Answer :
Answer:
3
Explanation:
In a nitrogen atom, since the no, of electrons is equal to its no. of protons, it has 7 electrons.
The electron configuration is 2, 5. (the first shell can only hold 2 electrons)
In each covalent bond, 2 electrons are shared between 2 atoms. usually, both atom contribute one electron. (unless it's dative covalent bond, which is not important at this point).
To obey octet rule, the outermost electron shell must have 8 electrons. Which means, the nitrogen atom need 3 more electrons to achieve that.
So with 3 covalent bonds, the nitrogen can get share 3 of its electrons, and obtain 3 more from the other atom(s). It won't lose electrons because covalent bonds exist between shared electrons, unlike ionic bonds.
Final answer:
A nitrogen atom, following the octet rule, will form three covalent bonds to achieve a formal charge of zero. This number comes from the fact that nitrogen, being in Group 15, has five valence electrons and needs three more to reach a full octet, thus forming three covalent bonds.
Explanation:
Assuming the octet rule is obeyed, a nitrogen atom will form three covalent bonds to give a formal charge of zero. Nitrogen is an element in Group 15, which means it has five valence electrons. To achieve a full octet of eight electrons, nitrogen forms three covalent bonds, meaning it shares three pairs of electrons with other atoms. An example of this can be observed in the molecule NH3 (ammonia), where nitrogen forms three covalent bonds with three hydrogen atoms.
Having a formal charge of zero indicates that the atom is at its most stable state. The stability is determined by guidelines such as minimizing formal charges, having no formal charge with a magnitude greater than one, placing negative formal charges on more electronegative elements, and having the less electronegative atom in the center position, among others.
Learn more about covalent bonds here:
https://brainly.com/question/16655971
#SPJ3
