Quantum number Symbol Function indicates the spin of the electron defines the spatial orinetation of an orbital The principal quantum number The angular-momentum quantum number defines the three- dimensional shape of an orbital The magnetic quantum number defines the size and energy level of an orbital mg The spin quantum number

Quantum number Symbol Function indicates the spin of the electron defines the spatial orinetation of an orbital The principal quantum number The angular-momentum quantum number defines the three- dimensional shape of an orbital The magnetic quantum number defines the size and energy level of an orbital mg The spin quantum number

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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13
Which of the following could represent the electron configuration of an excited state phosphorus atom? [Ne]3s23p25s1 [Ne]3s23p3 [Ne]3s13p3 [Ne]3s23p35s1 [Ne]3s23p4
Consider a helium ion with one electron in the ground state. It turns out that it would take about 28 eV to remove this electron through ionization. Blue photons have an energy of about 4 eV. Can this electron emit about 7 blue photons. Is this true? Why or why not?
List the values of all four quantum numbers for each of the valence electrons of radium (Ra). State how these two sets of quantum numbers satisfy Pauli exclusion principle. List all the possible values of magnetic quantum number for the electrons in praseodymium? How many magnetic quantum number values are possible for the electrons in the energy level that is closest to the nucleus of praseodymium? List the values.
Absorption of light provides energy to move an electron from a lower energy orbital to a higher energy orbital. A lower energy light, such as red, is sufficient to move the electron if the energy gap between the orbitals is O red O small O blue O large
Which of the following quantum numbers describes about orientation of orbitals? Va. Magnetic quantum number Principal quantum number * Angular momentum quantum number O d. Spin quantum number
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
Complete the table below by filling in the principal quantum number n and angular momentum quantum number / for each electron subshell listed. subshell 4f 4d 7p 6s principal quantum number n 1 7 angular momentum quantum number / 1 0 0 X Ś
Radio waves from an FM radio station have a frequency of 106.1 MHz. Calculate the energy of one photon of light at this frequency.
If 0.0600 mol H2(g) reacts with 0.0220 mol Nalg), how much ammonia is expected to be produced? O a. 2.41x 1022 molecules O b. 3.61x 102² molecules Ос 1.02 8 O d. 0.7g O e. 2.65x 1022 molecules Which one of the following electron configurations is for an atom in the ground state? O a. [Ne]3s23p34s O b. [Kr]5s+4ds E of 2 Oc. [Ar]4s23d O d. [He]3s23p3 O e. 1s2s23p4523d ENG 4) a ^ F1 F2 F3 F4 F5 F6 F7 F9 F10 @ %23 & 3 7 V 8A Q W Y UI S D FJG YH1J K の * 00 本 A LO 4\
49. Which of the following correctly identifies how Louis de Broglie's concept of the electron as a particle-wave helped to explain energy levels for an electron in an atom. A. de Broglie described the electron orbit as a circular standing wave pattern with a specific angular momentum as required by the Bohr hypothesis. B. de Broglie described the electron as a planar wave with a non- specific frequency as required by the Bohr hypothesis. C. de Broglie described the electron as a wave whose range of frequencies was continuous and thus allowed for all the possible electron energies predicted by Bohr. D. de Broglie described the electron as a spherical wave whose wavelength was dependent upon the speed with which it orbits the nucleus, as needed to explain the Bohr hypothesis.
Complete the table below by providing a set of quantum numbers for the last four electrons in an phosphorus atom