An element has electronic configuration [Xe] `4f^(7), 5d^(1),6s^(2)`. It belongs to ____ block of this periodic table.

Options

A. Option 1. s
B. Option 2. p
C. Option 3. d
D. Option 4. f

Answer

To determine which block of the periodic table the element with the electronic configuration [Xe] 4f^7, 5d^1, 6s^2 belongs to, we can follow these steps:

### Step 1: Identify the Electronic Configuration
The electronic configuration given is [Xe] 4f^7, 5d^1, 6s^2. Here, [Xe] represents the core electrons, and the remaining configuration describes the valence electrons.

### Step 2: Determine the Last Subshell Filled
In the configuration, the last subshell that receives electrons is the 4f subshell. The presence of 4f^7 indicates that the last electron is entering the f-orbital.

### Step 3: Identify the Block
The periodic table is divided into blocks based on the subshell that is being filled:
- s-block: Last electron in s subshell
- p-block: Last electron in p subshell
- d-block: Last electron in d subshell
- f-block: Last electron in f subshell

Since the last electron in this case is in the f-orbital (4f), it indicates that the element belongs to the f-block of the periodic table.

### Step 4: Classify the Element
Elements that have electrons filling the 4f subshell are known as lanthanides. The configuration shows that this element is part of the lanthanide series.

### Conclusion
Thus, the element with the electronic configuration [Xe] 4f^7, 5d^1, 6s^2 belongs to the f-block of the periodic table.

### Final Answer
The element belongs to the f-block of the periodic table.

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