The electron configuration of Co 2 + . Concept introduction: Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy. The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d). 3d elements show large variation in their oxidation states.

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Answer 1

Question

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

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Answer 2

Question

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

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Answer 3

Question

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

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Answer 4

Question

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

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Answer 5

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

Answer 6

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Answer 7

Chapter 20, Problem 20.1P

Interpretation Introduction

To determine:

The electron configuration of Co2+.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Answer 8

Expert Solution

Answer to Problem 20.1P

Solution:Co2+

: 1s2 2s2 2p6 3s2 3p6 3d7

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Atomic number of cobalt is 27. Thus, it has 27 electrons in its elemental state.

The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Co2+has 2 electrons less than that in its elemental state, thus it has 25 electrons.

Now, electrons are first removed from 4s2orbitals.

Thus, the electronic configuration of Co2+will be:

1s2 2s2 2p6 3s2 3p6 3d7

(c)

Answer 13

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Answer 14

Interpretation Introduction

To determine:

The electron configuration of metal in MnO2.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Answer 15

Expert Solution

Answer to Problem 20.1P

Solution:MnO2

: 1s2 2s2 2p6 3s2 3p6 3d3

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Atomic number of manganese is 25. Thus, it has 25 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Oxygen has an oxidation state of -2, thus in MnO2, 2 oxygen atoms have -4 charge on them. Since molecule is neutral, Mnmust have an atomic charge of +4. Thus, it has 4 electrons less than that in its elemental state, thus it has 21 electrons. The electrons are first removed from 4s orbital as follows:

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

(d)

Answer 20

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.

Now filling up 27 electrons of Cu2+

to get its electronic configuration:

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

Answer 21

Interpretation Introduction

To determine:

The electron configuration of metal in CuCl42−.

Concept introduction:

Electronic configuration of an atom shows how electrons are placed in the orbitals in order of increasing energy.

The filling of the sublevels progresses in order up to Period 4. However, in the sublevel blocks in Period 4 the 4s sublevel fills before the 3dsublevel.This occurs because the electrons in the 4ssublevel have slightly lower energy than the electrons in the 3d sublevel. This series of 10 elements is called the first transition series (3d).

3d elements show large variation in their oxidation states.

Answer 22

Expert Solution

Answer to Problem 20.1P

Solution:CuCl42−: 1s2 2s2 2p6 3s2 3p6 3d9

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Atomic number of copper is 29. Thus, it has 29 electrons in its elemental state. The arrangement of atomic orbitals in increasing order of their energies is as follows:

1s 2s 2p 3s 3p 4s 3d

The maximum occupancy of electrons for s, p, and dorbitals is 2, 6, and 10 respectively.

Thus, the electronic configuration will be:

1s2 2s2 2p6 3s2 3p6 4s1 3d10

This is because half filled, and full filled orbitals are more stable.

Chlorine has an oxidation state of -1, thus in CuCl42−, 4 chlorine atoms have -4 charge on them. Since molecule has a charge of -2, Cumust have an atomic charge of −(−4−(−2))=+2. Thus, it has 2 electrons less than that in its elemental state, thus it has 27 electrons.