In ammonia, a central nitrogen atom is bonded to three hydrogen atoms. Similarly, boron trifluoride has a central boron atom bonded to three fluorine atoms. However, ammonia is pyramidal and boron trifluoride is trigonal planar in shape. Which statement justifies this difference in their structure?

AThe lone pair of electrons in boron trifluoride increases the bond angle between the bonding pairs, giving it a planar structure.

BThe lone pair of electrons in boron trifluoride decreases the bond angle between the bonding pairs, giving it a planar structure.

CThe lone pair of electrons in boron trifluoride stabilizes the bond angle between the bonding pairs, giving it a planar structure.

DThe lone pair of electrons in ammonia increases the bond angle between the bonding pairs, giving it a pyramidal structure.

EThe lone pair of electrons on the nitrogen in ammonia decreases the bond angle between the bonding pairs, giving it a pyramidal structure.

The lone pair of electrons on the nitrogen in ammonia decreases the bond angle between the bonding pairs, giving it a pyramidal structure.

In that case, Your answer is E.

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saadhussain514 saadhussain514 · Answer 2 · 2018-08-25T04:00:59-04:00

Correct answer choice is :

E) The lone pair of electrons on the nitrogen in ammonia decreases the bond angle between the bonding pairs, giving it a pyramidal structure.

Explanation:

Ammonia is a mixture of nitrogen and hydrogen with the code NH₃. The simplistic pnictogen hydride, ammonia, is a neutral gas with a distinctive sour smell. Vulnerability to high frequencies of ammonia in the air creates important burning of the eyes, nose, throat and respiratory field and can occur in darkness, lung damage or death. Breath of lower frequencies can produce coughing, and nose and throat inflammation.