Given below are statements about some molecules/ions. Identify the CORRECT statements. A. The dipole moment value of NF_3 is higher than that of…

Statement A: In $NH_3$NH3​, the orbital dipole due to the lone pair is in the same direction as the resultant dipole moment of the $N-H$N−H bonds. In $NF_3$NF3​, the orbital dipole is in the opposite direction to the resultant dipole moment of the $N-F$N−F bonds. Thus, dipole moment of $NH_3$NH3​ ($1.47\ D$1.47 D) is higher than $NF_3$NF3​ ($0.23\ D$0.23 D). Statement A is incorrect.

Statement B: $BeH_2$BeH2​ is a linear molecule ($sp$sp hybridization). The two $Be-H$Be−H bond dipoles are equal and opposite, so they cancel each other out, making the net dipole moment zero. Statement B is correct.

Statement C: $O_2^{2-}$O22−​ has 18 electrons. Its bond order is $\frac{10-8}{2} = 1$210−8​=1. $F_2$F2​ also has 18 electrons and its bond order is 1. Statement C is correct.

Statement D: In the Lewis structure of ozone ($O_3$O3​), the central oxygen atom forms one double bond and one single bond and has one lone pair. Formal charge = $V - L - \frac{B}{2} = 6 - 2 - \frac{6}{2} = +1$V−L−2B​=6−2−26​=+1. Statement D is incorrect.

Statement E: $NO_2$NO2​ is an odd-electron molecule (17 valence electrons). The nitrogen atom has only 7 electrons in its valence shell, so it does not satisfy the octet rule. Statement E is incorrect.

Therefore, only statements B and C are correct.