The electronic configuration for the given ions should be determined. Concept Introduction: Periodic Table: The available chemical elements are arranged considering their atomic number , the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table. In periodic table the horizontal rows are called periods and the vertical column are called group. There are seven periods and 18 groups present in the table and some of those groups are given special name as follows, Group-1 → Alkali metal Group-2 → Alkaline metals Group-16 → Chalcogens Group-17 → Halogens Group-18 → Noble gases Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z . The superscript presents on the left side of the symbol of the element. Cation: Removal of electron from the atom results to form positively charged ion called cation. Anion: Addition of electron to atom results to form negatively charged ion called anion. The net charge present in the element denotes the presence or absence of electrons in the element. Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom. The rules followed by the electrons are as follows, The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital( Aufbau principle) , pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled ( Hund’s Rule ) and finally, no two electrons that have same set of quantum numbers ( Pauli’s Exclusion Principle ).

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Answer 1

Question

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

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1. Consider the following molecular-level diagrams of a titration. O-HA molecule -Aion °° о ° (a) о (b) (c) (d) a. Which diagram best illustrates the microscopic representation for the EQUIVALENCE POINT in a titration of a weak acid (HA) with sodium. hydroxide? (e)

Answers to the remaining 6 questions will be hand-drawn on paper and submitted as a single file upload below: Review of this week's reaction: H₂NCN (cyanamide) + CH3NHCH2COOH (sarcosine) + NaCl, NH4OH, H₂O ---> H₂NC(=NH)N(CH3)CH2COOH (creatine) Q7. Draw by hand the reaction of creatine synthesis listed above using line structures without showing the Cs and some of the Hs, but include the lone pairs of electrons wherever they apply. (4 pts) Q8. Considering the Zwitterion form of an amino acid, draw the Zwitterion form of Creatine. (2 pts) Q9. Explain with drawing why the C-N bond shown in creatine structure below can or cannot rotate. (3 pts) NH2(C=NH)-N(CH)CH2COOH This bond Q10. Draw two tautomers of creatine using line structures. (Note: this question is valid because problem Q9 is valid). (4 pts) Q11. Mechanism. After seeing and understanding the mechanism of creatine synthesis, students should be ready to understand the first half of one of the Grignard reactions presented in a past…

Propose a synthesis pathway for the following transformations. b) c) d)

Answer 2

Question

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

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Answer 3

Question

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

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Answer 4

Question

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

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See solution

Answer 5

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 6

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 7

Chapter 4.5, Problem 8PPA

(a)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 8

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 9

(b)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 10

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 11

(c)

Interpretation Introduction

Interpretation: The electronic configuration for the given ions should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

Electronic configuration: It is used to represent the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

Answer 12

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Answer 13

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Answer 15

Ch. 4.1 - Prob. 4.1WE Ch. 4.1 - Prob. 1PPA Ch. 4.1 - Prob. 1PPB Ch. 4.1 - Prob. 1PPC Ch. 4.1 - Prob. 4.1.1SR Ch. 4.1 - Prob. 4.1.2SR Ch. 4.1 - Prob. 4.1.3SR Ch. 4.2 - Prob. 4.2WE Ch. 4.2 - Without using a periodic table, give the...Ch. 4.2 - Identify the elements represented by (a)...

Solution Summary: The author explains that the electronic configuration for the given ions should be determined.

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