Explain why the transition metals in periods 5 and 6 have nearly identical radii in each group.

Short Answer

Expert verified
The transition metals in Periods 5 and 6 have nearly identical radii in each group because the increase in effective nuclear charge due to the higher number of protons is balanced by the increased electron shielding effect from the additional 4f electrons. This causes the effective nuclear charge experienced by the outermost electrons to remain almost constant, leading to nearly identical atomic radii for these elements in each group.

Step by step solution

01

Recall the Electron Configuration of Transition Metals

Transition metals are located in the d-block of the periodic table. They have their outermost electrons in the d-subshell. The electron configuration of these elements can be represented in the form: [Noble Gas] \(\mathrm{n-1}\) d \(\mathrm{x}\) n s \(\mathrm{y}\), where n is the principal quantum number (period), x and y are the number of electrons in the d and s subshells, respectively.
02

Understand the Effective Nuclear Charge

The effective nuclear charge is the net positive charge experienced by an electron in an atom. It is affected by the number of protons in the nucleus (atomic number) and the electron shielding effect caused by the inner electron shells. As we move down a group in the periodic table, the atomic number increases, which also increases the effective nuclear charge.
03

Explain the Electron Shielding Effect

The electron shielding effect occurs when the inner electron shells shield the outer electrons from the full attraction of the nucleus. This causes the outer electrons to experience a reduced effective nuclear charge. When transitioning from periods 5 to 6, the electron shielding in the 4f subshell increases.
04

Relate the Effective Nuclear Charge and Electron Shielding to Atomic Radii

As the effective nuclear charge increases, the attraction between the nucleus and the outer electron shell increases, causing the atomic radius to decrease. However, an increase in electron shielding counteracts this effect by reducing the effective nuclear charge, causing the atomic radius to remain fairly constant.
05

Conclude with the Reason for Nearly Identical Radii

In the case of transition metals in Periods 5 and 6, the increase in effective nuclear charge due to the higher number of protons is balanced by the increased electron shielding effect from the additional 4f electrons. As a result, the effective nuclear charge experienced by the outermost electrons remains almost constant, leading to nearly identical atomic radii for these elements in each group.

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