# How do you write Lewis formulas for the reactant and product species in the following chemical equation, including nonbonding electrons? N(g) + NO(g) -> N NO(g)

## Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond.

Aug 2, 2017

We gots formal separation of charge for $\text{nitrous oxide}$.....

#### Explanation:

$N \equiv \stackrel{+}{N} - {O}^{+}$; going form the nitrogen around the left there are 5, 4, and 7 valence electrons, giving 7, 6, and 8 electrons associated with each atom, and formal electronic charges of $\stackrel{0}{N}$, $\stackrel{+ I}{N}$, and $\stackrel{- I}{O}$

For nitrogen monoxide we have a radical species, with 11 electrons to distribute......*stackrel(..)N=stackrel(ddot)O: is the usual representation. Clearly, the would react with atomic nitrogen gas.....

$N \left(g\right) + N = O \left(g\right) \rightarrow {N}_{2} O \left(g\right)$

Can you do $N {O}_{2}$ and ${N}_{2} {O}_{4}$? The former is a radical species, and both Lewis structures display charge separation.