We are being asked to determine the false statements for NH3 and NF3.
In order to answer each statement, we need to determine first the Lewis structures of both structures, and their geometries.
We determine the Lewis structures with the following steps:
Step 1: Determine the central atom in the structure.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Which statement for NH3 and NF3 is false? Electronegativities: N = 3.0, H = 2.1, F = 4.0.
a. The NF3 molecule is more polar than the NH 3 molecule.
b. The bond angles in NF3 are smaller than those in NH3.
c. The bond dipoles in NF3 are directed toward the more electronegative fluorine atoms.
d. Both molecules have one unshared pair of electrons in the outer shell of nitrogen.
e. Both are sp3 hybridized at nitrogen.
f. The bond dipoles in NF3 oppose the effect of the unshared pair of electrons.
g. The nitrogen atom can be described as utilizing sp3 hybrid orbitals in the nitrogen trifluoride molecule.
h. The bond dipoles of NF3 are directed toward fluorine, whereas those in NH 3 are directed toward nitrogen.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Molecular Polarity concept. You can view video lessons to learn Molecular Polarity. Or if you need more Molecular Polarity practice, you can also practice Molecular Polarity practice problems.
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Based on our data, we think this problem is relevant for Professor Visalia's class at College of the Sequoias.