8 years ago. Source(s): retired chem teacher USA. Define bond order; explain its relationship to bond length or bond energy. Arrange the following bonds in order of increasing bond strength. Knowing that the tin atomic radius is 141 pm, estimate the bond distances in Sn—Cl, Sn—Br and Sn—I. Evaluate enthalpies of reactions using bond energies. N2 has a triple bond so its bond length is the shortest. Bond order= (No. and Cl2 and Br2 have single bonds so their bond length is the longest. Bond length is the distance between two nuclei of atoms that are covalently bonded together. In general, the equilibrium bond length is larger for excited electron configurations than for ground state electron configurations. A bond length for the HCl molecule can be calculated from the HCl spectrum by assuming that it is a rigid rotor and solving the Schrodinger equation for that rotor. (A) C-I < C-Br < C-Cl < C-F (B) C-F < C-Cl < C-Br < C-I (C) C-Br < C-I < C-Cl < C-F (D) C-I < C-Br < C-F< C-Cl (E) none of the above orders is correct . To correlate bond strength with bond length; To define and used average bond energies; In proposing his theory that octets can be completed by two atoms sharing electron pairs, Lewis provided scientists with the first description of covalent bonding. Bond length in diatomic molecules = sum of the atomic radii . Cottrell, "The Strengths of Chemical Bonds," 2nd ed., Butterworths, London, 1958; B. deB. A. For a free diatomic molecule the Hamiltonian can be anticipated from the classical rotational kinetic energy. The bond lengths in Cl2, Br2 and I2 are 200, 228 and 266 pm, respectively. 0 0. Determination of the I2 bond-length distribution in liquid, solid and solution, by extended X-ray absorption fine structure spectroscopy October 1997 The Journal of Chemical Physics 107(15):5720-5726 Which of the following molecules has the shortest bond length? O2 has a double bond so its bond length is a little longer. Gaseous iodine is composed of I 2 molecules with an I–I bond length of 266.6 pm. To answer this question firstly we have to calculate the bond orders. (The record is held by iodine's neighbour xenon: the Xe–Xe bond length is 308.71 pm.) In this section, we expand on this and describe some of the properties of covalent bonds. Robby. Select 1: a. H2 b. Cl2 c. I2 d. F2 e. Br2. How to Calculate Bond Length. It is even longer (271.5 pm) in solid orthorhombic crystalline iodine, which has the same crystal structure as chlorine and bromine. The higher the bond order is, the shorter the bond length. The bond lengths in Cl2, Br2 and I2 are 200, 228 and 266 pm, respectively. (A)N2 (B)O2 (C) Cl2 (D)Br2 (E)I2. Bond length is usually in the range of 0.1 to 0.2 nm. The minimum of a potential energy curve occurs at the equilibrium bond length, and corresponds to the most stable nuclear conformation for that electronic configuration. 8.9.1(a): Potential Well Diagram for H 2, where the energy of the H-H bond is plotted as a function of the internuclear distance (radius) (b). Reference: Huheey, pps. The I–I bond is one of the longest single bonds known. and the energy eigenvalues can be anticipated from the nature of angular momentum. Region (3) is the equilibrium bond length which represents the bottom of the potential well and is the length at which the molecules oscillate back and forth around. Define bond length and bond energy and note the relationship between the two. In this section, we expand on this and describe some of the properties of covalent bonds. A-21 to A-34; T.L. Compare the estimated values to the experimental values of 233, 250 and 270 pm, respectively. of bonding electrons-No. When two similar atoms are bonded together, half of the bond length is referred to as covalent radius. A. Since atomic radius of iodine is largest its bond length in diatomic state is largest when compared to given options. Recognize covalent substances and characterize ionic character as difference in electronegativity. Describe trends in bond lengths of a series of related compounds. The Answer to your question is N2 this is because there is a triple bond between the two nitrogen atoms therefore it is extremelyy strong. Fig. To correlate bond strength with bond length; To define and used average bond energies; In proposing his theory that octets can be completed by two atoms sharing electron pairs, Lewis provided scientists with the first description of covalent bonding. Knowing that the tin atomic radius is 141 pm, estimate the bond distances in …