The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name. Concept introduction: The fundamentals of Lewis formula or Lewis structure can be described as: 1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge. 2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood. 3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

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Answer 1

Question

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

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#1. Retro-Electrochemical Reaction: A ring has been made, but the light is causing the molecule to un- cyclize. Undo the ring into all possible molecules. (2pts, no partial credit) hv

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I have a question about this problem involving mechanisms and drawing curved arrows for acids and bases. I know we need to identify the nucleophile and electrophile, but are there different types of reactions? For instance, what about Grignard reagents and other types that I might not be familiar with? Can you help me with this? I want to identify the names of the mechanisms for problems 1-14, such as Gilman reagents and others. Are they all the same? Also, could you rewrite it so I can better understand? The handwriting is pretty cluttered. Additionally, I need to label the nucleophile and electrophile, but my main concern is whether those reactions differ, like the "Brønsted-Lowry acid-base mechanism, Lewis acid-base mechanism, acid-catalyzed mechanisms, acid-catalyzed reactions, base-catalyzed reactions, nucleophilic substitution mechanisms (SN1 and SN2), elimination reactions (E1 and E2), organometallic mechanisms, and so forth."

Answer 2

Question

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

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Answer 3

Question

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

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Answer 4

Question

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

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Answer 5

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 6

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 7

Chapter 4, Problem 1CGP

(a)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given ion has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The Lewis formula or structure of the given molecule has to determine with a comparison between the earlier name and final name.

Concept introduction:

The fundamentals of Lewis formula or Lewis structure can be described as:

1. The valence electron provided by the atom have to add. For a negatively charged ion, an electron has to add for per negative charge. Similarly, for a positively charged species, one electron have to subtract for each positive charge.

2. Usually, the larger atom or the less electronegative atom is the central atom of a species. The chemical symbols of the atoms to show their relative neighborhood.

3. One pair of the electron has to place between each pair of bonded atoms. The two electrons will be equally shared by the two atoms. Then more pair of an electron can be supplied for form multiple bonds or to provide lone pairs until each atom has its octet (doublet for hydrogen). The bond pairs may also be replaced by a single line.

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 4 - Prob. 1RQ Ch. 4 - Prob. 2RQ Ch. 4 - What are the structural differences among chlorine...Ch. 4 - Prob. 4RQ Ch. 4 - What are the charges on simple ions formed from...Ch. 4 - Prob. 6RQ Ch. 4 - In what group of the periodic table would elements...Ch. 4 - Prob. 8RQ Ch. 4 - Prob. 9RQ Ch. 4 - Prob. 10P

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