Find out the group of the element having the electronic configuration, `1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6)3d^(6)4s^(2)`.

Answer

To determine the group of the element with the electronic configuration `1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 3d^(6) 4s^(2)`, follow these steps:

### Step 1: Identify the Last Electron Configuration
The given electronic configuration can be broken down as follows:
- `1s^(2)`: 2 electrons in the first shell
- `2s^(2) 2p^(6)`: 8 electrons in the second shell
- `3s^(2) 3p^(6)`: 8 electrons in the third shell
- `3d^(6)`: 6 electrons in the d subshell
- `4s^(2)`: 2 electrons in the s subshell

The last electron enters the `3d` subshell.

### Step 2: Determine the Block of the Element
Since the last electron enters the `d` subshell, this element belongs to the d-block of the periodic table.

### Step 3: Count the Electrons in the s and d Subshells
To find the group number for d-block elements, we add the number of electrons in the outermost s subshell and the d subshell:
- Number of s electrons = 2 (from `4s^(2)`)
- Number of d electrons = 6 (from `3d^(6)`)

### Step 4: Calculate the Group Number
Now, add the number of s and d electrons:
\[ \text{Group Number} = \text{s electrons} + \text{d electrons} = 2 + 6 = 8 \]

### Conclusion
The element with the given electronic configuration belongs to **Group 8** of the periodic table.

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