How would you describe the strength of the bonds that result from resonance in SO3?
1 answer:
Answer:
All bonds are equivalent in length and strength within the molecule.
Gaseous SO3 is a trigonal planar molecule that exhibit a D3h symmetry group.
Sulfur has sp2 hybridization and it has 6 outer electrons which make the bonds with the oxygen.
Its constituent sulfur atom has an oxidation state of +6 and a formal charge of 0.
The Lewis structure is made up of one S=O double bond and two S–O dative bonds that doesn't not engage the d-orbitals. ( Thus, SO3 molecule has three double bonded oxygen to the central sulfur atom). This explains the strength.
It gaseous form had a zero electrical dipole moment because of the 120° angle between the S-O bonds.
Explanation:
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Answer:
Approximately (rounded to two significant figures.)
Explanation:
The unit of concentration is the same as
(moles per liter.) On the other hand, the volume of both the
solution and the original
solution here are in milliliters. Convert these two volumes to liters:
.
.
Calculate the number of moles of in that
of
solution:
.
reacts with
at a one-to-one ratio:
.
Coefficient ratio:
.
In other words, one mole of would neutralize exactly one mole of
. In this titration,
of
was required. Therefore, the same amount of
should be present in the original solution:
.
Calculate the concentration of the original solution:
.
Answer:
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Explanation:
