General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
11th Edition
ISBN: 9780134097329
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
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Textbook Question
Chapter 23, Problem 1E

By means of orbital diagrams, write electron configurations for the following transition element atom and ions (a) V ;(b) C r 2 + ; (c) M n 2 + ; (d) F e 2 + ; (e) C u 2 + ; (f) N I 2 + .

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

To write the electronic configuration of V by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:
  2. It states that the electron goes in orbital which has lowest energy.

    The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of V is 1s22s22p63s23p64s23d3

              1s2     2s2         2p6            3s2          3p6            4s2          3d3

Explanation of Solution

The atomic number of Vanadium, V is 23. V is neutral atom, hence the total number of electrons = 23

According to Aufbau principle, the lowest energy orbital is 1s which can have maximum 2 electrons. Next is 2s which has 2 electrons. Similarly, 2p has 6 electrons, 3s has 2 electrons 3p can have 6 electrons, 4s has 2 electrons. So far, total electrons added to orbitals are 20 electrons out of 23. Next comes 3d, it can have 10 electrons maximum but V has only 3 electrons left, which goes in 3d. The orbital diagram of V is:

              1s2     2s2         2p6            3s2          3p6            4s2          3d3

The electronic configuration of V is: 1s22s22p63s23p64s23d3

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

To write the electronic configuration of Cr2+ by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:

    It states that the electron goes in orbital which has lowest energy.

  2. The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of Cr2+ is 1s22s22p63s23p63d4.

            1s2     2s2         2p6            3s2          3p6                     3d4

Explanation of Solution

The atomic number of chromium ion, Cr is 24.

In the electronic configuration of Cr, there is an exception and the electronic configuration is written as: 1s22s22p63s23p64s13d5. Since the 3d5 is more stable configuration ( half filled configuration) than 3d4, one electrons from 4s2 shifts to 3d which makes the configuration 4s1 3d5 instead of 4s2 3d4.

Here, Cr has +2 charge on it, which means 2 electrons have been lost so total electrons present in Cr2+ is 24 − 2 = 22 electrons. The electrons start losing from outermost orbital.

Here, outermost orbital is 4s so it loses one electron and one from 3d.

The orbital diagram is:

            1s2     2s2         2p6            3s2          3p6                     3d4

The electronic configuration of Cr2+ is 1s22s22p63s23p63d4.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

To write the electronic configuration of Mn2+ by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:

    It states that the electron goes in orbital which has lowest energy.

  2. The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of Mn2+ is 1s22s22p63s23p63d5

            1s2     2s2         2p6            3s2          3p6                     3d5

Explanation of Solution

The atomic number of Manganese, Mn is 25.

The electronic configuration of Mn is 1s22s22p63s23p64s23d5.

Here, Mn shows charge of +2 means 2 electrons are lost from outermost orbital, 4d.

Hence, total electrons present in Mn2+ are 23.

            1s2     2s2         2p6            3s2          3p6                     3d5

The electronic configuration of Mn2+ is 1s22s22p63s23p63d5

Expert Solution
Check Mark
Interpretation Introduction

(d)

Interpretation:

To write the electronic configuration of Fe2+ by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:

    It states that the electron goes in orbital which has lowest energy.

  2. The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of Fe2+ is 1s22s22p63s23p63d6.

             1s2     2s2         2p6            3s2          3p6                     3d6

Explanation of Solution

The atomic number of Iron, Fe is 26.

The electronic configuration of Fe is 1s22s22p63s23p64s23d6.

Here, Fe shows charge of +2 means 2 electrons are lost from outermost orbital, 4d.

Hence, total electrons present in Fe2+ are 24.

The orbital diagram of Fe2+ is:

             1s2     2s2         2p6            3s2          3p6                     3d6

The electronic configuration of Fe2+ is 1s22s22p63s23p63d6.

Expert Solution
Check Mark
Interpretation Introduction

(e)

Interpretation:

To write the Electronic configuration of Cu2+ by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:

    It states that the electron goes in orbital which has lowest energy.

  2. The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of Cu2+ is 1s22s22p63s23p63d9.

             1s2     2s2         2p6            3s2          3p6                     3d9

Explanation of Solution

The atomic number of Copper, Cu is 29.

The electronic configuration of Cu is 1s2 2s2 2p6 3s2 3p6 4s1 3d10. Cu shows exception in configuration as 4s1 3d10 instead 4s2 3d9 because 10 electron in 3d orbital is stable configuration so out of 2 electrons, one electron from 4s jumps to 3d leaving 1 electron in 4s and 10 electron in 3d.

Here, Cu shows charge of +2 means 1 electron from outermost 4s and one electron from 3d are lost. Hence, total electrons present in Cu2+ are 27.

             1s2     2s2         2p6            3s2          3p6                     3d9

The orbital diagram of Cu2+ is:

The electronic configuration of Cu2+ is 1s22s22p63s23p63d9.

Expert Solution
Check Mark
Interpretation Introduction

(f)

Interpretation:

To write the electronic configuration of Ni2+ by using orbital diagram.

Concept introduction:

Orbital Diagram: It is pictorial representation of electrons in any atom. It represents shell number “n”, subshell “l” as well as spin of electrons. The orbitals present in subshell are represented by lines or boxes. In one orbital there can be maximum 2 electrons.

