The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified. Concept Introduction: Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot. Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model. Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals. Ø Lone-pair electrons are valence electrons that are not used in bonding. Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion. Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons). Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

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Answer 1

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Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

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Use the Henderson-Hasselbalch equation to calculate pH of a buffer containing 0.050M benzoic acidand 0.150M sodium benzoate. The Ka of benzoic acid is 6.5 x 10-5

Answer 2

Question

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

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Answer 3

Question

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

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Answer 4

Question

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

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Answer 5

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Answer 6

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Answer 7

Chapter 3.8, Problem 3.23YT

Interpretation Introduction

Interpretation:

The given equation has to be rewritten using Lewis structure; all the free radicals present have to be identified.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.

Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.

Ø Lone-pair electrons are valence electrons that are not used in bonding.

Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Answer 8

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Answer 10

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Answer 11

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Solution Summary: The author explains Lewis structure, which satisfies the octet rule of valence electrons and lone pairs in a molecule.

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