PART A - FLAME TESTS 1. Record the colors observed in the alkali metal flame tests: Lithium:red Sodium:Nclow 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. Potassium: Purple transitions & electronic Electronic structue to answer the auestions. 2p 2p 2s 2s 1s Li Excited-State 1s Li Ground-State 2. Visible light can be sorted by color (wavelength and frequency) from lower energy to higher energy: Red orange yellow Lower green blue violet Energy Higher 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 or 3p-3s gap in Na (circle one) 076e-Fireworks-Spring2020.docx 076-3 Last printed 1/10/20 7:31 AM

PART A - FLAME TESTS 1. Record the colors observed in the alkali metal flame tests: Lithium:red Sodium:Nclow 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. Potassium: Purple transitions & electronic Electronic structue to answer the auestions. 2p 2p 2s 2s 1s Li Excited-State 1s Li Ground-State 2. Visible light can be sorted by color (wavelength and frequency) from lower energy to higher energy: Red orange yellow Lower green blue violet Energy Higher 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 or 3p-3s gap in Na (circle one) 076e-Fireworks-Spring2020.docx 076-3 Last printed 1/10/20 7:31 AM

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 58AP: (a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The...

See similar textbooks

Similar questions

Given the valence electron orbital level diagram and the description, identify the element or ion. a. A ground state atom b. An atom in an excited state (assume two electrons occupy the 1s orbital) c. A ground state ion with a charge of 1
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
Spectroscopists have observed He+ in outer space. This ion is a one-electron species like a neutral hydrogen atom. Calculate the energy of the photon emitted for the transition from the n = 5 to the n = 3 state in this ion using the equation: En = − Z2/n2 (2.179 × 10−18 J). Z is the positive charge of the nucleus and n is the principal quantum number. In what part of the electromagnetic spectrum does this radiation lie?
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.
Planck originated the idea that energies can be quantized. What does the term quantized mean? What was Planck trying to explain when he was led to the concept of quantization of energy? Give the formula he arrived at and explain each of the terms in the formula.
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
Using vertical lines, indicate the transitions from Exercise 57 on an energy-level diagram for the hydrogen atom (see Fig. 2-9).
6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy levels, are we using deductive or inductive reasoning?
Scientists use emission spectra to confirm the presence of an element in materials of unknown composition. Why is this possible?
Answer the following questions: (a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom. (b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ?
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
Answer the following questions as a summary quiz on this chapter. (a) The quantum number n describes the ________ of an atomic orbital, and the quantum number describes its ________. (b) When n = 3, the possible values of are _________. (c) What type of orbital corresponds to = 3? ________ (d) For a 4d orbital, the value of n is _______, the value of is ________, and a possible value of m is _________. (e) Each of the following drawings represents a type of atomic orbital. Give the letter designation for the orbital, give its value of , and specify the number of planar nodes. Letter = ______ ______ value = ______ ______ Planar nodes = _______ ______ (f) An atomic orbital with three planar nodes through the nucleus is a(n) ______ orbital. (g) Which of the following orbitals cannot exist according to modem quantum theory: 2s, 3p, 2d, 3f, 5p, 6p? (h) Which of the following is not a valid set of quantum numbers? (i) What is the maximum number of orbitals that can be associated with each of the following sets of quantum numbers? (One possible answer is none. ) (i) n = 2 and =1 (ii) n = 3 (iii) n = 3 and = 3 (iv) n = 2, = 1, and m = 0