The observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm to be explained. The elimination of any resonance structure of N 2 O on the basis of formal charge is to be identified. The consistency of this elimination is to be checked with the given observation. Concept introduction: The Lewis structure is also known as dot structure. This structure depicts the bonding between atoms and the lone pairs of electrons if exists. Formal charge is a charge given to an atom with assumption that electrons are shared equally between atoms in all chemical bonds irrespective of their electronegativity. To determine: The rationalization of the observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm ; if any of the resonance structure of N 2 O can be eliminated on the basis of formal charge; if this elimination is consistent with the given observation. To determine: The rationalization of the observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm .
The observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm to be explained. The elimination of any resonance structure of N 2 O on the basis of formal charge is to be identified. The consistency of this elimination is to be checked with the given observation. Concept introduction: The Lewis structure is also known as dot structure. This structure depicts the bonding between atoms and the lone pairs of electrons if exists. Formal charge is a charge given to an atom with assumption that electrons are shared equally between atoms in all chemical bonds irrespective of their electronegativity. To determine: The rationalization of the observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm ; if any of the resonance structure of N 2 O can be eliminated on the basis of formal charge; if this elimination is consistent with the given observation. To determine: The rationalization of the observation that the N − N bond length in N 2 O is 112 pm and that the N − O bond length is 119 pm .
Solution Summary: The author analyzes how the Lewis structure depicts the bonding between atoms and the lone pairs of electrons if exists.
Definition Definition Connection between particles in a compound. Chemical bonds are the forces that hold the particles of a compound together. The stability of a chemical compound greatly depends on the nature and strength of the chemical bonding present in it. As the strength of the chemical bonding increases the stability of the compound also increases.
Chapter 8, Problem 106E
Interpretation Introduction
Interpretation:
The observation that the
N−N bond length in
N2O is
112pm and that the
N−O bond length is
119pm to be explained. The elimination of any resonance structure of
N2O on the basis of formal charge is to be identified. The consistency of this elimination is to be checked with the given observation.
Concept introduction:
The Lewis structure is also known as dot structure. This structure depicts the bonding between atoms and the lone pairs of electrons if exists.
Formal charge is a charge given to an atom with assumption that electrons are shared equally between atoms in all chemical bonds irrespective of their electronegativity.
To determine: The rationalization of the observation that the
N−N bond length in
N2O is
112pm and that the
N−O bond length is
119pm; if any of the resonance structure of
N2O can be eliminated on the basis of formal charge; if this elimination is consistent with the given observation.
To determine: The rationalization of the observation that the
N−N bond length in
N2O is
112pm and that the
N−O bond length is
119pm.
An open vessel containing water stands in a laboratory measuring 5.0 m x 5.0 m x 3.0 m at 25 °C ; the vapor pressure (vp) of water at this temperature is 3.2 kPa. When the system has come to equilibrium, what mass of water will be found in the air if there is no ventilation? Repeat the calculation for open vessels containing benzene (vp = 13.1 kPa) and mercury (vp = 0.23 Pa)
Every chemist knows to ‘add acid to water with constant stirring’ when diluting a concentrated acid in order to keep the solution from spewing boiling acid all over the place. Explain how this one fact is enough to prove that strong acids and water do not form ideal solutions.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell