Concept explainers
(a)
Interpretation:
The expected ground-state electron configuration and number of unpaired electrons in
Concept Introduction:
In
The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same
(b)
Interpretation:
The expected ground-state electron configuration and number of unpaired electrons in
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The expected ground-state electron configuration and number of unpaired electrons in
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The expected ground-state electron configuration in
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
- Describe the structure of a P2 molecule in valence-bond terms. Why is P4 a more stable form of molecular phosphorus than P2?arrow_forwardWhich type(s) of isomerism could [Ni(NH3)4(NO2)2]SO4 exhibit?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
- how would I identify which of these Lewis structures (A, B, C or D) is correct for PO33- and what is the VSEPR shape of the compound?arrow_forwardWrite the ground-state electron configuration of O2 and calculate the bond order.arrow_forwardDraw the Lewis structures of cyanate (OCN-) and fulminate (CNO-) ions and calculate their formal charges. Discuss their stability by giving resonance structures.arrow_forward
- Write a Lewis structure for the amide ion, NH2─, and assign formal charges to each atom.arrow_forwardWhich 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_forwardGive two requirements that should be satisfied for a molecule to be polar. Explain why CF4 and XeF4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has a net dipole moment). Is CO2 polar? What about COS? Explain.arrow_forward
- For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. SO2 b. SO3 c. d. e. SO32 f. SO42 g. SF2 h. SF4 i. SF6 j. F3SSF k. SF5+arrow_forwardThe cations O2+ and N2+ are formed when molecules of O2 and N2 are subjected to intense, high-energy solar radiation in Earths upper atmosphere. Write the electron configuration for O2+. Predict its bond order and magnetic behavior.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningGeneral 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 LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning