Energy in eV חח 0 -0.85 -1.51 -3.40 -13.60 Lyman series (ultraviolet, n₁ = 1) Paschen series (infrared, n₁ =3) Visible spectrum Balmer series (n₁=2) n = ∞ -n=5 n=4 n=3 n=2 n=1
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Which of the spectral lines of the hydrogen atom given below corresponds to a energy transition with the highest frequency?
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- A 10. The energy levels for a Bohr atom are shown below. n = 5 n = 4 n = 3 Toggle bookmark -4.90 eV -7.65 eV -13.6 eV -30.6 eV n = 2 -122.4 ev n = 1 If an electron moves from n = 1 to n = 5, what wavelength of light is absorbed? (h = 6.626 x 10-34,1 eV = 1.6 x 10-19 J) O 209 nm 10.6 nm 13.5 nm 452 nmThe wavelengths of the Lyman series for hydrogen are given by: = RH(1-1), n = 2, 3, 4, ... For the second of this series; calculate the energy (in eV). Note: 1.60 x 10^-19 J = 1.0 eV O 4.10 x 10^3 eV 2.12 x 10^3 eV 3² O 1.21 x 10^3 eV 3.30 x 10^3 eVThe wavelengths of the Lyman series for hydrogen are given by = R 1 (a) Calculate the wavelengths of the first three lines in this series. nm nm RH(1 - -/- 2 ), n = n nm x-ray region O infrared region O ultraviolet region ‚n = 2, 3, 4, ... (b) Identify the region of the electromagnetic spectrum in which these lines appear. O visible light region gamma ray region
- -1 7 ~ Energy (eV) w + -5 6s 5s 4s: 3s 615.8 515.2. 1139.6- 5p 4p 3P 589.2. 5d 4d 498.1 568.6 (b) 819.1 3d 5f 4f Figure b) Sodium with wavelengths listed in nm, and because 3p level is actually listed as the average of the two closely spaced levels, the wavelengths listed to this level are given as the average to the two closely spaced levels. All other fine structure splitting is negligible. 8 (a) What is the ground state of sodium? Assuming the 5s level of sodium is at -1 eV, and an electron decays from 5s to the 3p state and then from 3p to the 3s state, b) how much energy would each emitted photon carry? c) From these values calculate the ionization energy of sodium? (d) If Z'eff En = (-13.6ev) err n² what would be the effective nuclear charge felt by the 3s electron?In the equation below, the Balmer series involves the emission lines (wavelengths) obtained when electrons go from higher energy (excited) level to 1 1 R n' 1 where, R = 1.097 x 107 m-1 %3D -- A. The ground level (n = 1) B. The first atomic level (n = 2) C. The third atomic level (n = 3) D. The fourth atomic level (n = 4) E. The fifth atomic level (n = 4) %3D %3DCesium has a work function of 2.14 eV. What is the wavelength (nm) of a photon with the threshold energy to release an electron from the metal (with no kinetic energy)? [?] nm Hints: h = 6.63x10-34 J-s 1.00 eV 1.60×10-19 J = Enter
- The wavelengths of the Lyman series for hydrogen are given by = RH(1-2), = 2, 3, 4, ... 1/2 (a) Calculate the wavelengths of the first three lines in this series. nm nm nm (b) Identify the region of the electromagnetic spectrum in which these lines appear. O ultraviolet region O infrared region O x-ray region O visible light region O gamma ray regionThe K series of the discrete spectrum of tungsten contains wavelengths of 0.0185 nm, 0.0200 nm, and 0.0215 nm. The K-shel lontzation onargy is 69.5 kev. Determine the ionization energies of the L, M, and N shels ke ke kev Need Help? Read Master Subnt Anoa 13. DETAILS SERCP11 28.A.P.047. MY NOTES ASK YOUR TEACHER PRACTICE ANOTHER (0) How much energy is required to cause an electron in hydrogen to move from the n-2 state to the n-3 state? ev (b) If the eloctrons gain this energy by collision between hydrogen atoms in a high temperature gas, find the mimmum temperature of the heated hydrogen gas. The thermal energy of the heated atoms is given by 3kT/2. wihere k is the Boliemann conctant. Need Help? Read 14. DETAILS SERCP11 28.AP.048. MY NOTES ASK YOUR TEACHER PRACTICE ANOTHER A puled ruby liner emits lght at 604,3 nm. For a 14.7-ps pulse containing 3.40 Jof energy, find the folowing (a) the physical length of the pulse as it travak through space mmWavelength of the Balmer series is emitted as the electron in the hydrogen atom falls from, according to the above figure) n = (3 to ∞) to n = 2. What would be the specific wavelength of such a line for ni = 4? [Hint :1/λ = RH(1/nf2 – 1/ni2), RH being Rydberg constant = 1.097 × 107 /m] Group of answer choices 562 nm 486 nm 1122 nm 780 nm
- 2. Complete the table. Work Work Frequenc Maximum KE of Metal Function Function y Ejected electrons /J Solids in eV in Joules used /Hz Sodium 2.28 6 x 1014 Potassium 3.68 х 10:19 0.32 х 10:19 Lithium 2.9 1х 1015 Aluminium 4.1 0.35 х 10:19 Zinc 4.3 1.12 x 1019 Сopper 7.36 х 1019 1х 10153:09 O O O 63° A X • N N O 5G „ll Quizzes a (absorption) Brackett series Paschen series Lyman series (emission) Balmer series Paschen series (emission) n= 2 n=3 n=4 .... Lyman series n-5 (a) (b) e These pictures refer to the energy levels of a hydrogen atom. You can find the error in both parts, (a) and (b). The arrows labeled "emission" in (a), and all the arrows in (b), indicate a transition in which an electron jumps from a higher- energy state to a lower-energy state. The different "series" of emission lines are characterized by the index n of the low- energy state in which the electron ends up. In particular, the Lyman series consists of all transitions that end up in the n=1 energy level, with an initial energy level that corresponds to the label n = 2, 3, 4, 5, etc. One of these values of n is not shown as an arrow in the Lyman emission series in figures (a) or (b). This is a significant error because that particular spectral line is very important in astronomy. Pick the value…h = 6.63x10-34 Js, = h/(2T), hc = 1240 eV nm ao = 0.053 nm G = 6.67x10-11 Nm²/kg² 1. The Bohr model predicts that a hydrogen atom will have discrete orbital 'stationary' states, given by E=-13.6eV/n², where n = 1,2,3... A) Determine the lowest three stationary state energies of this atom, in eV. B) Calculate the wavelength of the photon produced as the electron drops from n=3 to n=2. C) Determine the change in angular momentum of the electron in part (B), according to the Bohr Model. D) Calculate the de Broglie wavelength of the electron at n=2. E) A photon is absorbed by this atom when the electron is at its ground state, causing it to escape the nucleus. (This is called 'ionization'). Calculate the maximum wavelength of this photon