Wouldn't both of those be 180 degrees or linear? a) SO3 b) SF2 c) HCN d) H2S e) PF3 See all problems in Bond Angles. In all the four cases, the molecules undergo Sp 3 hybridization forming four hybrid orbitals, two of which are occupied by 1p of electrons and two by bp electrons. In this work, we present detailed calculations of the electronic structure of H2S, SF2, and HSF. Of the following molecules given below, which has the largest bond angle? as electronegativity of O is more than S so bond angle of H2O more than H2S. oxygen atom in water molecule has two lone pairs; due to small size of oxy , the lone pair-lone pair and the bond-pair bond-pair repulsion is large and as a result tend to push the molecule apart ; however in H2S, the sulphur atom is greater in size and the lone pair tend to be far apart, thereby considerably reducing the repulsions and also the bond angle. that is the reason. a. OCS - linear,180 deg, two double bonds. (a) SO3 (b) SF2 (c) HCN (d) H2S (e) PF3. A quick explanation of the molecular geometry of NO2 - (the Nitrite ion) including a description of the NO2 - bond angles. https://geometryofmolecules.com/sf2-lewis-structure-polarity-and-bond-angles For similar reasons, \$\ce{HOF}\$ will have a bond angle closer to \$109.5^\circ\$. The bond length for the nearly linear bonds is 1.646 A±0.003 A; for the other pair it is 1.545 A±0.003 A. a) angle O–S–O in SO42– ...as medium difficulty. Which molecule has the largest bond angle? 2019 04:00, akshat8712. I know that bond angle of \$\ce{SF2}\$ will be less than the bond angle of \$\ce{OF2}\$ because of larger size of sulfur atom. Thus they are expected to have 109 ° 28' angle but this does not happen. For similar reasons, \$\ce{HOF}\$ will have a bond angle closer to \$109.5^\circ\$. SF2 is a bent V-shape molecule with a bond angle of 98 degrees and there exists a difference between fluorine and sulfur atoms of around 3.98-2.58 = 1.4. Answer Save. 1 Answer. The answer is c but I can't figure out why it is better than b. The bond angles of \$\ce{NH2}\$, \$\ce{NH2-}\$ and \$\ce{NH2+}\$ are all very similar, \$103^\circ\$, \$104^\circ\$, and \$115^\circ\$ respectively. b. FNO - bent, 120 deg. I thought it was either b or c based on my drawings. d. While all three compounds have similar bent singlet ground states, the potential energy surfaces of various low lying electronic states as a function of bond angle reveal very different behaviors, in particular for linear geometries. With that you can count the bonding pairs and lone pairs and that will tell you the bond angles and molecular geometry. \$\begingroup\$ This answer explains why \$\ce{SF2}\$ will have a bond angle close to \$90^\circ\$ and \$\ce{OF2}\$ will have a bond angle closer to \$109.5^\circ\$. ... Our tutors rated the difficulty ofWhich has the largest bond angle? 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