The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained. 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. 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. Atomic radius: Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary. The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table. Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus. Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus. To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Question

Want to see the full answer?

Answer 1

Question

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

what is the drawn mechanism for diethyl carbonate and 4 - bromo - N, N -dimethylaniline to create crystal violet?

Which of the following compounds are constitutional isomers of each other? I and II O II and III O III and IV OI and IV O II and IV CI H CI H CI H H CI H-C-C-CI C-C-C-CI H-C-C-CI H-C-C-CI H CI Ĥ ĆI A A Ĥ ĆI || IV

Please correct answer and don't used hand raiting

Answer 2

Question

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Answer 6

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

Answer 7

Chapter 4, Problem 4.115QP

Interpretation Introduction

Interpretation:

The effective nuclear charge of 4-p electrons in gallium is 6.22 irrespective of the 18 additional electrons with it and the deviation should be explained.

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.

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.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

The atomic size follow the regular trend that it gets decreases as we move from left to right of the table and gets increases as we go from top to bottom of the table.

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus.

Effective nuclear charge: It is the charge experienced by the valence electrons from the nucleus.

To determine: The reason for less effective nuclear charge for the gallium atom irrespective of electrons present in it.

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. 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)...

Videos

Want to see the full answer?

Chapter 4 Solutions