Transition Metal Electronic Configuration Fundamentals
Transition metal elements are a fascinating group found in the d-block of the periodic table. Their identity is primarily linked to the way their electrons are arranged, specifically concerning the 'd' orbitals.
Defining Transition Metals
The core characteristic that defines a transition metal is having incompletely filled d sub-shells in their neutral atomic state or in common oxidation states. This means that electrons are actively being added to the d orbitals of the penultimate energy shell (the shell just before the outermost one).
Analyzing Electronic Configuration Options
Let's examine each provided general electronic configuration to see which one accurately represents a transition metal:
-
Option 1: \((n-2)d^{1-10}ns^2\)
This configuration is incorrect because it suggests that the d-orbitals of the \((n-2)\) shell are being filled. For transition metals, it's the \((n-1)\) shell's d-orbitals that are typically involved.
-
Option 2: \((n-2)f^{1-14}(n-1)d^{0-1}ns^2\)
This configuration involves the filling of \(f\) orbitals (\((n-2)f^{1-14}\)), which are characteristic of the lanthanide and actinide series (f-block elements), not the d-block transition metals.
-
Option 3: \(ns^2np^6nd^{1-10}\)
This configuration is inaccurate. The filling of the \(nd\) subshell after the \(ns\) and \(np\) subshells of the same principal energy level (\(n\)) is not typical for transition metals. Furthermore, a filled \(ns^2np^6\) configuration often signifies a noble gas electron arrangement.
-
Option 4: \((n-1)d^{1-10}ns^{0-2}\)
This is the correct general electronic configuration for transition metals.
- \((n-1)d^{1-10}\): This part accurately shows that the d-orbitals of the penultimate shell (one shell less than the outermost, \(n\)) are being filled with electrons, ranging from 1 to 10. This is the defining feature.
- \(ns^{0-2}\): This part indicates that the outermost shell's s-orbitals contain 0 to 2 electrons. This accounts for cases where the outermost s-orbital might be empty (like in Palladium, Pd: \([Kr] 4d^{10} 5s^0\)) or contain two electrons (like in Scandium, Sc: \([Ar] 4s^2 3d^1\)), or even one electron (like in Chromium, Cr: \([Ar] 4s^1 3d^5\)).
- Option 5: (No configuration provided)
Conclusion on Transition Metal Configuration
Based on the analysis, the electronic configuration that correctly represents a transition metal element involves the filling of the \((n-1)d\) subshell while the outermost \(ns\) subshell contains 0 to 2 electrons. This matches Option 4.
Similar Questions
Which of the following carbon allotropes is/are good conductor(s) of electricity ?
1. Diamond
2. Graphite
3. Fullerene
Select the correct answer using the code given below :
CI - is not isoelectronic with
Important Questions from Classification of Elements and Periodicity in Properties
What is the valency of Lithium?
The maximum number of electrons that can be accommodated in the outermost orbit is _______.
If the atomic size increases, the nonmetallic character will
State the electronic configuration of Argon.
The ore of aluminium ‘bauxite’ is:
