The strength of forces between atoms in a covalent bond can be quantified by the bond dissociation energy. Bond dissociation energy is the energy required to break a single covalent bond between two atoms in a molecule. It is typically measured in units of kilojoules per mole (kJ/mol).

The bond dissociation energy of a covalent bond depends on several factors, including:

1. Electronegativity: The difference in electronegativity between the two atoms forming the bond. The greater the electronegativity difference, the stronger the bond. This is because the more electronegative atom attracts electrons more strongly, creating a stronger bond.

2. Bond order: The number of electron pairs shared between the two atoms. The higher the bond order, the stronger the bond. This is because more electron pairs mean more electrons are shared between the atoms, creating a stronger attraction.

3. Bond length: The distance between the two atoms forming the bond. The shorter the bond length, the stronger the bond. This is because the closer the atoms are to each other, the stronger the attraction between them.

In general, covalent bonds are stronger than ionic bonds and hydrogen bonds. The strongest covalent bonds are typically found between atoms with high electronegativity differences and high bond orders.

Some examples of bond dissociation energies for common covalent bonds:

- H-H bond: 436 kJ/mol

- C-C bond: 348 kJ/mol

- C-H bond: 413 kJ/mol

- N-H bond: 391 kJ/mol

- O-H bond: 463 kJ/mol

These values illustrate the range of bond strengths that can exist in covalent bonds.