(a)
Interpretation:
The abbreviated electronic configuration for 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 electronic configuration for 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 electronic configuration for 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 electronic configuration for 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 electronic configuration for 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
- (a) What is the range in electronegativity across the first (3d)transition series? (b) What is the range across Period 4 of main-group elements? (c) Explain the difference.arrow_forwardWhich transition metal atom is present in each of the following biologically important molecules: (a) siderophores, (b) hemocyanine.arrow_forwardThe complexes [V(H2O)6]3+ and [VF6]3- are both known. Which of the two complexes would you expect to absorb light of higher energy?arrow_forward
- 1.) The 3rd ionization energy of Fe is Ei3= +2952kj/mole. What is the longest wavelength of light that could ionize Fe2+ to Fe3+? 2.) What is the mass of K2C2O4 produced using the 12.0g of oxalic acid if the percent yield of the reaction was 87.5%?arrow_forwardDescribe how magnetism in lanthanides series arisesarrow_forward(a) What is the lanthanide contraction? (b) How does it affectatomic size down a group of transition elements? (c) How doesit influence the densities of the Period 6 transition elements?arrow_forward
- Identify the first row transition metal that satisfies the requirements given: [Mn(H2O)6]2+ having two unpaired electrons (list all possibilities). Please provide a step by step explanation.arrow_forwardFor each of the following ions, draw diagrams like thosein Figure 8.18 to show orbital occupancies in both weakand strong octahedral fields. Indicate the total number ofunpaired electrons in each case.(a) Mn2+ (c) Cr3+ (e) Fe2+(b) Zn2+ (d) Mn2+arrow_forwardSuggest why the fluoride compound in which chromium has its highest oxidation state is CrF6 whereas the highest oxidation state chromium has in a chloride is CrCl4arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning