The values of rotational constant, B for SF 6 and UF 6 are to be calculated. The differences between their B values, taking into account their atomic masses is to be commented. Concept introduction: In a molecule, the rotational energy level corresponds to the different probable ways in which the portion of a molecule rotates around the chemical bond that binds it to the rest of the molecule. Every rotational energy level possesses degeneracy. The two-body system is represented as a one-body system by a reduced mass. It is expressed by a quantity μ . The inertial mass of the moving body with respect to the body which is at rest is simplified to a reduced mass when there are only mutual interactions between the two bodies. The spherical top refers to a symmetric rotor that has the same value for all moments of inertia. For spherical tops, I a = I b = I c .

Question

(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .

Answer 1

Question

100%

Chapter 14, Problem 14.16E

Interpretation Introduction

Interpretation:

The values of rotational constant, B for SF6 and UF6 are to be calculated. The differences between their B values, taking into account their atomic masses is to be commented.

Concept introduction:

In a molecule, the rotational energy level corresponds to the different probable ways in which the portion of a molecule rotates around the chemical bond that binds it to the rest of the molecule. Every rotational energy level possesses degeneracy.

The two-body system is represented as a one-body system by a reduced mass. It is expressed by a quantity μ. The inertial mass of the moving body with respect to the body which is at rest is simplified to a reduced mass when there are only mutual interactions between the two bodies.

The spherical top refers to a symmetric rotor that has the same value for all moments of inertia. For spherical tops, Ia=Ib=Ic.

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .

If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?

The pentafluorides of the larger members of Group 5A(15)have been prepared, but N can have only eight electrons. A claim has been made that, at low temperatures, a compound with the empirical formula NF₅ forms. Draw a possible Lewis structure for this compound.