Ground state electronic configurations of P 3 − ion has to be written using Hund’s rule. Concept Introduction: Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

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Answer 1

Question

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

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Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 1.3 × 10 4: Cl2(g) + CHCl3(g) HCl(g) + CC₁(g) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.6 mol of HCI and 1.6 mol of CCl4. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little Cl2 and CHCl3. ☐ x10 There will be very little HCI and CCl4. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. HCl(g)+CC14(g) 12 Cl2(9)+CHCl3(9) K = 0 ☐ What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 Cl₂(9)+2CHCl3(9) 2 HCl(9)+2CC₁₁(9) K = ✓ 00. 18 Ar

Answer 2

Question

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

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Answer 3

Question

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

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Answer 4

Question

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

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Answer 5

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 6

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

Answer 7

Chapter 5, Problem 5.35P

(a)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of P3− ion has to be written using Hund’s rule.

Concept Introduction:

Each orbital has two electrons and they both are in opposite spin. Electrons are filled up in the orbitals of a sub-shell by following Hund’s rule. This rule tells that all the orbitals are singly filled in a sub-shell and then the pairing occurs.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 12

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 13

(d)

Interpretation Introduction

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 5 - Prob. 5.1P Ch. 5 - Prob. 5.2P Ch. 5 - Prob. 5.3P Ch. 5 - Prob. 5.4P Ch. 5 - Prob. 5.5P Ch. 5 - Prob. 5.7P Ch. 5 - Prob. 5.8P Ch. 5 - Prob. 5.9P Ch. 5 - Prob. 5.10P Ch. 5 - Prob. 5.11P

Concept explainers

Videos

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

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Chapter 5 Solutions

Concept explainers

Videos

Interpretation: Ground state electronic configurations of Br− ion has to be written using Hund’s rule. Concept Introduction: Refer part (a).

Interpretation: Ground state electronic configurations of Se2− ion has to be written using Hund’s rule. Concept Introduction: Refer part (a).

Interpretation: Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule. Concept Introduction: Refer part (a).

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Chapter 5 Solutions

Interpretation:

Ground state electronic configurations of Br− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Interpretation:

Ground state electronic configurations of Se2− ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).

Interpretation:

Ground state electronic configurations of Ba2+ ion has to be written using Hund’s rule.

Concept Introduction:

Refer part (a).