Consider the following statements :
(I) The radius of an anion is larger than that of the parent atom
(II) The ionization energy generally increases with increasing atomic number in a period.
(III) The electronegativity of an element is the tendency of an isolated atom to at tract an electron.
Which of the above statements is/are correct?

Options

A. I alone
B. II alone
C. I and II
D. II and III

Explanation

To solve the question, we need to evaluate each of the three statements provided:

### Step 1: Analyze Statement I
**Statement I:** The radius of an anion is larger than that of the parent atom.

- **Explanation:** An anion is formed when an atom gains one or more electrons. The addition of electrons increases electron-electron repulsion in the outer shell, causing the electron cloud to expand. Therefore, the radius of an anion is indeed larger than that of its parent atom.

**Conclusion:** Statement I is **True**.

### Step 2: Analyze Statement II
**Statement II:** The ionization energy generally increases with increasing atomic number in a period.

- **Explanation:** Ionization energy is the energy required to remove an electron from an atom. As we move from left to right across a period, the atomic number increases, and the effective nuclear charge experienced by the outer electrons also increases. This leads to a stronger attraction between the nucleus and the electrons, resulting in higher ionization energy.

**Conclusion:** Statement II is **True**.

### Step 3: Analyze Statement III
**Statement III:** The electronegativity of an element is the tendency of an isolated atom to attract an electron.

- **Explanation:** Electronegativity is defined as the tendency of an atom to attract a pair of electrons when it is part of a compound, not just a single electron. The statement is incomplete because it does not mention the attraction of a pair of electrons.

**Conclusion:** Statement III is **False**.

### Final Conclusion:
- **Correct Statements:** I and II are correct.
- **Incorrect Statement:** III is incorrect.

Thus, the correct answer is that **Statements I and II are correct**.

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