Consider these electronic configurations for neutral atoms:
(i) `1s^(2)2s^(2)2p^(6)3s^(1)`
(ii). `1s^(2)2s^(2)2p^(6)4s^(1)`
Which of the following statements is/are false?

Options

A. X represents an alkali metal.
B. Energy is required to change X into Y.
C. Y represents ground state of the element.
D. Less energy is required to remove an electron from Y than from X.

Answer

To solve the question regarding the electronic configurations of the neutral atoms given as (i) `1s^(2)2s^(2)2p^(6)3s^(1)` and (ii) `1s^(2)2s^(2)2p^(6)4s^(1)`, we will analyze each statement provided in the question to determine which of them is false.

### Step-by-Step Solution:

1. **Identify the Elements**:
- For configuration (i) `1s^(2)2s^(2)2p^(6)3s^(1)`:
- Count the total number of electrons:
\(2 + 2 + 6 + 1 = 11\)
- This corresponds to Sodium (Na), which is an alkali metal.

- For configuration (ii) `1s^(2)2s^(2)2p^(6)4s^(1)`:
- Count the total number of electrons:
\(2 + 2 + 6 + 1 = 11\)
- This is also Sodium (Na) but in an excited state since the electron has moved from the 3s orbital to the 4s orbital.

2. **Analyze the Statements**:
- **Statement A**: "X represents an alkali metal."
- This is true as both configurations represent Sodium, which is an alkali metal.

- **Statement B**: "Energy is required to change X into Y."
- This is true as moving an electron from the 3s orbital to the 4s orbital requires energy (excitation).

- **Statement C**: "Y represents the ground state of the element."
- This is false. Y represents the excited state of Sodium, not the ground state.

- **Statement D**: "Less energy is required to remove an electron from Y than from X."
- This is true. The electron in Y (4s) is farther from the nucleus than in X (3s), thus requiring less energy to remove.

3. **Conclusion**:
- The false statement is **Statement C**: "Y represents the ground state of the element."

### Final Answer:
The false statement is **C**.