In which of the following ionization processes the bond energy increases and the magnetic behaviour changes from paramagnetic to diamagnetic?
1. \(\mathrm{O_{2}\rightarrow O_{2}^{+} }\)
2. \(\mathrm{C_{2}\rightarrow C_{2}^{+} }\)
3. \(\mathrm{NO\rightarrow NO^{+} }\)
4. \(\mathrm{N_{2}\rightarrow N_{2}^{+} }\)

The most preferred structure among the following with the lowest energy for SO₃ is: 

1.		2.
3.		4.

In which of the following molecules the central atom does not have sp³ hybridization?

1. SF₄

2. $B{F}_4^{-}$

3. $N{H}_4^{+}$

4. CH₄

Which of the two species, NO₃⁻ or H₃O⁺, has the correctly described properties listed below?

Which of the following pairs of oxygen species and their magnetic behaviour is correct?

1. $\mathrm{O},$ ${\mathrm{O}}_2^{2-}$ - Both paramagnetic
2. ${\mathrm{O}}_2^{-},$ ${\mathrm{O}}_2^{2-}$ - Both diamagnetic
3. ${\mathrm{O}}^{+},$ ${\mathrm{O}}_2^{2-}$ - Both paramagnetic
4. ${\mathrm{O}}_2^{+},$ ${\mathrm{O}}_2$ - Both paramagnetic

Four diatomic species are listed below. Identify the correct order in which the bond order is increasing in them.
1. O₂^– < NO < C₂^2– < He₂⁺  
2. C₂^2– < He₂⁺ < O₂^– < NO  
3. He₂⁺ < O₂^– < NO < C₂^2–
4. NO < O₂^– < C₂^2– < He₂⁺  

Which orbital does the additional electron occupy when O₂ is converted to the O₂⁻ ion?