The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum. Concept introduction: The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength. The position of the peak in the spectrum, called λ max , is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital. The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Question

Want to see the full answer?

Answer 1

Question

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

( solve with explanation ) if u hv already answered plz do not answer , do not copy from here and there

How many signals would be in a CNMR AND HNMR for this product? Please explain in depth.

Based on the picture below what is the: Number of signals, and the parts of sheding and spliting?

Answer 2

Question

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Answer 6

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Answer 7

Chapter 15, Problem 15.3P

Interpretation Introduction

Interpretation:

The approximate energy difference between the HOMO and LUMO is to be calculated from the given UV-vis spectrum.

Concept introduction:

The UV-vis spectrum of a is a plot of relative absorbance as a function of the wavelength.

The position of the peak in the spectrum, called λmax, is the wavelength at which the absorbance reaches a local maximum. This is the wavelength of the photon that is absorbed by the active molecule and corresponds to the transition of an electron from its ground state to an empty higher energy orbital.

The transition of an electron from the HOMO to the LUMO requires the least energy of all possible electron transitions on that molecule. This is because an electron in the HOMO has the highest energy of all electrons in the ground state, and the LUMO is the lowest energy empty orbital available. This energy then corresponds to the longest wavelength band (or peak) in the UV-vis spectrum.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 15 - Prob. 15.1P Ch. 15 - Prob. 15.2P Ch. 15 - Prob. 15.3P Ch. 15 - Prob. 15.4P Ch. 15 - Prob. 15.5P Ch. 15 - Prob. 15.6P Ch. 15 - Prob. 15.7P Ch. 15 - Prob. 15.8P Ch. 15 - Prob. 15.9P Ch. 15 - Prob. 15.10P

Solution Summary: The author calculates the approximate energy difference between the HOMO and LUMO from the given UV-vis spectrum.

Want to see the full answer?

Chapter 15 Solutions