This discussion on For the compounds CH3Cl, CH3Br, CH3I and CH3F, the correct order of increasing C-halogen bond length is :a)CH3F CH3F > CH3Br > CH3I . The constants P, q, and r are functions of the bond lengths and masses of the atoms. Ref: HORVATH,AL (1982) ECOSAR Class Program (ECOSAR v0.99h): Class(es) found: Neutral Organics Henrys Law Constant (25 deg C) [HENRYWIN v3.10]: Can you explain this answer? 2- Determine the molecular geometry for each molecule. 4- In which cases do you expect deviations from the idealized bond angle? is done on EduRev Study Group by JEE Students. Thus an H–F bond is stronger than an H–I bond, H–C is stronger than H–Si, H–N is stronger than H–P, H–O is stronger than H–S, and so forth. In sp2 hybrid orbitals have more of s -character and hence the carbon if chlorobenzene withdraws the electron pair between C-Cl with greater force. As a result, C-Cl bond is shorter than CH3-Cl. More crowding = more repulsion = longer bond length. One way to think about it is that a sp3 center with 109.5 degree angles is more crowded than an sp2 center with 120 degree angles. As the polar nature of CH-X bond is expected to increase with increase in the electronegativity difference between carbon and halogen atom. & we know electronegativites of the halogens are: F 4.0 Cl 3.5 Br 2.8 I 2.5 Hence the order of bond dipole moment here is CHF3> CHCl3>CHBr3>CHI3 Hope you have got it..(: This is only the major reason. For CH3Br, these constants are given by the following expressions. 4 years ago a) PF3 (b) SBr2 (c) CH3Br (d) BCl3 I'd really appreciate your help! Also identified as methyl bromide, methyl fume, and mono-bromomethane, it is a fabricated chemical compound that is manufactured biologically and industrially. NH4 is a polyatomic ion, meaning it is a compound (composed of multiple elements) that has an overall net charge (in this case, being +1). JEE Main 2014: For the compounds CH3Cl, CH3Br, CH3I and CH3F, the correct order of increasing C-halogen bond length is: (A) CH3F < CH3Cl < CH3C < CH https://www.khanacademy.org/.../v/bond-length-and-bond-energy Another way to think about it is that the e-pair in an s orbital is sitting on the nucleus. 3- Determine the idealized bond angle for each molecule. (i) The carbon in C-Cl bond in chlorobenzene is sp2 hybridised, while in CH3-Cl is sp3 hybridised. The reason for this is that the region of space in which electrons are shared between two atoms becomes proportionally smaller as one of the atoms becomes larger (part (a) in Figure 8.11).