[tex]\boxed{{\text{3}}\;{\text{covalent bonds}}}[/tex] are formed by nitrogen if each of its unpaired electrons participates in one bond.
Further Explanation:
The bond that is formed by the mutual sharing of electrons between the bonded atoms is called a covalent bond. It is also known as a molecular bond. Covalent compounds are those compounds which are formed by the electron sharing between two or more non-metals.
The octet rule is the rule in accordance to which the elements have the tendency to bond with other elements and acquire eight electrons in their valence shells. This results in achieving a stable noble gas configuration.
For example, the formation of [tex]{\text{NaCl}}[/tex] occurs according to the octet rule. The electronic configuration of sodium is [tex]{\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^{\mathbf{6}}}{\mathbf{3}}{{\mathbf{s}}^{\mathbf{1}}}[/tex] while that of chlorine is [tex]{\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^{\mathbf{6}}}{\mathbf{3}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{3}}{{\mathbf{p}}^{\mathbf{5}}}[/tex] .
Chlorine is one electron short of the stable noble gas configuration and sodium can achieve stable configuration by losing an electron. So sodium loses an electron and forms cation and chlorine gains that electron to complete its octet.
In case of nitrogen:
The atomic number of nitrogen is 7. Its ground state electronic configuration is [tex]{\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^{\mathbf{3}}}[/tex] . The partial orbital diagram is the diagrammatic representation of the distribution of electrons in the valence shell only. In case of nitrogen, the valence shell is 2s and 2p.(Refer to the attached image).
Nitrogen atom consists of five electrons in its valence shell. Out of these five electrons, two are paired and present in 2s while three remain unpaired in 2p. If all three unpaired electrons are to be used, it will accept three electrons from the neighboring atoms to make three covalent bonds. The octet of nitrogen is completed with the formation of three covalent bonds with neighboring atoms.
Learn more:
1. Identification of ionic bonding: https://brainly.com/question/1603987
2. Chemical bonds in NaCl: https://brainly.com/question/5008811
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Ionic and covalent compounds
Keywords: covalent bonds, nitrogen, unpaired electrons, bond, 3, paired electrons, covalent compounds, molecular bond, covalent bond, mutual sharing of electrons, five electrons, partial orbital diagram, distribution of electrons.
