(a)
Interpretation:
The abbreviated orbital diagram and number of unpaired electrons in metal ion
Concept introduction:
A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons. The abbreviated electronic configuration of an element depicts the electronic configuration of the elements by making use of noble gas configuration as they have fully-filled electron shells.
(b)
Interpretation:
The abbreviated orbital diagram and number of unpaired electrons in metal ion
Concept introduction:
A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons. The abbreviated electronic configuration of an element depicts the electronic configuration of the elements by making use of noble gas configuration as they have fully-filled electron shells.
(c)
Interpretation:
The abbreviated orbital diagram and number of unpaired electrons in metal ion
Concept introduction:
A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons. The abbreviated electronic configuration of an element depicts the electronic configuration of the elements by making use of noble gas configuration as they have fully-filled electron shells.
(d)
Interpretation:
The abbreviated orbital diagram and number of unpaired electrons in metal ion
Concept introduction:
A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons. The abbreviated electronic configuration of an element depicts the electronic configuration of the elements by making use of noble gas configuration as they have fully-filled electron shells.
(e)
Interpretation:
The abbreviated orbital diagram and number of unpaired electrons in metal ion
Concept introduction:
A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons. The abbreviated electronic configuration of an element depicts the electronic configuration of the elements by making use of noble gas configuration as they have fully-filled electron shells.
Want to see the full answer?
Check out a sample textbook solutionChapter 19 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- 5. What would you predict about the solubilities of beryllium salts and radium salts relative to the other Group IIA metal salts?arrow_forwardWrite the electron configuration for each ion. Determine whether the ion is paramagnetic or diamagnetic based on its electron configuration 1. Fe3+ 2. Br-3. Sn2+ 4. Cr3+ 5. F- show your solutionsarrow_forwardDefine actinidesarrow_forward
- 17. Write the ground state electron configuration for each atom and ion pair. a. Ni, Ni+ c. Y, Y* b. Mn, Mn* d. Ta, Taarrow_forwardPotassium and Sulfide ions are isoelectronic. Explain the term isoelectronic with reference to these ions.arrow_forward<p>When a transition metal atom forms an ion, which electrons are lost first?arrow_forward
- please answerarrow_forwardWhy do Iodine crystals cause carbon tetrachloride solutions to change its colors? And why it (iodine crystals) did not react to the water?arrow_forwardWhich lanthanide has the maximum number of unpairedelectrons in both its atom and 3+ ion? Give the number of un-paired electrons in the atom and ion.arrow_forward
- In the lab, you should have observed that the reactivity of metals increased down a group. Explain how electron shielding contributes to this trend in reactivity. !!arrow_forward1. Which halogen has the highest ionization energy? Explain why. 2. Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.arrow_forwardLanthanide contraction caused the similarities of the radius of the 4d and 5d metals and is responsible for the low reactivity of the 2nd and 3rd transition series.* True or falsearrow_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 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 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 Learning