To solve the question, we need to evaluate each of the statements provided and determine which ones are correct based on our understanding of atomic structure and electron behavior in atoms.
### Step-by-Step Solution:
1. **Evaluate Statement (i)**: "The energy of an electron in an atom is always negative, because it is negatively charged."
- The energy of an electron in an atom is not negative because it is negatively charged. Instead, it is negative because the electron is bound to the nucleus. The reference point for energy is taken at an infinite distance where the energy is considered zero. Thus, this statement is **incorrect**.
2. **Evaluate Statement (ii)**: "The charge of an electron in an atom is negative."
- This statement is true. The charge of an electron is indeed negative, approximately -1.6 × 10^-19 coulombs. Thus, this statement is **correct**.
3. **Evaluate Statement (iii)**: "When an electron is at an infinite distance from the nucleus so that there is no electrical interaction, then orbitarily the energy of electron is taken to be zero."
- This statement is generally accepted in atomic physics. At an infinite distance, the potential energy of the electron is considered to be zero because there is no interaction with the nucleus. Thus, this statement is **correct**.
4. **Evaluate Statement (iv)**: "As the electron moves closer to the nucleus, energy is released and so its energy becomes less than zero i.e., negative."
- This statement is also true. As the electron moves closer to the nucleus, it loses potential energy, which is released as energy. Consequently, the energy of the electron becomes more negative (less than zero). Thus, this statement is **correct**.
### Conclusion:
- The correct statements are (ii), (iii), and (iv).
### Final Answer:
- The correct statements are: **(ii), (iii), and (iv)**.
