An element has outer shell configuration of `5f^0 6d^2 7s^2`. This element will lie in the

Options

A. s-block
B. p-block
C. d-block
D. f-block

Answer

To determine the block in which the element with the outer shell configuration of `5f^0 6d^2 7s^2` lies, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Outer Shell Configuration**:
The given outer shell configuration is `5f^0 6d^2 7s^2`. This means that:
- The `5f` subshell has 0 electrons (it is empty).
- The `6d` subshell has 2 electrons.
- The `7s` subshell has 2 electrons.

2. **Determine the Block**:
- The `s` block consists of elements that have their outermost electrons in the `s` subshell.
- The `p` block consists of elements that have their outermost electrons in the `p` subshell.
- The `d` block consists of elements that have their outermost electrons in the `d` subshell.
- The `f` block consists of elements that have their outermost electrons in the `f` subshell.

In this case, since the `5f` subshell is empty (`5f^0`), we need to look at the `6d` and `7s` subshells. The presence of electrons in the `6d` and `7s` subshells indicates that this element is primarily filling the `d` and `s` subshells.

3. **Identify the Series**:
- The `5f` series corresponds to the actinides, which are located in the f-block of the periodic table.
- However, since the `5f` subshell is empty, we focus on the `6d` and `7s` electrons.

4. **Conclusion**:
- Given that the `5f` subshell is empty and the element has electrons in the `6d` and `7s` subshells, it indicates that this element is part of the f-block elements (specifically, the actinides).
- Therefore, the element lies in the **f-block** of the periodic table.

### Final Answer:
The element will lie in the **f-block**.

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