Exams › JEE Main › Chemistry
Stability of the species Li2, Li2− and Li2+ increases in the order of:
- Li2 < Li2+ < Li2−
- Li2− < Li2+ < Li2
- Li2 < Li2− < Li2+
- Li2− < Li2 < Li2+
Correct answer: Li2− < Li2+ < Li2
Solution
The stability of these lithium species is influenced by their electron configurations; Li2 has a stable bond with a complete electron configuration, while Li2− has an extra electron that leads to increased repulsion, making it less stable, and Li2+ has one less electron, resulting in a stronger bond and thus higher stability than Li2−.
Related JEE Main Chemistry questions
- Although the electronegativity gap between N and F is larger than that between N and H, ammonia has a dipole moment of 1.5 D while nitrogen trifluoride has only 0.2 D. The reason is that
- When N₂ is converted into N₂⁺, the dissociation energy of the N–N bond ______, and when O₂ is converted into O₂⁺, the dissociation energy of the O–O bond ______.
- From the ions listed below, which pair has geometries that can be accounted for by the same type of orbital hybridization? NO₂⁻, NO₃⁻, NH₂⁻, NH₄⁺, SCN⁻
- Atoms A and B have electronegativities of 1.20 and 4.0, respectively. What is the percentage ionic character of the A–B bond?
- In the phosphate ion, PO₄³⁻, what is the formal charge on an oxygen atom that is singly bonded to phosphorus in a P–O bond?
- Among the following species, which one has no unpaired electrons?
⚔️ Practice JEE Main Chemistry free + battle 1v1 →