The structure of borazine, B3N3H6, is a six-membered ring
of alt...

Question

The structure of borazine, B3N3H6, is a six-membered ring 
of alternating B and N atoms. There is one H atom bonded 
to each B and to each N atom. The molecule is planar. 
(a) Write a Lewis structure for borazine in which the formal 
charge on every atom is zero.

Accepted Answer

Hey everyone, we're asked to draw out the lewis structure of rock scene and to make sure that the formal charge on each atom is zero. Now, they've given us a description on how our Barac scene is structured. But first let's go ahead and calculate the total number of valence electrons will have to draw out for our boron. We have three of boron. And we're going to multiply this by three. Since boron is in our group 38, this will get us to nine valence electrons for our hydrogen. We have three of hydrogen and we're going to multiply this by one and this will get us three valence electrons For our oxygen. We have three of oxygen and we're going to multiply this by six since oxygen is in a group six a this will get us to 18 valence electrons. In total, we have to draw out 30 valence electrons. Now let's go ahead and draw our lewis structure. We're told that we have a six member ring that is made up of alternating oxygen and boron drawing this out. We have boron, oxygen, boron, oxygen, boron and oxygen. And we're also told that the overall shape is plainer and one hydrogen is bonded to each boron adam. Now to get to 30 valence electrons will have to add two lone pairs onto each oxygen. Now let's go ahead and determine the formal charge of each atom. We know that formal charge is going to be equal to the group number minus the sum of our bonds, plus our non bonding electrons where the formal charge of boron. We know that our group number is going to be three and we're going to subtract three plus zero since we have three bonds connecting to our boron and zero non bonding electrons. This will get us to an overall formal charge of zero for a formal charge of our hydrogen. We know that our group number is going to be one and we're going to subtract one plus zero and this will get us to a formal charge of zero as well for a formal charge of oxygen. We know our group number is six and we're going to subtract two bonds plus four non bonding electrons. This will get us so formal charge of zero as well. Now I hope that made sense. And let us know if you have any questions.

The structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (a) Write a Lewis structure for borazine in which the formal charge on every atom is zero.

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