Calculate the wavelength associated with the electronic transition of a hydrogen atom, when the electron changes from a 3s orbital to a 4p orbital. Is it an emission or absorption process?

The photoelectric work function of a metal is the minimum energy (of a photon) needed to eject a single electron from the surface of the metal by irradiating it with a wavelength of light with that minimum energy. For potassium (K), the work function equals 3.669 x 10 19 J (per photon). a) What is the minimum frequency ( v ) of the photon of light required to eject an electron from the surface of potassium metal? [ Select ] sec- b) What is the wavelength of this photon of light? [ Select ] nm c) What part of the electromagnetic spectrum does this photon of light come from? [ Select ]

X-rays are commonly applied in medical practices. It is a form of electromagnetic radiationused to produces images of bones and other body parts. Medical practitioners are able toexamine bone fracture and abnormalities in body organs by using this technique. Given wavelength of an x-ray photon is 2.70 Å, compute its frequency (in hertz) and energy (in joules). (1 Å = 10-8 cm)

A liquid is exposed to infrared radiation with a wavelength of 9.44×10−4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 44.00 J of heat?

Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers n = 1, l = 1, me = 0 n = 4, l = 2, me = 2 n = 2, l = 1, me = -1 n = 3, l = 2, me = -3 n = 5,l = 3, me = 1 4f 3s 2d 4p 5f not allowed Answer Bank 3d 4s 2p 5d 3p 4d 1p 1s 5s 5p 2s 3f

Ozone in the stratosphere absorbs ultraviolet light of wavelengths shorter than 320 nm, thus filtering out the most energetic radiation from sunlight.  During this absorption, an ozone molecule absorbs a photon, which breaks an oxygen-oxygen bond, yielding an oxygen molecule and an oxygen atom: O3(g) + hν → O2(g) + O(g)  (Here, hν denotes a photon.)  Suppose a flask of ozone is irradiated with a pulse of UV light of wavelength 275 nm.  Assuming that each photon of this pulse that is absorbed breaks up one ozone molecule, calculate the energy absorbed per mole of O2 produced, giving the answer in kJ/mol.

A certain microwave oven delivers 750. watts (J/s) of power to a coffee cup containing 100.0 g water at 22.0°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/°C*g, and assume only the water absorbs the energy of the microwaves. The speed of light is 3.0*108 and the Planck‘s constant is 6,63 * 10-34 J/s.