Concept explainers
(a)
Interpretation:
Well labeled molecular energy level diagram 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
2. For atomic number more than 14 order of energy is,
(b)
Interpretation:
Molecular energy level diagram of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Whether electrons have higher probability to exist at oxygen or nitrogen orbital has to be determined.
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forward(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .arrow_forwardThere are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.arrow_forward
- If the dipole moment of a diatomic molecule is found to be 1.04 D, and its bond length is found to be 124 pm, what is the fractional charge on the atoms of the molecule in Coulombs (C)?arrow_forwardDescribe the structure of a P2 molecule in valence-bond terms. Why is P4 a more stable form of molecular phosphorus than P2?arrow_forward1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_forward
- From their Lewis structures, determine the number of sand π bonds in each of the following molecules or ions:(a) CO2; (b) cyanogen,(CN2); (c) formaldehyde, H2CO;(d) formic acid, HCOOH, which has one H and two O atomsattached to C.arrow_forward(a) What is the physical basis for the VSEPR model?(b) When applying the VSEPR model, we count a double ortriple bond as a single electron domain. Why is this justified?arrow_forwardWhat are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(a) ClF5(b) ClO2−(c) TeCl42−(d) PCl3(e) SeF4(f) PH2−arrow_forward
- The Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forward(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forward(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a π*2p molecular orbital, or (iii) The π*2pMO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning