Answer :
Assuming the octet rule is obeyed and have a formal charge of zero, a nitrogen atom typically forms three covalent bonds with other atoms.
These bonds can be with hydrogen atoms or other elements, and the arrangement of shared electrons ensures a stable electron configuration for all atoms involved.
A nitrogen atom forms covalent bonds to achieve a formal charge of zero by adhering to the octet rule. Nitrogen has five valence electrons in its outer shell, requiring three additional electrons to complete its octet. By sharing three electrons with other atoms through covalent bonding, nitrogen can reach a stable electron configuration.
Covalent bonds involve the sharing of electrons between atoms to satisfy the octet rule. Nitrogen can form three covalent bonds, such as in ammonia (NH3), where it shares one electron with each of the three hydrogen atoms. In this case, each hydrogen atom contributes one electron, and nitrogen contributes three electrons, creating a stable, shared electron arrangement with a formal charge of zero for nitrogen.
Similarly, nitrogen can form covalent bonds with other elements to achieve a formal charge of zero. For example, in nitrogen gas (N2), two nitrogen atoms share three electrons each, resulting in a triple bond with a total of six shared electrons. Each nitrogen atom in this molecule achieves a complete octet and has a formal charge of zero.
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