(a)
Interpretation:
The
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.
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
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The
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
- Mixing SbCl3 and GaCl3 in a 1:1 molar ratio using liquid sulfur dioxide as a solvent gives a solidionic compound with the empirical formula GaSbCl6. A controversy arose over whether this compoundis [SbCl2]+[GaCl4]− or [GaCl2]+[SbCl4]−.(a) Predict the molecular structure of the two anions from the two choices using VSEPR theory.(b) It is learned that the cation in the compound has a bent structure. Based on this fact, whichformulation is the correct one?arrow_forwardWrite electron configurations for the following ions. Ru3+ As3- Y3+ Pd2+arrow_forwardDefine the following phenomena with reference to main group compounds: (d) multicenter electron deficient bondingarrow_forward
- Write the electron configuration for each of the following ions and determine which one possess noble-gas configurations: (a) Sr2+; (b) Ti2+; (c) Se2-; (d) Ni2+; (e) Br-; (f) Mn3+.arrow_forwardWhich member of each pair has more covalentcharacter inits bonds: (a) LiCl or KCl; (b) AlCl₃ or PCl₃; (c) NCl₃ or AsCl₃?arrow_forwardWhat is the ground state electron configuration of a Co²+ ion? O1s22s22p 3s³3p64s²3d5 O 1s22s²2p 3s³3p63d7 O 1s22s22p 3s 3p 4s²3d7 O1s²2s22p 3s³3p64s¹3d6arrow_forward
- [Ne]3s²3p* is the noble gas configuration of oxygen O Sulphur O nitrogen carbonarrow_forward1- Give the electron configurations for the following ions? Al * (Z=13) Fe* (Z=26) and 2- Calculate the number of covalent bonds of Fluorine (F), Z of F equal (9)?arrow_forwardThree biologically Important diatomic species,either because they promote or inhibit life, are (a) CO, (b) NO, and (c) CN−. The first binds to hemoglobin, the second is a chemical messenger, and the third interrupts the respiratory electron transfer chain. Their biochemical action is a reflection of their orbital structure. Deduce their ground-state electron configurations using sigma and pi. (Draw MO)arrow_forward
- Determine the average Cl-F bond energy, in units of kJ mol¯, in CIF5, using t following data: • Cl2(g) + 5 F2(g) → 2 CIF5(g) A,H° = -477 kJ mol-1 159 kJ mol-1 • bond energy F-F: • bond energy Cl-Cl: 243 kJ mol-1arrow_forwardN2 and CN' are both isoelectronic. (i) Draw the molecular orbital diagram for N2 and CN molecules. (ii) Explain why CN is a toxic substance but N2 isn't. (iii) N2(g) is an inert gas that is suitable for a wide range of application. Would you expect N2" to be a stable diatomic species in the gaseous state? Explain your answer.arrow_forwardThree biologically Important diatomic species,either because they promote or inhibit life, are (a) CO, (b) NO, and (c) CN−. The first binds to hemoglobin, the second is a chemical messenger, and the third interrupts the respiratory electron transfer chain. Their biochemical action is a reflection of their orbital structure. Deduce their ground-state electron configurations using sigma and pi. (Draw MO). Show how you get electron configuration below using MO?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY