Exams › JEE Main › Chemistry

Consider the species N2, CO, CN- and NO+. Which statement is correct for all of them?

1. All of them are paramagnetic
2. They are isoelectronic with one another
3. All of them possess a dipole moment
4. All of them are linear

Correct answer: They are isoelectronic with one another

Solution

N2 (14e), CO (6+8=14e), CN- (6+7+1=14e) and NO+ (7+8-1=14e) all have 14 electrons, so they are isoelectronic; being diatomic they are linear but homonuclear N2 has no dipole moment, and all are diamagnetic.

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 →