**Question:**Three prominent spectral lines of wavelength λ are observed at 499nm, 508nm, and 523nm. What is the most likely composition of this sample?**Options:**Select one:- a. Helium- b. Lithium- c. Hydrogen- d. Chlorine- e. Oxygen- f. Neon**Analysis of Spectral Lines:** To determine the composition of the sample, match the given spectral wavelengths with known atomic spectra from the options provided. Each element emits or absorbs specific wavelengths of light, creating a unique spectral fingerprint.

Answered: Image /qna-images/answer/2a838bba-e344-4130-92c7-cf4cbb3ac889.jpg

Answered: Three prominent spectral lines of…

Similar questions

QUESTION 10 Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s. a. hc/1.89 b. 1.89 x h x c c. 1.89/hxc d. (1.51 + 3.4)/hc e. hc/3.4
A neutral atom of the element boron (B) has 5 electrons. Four of the electrons are removed, forming an ion with the one remaining electron. a) Sketch an energy level diagram for this ion, showing the ground state and the first two excited states. Label each state with the value of its energy. b) Calculate the two longest wavelengths at which this ion can absorb radiation. Assume all absorption occurs from the ground state. c) What is the minimum amount of energy needed to remove the electron from the ground state of this ion?
19. A certain atom holds an electron with an initial energy of 6.4 eV above the ground state energy. At some time later the energy is 3.2 eV above ground state. What is the frequency associated with the emission of the photon for this transition? A. 9.4x10¹4 Hz B. 7.7x10¹4 Hz C. 2.1x10¹4 Hz D. 8.9x1014 Hz
1a. One photon of light emitted from a hydrogen lamp is measured to have an energy of 0.6618eV. What electron transition is responsible for this photon? Hint: one of the energy levels involved is n = 3. 1b. What is the emission spectrum for a given element and why do different elements have different emission spectra?
What is the energy of a photon of wavelength 5.50 x 10-7 m, in Joules? [? [ ? ] × 10 [²] J Hint: c = Af
2. A photon is emitted from a hydrogen atom that undergoes an electronic transition from the state n=3 to the state n =2. Calculate (a) the energy, (b) the wavelength, and (c) the frequency of the emitted photon.
9
Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108m/s. a. 1.89 x h x c b. hc/3.4 c. (1.51 + 3.4)/hc d. hc/1.89 e. 1.89/hxc
4. The energy of the atom is in part determined by the electrical potential energy of the electron interacting with the proton nucleus, and when the electron is close to the nucleus it is very tightly bound. That's why the energy is negative, and larger in magnitude the smaller n. What does this tell you about the size of the atom for large n? Explain your reasoning.

Three prominent spectral lines of wavelength are observed at 499nm, 508nm, and 523nm. What is the most likely composition of this sample? Select one: Оа. Helium O b. Lithium O c. Hydrogen O d. Chlorine Ое. Охудen O e. O f. Neon