JEE Main · 2025 · 22 Jan 2025 · Shift 1 · Chemical Bonding and Molecular Structure

Checking each species for geometry:

$S{O}_2$ — bent ($s{p}^2$, one lone pair on S)
$BeC{l}_2$ — linear ($sp$, no lone pair)
$C{O}_2$ — linear ($sp$, no lone pair)
$N_3^{-}$ — linear ($sp$, resonance-delocalised)
$N{O}_2$ — bent ($s{p}^2$, unpaired electron)
$F_{2}O$ — bent ($s{p}^3$, two lone pairs on O)
$Xe{F}_2$ — linear ($s{p}^{3}d$, three equatorial lone pairs)
$N{O}_2^{+}$ — linear ($sp$, isoelectronic with $C{O}_2$)
$I_3^{-}$ — linear ($s{p}^{3}d$, three equatorial lone pairs)
$O_3$ — bent ($s{p}^2$, one lone pair on central O)

Linear species: $BeC{l}_2,C{O}_2,N_3^{-},Xe{F}_2,N{O}_2^{+},I_3^{-}$ — six in total.