2. A hydrogen atom is excited to the n = 8 level. Its decay to the...
9. An excited hydrogen atom emits light with a frequency of 1.141 x 10 HZ energy level for which n=4. In what principal quantum level did the electron begin
When an excited electron in a hydrogen atom falls from n = 6 to n=2, a photon of violet light is emitted. If an excited electron in an Het ion falls from n = 5, which energy level must it fall to (nı) for violet light of a similar wavelength to be emitted? ni =
Q22. A hydrogen atom is in its first excited state (n - 2). The angular momentum in the Bohr's m quantized: mevr-nh, where n 1, 2, 3,... and radii are given by rn- neao, ao-0.0529 nm. The linear momentum of the electron in kg m/s is a) 3 X 1024 b) 2 X 1024 c) 1X 1024 d) 4X104 e) 3 X 10-15
4. A hydrogen atom is excited by causing an electronic transition from (i) n = 2 to n3 and (ii) n=1 to n = 2 principle energy level. a) Which case needs more energy, (i) or (ii)? Why? b) If light is used as the energy source, which case absorbs a light with a longer wavelength? Why?
9.6 A hydrogen atom in its ground state (n = 1) is excited to the n = 5 level by absorbing photons. It then makes a transition to the n = 3 level and then from n = 3 level directly to the ground level. (a) What is the wavelength of absorbed photon? (b) What are the wavelengths of the emitted photons? [Answer: (a) 95 nm, (b) 1282 nm and 103 nm] Please show work and explain how. I do...
An electron in the Hydrogen atom is in the excited state with energy E2. a) According to the Bohr model, what is the radius of the atom in this state, in Angstroms? b) What is the wavelength le of the electron, in Angstroms? c) What is the momentum of the electron, in kg-m/s ? d) This atom decays from the excited state with energy E2 to the ground state with energy E1 . What is the energy of the emitted photon?...
A highly excited atom of hydrogen makes a transition from the n = 11 to the n = 10 state and emits a photon. What is the energy of this photon in joules? What is the wavelength in meters of the photon emitted when this highly excited hydrogen atom of hydrogen makes its transition from the n = 11 to the n = 10 state?
Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n 4 to the n=1 principal energy level. Recall that for hydrogen En-2.18x 10-18 J(1/n2). (h 6.63 x 10 34 J s) Select one: a. 3.08 x 1015s' b. 1.03x 108 s1 c. 2.06 x 1014s O d. 1.35 x 10-51 s1 e. 8.22 x 1014g
8· A hydrogen atom is in its ground state (n = 1). Find the wavelengths of photons it needs to absorb in order to (a) get excited to n-5 or (b) to eject a 10-eV electron.
4 Suppose hydrogen atoms absorb energy so that electrons are excited to the n-7 energy level. Electrons then undergo these transitions, among others (a) n 7 to n- (b) n 7 to n-6 (c) n-2 to n-1 Enter the letter (a, b, or c) for each. the smallest energy? the highest frequency? the shortest wavelength? What is the frequency of a photon resulting from the transition n-6 → n-1? h -6.62 x 10-34 J-s 4 Suppose hydrogen atoms absorb energy...