Subshell Number of orbitals Number of maximum electrons
s 1 2
p 3 6
d 5 10
f 7 14

The spin of electron is represented by arrows. The up arrow means 1/2 spin and down arrow means - 1/2 spin. There are some rules to fill electrons in these orbitals as:

  1. Aufbau Principle:

    It states that the electron goes in orbital which has lowest energy.

  2. The series of orbital from lowest to highest energy:

    1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 7p 

  3. Pauli’s Exclusion Principle:

    It states that no two electron can have all the same quantum number, that’ why in an orbital, the spin or one electron is up and spin of second electrons is down.

  4. Hund’s Rule:

    It states that each orbital in a subshell is single occupied with one electron before any one electron is occupied double and also the spin of all electrons.

Electronic configuration:

It is notation which shows the distribution of electrons in orbitals of atoms, ion or molecule. The configuration lists the shell by principal quantum number, n= 1,2,3,4…. and subshell by azimuthal quantum number, l = s, p, d, f and electrons that can be present in it. With the help of orbital diagram electronic configuration can be written.

Answer to Problem 1E

The electronic configuration of Ni2+ is 1s22s22p63s23p63d8.

             1s2     2s2         2p6            3s2          3p6                     3d8

Explanation of Solution

The atomic number of Nickel, Ni is 28.

The electronic configuration of Ni is 1s22s22p63s23p64s23d8.

Here, Ni shows charge of +2 means 2 electrons from outermost 4s are lost. Hence total electrons present in Ni2+ are 26.

The orbital diagram of Ni2+ is:

             1s2     2s2         2p6            3s2          3p6                     3d8

The electronic configuration of Ni2+ is 1s22s22p63s23p63d8.

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Chapter 23 Solutions

General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)

Ch. 23 - Complete and balance the following equations. If...Ch. 23 - By means of e chemical equation, give an example...Ch. 23 - Prob. 13ECh. 23 - Prob. 14ECh. 23 - Prob. 15ECh. 23 - Prob. 16ECh. 23 - Prob. 17ECh. 23 - According to Figure 23-8, G decreases with...Ch. 23 - Prob. 19ECh. 23 - Prob. 20ECh. 23 - Write plausible half-equations to represent each...Ch. 23 - Prob. 22ECh. 23 - Use electrode potential data from this chapter or...Ch. 23 - You are given these three reducing agents: Zn(s);...Ch. 23 - Prob. 25ECh. 23 - Prob. 26ECh. 23 - Prob. 27ECh. 23 - Use data from the text to construct a standard...Ch. 23 - When a soluble lead compound is added to a...Ch. 23 - Prob. 30ECh. 23 - Prob. 31ECh. 23 - If CO2(g) under pressure is passed into...Ch. 23 - Use equation (23.19) to determine [Cr2O72] in a...Ch. 23 - If a solution is prepared by dissolving 1.505 g...Ch. 23 - Prob. 35ECh. 23 - Prob. 36ECh. 23 - Prob. 37ECh. 23 - Prob. 38ECh. 23 - Will reaction (23.25) still be spontaneous in the...Ch. 23 - Prob. 40ECh. 23 - Prob. 41ECh. 23 - Prob. 42ECh. 23 - Prob. 43ECh. 23 - Prob. 44ECh. 23 - Prob. 45ECh. 23 - Prob. 46ECh. 23 - Prob. 47ECh. 23 - At 400C , 2Hg(I)+O2(g)2HgO(s) for the reaction...Ch. 23 - Prob. 49ECh. 23 - Prob. 50ECh. 23 - Prob. 51ECh. 23 - Prob. 52ECh. 23 - Prob. 53ECh. 23 - Prob. 54ECh. 23 - The text notes that in small quantities, zinc is...Ch. 23 - Prob. 56ECh. 23 - What formulas would you expect for the metal...Ch. 23 - For the straight-line graphs in Figure 23-8...Ch. 23 - Prob. 59ECh. 23 - Prob. 60ECh. 23 - Prob. 61ECh. 23 - Prob. 62ECh. 23 - Prob. 63ECh. 23 - Prob. 64ECh. 23 - Prob. 65ECh. 23 - Prob. 66ECh. 23 - Prob. 67ECh. 23 - Prob. 68ECh. 23 - Prob. 69ECh. 23 - Prob. 70ECh. 23 - Prob. 71ECh. 23 - For a coordination number of four, the radius of...Ch. 23 - Prob. 73ECh. 23 - Prob. 74FPCh. 23 - Several transition metal ions are found in cation...Ch. 23 - Prob. 76SAECh. 23 - Briefly describe each of the following ideas. phe...Ch. 23 - Prob. 78SAECh. 23 - Prob. 79SAECh. 23 - Prob. 80SAECh. 23 - Prob. 81SAECh. 23 - Prob. 82SAECh. 23 - Prob. 83SAECh. 23 - Prob. 84SAECh. 23 - Prob. 85SAECh. 23 - Provide the missing name or formula for the...Ch. 23 - Prob. 87SAECh. 23 - Prob. 88SAECh. 23 - Prob. 89SAECh. 23 - Prob. 90SAE
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