1. Record the colors observed in the alkali metal flame tests: Lithium: Sodium: Potassium: The emissions in these flame tests are produced when the valence electron in gas phase Group IA atoms falls from a higher energy orbital to a lower energy orbital. Demonstrate your understanding of this process by using three arrows to represent the three electrons in an atom of lithium and show how one of the valence electron "falls" from a higher-energy orbital in the excited-state configuration to a lower energy orbital in the ground-state configuration. 2p 2p 2s 2s 1s 1s Li Excited-State Li Ground-State 2. Visible light can be sorted by color (wavelength and frequency) from lower energy to higher energy: Red orange yellow green blue violet Higher Energy Lower Energy Given the color of light emitted when the electron drops from the higher-energy orbital to the lower-energy orbital, which energy gap do you predict to be larger? Which gap represents a greater energy change for the electron transition? 2p-2s gap in Li 3p-3s gap in Na or

1. Record the colors observed in the alkali metal flame tests: Lithium: Sodium: Potassium: The emissions in these flame tests are produced when the valence electron in gas phase Group IA atoms falls from a higher energy orbital to a lower energy orbital. Demonstrate your understanding of this process by using three arrows to represent the three electrons in an atom of lithium and show how one of the valence electron "falls" from a higher-energy orbital in the excited-state configuration to a lower energy orbital in the ground-state configuration. 2p 2p 2s 2s 1s 1s Li Excited-State Li Ground-State 2. Visible light can be sorted by color (wavelength and frequency) from lower energy to higher energy: Red orange yellow green blue violet Higher Energy Lower Energy Given the color of light emitted when the electron drops from the higher-energy orbital to the lower-energy orbital, which energy gap do you predict to be larger? Which gap represents a greater energy change for the electron transition? 2p-2s gap in Li 3p-3s gap in Na or

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...

See similar textbooks

Similar questions

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, Cl. You may write either the full or condensed electron configuration. x x. He-, 5.
dont give handwritten (only typed)
introducing calcium chloride into a flame imparts an intense orange color to the flame. To format the electron configuration correctly make sure to superscript where needed, do not add spaces to your answer and italics are not possible in this module.
What is the total number of orbitals associated with the principal quantum number 4? What is the total number of orbitals associated with the principal quantum number 3? What is the total number of orbitals associated with the principal quantum number 5? The quantum number represents the energy level. What is this quantum number?
Part 6: 6a. What trend in atomic radius occurs as you go up a group on the periodic table? Explain why this occurs. 6b. Write the complete electron configuration for Sr*. 6c. What element is the electron configuration for Sr+ isoelectric with? 6d. Write the abbreviated electron configuration for Bi. 6e. Write four quantum numbers to describe the highest energy electron in the Sr atom. The answer must include the four symbols and four correct numbers.
The Emission spectrum of an element is unique. Explain why the emission spectrum is sometimes referred to as an element’s fingerprint. Determine the nature of an unknown chemical. Relate it with Bohr’s Theory
The dazzling colors produced by fireworks result from excited gaseous atoms or molecules emitting light. The normal electron configuration of an atom is known as the "ground state." In ground state, all electrons are in the lowest energy levels available. When atoms or ions are heated, some electrons may absorb enough energy to allow them to "jump" to higher energy levels. The atom or ion is then said to be in the "excited state." The electrons cannot remain in this excited state for long and will emit energy in the form of light when they return to ground state. It is this light we see when an atom is heated in a flame. The frequency or color of light emitted depends on the energy difference between the excited state and the ground state. Chose the correct ground state configuration for Sr O 1:2322p 3s23p 43² 3d104p65s2 O 1:22p 3323p°4=?3410 4p7 O 1:?2,2p 3s23p 4s24p 441052 p75st
show your solution.
21 This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10 can find the meaning of any SI prefix in the ALEKS Data tab.) 1400 1200 energy (z)) 1000 Continue 56°F Clear 800 600 400 200 0 If the electron makes the transition shown by the red arrow, from B to A, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits Use this diagram to complete the table below. C B A Q Search nm C x10 X Ś DELL © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cente O P prt sc You home Submit end
1. Is there any observable pattern for ionization energy on the periodic table? What is it? 2. Is there any observable pattern for electron affinities on the periodic table? What is it?