when atoms share electrons to achieve a more stable electron configuration. Covalent bonds are relatively strong and hold the atoms together within a molecule. Examples include the bonds between atoms in water (H₂O) or methane (CH₄).

• Nonpolar covalent bonds: Nonpolar covalent bonds involve the equal sharing of electrons between atoms. This type of bond occurs when the electronegativity difference between atoms is minimal.

• Polar covalent bonds: In polar covalent bonds, electrons are shared between atoms, but the sharing is unequal due to differences in electronegativity. This leads to partial positive and negative charges within the molecule.

The strength of covalent bonds can vary. Single covalent bonds are generally weaker than double or triple bonds. The strength depends on factors like bond length and bond energy. Covalent network structures (like in diamond or quartz) can be very strong due to the three-dimensional network of covalent bonds.

Ionic bonds: Ionic bonds are intramolecular bonds. They involve the transfer of electrons from one atom to another, resulting in the formation of positively charged cations and negatively charged anions that are held together by electrostatic forces. An example is the bond in sodium chloride (NaCl).

Intramolecular ionic bonds can be strong due to the electrostatic attraction between oppositely charged ions in a crystal lattice. Ionic compounds often have high melting and boiling points.

Metallic bonds: Metallic bonds are intramolecular forces that occur between metal atoms. In this bonding type, electrons are delocalized and move freely throughout the metal lattice, contributing to the unique properties of metals, such as electrical conductivity and malleability.

Covalent network bonds: These are strong intramolecular bonds that involve a three-dimensional network of covalent bonds throughout a substance. Examples include diamond and quartz. These substances have very high melting points and are typically hard and brittle.

Van der Waals forces: 

• London Dispersion Forces: Weakest intermolecular forces, arising from temporary fluctuations in electron distribution around atoms and molecules.

• Dipole-Dipole Interactions: Intermolecular forces between polar molecules with permanent dipole moments.

Hydrogen bonds: Hydrogen bonds are a type of dipole-dipole interaction where a hydrogen atom is covalently bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom.

Ion-Dipole Interactions: These interactions occur between an ion and a polar molecule, where the ion is attracted to the partial charges on the polar molecule.

Dipole-Induced Dipole Interactions: These interactions occur between a polar molecule and a nonpolar molecule, where the presence of the polar molecule induces a temporary dipole moment in the nonpolar molecule.