‘Energy state’ should be identified. Concept introduction: The electron jumps from n=1 to n=2 is called the 1 s t excitation and n=2 to n=3 is 2 n d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom. The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ ¯ = R [ 1 n 1 2 − 1 n 2 2 ] . Given: The wave length ( λ ) of the UV light is 1.03 × 10 − 7 m . The initial shell from which the electron jumps i.e. n 1 = 1 To determine: On absorption of ultra violet light at the ground state of wave length 1.03 × 10 − 7 m the position of the electron.

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Answer 1

Question

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

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Answer 2

Question

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Expert Solution & Answer

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See solution

Answer 3

Question

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Expert Solution & Answer

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Answer 4

Question

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Expert Solution & Answer

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Answer 5

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Answer 6

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Answer 7

Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^s^t excitation and n=2 to n=3 is 2ⁿ^d excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is υ¯=R[1n12−1n22].

Given:

The wave length ( λ ) of the UV light is 1.03×10−7m. The initial shell from which the electron jumps i.e. n1 = 1

To determine:

On absorption of ultra violet light at the ground state of wave length 1.03×10−7m the position of the electron.

Answer 8

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Answer 9

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Answer 10

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Answer 11

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