Concept explainers
(a)
Interpretation:
The ground-state electronic configuration of isoelectronic
Concept Introduction:
The fundamental principles that are followed to write an electronic configuration include three rules as follows:
Electron in a
Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.
Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.
(b)
Interpretation:
Number of unpaired electrons in
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Neutral atom that has the same electron configuration as
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemical Principles: The Quest for Insight
- Which of the following represent configurations of indium ions in compounds? Explain your decision in each ease. a In4+ [Kr]4d9 b In+ [Kr]4d10 5s2 c In3+ [Kr]4d10 d In [Kr]4d10 5s1arrow_forwardSeveral Lewis structures can be written for perbromate ion, , the central Br with all single Br—O bonds, or with one, two, or three Br=O double bonds. Draw the Lewis structures of these possible resonance structures, and use formal charges to predict which makes the greatest contribution to the resonance hybrid.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
- Would you expect BrF3 to be as reactive with LiF(s) as it is with CsF(s)? Why (not)?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_forwardPredict the ordering, from shortest to longest, of the bondlengths in CO, CO2, and CO32 - .arrow_forward
- What is the resonance form that describes the distribution of electrons in SeO2 ?arrow_forward1) Which of the following elements are capable of forming compounds in which the indicated atom can have more than 4 valence e- pairs? In each case, explain why and why not.arrow_forwardAlthough the peroxide ion, O22-, and the acetylide ion, C22-, have long been known, the diazenide ion N22- has only been prepared much more recently. By comparison with the other diatomic species, predict the bond order, bond distance, and number of unpaired electrons for N22-.arrow_forward
- What are the hybridizations of nitrogen in NF3 and NH3 respectively?arrow_forwardHigh-resolution photoelectron spectroscopy has provided information on the energy levels and bond distance in the ion. Prepare a molecular orbital energy level diagram for this ion Ar2+. How would you expect the bond distance in to compare with 198.8 pm, the bond distance in Cl2arrow_forwardIt 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
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher: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 LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning