The structure of borazine, B3N3H6, is a six-membered ringof alternating B and N atoms. There is one H atom bondedto each B and to each N atom. The molecule is planar.(a) Write a Lewis structure for borazine in which the formalcharge on every atom is zero. (b) Write a Lewis structurefor borazine in which the octet rule is satisfied forevery atom. (c) What are the formal charges on the atomsin the Lewis structure from part (b)? Given the electronegativitiesof B and N, do the formal charges seem favorableor unfavorable? (d) Do either of the Lewis structuresin parts (a) and (b) have multiple resonance structures?(e) What are the hybridizations at the B and N atoms inthe Lewis structures from parts (a) and (b)? Would you expectthe molecule to be planar for both Lewis structures?(f) The six B—N bonds in the borazine molecule are allidentical in length at 1.44 Å. Typical values for the bondlengths of B¬N single and double bonds are 1.51 Å and1.31 A°, respectively. Does the value of the B—N bondlength seem to favor one Lewis structure over the other?(g) How many electrons are in the π system of borazine?
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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. (b) Write a Lewis structure
for borazine in which the octet rule is satisfied for
every atom. (c) What are the formal charges on the atoms
in the Lewis structure from part (b)? Given the electronegativities
of B and N, do the formal charges seem favorable
or unfavorable? (d) Do either of the Lewis structures
in parts (a) and (b) have multiple resonance structures?
(e) What are the hybridizations at the B and N atoms in
the Lewis structures from parts (a) and (b)? Would you expect
the molecule to be planar for both Lewis structures?
(f) The six B—N bonds in the borazine molecule are all
identical in length at 1.44 Å. Typical values for the bond
lengths of B¬N single and double bonds are 1.51 Å and
1.31 A°
, respectively. Does the value of the B—N bond
length seem to favor one Lewis structure over the other?
(g) How many electrons are in the π system of borazine?
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