61. Each of the following is either linear , angular (bent), planar tetrahedral, or octahedral . Indicate the correct shape of (a) H_(2)S (b) N_(2)O_(4) ; (c) HCN; (d) SbCl_(6)^- (e) BF_(4)^-

To determine the shape of each molecule, we can use the VSEPR (Valence Shell Electron Pair Repulsion) theory. According to this theory, the shape of a molecule is determined by the repulsion between the electron pairs in the valence shell of the central atom.(a) : In , sulfur is the central atom. It has two bonded atoms (hydrogen) and two lone pairs of electrons. According to VSEPR theory, the shape of is bent or angular.(b) : In , nitrogen is the central atom. It has two bonded atoms (nitrogen) and two lone pairs of electrons. According to VSEPR theory, the shape of is planar tetrahedral.(c) HCN: In HCN, carbon is the central atom. It has one bonded atom (hydrogen) and one triple bond with nitrogen. According to VSEPR theory, the shape of HCN is linear.(d) : In , antimony is the central atom. It has six bonded atoms (chlorine) and no lone pairs of electrons. According to VSEPR theory, the shape of is octahedral.(e) : In , boron is the central atom. It has four bonded atoms (fluorine) and no lone pairs of electrons. According to VSEPR theory, the shape of is tetrahedral.Therefore, the correct shapes for each molecule are:(a) : Bent or angular(b) : Planar tetrahedral(c) HCN: Linear(d) : Octahedral(e) : Tetrahedral