What is the wavelength necessary to completely remove an electron from the fourth shell (n = 4) of a hydrogen atom, given the Rydberg constant R = 1.097 x 10^7 m^-1?

Consider the two waves shown here (figure 1), which we will consider to represent two electromagnetic radiations.

A C–C bond has an average bond strength of 350 kJ/mol. What is the longest wavelength (lowest energy) light, in nm, that can break the average C–C bond? (1 m = 10⁹ nm)

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.32 × 10^14 Hz. (Use the speed of light, c = 3.00 × 10^8 m/s)

What is the wavelength necessary to completely remove an electron from the second shell (n = 2) of a hydrogen atom, given the Rydberg constant R∞ = 1.097 × 10^7 m^-1?

Calculate the wavelength of light produced if an electron moves from n=5 state to n=3 state in a hydrogen atom. Use the Rydberg formula: 1/λ = R_H (1/n1² - 1/n2²), where R_H = 1.097 x 10^7 m^-1.

Which of the following transitions requires the absorption of the most energetic photon?

Determine the frequency, in hertz, of radiation having an energy of 8.66 x 10^-21 J/photon. (Use Planck's constant, h = 6.626 x 10^-34 J·s)