Which of the following statements is incorrect for Be?

Options

A. Most of its compounds are largely covalent
B. `BeCl_(2)` has bridged covalent structure and is a linear molecule above 1200 K
C. It has distintive group properties due to samller size and high electronegativity
D. It from `Be^(2+)` ions because of the lower value the sum of Ist and 2nd L.E.

Answer

To determine which statement about Beryllium (Be) is incorrect, we need to analyze each statement provided in the question.

**Step 1: Analyze the statements about Beryllium.**

1. **Statement 1:** Most of its compounds are largely covalent.
- Beryllium compounds, such as BeCl₂, exhibit significant covalent character due to the small size and high charge density of the Be²⁺ ion. This statement is correct.

2. **Statement 2:** Beryllium chloride has a rich covalent structure and is a linear molecule above 1200 Kelvin.
- Beryllium chloride (BeCl₂) does indeed have a covalent structure and can exist in a linear form at elevated temperatures. This statement is also correct.

3. **Statement 3:** It has distinctive group properties due to small size and high electronegativity.
- Beryllium is unique among the alkaline earth metals due to its small size and high electronegativity, which leads to its distinct properties. This statement is correct.

4. **Statement 4:** It formed Beryllium ion because of low value of sum of first and second ionization energy.
- This statement is incorrect. Beryllium has a relatively high ionization energy due to its small size and the strong attraction between the nucleus and the electrons. The sum of the first and second ionization energies is not low; in fact, it is quite high, which is why Be tends to form covalent compounds rather than ionic ones.

**Conclusion:**
The incorrect statement regarding Beryllium is the fourth one, which suggests that it forms a Beryllium ion due to low ionization energy.

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