# For an atomic orbital what does the quantum number n and l describes should be given. Concept introduction: Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a) Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b) Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c) Magnetic quantum number is represented by m l and this number indicates the orientation of the orbital. d) Spin quantum number is represented by m s and this number indicates the spin of the electron.

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter 6, Problem 68GQ

(a)

Interpretation Introduction

## Interpretation: For an atomic orbital what does the quantum number n and l describes should be given.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a) Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b) Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c) Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d) Spin quantum number is represented by ms and this number indicates the spin of the electron.

(b)

Interpretation Introduction

### Interpretation: The possible values of l when n = 3 should be determined.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The values of l when the principal quantum number is n are from 0 to (n −1). Each l value indicates subshell.

(c)

Interpretation Introduction

### Interpretation: The type of orbital that corresponds to l = 3 should be determined.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The values of l when the principal quantum number is n are from 0 to (n −1). Each value of l indicates subshell.

(d)

Interpretation Introduction

### Interpretation: The value of n, l and a possible value of ml should be determined.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The principal quantum number and number of subshells are same in a shell.The values of l when the principal quantum number is n are from 0 to (n −1). Each value of l indicates subshell.The values of ml when the orbital angular quantum number is l are from −l to +l.

(e)

Interpretation Introduction

### Interpretation: The appropriate letters, l value and number of planar nodes should be given in the table for the given orbital pictures.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The values of l when the principal quantum number is n are from 0 to (n −1). Each value of l indicates subshell.Nodal surfaces: the surface which passing through nucleus where there is zero chance of finding electrons.

(f)

Interpretation Introduction

### Interpretation: The atomic orbital having three planar nodes through the nucleus should be determined.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.Nodal surfaces: the surface which passing through nucleus where there is zero chance of finding electrons.The values of l when the principal quantum number is n are from 0 to (n −1). Each value of l indicates subshell.

(g)

Interpretation Introduction

### Interpretation: The orbitals that cannot exist according to modern quantum theory should be determined from the given orbitals.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The values of l when the principal quantum number is n are from 0 to (n −1). Each l value indicates subshell

(h)

Interpretation Introduction

### Interpretation: The invalid set of quantum numbers should be determined from the given sets of quantum numbers.Concept introduction:Quantum numbers are numbers, which explains the existence and the behavior of electron in an atom. a. Principle quantum number is represented by n and this number describes the energy of the orbital and the size of an atom. b. Angular momentum quantum number (or azimuthal quantum number) is represented by l and this number indicates the shape of the orbitals. c. Magnetic quantum number is represented by ml and this number indicates the orientation of the orbital. d. Spin quantum number is represented by ms and this number indicates the spin of the electron.The values of l when the principal quantum number is n are from 0 to (n −1). Each l value indicates subshell.The values of ml when the orbital angular quantum number is l are from −l to +l.

(i)

Interpretation Introduction

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