(a) nitromethane is an organic compound with the molecular formula ch3no2. draw a complete lewis structure that shows all bonds, unshared electron pairs, and minimized formal charges, where appropriate.

The Lewis Structure of Nitromethane is attached below.

It can be found from structure that it consists of a single carbon atom bonded to three hydrogen atoms and a nitrogen atom of Nitro functional group via single covalent (sigma) bonds.

The functional group (-NO₂) is highlighted in blue.

Also, the formal charges on all atoms is zero except for Nitrogen atom and and oxygen atom of Nitro group which was calculated +1 and -1 respectively using following formula.

Formal Charge  =  [# of valence e⁻] - [e⁻ in lone pairs + 1/2 # of bonding e⁻]

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.