From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with C l - .

Question

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Answer 1

Question

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

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Answer 2

Question

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

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Answer 3

Question

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

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Answer 4

Question

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

Answer 6

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.

Conclusion

Transition elements having partially filled d-subshell form coloured compounds.

Answer 7

Chapter 23, Problem 23.1VP

Interpretation Introduction

To identify:

From the four highlighted metals in Figure P32.1, the cations of which of the two form coloured compound with Cl-.

Answer 8

Expert Solution & Answer

Answer to Problem 23.1VP

Solution:

Cations of chromium (green) and cobalt (yellow) form coloured compound with Cl-.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

The highlighted elements are calcium (red), chromium (green), cobalt (yellow), and zinc (blue).

Transition metal compounds are often colored because of partially filled d-orbitals. The d-orbitals are generally split into two groups of different energies. The difference in the energies of the two groups is designated ∆. An electron from a lower energy d-orbital can absorb a photon of energy equal to ∆ and move to be promoted to a higher energy d-orbital from the same subshell. If the energy of the photon corresponds to the visible region, the compound appears colored.

Calcium belongs to s-block element and does not have d-electrons. Hence, it does not form coloured compounds.

Cations of chromium and cobalt have d-electrons which undergo d-d transition, and therefore, appear colored.

Zinc is also a d-block element but it has a completely filled 3d subshell. Therefore, a d-d transition is not possible and its compounds are colorless.