(a) Interpretation: The reason for not forming pentafluoride by nitrogen should be suggested. Concept introduction: In the group-15, the valence shell configuration of all elements is ns 2 , np 3 hence they have 5 valence electrons with half-filled valence shell. The group-15 starts from nitrogen (N) and ended at Bismuth (Bi); nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).Nitrogen is the first and smallest element of the group with 2s 2 , 2p 3 valence shell configuration. It exhibits anomalous behavior due to small size and high electro-negativity compare to other elements of the group.
(a) Interpretation: The reason for not forming pentafluoride by nitrogen should be suggested. Concept introduction: In the group-15, the valence shell configuration of all elements is ns 2 , np 3 hence they have 5 valence electrons with half-filled valence shell. The group-15 starts from nitrogen (N) and ended at Bismuth (Bi); nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).Nitrogen is the first and smallest element of the group with 2s 2 , 2p 3 valence shell configuration. It exhibits anomalous behavior due to small size and high electro-negativity compare to other elements of the group.
Solution Summary: The author explains the reason for not forming pentafluoride by nitrogen using the VSEPR theory.
The reason for not forming pentafluoride by nitrogen should be suggested.
Concept introduction:
In the group-15, the valence shell configuration of all elements is ns2, np3 hence they have 5 valence electrons with half-filled valence shell. The group-15 starts from nitrogen (N) and ended at Bismuth (Bi); nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).Nitrogen is the first and smallest element of the group with 2s2, 2p3 valence shell configuration. It exhibits anomalous behavior due to small size and high electro-negativity compare to other elements of the group.
Interpretation Introduction
(b)
Interpretation:
The structure of NF3 molecule should be rationalized using VSEPR theory.
Concept introduction:
VSEPR is the theory purposed to explain the geometry of those molecules mainly which have lone pairs on the central atom as due to presence of lone pair and bond pairs, the repulsion plays important role in the determination of molecular geometry of the molecule.
Ammonia reacts with boron trifluoride to form a stablecompound, as we saw in Section 8.7. (a) Draw the Lewisstructure of the ammonia–boron trifluoride reaction product.(b) The B—N bond is obviously more polar than theC—C bond. Draw the charge distribution you expect on theB—N bond within the molecule (using the delta plus anddelta minus symbols mentioned in Section 8.4). (c) Borontrichloride also reacts with ammonia in a similar way tothe trifluoride. Predict whether the B—N bond in the trichloridereaction product would be more or less polar thanthe B—N bond in the trifluoride product, and justify yourreasoning
Ammonia reacts with boron trifluoride to form a stablecompound, as we saw in Section 8.7. (a) Draw the Lewisstructure of the ammonia–boron trifluoride reaction product.(b) The B—N bond is obviously more polar than the C—C bond. Draw the charge distribution you expect on theB—N bond within the molecule (using the delta plus anddelta minus symbols mentioned in Section 8.4). (c) Borontrichloride also reacts with ammonia in a similar way tothe trifluoride. Predict whether the B—N bond in the trichloridereaction product would be more or less polar thanthe B—N bond in the trifluoride product, and justify yourreasoning.
Which Group 5A element cannot form molecules with five covalent bonds?
Select one:
a. N
b. P
c. As
d. Sb
e. Bi
Chapter 22 Solutions
General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell