The Lewis structure of ( CO ) molecule has to be drawn. 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

Question

Chapter 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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.

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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.

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 2

Question

Chapter 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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.

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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.

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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.

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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.

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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.

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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.

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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.

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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.

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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 3.7, Problem 3.19YT

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of (CO) molecule has to be drawn.

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

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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 9

(b)

Interpretation Introduction

Interpretation: The Lewis structure of SO2 molecule should be determined.

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.

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 10

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 11

(c)

Interpretation Introduction

Interpretation: The Lewis structure of SO3 molecule should be determined.

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 12

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Answer 13

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Answer 14

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Answer 15

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Solution Summary: The author explains how the Lewis structure of (CO) molecule is drawn. The octet rule of valence electrons and lone pairs also exist in

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