Answer correctly ## Calculating the Wavelength of a Spectral Line from an Energy DiagramThis section focuses on understanding the energy levels of electrons in an atom, as depicted in an energy diagram.### Diagram ExplanationThe displayed energy diagram illustrates the allowed energy levels of an electron in a specific atom. The diagram uses the SI prefix "zepto" (10⁻²¹) for measurements. ### Diagram Details- **Energy Levels**: The vertical axis of the diagram represents energy. Horizontal lines across the diagram symbolize different energy levels.- **Transitions**: Arrows between these lines indicate potential transitions an electron can make between energy states.### Activity Instructions- **Interactive Table**: Use information from the diagram to fill out the accompanying table.- **Ground State Energy Question**: "What is the energy of the electron in the ground state?" prompts learners to identify the energy at the lowest level.### Tools and Resources- **Explanation Button**: Provides additional information and context for understanding the diagram.- **Check Button**: Allows users to verify their answers.#### Note: - © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessibilityLearners are encouraged to explore how electron transitions between different energy levels lead to the emission or absorption of light at specific wavelengths, fundamental to understanding atomic spectra. **Title: Electronic Structure and Chemical Bonding: Calculating the Wavelength of a Spectral Line from an Energy Transition**---**Instructions:**Use the diagram to complete the table below.1. **Questions:** - What is the energy of the electron in the ground state? - [ ] ZJ - What is the energy of the electron in the first excited state? - [ ] ZJ - If the electron makes the transition shown by the red arrow, from A to B, will a photon be absorbed or emitted? - [ ] absorbed - [ ] emitted - Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. - [ ] nm**Interactives:**- **Explanation Button:** Provides detailed explanations for the concepts.- **Check Button:** Allows learners to verify their answers.**Diagram Description:**The diagram is not visible in detail, but it likely depicts an energy level diagram showing transitions between different energy states. The transition from A to B is indicated by a red arrow, signifying either photon absorption or emission based on the direction of the transition. The diagram assists in visualizing quantum jumps within an electron orbit, crucial for calculating spectral lines.---Explore these concepts further to understand the fundamental principles of quantum mechanics and electron transitions!

Answered: Image /qna-images/answer/f888e707-ae41-487c-8594-5e62d1c7c250.jpg

Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to B, will a photon be absorbed or emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. 02.J O absorbed O emitted nm X

Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to B, will a photon be absorbed or emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. 02.J O absorbed O emitted nm X

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter5: Electrons In The Atom

Section: Chapter Questions

Problem 89A

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Draw electron configurations for each of the following elements according to the Bohr model. Indicate which electrons are valence electrons. a. Mg b. S c. He d. K
Determine whether each statement that follows is true or false: a Electron energies are quantized in excited states but not in the ground state. b Line spectra of the elements are experimental evidence of the quantization of electron energies. c Energy is released as an electron passes from ground state to an excited state. d The energy of an electron may be between two quantized energy levels. e The Bohr model explanation of line spectra is still thought to be correct. f The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus. g Orbitals are regions in which there is a high probability of finding an electron. h All energy sublevels have the same number of orbitals. i The 3p orbitals of an atom are larger than its 2p orbitals but smaller than its 4p orbitals. j At a given sublevel, the maximum number of d electrons is 5. k The halogens are found in Group 7A/17 of the periodic table. l The dot structure of the alkaline earths is X, where X is the symbol of element in the family. m Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms. n Atomic numbers 23 and 45 both belong to transition elements. o Atomic number 52, 35, and 18 are arranged in order of increasing atomic size. p Atomic number 7, 16, and 35 are all nonmetals.
Which statement is true of the quantum mechanical model, but not of the Bohr model? a. Electrons orbit the nucleus in simple circular orbits, just like planets orbit the Sun. b. The exact path that an electron follows within an atom cannot be specified. c. The electron is attracted to the nucleus of the atom.
According to the Bohr theory, which of the following would have the higher energy? a. An electron in an orbit close to the nucleus b. An electron in an orbit located farther from the nucleus
Explain electron from a quantum mechanical perspective, including a discussion of atomic radii, probabilities, and orbitals.
Advances in technology and science often progress hand-in-hand. What advance in technology was necessary to set the stage for the discovery of the electron?
In J. J. Thompson’s experiment depicted in Figures 1.10 and 1.11, assume that the electrons are initially traveling at a speed of 8.00106ms1 in the +x direction and the electrostatic plates have a length of l=0.10m , between which the electrons are deflected toward the -y direction (downward) by an electric field of magnitude 200Vm1 . (Note that 1volt=1V=1JC1 .) Calculate S, the magnitude of the downward displacement, if the fluorescent screen is located 0.90 m beyond the exit of the region between the two electrostatic plates. No magnetic field is applied to counteract the electrostatic force. (Caution: L is not 1.0 m nor 0.9 m; see Figure 1.11.)
In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. In one transition between energy states, an electron moves from n=1 to n=2. Is energy absorbed or emitted in the process? Does the electron move closer to or farther from the nucleus?
6.11 Define the term photon.
Give electron configurations according to the Bohr model for each of the following elements. Indicate which of these elements you expect to be the most reactive and the least reactive. a. He b. Al c. Be d. Ne e. O
An atom that has five 3p electrons in its ground state is: a. Si b. P c. Cl d. O
Consider the transition from the energy levels n=5 to n=3. (a) What is the frequency of light associated with this transition? (b) In what spectral region does the transition occur? (c) Is energy absorbed?