23.3.1 Color and Transition Metals

Question 1

Which statement about hexafluorocobaltate(III) and hexaamminecobalt(III) is not correct?

Answer 1

Transition metals do not absorb light in a visible region. This is because the energy differences among the different d orbitals are very small.

Question 2

Which statement about color or the color chart is not correct?

Answer 2

In transition metals, the d orbitals are very far apart; therefore, any changes in ΔE are very large, resulting in colors in the ultraviolet range.

Question 3

Which statement about transition metals is not correct?

Answer 3

Transition metals in solution exhibit a small range of color differences.

Question 4

Which statement about orbitals and magnetic fields is not correct?

Answer 4

A diamagnetic substance is attracted to a magnetic field.

Question 5

Which statement about hexafluorocobaltate(III) ion is not correct?

Answer 5

The cobalt in this complex ion has an oxidation state of 2+.

Question 6

Which statement about hexaamminecobalt(III) ion is not correct?

Answer 6

Hexaamminecobalt(III) ion has an overall charge of 3−.

Question 7

Look at the two different electron orbital arrangements for cobalt. Which statement about these arrangements is not correct?

Answer 7

In the ion with three electrons removed, the 3d orbitals have a higher energy level and thus contain all of the electrons.

Question 8

Which statement about color is not correct?

Answer 8

Color exists in most transition metal solutions because the solution emits light.

Question 9

Look at the ΔE color spectrum chart. Which statement about the chart is not correct?

Answer 9

For the transition metals, the energy change is always negative when going from a lower level to a higher level.

Question 10

Which choice best explains why transition metals exhibit a wide variety of colors?

Answer 10

Transition metals have partially filled d orbitals, and the different d orbitals are at different energy levels when ligands are attached.