The ground-state electronic configuration of P 2 − has to be determined. Concept Introduction: The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is n s 1 − 2 , that of p block elements is n s 2 n p 1 − 6 , that of d − block elements is ( n − 1 ) d 1 − 10 n s 0 − 2 and that of f block elements is ( n − 2 ) f 1 − 14 ( n − 1 ) d 0 − 10 n s 2 . Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows: 1 s < 2 s < 2 p < 3 s < 3 p < 4 s < 3 d < 4 p < 5 s < 4 d < 5 p < 6 s < 4 f < 5 d < 6 p < 7 s Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

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Answer 1

Question

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 2

Question

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

Answer 7

Chapter 8, Problem 8.31QE

(a)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of P2− has to be determined.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d−block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 8 - Define an isoelectronic series. Give the symbols...Ch. 8 - Prob. 8.2QE Ch. 8 - Graph the atomic radii versus atomic number of the...Ch. 8 - Prob. 8.4QE Ch. 8 - Prob. 8.5QE Ch. 8 - Prob. 8.6QE Ch. 8 - Prob. 8.7QE Ch. 8 - Prob. 8.8QE Ch. 8 - Prob. 8.9QE Ch. 8 - Prob. 8.10QE

Solution Summary: The author explains how the ground-state electronic configuration of P2- has to be determined.

Videos

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).

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Chapter 8 Solutions

Solution Summary: The author explains how the ground-state electronic configuration of P2- has to be determined.

Videos

Interpretation: The ground-state electronic configuration of Fe2+ has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The ground-state electronic configuration of Co3+ has to be determined. Concept Introduction: Refer to part (a).

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Chapter 8 Solutions

Interpretation:

The ground-state electronic configuration of Fe2+ has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The ground-state electronic configuration of Co3+ has to be determined.

Concept Introduction:

Refer to part (a).