What is the longest wavelength of electromagnetic radiation capable of ionizing this hydrogen atom in an excited state? Report your answer in nanometers. λ = 121.58 nm

Compare the energy (in joules) carried by an X-ray photon (wavelength=0.20nm) with that carried by an AM radio wave photon (=0.20m) . Calculate the energy of 1.00 mol of each type of photon. What effect do you expect each type of radiation to have for inducing chemical reactions in the substances through which it passes?

What experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?

This laser emits green light with a wavelength of 533 nm. (a) What is the energy, in joules, of one photon of light at this wavelength? (b) If a particular laser produces 1.00 watt (W) of power (1 W = 1 J/s), how many photons are produced each second by the laser?

6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?

Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using the spectroscope they invented in 1859. The name came from the Latin caesius ("sky blue") because of the prominent blue line observed for this element at 455.5 nm. Calculate the frequency and energy of a photon of this light.

• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.

Using the Bohr model of an electron orbiting a nucleus, the angular momentum of Earth's orbit around the Sun is about 2.67 x 1040 g m2 s−1. Using the Bohr quantization condition, what is the quantum number n for Earth's orbit? If the Earth transitions from this orbit to n-1 (emitting a graviton, which is the gravitational anagloue of the photon), how much energy would be released? Find the frequency of the graviton.

An electron is trapped in a tiny hole in an array of aluminum atoms (assume that they behave as uniform hard spheres). In this situation, the energy of the electron is quantized, and the lowest–energy transition (nx, ny, nz = 1,1,2➔ nx, ny, nz = 1,1,1) (particle in a box in 3 –dimensions) corresponds to a wavelength of 9.50 nm. Assuming that the hole can be approximated as a cube (face-centered), what is the radius of a spherical ion that will just fit in this hole?

Calculate the maximum wavelength of electromagnetic radiation if it is to cause detachment of electrons from the surface of metallic tungsten, which has a work function of 7.29 × 10-19 J. If the maximum speed of the emitted photoelectrons is to be 2.00 × 106 m s-1 , what should the wavelength of the radiation be?