The expected ground-state electron configuration in Zr 4 + should be given. Concept Introduction: The fundamental principles that are followed to write an electronic configuration include three rules as follows: Electron in a s orbital is relatively low in energy than a p x electron because the s orbital is in nearer vicinity of nucleus than p x orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows: Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron. Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital. In chemical reactions , only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [ He ] 2s 2 2p 3 . The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

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Answer 1

Question

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

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Answer 2

Question

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

Answer 7

Chapter 2, Problem 2A.6E

(a)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration in Zr4+ should be given.

Concept Introduction:

The fundamental principles that are followed to write an electronic configuration include three rules as follows:

Electron in a s orbital is relatively low in energy than a px electron because the s orbital is in nearer vicinity of nucleus than px orbital. This is basis of Aufbau rule that suggests electrons occupy orbitals in order so that lowest energy orbital gets filled first. For instance the order is illustrated as follows:

Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.

Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers. Quantum-mechanical equivalent for this state means that two electrons are not allowed to have the same space simultaneously. Since one electron may certain discrete same set of n, l and m values, however, the fourth spin quantum number should be different. This provides a unique address to every electron. Since the possible magnitudes of spin can be either +1/2 or -1/2 thus at maximum two electrons can occupy any given orbital.

In chemical reactions, only outer electrons are involved thus the electronic configuration is simplified when the core electrons are represented by the closest noble gases followed by valence electrons. For instance, nitrogen with atomic number seven is written as [He]2s22p3.

The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same n value, electrons are lost from the subshell with highest l value.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

Answer 12

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

Answer 13

(b)

Interpretation Introduction

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 2 - Prob. 2A.1AST Ch. 2 - Prob. 2A.1BST Ch. 2 - Prob. 2A.2AST Ch. 2 - Prob. 2A.2BST Ch. 2 - Prob. 2A.3AST Ch. 2 - Prob. 2A.3BST Ch. 2 - Prob. 2A.4AST Ch. 2 - Prob. 2A.4BST Ch. 2 - Prob. 2A.1E Ch. 2 - Prob. 2A.2E

Solution Summary: The author explains the basic principles that are followed to write an electronic configuration, including Hund's rule, Pauli Exclusion Principle, and valence electrons.

Videos

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).

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Chapter 2 Solutions

Solution Summary: The author explains the basic principles that are followed to write an electronic configuration, including Hund's rule, Pauli Exclusion Principle, and valence electrons.

Videos

Interpretation: The expected ground-state electron configuration of Os3+ should be given. Concept Introduction: Refer to part (a).

Interpretation: The expected ground-state electron configuration of Cs+ should be given. Concept Introduction: Refer to part (a).

Interpretation: The expected ground-state electron configuration of P3− should be given. Concept Introduction: Refer to part (a).

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Chapter 2 Solutions

Interpretation:

The expected ground-state electron configuration of Os3+ should be given.

Concept Introduction:

Refer to part (a).

Interpretation:

The expected ground-state electron configuration of Cs+ should be given.

Concept Introduction:

Refer to part (a).

Interpretation:

The expected ground-state electron configuration of P3− should be given.

Concept Introduction:

Refer to part (a).