Concept explainers
(a)
Interpretation:
The electronic configuration for metal ion
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. While writing the electronic configuration, it is assumed that atom is present in its isolated gaseous state. Electrons are filled in order of the increasing energies of the various sublevels.
Answer to Problem 32QAP
The electronic configuration for Cd2+ is
Explanation of Solution
Cadmium is a 4d
When it two electrons this leads to the formation of Cd2+ cation, and its electronic configuration becomes:
This filling of electrons in the atomic orbitals takes place according to the Aufbau principal which states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
(b)
Interpretation:
The electronic configuration for metal ion
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel.When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. While writing the electronic configuration, it is assumed that atom is present in its isolated gaseous state. Electrons are filled in order of the increasing energies of the various sublevels.
Atomic number of an element gives the total number of electrons present in an atom. In case of transition metal cations, the electrons that are present beyond the noble gas are located in their inner d- orbitals (3d orbitals in case of 3d transition metal elements), this means that they have no outer s- electrons and the distribution of electrons is according to Hund’s rule which states that when orbitals of equal energy are available, then electrons enter singly in the respective orbitals, this gives rise to maximum number of unpaired electrons in transition metal cations.
Answer to Problem 32QAP
The electronic configuration for Fe2+ is
Explanation of Solution
Iron is a 3d transition metal element and its atomic number is 26. Its electronic configuration can be written as follows:
When it two electrons this leads to the formation of Fe2+ cation, and its electronic configuration becomes:
This filling of electrons in the atomic orbitals takes place according to the Aufbau principal. It states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly, lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
(c)
Interpretation:
The electronic configuration for metal ion
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration, one can get details of the number of electrons present in each sublevel. When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. While writing the electronic configuration, it is assumed that atom is present in its isolated gaseous state. Electrons are filled in order of the increasing energies of the various sublevels.
Atomic number of an element gives the total number of electrons present in an atom. In case of transition metal cations, the electrons that are present beyond the noble gas are located in their inner d- orbitals (3d orbitals in case of 3d transition metal elements), this means that they have no outer s- electrons and the distribution of electrons is according to Hund’s rule which states that, when orbitals of equal energy are available, then electrons enter singly in the respective orbitals, this gives rise to maximum number of unpaired electrons in transition metal cations.
Answer to Problem 32QAP
Theelectronic configuration for Pt2+ is
Explanation of Solution
Platinum is a 5d transition metal element and its atomic number is 78. Its electronic configuration can be written as follows:
When it two electrons this leads to the formation of Pt2+ cation, and its electronic configuration becomes:
This filling of electrons in the atomic orbitals takes place according to the Aufbau principal. It states that, when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
(d)
Interpretation:
The electronic configuration for metal ion
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. While writing the electronic configuration, it is assumed that atom is present in its isolated gaseous state. Electrons are filled in order of the increasing energies of the various sublevels.
Atomic number of an element gives the total number of electrons present in an atom. In case of transition metal cations, the electrons that are present beyond the noble gas are located in their inner d- orbitals (3d orbitals in case of 3d transition metal elements), this means that they have no outer s- electrons and the distribution of electrons is according to Hund’s rule. It states that when orbitals of equal energy are available, then electrons enter singly in the respective orbitals, which gives rise to maximum number of unpaired electrons in transition metal cations.
Answer to Problem 32QAP
The electronic configuration forMn2+ is
Explanation of Solution
Manganese is a 3d transition metal element and its atomic number is 25. Its electronic configuration can be written as follows:
When it two electrons this leads to the formation of Mn2+ cation, and its electronic configuration becomes:
This filling of electrons in the atomic orbitals takes place according to the Aufbau principal. It states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly, lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
(e)
Interpretation:
The electronic configuration for metal ion
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration, one can get details of the number of electrons present in each sublevel. When the electronic configuration of an atom is written, it describes the number of electrons present in each sublevel by the superscript. While writing the electronic configuration, it is assumed that atom is present in its isolated gaseous state. Electrons are filled in order of the increasing energies of the various sublevels.
Atomic number of an element gives the total number of electrons present in an atom. In case of transition metal cations, the electrons that are present beyond the noble gas are located in their inner d- orbitals (3d orbitals in case of 3d transition metal elements), this means that they have no outer s- electrons and the distribution of electrons is according to Hund’s rule which states that when orbitals of equal energy are available, then electrons enter singly in the respective orbitals. This gives rise to maximum number of unpaired electrons in transition metal cations.
Answer to Problem 32QAP
The electronic configuration forNi3+ is
Explanation of Solution
Nickel is a 3d transition metal element and its atomic number is 28. Its electronic configuration can be written as follows:
When it three electrons it leads to the formation of Ni3+ cation, and its electronic configuration becomes:
This filling of electrons in the atomic orbitals takes place according to the Aufbau principal. It states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly, lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
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Chapter 19 Solutions
Chemistry: Principles and Reactions
- Please don't provide handwriting solutionarrow_forwardAssign reasons for each of the following :(i) Transition metals generally form coloured compounds.(ii) Manganese exhibits the highest oxidation state of +7 among the 3d series of transition elements.arrow_forwardWrite the ground state electronic configurations for: (a) Ca²+ (b) Cu (c) Crarrow_forward
- (a) What are the central metal ions in chlorophyll, heme,and vitamin B₁₂? (b) What similarity in structure do these com-pounds have?arrow_forwardWrite the electron configurations for each of the following elements and its ions:(a) Ti(b) Ti2+(c) Ti3+(d) Ti4+arrow_forwardFor each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # Unpaired Weak field # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd 2(d) Ni2 + (e) Co2 +arrow_forward
- For 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_forwardAre compounds of these ground-state ions paramagnetic?(a) Ti²⁺(b) Zn²⁺(c) Ca²⁺(d) Sn²⁺arrow_forwardHow many electrons are in the valence d orbitals in these transition-metal ions? (a) Cd2+arrow_forward
- (a) What is a coordinate covalent bond?(b) Is it involved when FeCl3 dissolves in water? Explain.(c) Is it involved when HCl gas dissolves in water? Explain.arrow_forwardIn the compound Pt(C2H3O2)2, what is the charge on the platinum?arrow_forwardWhat is the correct IUPAC name for a compound with the formula K2[Pt(CN)6]? (A) Potassium hexacyanoplatium(II) (B) Potassium hexacyanoplatinate(II) (C) Potassium hexacyanoplatinate(IV) (D) Potassium hexacyanoplatinum(IV)arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning