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Chapter 23: Problem 14

Among the period 4 transition metals \((\mathrm{Sc}-\mathrm{Zn}),\) which elements do not form ions where there are partially filled \(3 d\) orbitals?

Short Answer

Expert verified
The period 4 transition metals that do not form ions with partially filled 3d orbitals are Scandium (Sc), Titanium (Ti), Vanadium (V), Copper (Cu), and Zinc (Zn).

Step by step solution

01

Write down the electron configurations of the period 4 transition metals

We can determine the electron configurations of the period 4 transition metals through the periodic table: 1. Scandium (Sc): [Ar] 4s虏 3d鹿 2. Titanium (Ti): [Ar] 4s虏 3d虏 3. Vanadium (V): [Ar] 4s虏 3d鲁 4. Chromium (Cr): [Ar] 4s鹿 3d鈦� 5. Manganese (Mn): [Ar] 4s虏 3d鈦� 6. Iron (Fe): [Ar] 4s虏 3d鈦� 7. Cobalt (Co): [Ar] 4s虏 3d鈦� 8. Nickel (Ni): [Ar] 4s虏 3d鈦� 9. Copper (Cu): [Ar] 4s鹿 3d鹿鈦� 10. Zinc (Zn): [Ar] 4s虏 3d鹿鈦�
02

Identify the elements that form stable cations without partially filled 3d orbitals

Now, we need to determine which of these elements do not form ions with partially filled 3d orbitals. To do this, we'll examine their possible cations and the resulting electron configurations: 1. Scandium (Sc): Sc鲁鈦� has the electron configuration [Ar], with no remaining 3d electrons. 2. Titanium (Ti): Ti鈦粹伜 has the electron configuration [Ar], with no remaining 3d electrons. 3. Vanadium (V): V鈦碘伜 has the electron configuration [Ar], with no remaining 3d electrons. 4. Chromium (Cr): Cr虏鈦� has the electron configuration [Ar] 3d鈦�. 5. Manganese (Mn): Mn虏鈦� has the electron configuration [Ar] 3d鈦�. 6. Iron (Fe): Fe鲁鈦� has the electron configuration [Ar] 3d鈦�. 7. Cobalt (Co): Co鲁鈦� has the electron configuration [Ar] 3d鈦�. 8. Nickel (Ni): Ni虏鈦� has the electron configuration [Ar] 3d鈦�. 9. Copper (Cu): Cu鈦� has the electron configuration [Ar] 3d鹿鈦�. 10. Zinc (Zn): Zn虏鈦� has the electron configuration [Ar] 3d鹿鈦�.
03

List the elements that do not form ions with partially filled 3d orbitals

From the information in Step 2, we can determine that Scandium (Sc), Titanium (Ti), Vanadium (V), Copper (Cu), and Zinc (Zn) are the period 4 transition metals that do not form ions with partially filled 3d orbitals.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Configuration
Electron configuration refers to how electrons are distributed in different atomic orbitals. Understanding electron configuration is critical to comprehending chemical properties and behaviors. For atoms in their ground state, electrons are filled in such a way to achieve the lowest possible energy.
For the period 4 transition metals, electron configurations start with the noble gas configuration of Argon \(\text{[Ar]}\), followed by additional electrons in the 4s and 3d orbitals.
  • Scandium (Sc): \([\text{Ar}] \ 4s^2 \ 3d^1\)
  • Titanium (Ti): \([\text{Ar}] \ 4s^2 \ 3d^2\)
  • Vanadium (V): \([\text{Ar}] \ 4s^2 \ 3d^3\)
  • ... ending with Zinc (Zn): \([\text{Ar}] \ 4s^2 \ 3d^{10}\)
When filling the d shell, once the 4s orbital is filled, electrons begin populating the 3d orbitals. However, due to electron-electron interactions and energy considerations, there are exceptions like Chromium (Cr) and Copper (Cu), where an electron from the 4s is used to half fill or completely fill the 3d orbital for added stability.
Period 4 Elements
Period 4 elements on the periodic table are fascinating, particularly the transition metals from Scandium (Sc) to Zinc (Zn). These elements have electrons entering the 3d sublevel, setting them apart from other elements.
They are known for their unique chemical behaviors and variable oxidation states. In period 4, transition metals' noteworthy features include:
  • High melting points
  • Variable oxidation states
  • Formation of colored compounds
  • Magnetic properties, particularly among the first few elements
The filling of the 3d orbitals confers unique characteristics. For instance, the incomplete d orbitals allow transition metals to form various ions and exhibit distinct magnetic and hallucinogenic properties. Transition metals in period 4 also play crucial roles in biological systems and industrial processes, leveraging their ability to form stable complex ions.
Ion Formation
Ion formation in transition metals is an intriguing process due to their variable oxidation states. When transition metals form ions, they typically lose electrons from both the s and d orbitals. The number of electrons removed corresponds to their oxidation state.
For example:
  • Scandium (Sc) loses 3 electrons to form \(\text{Sc}^{3+}\), resulting in \(\text{[Ar]}\)
  • Titanium (Ti) can form \(\text{Ti}^{4+}\), emptying the 3d orbital
  • Copper (Cu) forms a stable \(\text{Cu}^+ \) ion with a full 3d orbital \(\text{[Ar] 3d}^{10}\)
Unlike main group metals that typically form one type of ion, transition metals can form numerous ions with different charges. The differing ion charges affect the color, magnetism, and reactivity of the transition compounds. A practical example is iron, which can exist as \(\text{Fe}^{2+}\) or \(\text{Fe}^{3+}\), contributing to its versatility in chemical reactions and forming diverse compounds, essential for various industrial applications.

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Most popular questions from this chapter

Solutions of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+},\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (both octahedral), and \(\left[\mathrm{CoCl}_{4}\right]^{2-}(\) tetrahedral) are colored. One is pink, one is blue, and one is yellow. Based on the spectrochemical series and remembering that the energy splitting in tetrahedral complexes is normally much less than that in octahedral ones, assign a color to each complex.

The lanthanide contraction explains which of the following periodic trends? (a) The atomic radii of the transition metals first decrease and then increase when moving horizontally across each period. (b) When forming ions the period 4 transition metals lose their \(4 s\) electrons before their \(3 d\) electrons. (c) The radii of the period 5 transition metals (Y-Cd) are very similar to the radii of the period 6 transition metals (Lu-Hg).

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) triamminetriaquachromium(III) nitrate (b) dichlorobis(ethylenediamine)platinum(II) (c) pentacarbonyliron(0) (d) ammonium diaquabis(oxalato)Co(II) (e) tris(bipyridyl)cobalt(III) sulfate

The lobes of which \(d\) orbitals point directly between the ligands in (a) octahedral geometry, (b) tetrahedral geometry?

Determine if each of the following metal complexes is chiral and therefore has an optical isomer: (a) square planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right],(\mathbf{b})\) octahedral \(\left[\mathrm{Ni (\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},\) (c) octahedral cis-[V(en) \(\left._{2} \mathrm{ClBr}\right]\).
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