Concept explainers
(a)
Interpretation:
Valence shell electronic configuration and bond order of
Concept Introduction:
Molecular orbital diagram is a linear combination of atomic orbitals of similar energy and similar symmetry. It is formed by the proper overlap of the atomic orbitals.
There are 3 types of molecular orbitals as follows:
- 1. Bonding molecular orbital: They are formed by the constructive interference of atomic orbitals and electrons in it stabilize the molecule and are of lesser in energy.
- 2. Antibonding molecular orbital: This type of orbitals increases the energy of molecule and destabilizes it and weakens the bond between the atoms.
- 3. Non-bonding molecular orbital: These types of orbitals have energy similar to atomic orbitals that is addition or removal of electron does not change the energy of molecule.
The order of energy in molecular orbital follows two rules as follows:
- 1. For
atomic number less than or equal to 14 order of energy is,
- 2. For atomic number more than 14 order of energy is,
Bond order
(a)
Explanation of Solution
The symbol for oxygen is
Two negative charges are added to the total valence count.
Thus total valence electrons are sum of the valence electrons for each atom in
Hence, 14 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since, number of electrons in
Substitute 8 for number of electrons in bonding orbitals and 6 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.
Hence, the bond order of the molecule
(b)
Interpretation:
Valence shell electronic configuration and bond order of
Concept Introduction:
Refer to part (a).
(b)
Explanation of Solution
The symbol for nitrogen is
One negative charge is added to the total valence count.
Thus total valence electrons are sum of the valence electrons for each atom in
Hence, 11 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since, number of electrons in
Substitute 8 for number of electrons in bonding orbitals and 3 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.
Hence, the bond order of the molecule
(c)
Interpretation:
Electronic configuration and bond order of
Concept Introduction:
Refer to part (a).
(c)
Explanation of Solution
For
The symbol for carbon is
One negative charge is added to the total valence count.
Thus total valence electrons are sum of the valence electrons for each atom in
Hence, 9 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since, number of electrons in
Substitute 7 for number of electrons in bonding orbitals and 2 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.
Hence, the bond order of the molecule
Want to see more full solutions like this?
Chapter 2 Solutions
Chemical Principles: The Quest for Insight
- Describe the structure of a P2 molecule in valence-bond terms. Why is P4 a more stable form of molecular phosphorus than P2?arrow_forwardGive the ground-state electron configurations and bond orders of(i) Li2, (ii) Be2, and (iii) C2.arrow_forwardWhat are the favored geometrical arrangements for ABn molecules for which the A atom has 2, 3, 4, 5, and 6 pairs of electrons in its valence shell?arrow_forward
- Predict the ordering of the C—O bond lengths in CO, CO2, and CO32-arrow_forwardWhat is the molecular orbital diagram for CO^2+ and N2^-1? Are they diamagnetic or paramagnetic? Do they have unpaired electrons?arrow_forwardDraw the Lewis structure of HClO₃ (with minimized formal charges) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning