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. $\begingroup$ 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 $109.5^\circ$. With that you can count the bonding pairs and lone pairs and that will tell you the bond angles and molecular geometry. 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. 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. a) angle O–S–O in SO42– ...as medium difficulty. Answer Save. The answer is c but I can't figure out why it is better than b. Of the following molecules given below, which has the largest bond angle? Which molecule has the largest bond angle? In this work, we present detailed calculations of the electronic structure of H2S, SF2, and HSF. as electronegativity of O is more than S so bond angle of H2O more than H2S. 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. 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. (a) SO3 (b) SF2 (c) HCN (d) H2S (e) PF3. H2O,OF2,SF2,H2S arrangw it in increasing bond angle order H2O = 104 0 5 SF2= 104 0 5 H2S = 104 0 5 Thank You Ruchi Askiitians faculty Thus they are expected to have 109 ° 28' angle but this does not happen. 1 Answer. 2019 04:00, akshat8712. a) SO3 b) SF2 c) HCN d) H2S e) PF3 See all problems in Bond Angles. For similar reasons, $\ce{HOF}$ will have a bond angle closer to $109.5^\circ$. that is the reason. The bond angles of $\ce{NH2}$, $\ce{NH2-}$ and $\ce{NH2+}$ are all very similar, $103^\circ$, $104^\circ$, and $115^\circ$ respectively. F-N single bond, N=O double bond, 1 one pair on N. c. FCN - linear, 180 deg, F-C single bond, C-N tripe bond. 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. Wouldn't both of those be 180 degrees or linear? One FSF angle is 101°33′±30′, the opposite FSF angle is 186°56′±30′. a. OCS - linear,180 deg, two double bonds. b. FNO - bent, 120 deg. https://geometryofmolecules.com/sf2-lewis-structure-polarity-and-bond-angles A quick explanation of the molecular geometry of NO2 - (the Nitrite ion) including a description of the NO2 - bond angles. 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