(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: Principles and Reactions
- The inert-pair effect is sometimes used to explain the tendency of heavier members of Group 3A (13) to exhibit +1 and +3 oxidation states. What does the inert-pair effect reference? [Hint: Consider the valence electron configuration for Group 3A (13) elements.]arrow_forward25) Which nonradioactive group I metal would be the most reactive in water and why? A) Cesium would be the most reactive group I metal in water because it's one valence electron is the closest to the nucleus compared to the other metals. B) Cesium would be the most reactive group I metal in water because it's one valence electron is the farthest from the nucleus compared to the other metals. C) Cesium would be the most reactive group I metal in water because it has only one valence electron. 26) Which of the following elements have a tendency to gain electrons? A) N, O, AI B) CI, O, F C) CI, F, Gaarrow_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
- 5. What would you predict about the solubilities of beryllium salts and radium salts relative to the other Group IIA metal salts?arrow_forwardThe electron configuration of a Cr 3+ ion is [Ar]4s23d4. [Ar]4s13d2. [Ar]3d5. [Ar]3d3. [Ar]4s13d5.arrow_forwardWhy do Iodine crystals cause carbon tetrachloride solutions to change its colors? And why it (iodine crystals) did not react to the water?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_forwardDo the alkaline earth metals tend to gain or lose electrons in chemical reactions? How many?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_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 LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning