(a)
Interpretation:
Electron configuration of
Concept introduction:
Electronic distribution of atoms and molecules in atomic or molecular orbital is referred to as electron configuration.
Hund’s rule − For more than two orbitals with same energy, the electron is first filled in all the same energy orbitals and after the filling of all orbitals with 1 electron each, pairing of electron takes place.
(b)
Interpretation:
Electron configuration of
Concept introduction:
Electronic distribution of atoms and molecules in atomic or molecular orbital is referred to as electron configuration.
Hund’s rule − For more than two orbitals with same energy, the electron is first filled in all the same energy orbitals and after the filling of all orbitals with 1 electron each, pairing of electron takes place.
(c)
Interpretation:
Electron configuration of
Concept introduction:
Electronic distribution of atoms and molecules in atomic or molecular orbital is referred to as electron configuration.
Hund’s rule − For more than two orbitals with same energy, the electron is first filled in all the same energy orbitals and after the filling of all orbitals with 1 electron each, pairing of electron takes place.
(d)
Interpretation:
Electron configuration of
Concept introduction:
Electronic distribution of atoms and molecules in atomic or molecular orbital is referred to as electron configuration.
Hund’s rule − For more than two orbitals with same energy, the electron is first filled in all the same energy orbitals and after the filling of all orbitals with 1 electron each, pairing of electron takes place.
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LCPO CHEMISTRY W/MODIFIED MASTERING
- The orbital occupancies for the d orbitals of several com-plex ions are diagrammed below. (a) Which diagram corresponds to the orbital occupancy of thecobalt ion in [Co(CN)₆]³⁻? (b) If diagram D depicts the orbital occupancy of the cobalt ionin [CoF₆]ⁿ, what is the value of n? (c) [NiCl₄]²⁻ is paramagnetic and [Ni(CN)₄]²⁻ is diamagnetic.Which diagrams correspond to the orbital occupancies of thenickel ions in these species? (d) Diagram C shows the orbital occupancy of V²⁺ in the octa-hedral complex VL₆. Can you determine whether L is a strong-or weak-field ligand? Explain.arrow_forwardOne of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?arrow_forward2. Predict whether each of the following oxides is ionic or molecular? (a) SnO2 (b) Al½O3 (c) CO2 (d) Li¿Oarrow_forward
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- Give the oxidation state of the metal for each of the following oxides of the first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than oneoxidation state. It is possible to write these compound formulas in the equivalent format MO∙M2O3, to permit estimation of the metal’s two oxidation states.)(a) Sc2O3(b) TiO2(c) V2O5(d) CrO3(e) MnO2(f) Fe3O4(g) Co3O4(h) NiO(i) Cu2Oarrow_forwardHow many electrons are in the valence d orbitals in these transition-metal ions? (a) Co3+arrow_forward(c) Give the ground-state electron configuration for each of following substances: (1) Phosphorus (ii) Cr(II) ion (iii) Sulfide ion (iv) Ti(IV) ionarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning