Problem 14
Page 374
Section: Problems by Topic
Chapter 9: Chemical Bonding I:The Lewis Model
Given information
Using covalent Lewis structures, the reason as to why the compound that forms between nitrogen and hydrogen has the formula 
is to be explained. The reason why 
and 
are not stable is to be shown.
Step-by-step explanation
In a Lewis dot structure, the central metal atom of a molecule possesses 8 electrons in its valence shell, i.e. the Lewis structure follows the octet rule and the atom has an even number of total valence electrons.
Nitrogen belongs to period 
and has five valence electrons whereas hydrogen belongs to period 
and has only one valence electron. Therefore Nitrogen forms covalent bonds with hydrogen by sharing a pair of electrons to attain octet.
In , Nitrogen has a total of eight electrons; six electrons forming three covalent bonds with Hydrogen, and a lone pair (two unpaired electrons). It satisfies the Octet rule, thus it is stable.
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This problem is similar to
Principles of Chemistry Molecular Approach
Chemistry: A Molecular Approach
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Principles of Chemistry Molecular Approach
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- Problem 1
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- Problem 37d
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- Problem 43b