The most likely charge for ion formed from Cs has to be determined. 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 are 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. In case of d-block elements, the ns electrons are removed prior to ( n − 1 ) d electrons.

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Answer 1

Question

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 2

Question

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

Answer 7

Chapter 2, Problem 2A.16E

(a)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Cs has to be determined.

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 are 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. In case of d-block elements, the ns electrons are removed prior to (n−1)d electrons.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

Answer 12

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

Answer 13

(d)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

Answer 14

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

Answer 15

(e)

Interpretation Introduction

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

Answer 16

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Answer 17

Expert Solution & Answer

Answer 18

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Answer 19

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 that electrons in a s orbital are relatively low in energy because they are in nearer vicinity of nucleus.

Concept explainers

Videos

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).

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Chapter 2 Solutions

Solution Summary: The author explains that electrons in a s orbital are relatively low in energy because they are in nearer vicinity of nucleus.

Concept explainers

Videos

Interpretation: The most likely charge for ion formed from O has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The most likely charge for ion formed from Ca has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The most likely charge for ion formed from N has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The most likely charge for ion formed from I has to be determined. Concept Introduction: Refer to part (a).

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Chapter 2 Solutions

Interpretation:

The most likely charge for ion formed from O has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from Ca has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from N has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The most likely charge for ion formed from I has to be determined.

Concept Introduction:

Refer to part (a).