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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Choose the Lewis structure for the compound below: H2CCHOCH2CH(CH3)2 HH H :d H H H C. Η H H HH H H H H. H H H HH H H H H H- H H H C-H H H HHHH

Each of the highlighted carbon atoms is connected to hydrogen atoms.

く Complete the reaction in the drawing area below by adding the major products to the right-hand side. If there won't be any products, because nothing will happen under these reaction conditions, check the box under the drawing area instead. Note: if the products contain one or more pairs of enantiomers, don't worry about drawing each enantiomer with dash and wedge bonds. Just draw one molecule to represent each pair of enantiomers, using line bonds at the chiral center. More... No reaction. Explanation Check O + G 1. Na O Me Click and drag to start drawing a structure. 2. H + 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 000 Ar P

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

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.