Whats the wavelength of a photon of light that permits a hydrogen atom to go from its energy level 3 to its energy level 2? 434nm 121.6nm 486.1nm 656.3nm Whats the wavelength of a photon that could make a hydrogen atom jump from energy level 4 to energy level 2? 656.3nm 121.6nm 102.6nm 486.1nm

Find the energy of the following. Express your answers in units of electron volts, noting that 1 eV = 1.60  10-19 J.(a) a photon having a frequency of 7.20  1017 Hz eV (b) a photon having a wavelength of 5.00  102 nm eV

Example: An electron in a hydrogen atom drops from energy level E4 to energy level E2. What is the frequency of the emitted photon, and which line in the emission spectrum corresponds to this event? E6 E = -0.378 eV Step 1: Es E = -0.544 eV - E= -0.850 eV Find the energy of the photon. E E = Einitial - Efinal E3 E=-1.51 eV = (-0.850 eV) - (-3.40 eV) = 2.55 eV Step 2: Use Plank's equation for frequency. E₂ E= -3.40 eV 12 E E = hf; f = h (2.55 eV) (1.60 x 10-191 6.63 x 10-34 Js f= 6.15 x 10¹4 Hz Line 3 is in the visible part of the electromagnetic spectrum and appears to be blue. The frequency f = 6.15 x 10¹4 Hz lies within the range of the visible spectrum and is toward the violet end, so it is reasonable that light of this frequency would be visible blue light. Step 3: Find the corresponding line in the emission spectrum. Examination of the diagram shows that the electron's jump from energy level E4 to energy level E2 corresponds to Line 3 in the emission spectrum. 3 Incoming photon…

An electron at the n=5 energy level of hydrogen undergoes a transition to the n=3 energy level. What wavelength of photon does the atom emit in this process?   a) 1.28 x 10^-6 m b) 2.37 x 10^-6 m c) 4.22 x 10^-7 m d) 3.04 x 10^-6 m e) 5.92 x 10^-5 m

What is the energy of a hydrogen electron in the following energy states? A) n=5  b) n=3  c) what is the energy of a photon emitted when an electron transitions from the n=5 state to the n=3 state? d)what is the wavelength of this photon

A photon of light has a frequency of 5.00 x 1014 Hz. If the frequency of the photon was doubled then which of these would happen to the energy of this photon? a. it would double b. it would triple c. it would quadruple d. it would become one-fourth as much e. it would become half as much

3) What is the wavelength of a photon in nanometers, having energy of 2.00 eV? (e-3.00 - 10 m/s, h = 6.626 x 10-34 J-s, 1 eV = 1.60 × 10-19 J) s)

3. A. 279.7 kJ of energy are required to remove one mole of electrons from one mole of lithium atoms. What is the maximum wavelength of light that can remove one electron from one lithium atom? (h = 6.626 x 1034J•sec, c = 3.0 x 10* m/s) B. Assume that a hydrogen atom's electron has been excited to the n= 5 energy level. How many different wavelengths of light can be emitted as this excited electron loses energy? Include a diagram to support your answer.

1a) Light that has a frequency of about 5.55 * 1014 Hz (a wavelength of about 543 nm) appears green to our eyes. What is the energy in joules of the photons associated with this light?=__________ J     1b) The human eye is sensitive to yellow-green light having a frequency of about 5.5 * 1014 Hz (a wavelength of about 550 nm). What is the energy in joules of the photons associated with this light? =_____________J

) a) What temperature is required for a black body spectrum to peak in the X-ray band? (Assume that E = 1 keV). What is the frequency and wavelength of a 1 keV photon? b) What is one example of an astrophysical phenomenon that emits black body radiation that peaks near 1 keV? c) What temperature is required for a black body spectrum to peak in the gamma-ray band with E = 1 GeV? What is the frequency and wavelength of a 1 GeV photon? d) What is one example of an astrophysical phenomenon that emits black body radiation that peaks at 1 GeV?