Question

The energy of a vibrating molecule is quantized much like the energy of an electron in the hydrogen atom. The energy levels of a vibrating molecule are given by the equation
En=(n+12)hν
where n is a quantum number with possible values of 1,2,…, and ν is the frequency of vibration. The vibration frequency of HCl is approximately 8.85×1013s−1

Part A:

starting with a "stationary" molecule, what minimum energy is required to excite a vibration in HCl?

Part B:

What wavelength of light is required to excite this vibration?

Answer 1

Answer: According to the given question , Here

part A ) For number one just plug the numbers into the equation En=(n + .5)hv. N should equal 1 since that is the smallest (minimum of 1 and 2). H is a constant 6.63*10^-34 and v is the 8.85*10¹³. Answer should be something like 8.80*10^-20 .

Hecne it is all about the first part .

Part B) According to the question , Here we use this equation. E=hc/lamda.

Now lamda = hc / E = 6.63 * 10^-34  * 3 * 10⁸  / 8.80 * 10^-20   = 2.26 * 10^-6

Hence the valu of lamda = 226 nm

Hence it is all about the given question , Thank you :)