The atomic emission spectrum of sodium (LEFT) and the molecular flame emission spectrum of CaOH(RIGHT) are given below. Explain why the CaOH spectrum is much broader than the sodium emissionline.nision588590S505540520S500S40Wavelength, nmWavelengh, AA. Sodium atom has many vibrational and rotational states and thus many excited energy levels.B. Sodium is present largely as atoms that emit at only a few discrete wavelengths.C. The molecule CAOH has many vibrational and rotational states and thus many excited energy levels.D. A and BE. B and CIntensity

Answered: Image /qna-images/answer/13843eb8-72b3-4337-8779-21a4dac4ceaf.jpg

Answered: The atomic emission spectrum of sodium…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4. Explain why and what makes the spectrum of hydrogen different from the spectrum of helium.
Consider a hydrogen atom in the ground state. What is the energy of its electron? E = ?j Now consider an excited‑state hydrogen atom. What is the energy of the electron in the N = 3 level? E3 = ?j
О Which of the statements most accurately describes the following electron configuration? 1 ↓ 1 a. It is a valid configuration for a ground state atom. b. It violates the aufbau principle. c. It is invalid and violates multiple rules/principles. d. It violates the Pauli exclusion principle. e. It violates Hund's rule.
The quantum number that characterizes the electron in the lowest energy level of the hydrogen atom is n =1, l=0, m=0; and s= +½. Electron excitation can promote to higher energy levels. Which set of quantum numbers is forbidden for excited electrons? a. n = 1, l = 0, m = -1, s = +1/2 b. n = 3, l = 1, m = 0, s = +1/2 c. n = 3, l=2, m = -2, s=-1/2 d. n = 7, l = 4, m = -2, s = +1/2
Determine the wavelength of light emitted in an electron transition from n=4 to n=2 in a Be³⁺ ion. a. 40.2 nm b. 80.6 nm c. 30.4 nm d. 20.5 nm e. 60.4 nm
a. The following is not a possible set of quantum numbers. Which of the quantum numbers is not consistent with the others, or is just wrong? n=4 l=2 ml=0 ms=0 b.The following is not a possible set of quantum numbers. Which of the quantum numbers is not consistent with the others, or is just wrong? n=2 l=1 ml=-1 ms=0
5. An electron in a hydrogen atom makes a transition from ann= 2 orbital to an n = 5 orbital. a. For this electron transition, is energy being absorbed or released? Circle one. ABSORBED RELEASED b. Calculate the energy difference for this transition and the wavelength (in nanometers) of the photon involved in this transition.
The soft yellow glow of many streetlights is produced by small amounts of sodium metal present in the bulbs. In the line spectrum of sodium, this light has a wavelength of 589 nm. ES a Wavelength, nm 500 400 700 600 When sodium absorbs energy, its highest-energy electron jumps from the ground state to energy level 3p. When the electron relaxes back down, it releases this energy as 589-nm yellow light. Write the electron configuration for sodium in its ground state, and then write the electron configuration for the excited sodium atom. Top to bottom: k en biggs/Alamy Stock Photo; Macmillan Learning
Molybdenum metal must absorb radiation with a minimum frequency of 1.09 × 1015 s before it can eject an electron from its surface via the photoelectric effect. а. What is the minimum energy required to eject an electron? b. What wavelength of radiation will provide a photon of this energy? c. If molybdenum is irradiated with light of wavelength of 120 nm, what is the maximum possible kinetic energy of the emitted electrons? 6.626xx0 66 X10
What is the wavelength of light that has a frequency of 7.155 x 1014 s-1? Note that - 1 nm = 1 x 10-9 m Note: In problems dealing with frequencies, wavelengths, photon energies, or electron transitons in hydrogen atoms, you may need some of the following equations: 1 v = c where c = 2.99792458 x 108 m s1 Ep = h v where h = 6.6260755 x 1034 J s En = -RH / n2 where RH 2.1798741 x 10-18 j %3D
Write the ground-state electron configuration for calcium, Ca. You may write either the full or condensed electron configuration. x x. He -, | 8. Write out the ground-state electron configuration for chlorine, CI. You may write either the full or condensed electron configuration. x| x. He 8.
9. Calculate the energy in electron volts of an X-ray photon with a wavelength of 6.24 Å.

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