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