(a)
Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbitals is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- When cation is formed it means the electrons are removed from the outermost orbital of atom. If anion is formed means then the electrons are added to the atom in its outermost orbital.
- For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.
To identify: Ion with net charge of +1 with electronic configuration of
(a)
Answer to Problem 4.75QP
Answer
The ion with a net charge of +3 for (a) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Ion with net charge as +3 with electronic configuration
Argon is a noble gas and has a complete octet electronic configuration as
(b)
Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbitals is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- When cation is formed it means the electrons are removed from the outermost orbital of atom. If anion is formed means then the electrons are added to the atom in its outermost orbital.
- For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.
To identify: Ion with net charge of +3 with electronic configuration of
(b)
Answer to Problem 4.75QP
Answer
The ion with a net charge of +3 for (b) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Ion with net charge as +3 with electronic configuration
Argon is a noble gas and has a complete octet electronic configuration as
(c)
Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbitals is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- When cation is formed it means the electrons are removed from the outermost orbital of atom. If anion is formed means then the electrons are added to the atom in its outermost orbital.
- For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.
To identify: Ion with net charge of +3 with electronic configuration of
(c)
Answer to Problem 4.75QP
Answer
The ion with a net charge of +3 for (c) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Ion with net charge as +3 with electronic configuration
Krypton is a noble gas and has a complete octet electronic configuration as
(d)
Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.
Concept Introduction:
- Electronic configuration is the arrangement of the electrons of atoms in the orbital. For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
- According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
- According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled. When the orbitals is singly filled, all the electrons have same spin. In a doubly filled orbital, there are two electrons with opposite spin.
- When cation is formed it means the electrons are removed from the outermost orbital of atom. If anion is formed means then the electrons are added to the atom in its outermost orbital.
- For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.
To identify: Ion with net charge of +3 with electronic configuration of
(d)
Answer to Problem 4.75QP
Answer
The ion with a net charge of +3 for (d) is
Explanation of Solution
Electronic configuration of
The electronic configuration of
Ion with net charge as +3 with electronic configuration
Xenon is a noble gas and has a complete octet electronic configuration as
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Chapter 4 Solutions
Chemistry: Atoms First
- Use the noble-gas notation and write the ground-state electronic configurations of the following ions:(a) Ca2+ (b) Ga3+ (c) Cr3+arrow_forwardWhat is the electron configuration and orbital diagram of:(a) Na+(b) P3–(c) Al2+ (d) Fe2+(e) Sm3+arrow_forwardWrite the electron configuration and orbital diagram for each ion and predict whether each will be paramagnetic or diamagnetic.(a) Co2+ (b) N3- (c) Ca2+arrow_forward
- Write the ground-state electron configurations of the following ions/transition metal ions.. (a) Li+ (b) N3− (c) In3+ (d) Tl+ (a) Sc3+ (b) Cr3+ (c) Cu+ (d) Au+arrow_forwardWrite the complete electron configuration for each of the following ions (a) Ga3+: (b) Mg2+:arrow_forwardThe Ti2 + ion is isoelectronic with the Ca atom. (a) Write theelectron configurations of Ti2 + and Ca. (b) Calculate thenumber of unpaired electrons for Ca and for Ti2 + . (c) Whatcharge would Ti have to be isoelectronic with Ca2 + ?arrow_forward
- Write the ground-state electron configurations of the following transition metal ions. (a) Sc3+ (b) Cr3+ (c) Cu+ (d) Au+arrow_forwardWhich of these are paramagnetic in their ground state?(a) Ga(b) Si(c) Be(d) Tearrow_forward8.29 Write the ground-state electron configurations of the following transition metal ions: (a) Sc3+, Ti4+, (c) V5+, (d) Cr3+, (e) Fe2+, (f) Fe3+ (b)arrow_forward
- (a) As we go down the periodic table, which subshell is filled first, the 3d or the 4s subshell? (b) Which electronic configuration has a lower energy, [Ar]3d44s2 or [Ar]3d54s1? Note: The notation [Ar] represents the filled configuration for argon. Suggestion: Which has the greater number of unpaired spins? (c) Identify the element with the electronic configuration in part (b).arrow_forwardIdentify each element below, and give the symbols of the other elements in its group: (a) [Ar] 4s23d104p4 (b) [Xe] 6s24f 145d 2 (c) [Ar] 4s23d 5arrow_forwardWrite the electron configurations for the following atoms or ions:(a) B3+(b) O–(c) Cl3+(d) Ca2+(e) Tiarrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning