draw lewis structure for no⁺, showing formal charges.

Answer

Explanation:

Step1: Determine valence electrons

N has 5 valence electrons and O has 6 valence electrons. Since it is $NO^{+}$, we subtract 1 electron for the positive charge. So total valence electrons = 5 + 6- 1=10.

Step2: Connect atoms

Connect N and O with a single - bond. This uses 2 electrons, leaving 8 electrons.

Step3: Distribute remaining electrons

Place 3 lone - pairs on O to satisfy its octet. Now we have used 8 electrons and have 0 electrons left. But N does not have an octet. So we change the single - bond to a triple - bond.

Step4: Calculate formal charges

Formal charge of an atom = valence electrons - non - bonding electrons - $\frac{1}{2}$ bonding electrons. For N: 5 - 0 - $\frac{1}{2}\times6$ = + 1 For O: 6 - 2 - $\frac{1}{2}\times6$ = 0

The Lewis structure has a triple - bond between N and O, with 1 lone - pair on O. The formal charge on N is + 1 and on O is 0.

Answer:

The Lewis structure has a triple - bond between N and O, with 1 lone - pair on O. N has a formal charge of + 1 and O has a formal charge of 0.