Draw a lewis structure for h3o . show all unshared electrons and the formal charges, if any. assume that bonding follows the octet rule.

Lewis Structure of H₃O⁺ with Lone pair of electron labelled as RED and formal charge labelled as BLUE.

Lewis Structure was drawn utilizing following steps,

Step 1: Count the Total Number of Valence Electrons,

Oxygen           =  6

Hydrogen (3)  =  3______

Total                   9

                        -  1                 (for one +ve charge

                       =   8

Step 2: Make the structure as;

Put Oxygen atom in center surrounded by Hydrogen atoms. Make a single bond between each H and oxygen atom and subtract 2 electrons per bond. Therefore,

Electrons left  =  8 - 6  = 2

Step 3: Add remaining electrons to most electrnegative atom which is Oxygen in current case.

Step 4: Calculate Formal Charge on Oxygen using following formula,

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

Formal Charge  =  [6] - [2 + 6/2]

Formal Charge  =  6 -5

Formal Charge = + 1

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

the awnser is group 12