The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid. Concept introduction: The rules for the allowed quantum numbers combinations are as follows: All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers. The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on. The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2. The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2 For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell. Here, for s orbital value of l = 0 , for p orbital it is l = 1 , for d orbital it is l = 2 and for f it is 3. The relative energy of orbitals is represented as follows: A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

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Answer 1

Question

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

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Answer 2

Question

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

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Answer 3

Question

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

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Answer 4

Question

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

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Answer 5

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

Answer 6

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

Answer 7

Chapter 5, Problem 107APP

(a)

Interpretation Introduction

Interpretation: The elements with the given electronic configuration should be identified as a metal, non-metal or metalloid.

Concept introduction: The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be either -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

A s orbital can have maximum of 2 electrons, p orbital can have maximum of 6 electrons. Similarly, maximum electrons that a d and f orbital can have are 10 and 14 respectively.

Answer 8

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

Answer 9

(b)

Interpretation Introduction

Interpretation: The element with the largest atomic size should be identified.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

Answer 10

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

Answer 11

(c)

Interpretation Introduction

Interpretation: The element with the highest ionization energy should be identified.

Concept Introduction: Ionization energy is defined as the amount of energy required to remove an electron from its outermost shell. According to periodic trends, it decreases on moving top to bottom in a group due to increase in size and it increases on moving left to right in a period due to decrease in size.

Answer 12

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

Answer 13

(d)

Interpretation Introduction

Interpretation: The element with the smallest atomic size.

Concept Introduction: According to the periodic trends, the atomic size of the element increases on moving top to bottom in a group due to addition of one shell and decreases on moving left to right in a group due to increase in atomic number.

Answer 14

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Answer 16

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Answer 17

Ch. 5.1 - What is meant by the wavelength of UV light?Ch. 5.1 - How are the wavelength and frequency of light...Ch. 5.1 - What is the difference between "white” light and...Ch. 5.1 - Prob. 4PP Ch. 5.1 - Ultraviolet radiation (UVB) used to treat...Ch. 5.1 - AM radio waves have a frequency of 8105s1, whereas...Ch. 5.1 - If orange light has a wavelength of 6105cm, what...Ch. 5.1 - A wavelength of 850 nm is used for fiber-optic...Ch. 5.1 - Prob. 9PP Ch. 5.1 - Prob. 10PP

Solution Summary: The author explains that the three quantum numbers (n, l, and m) describe the orbital of an atom and they are integers.

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