Covalent bonding is formed through the sharing of electrons between atoms. When determining the formation of covalent bonds, the atomic number is more relevant than the atomic mass.
The atomic number of an element corresponds to the number of protons in the nucleus of an atom. It defines the element's identity and determines its position on the periodic table. In a covalent bond, atoms share electrons in order to achieve a stable electron configuration, typically by filling their valence shells.
The valence electrons are the outermost electrons in an atom's electron configuration, and they play a crucial role in covalent bonding. The number of valence electrons is directly related to the atomic number. For example, carbon (C) has an atomic number of 6, indicating that it has six protons. Carbon's electron configuration is 2, 4, meaning it has two electrons in the inner shell and four valence electrons in the outer shell.
During covalent bonding, atoms strive to achieve a full outer shell by sharing electrons with other atoms. For carbon, it needs four additional electrons to complete its outer shell. Therefore, it forms four covalent bonds, typically with other carbon atoms or atoms such as hydrogen, nitrogen, or oxygen.
The atomic mass, on the other hand, represents the weighted average of the masses of an element's isotopes. While atomic mass can provide information about the isotopic composition and overall mass of an atom, it does not directly determine how atoms bond or interact in covalent bonding.
In summary, the atomic number, which indicates the number of protons and valence electrons, is the primary factor determining covalent bonding, as atoms share electrons to achieve a stable electron configuration.