
Concept explainers
(a)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in peroxide ion has to be predicted using MO theory.
Concept Introduction:
Molecular orbital theory:
The atomic orbitals of the atoms constituted in a molecule are combined to produce new orbitals are called Molecular Orbitals.
Like atomic orbitals, a molecular orbital can accommodate maximum two electrons and the two electrons must have opposite spins (Pauli Exclusion Principle).
The numbers of MO’s are equals to the number of atomic orbitals are combined in such a way that the linear combination of similar atomic orbitals to form one bonding and one anti-bonding MO’s.
The bonding MO’s are lower in energy than the anti-bonding MO’s.
HOMO is the highest energized occupied orbital in the MO’s.
Relative energy levels of molecules are according to the energy levels of atomic orbitals.
LUMO is the lowest energized orbital in the MO’s.
Bond order can be calculated using below formula
(a)

Explanation of Solution
The total number of valence electrons present in Peroxide ion is
The molecular orbital diagrams of the peroxide ion can be written as,
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the Peroxide ion has single bond and no unpaired electrons.
(b)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in
Concept Introduction:
Refer part (a).
(b)

Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
(c)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in
Concept Introduction:
Refer part (a).
(c)

Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
(d)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds
Concept Introduction:
Refer part (a).
(d)

Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
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Chapter 6 Solutions
Chemistry: The Molecular Science
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- For the decomposition reaction of N2O5(g): 2 N2O5(g) → 4 NO2(g) + O2(g), the following mechanism has been proposed: N2O5 NO2 + NO3 (K1) | NO2 + NO3 → N2O5 (k-1) | NO2 + NO3 NO2 + O2 + NO (k2) | NO + N2O51 NO2 + NO2 + NO2 (K3) → Give the expression for the acceptable rate. → → (A). d[N205] dt == 2k,k₂[N₂O₂] k₁+k₁₂ (B). d[N2O5] =-k₁[N₂O] + k₁[NO₂] [NO3] - k₂[NO₂]³ dt (C). d[N2O5] =-k₁[N₂O] + k [NO] - k₂[NO] [NO] d[N2O5] (D). = dt = -k₁[N2O5] - k¸[NO][N₂05] dt Do not apply the calculations, based on the approximation of the stationary state, to make them perform correctly. Basta discard the 3 responses that you encounter that are obviously erroneous if you apply the formula to determine the speed of a reaction.arrow_forwardFor the decomposition reaction of N2O5(g): 2 N2O5(g) → 4 NO2(g) + O2(g), the following mechanism has been proposed: N2O5 NO2 + NO3 (K1) | NO2 + NO3 → N2O5 (k-1) | NO2 + NO3 NO2 + O2 + NO (k2) | NO + N2O51 NO2 + NO2 + NO2 (K3) → Give the expression for the acceptable rate. → → (A). d[N205] dt == 2k,k₂[N₂O₂] k₁+k₁₂ (B). d[N2O5] =-k₁[N₂O] + k₁[NO₂] [NO3] - k₂[NO₂]³ dt (C). d[N2O5] =-k₁[N₂O] + k [NO] - k₂[NO] [NO] d[N2O5] (D). = dt = -k₁[N2O5] - k¸[NO][N₂05] dt Do not apply the calculations, based on the approximation of the stationary state, to make them perform correctly. Basta discard the 3 responses that you encounter that are obviously erroneous if you apply the formula to determine the speed of a reaction.arrow_forwardR lactam or lactone considering as weak acid or weak base and whyarrow_forward
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