Review TConstants |PerIodic TabieLearning Goal:To learn the restrictions on each quantum number.Part AQuantum numbers can be thought of as labels for an electron. Everyelectron in an atom has a unique set of four quantum numbers.What is the only possible value of m, for an electron in an s orbital?The principal quantum numbern corresponds to the shell in which theelectron is located. Thus n can therefore be any integer. For example,an electron in the 2p subshell has a principal quantum number ofn = 2 because 2p is in the second shell.Express your answer numerically.• View Available Hint(s)The azimuthal or angular momentum quantum number l correspondsto the subshell in which the electron is located. s subshells are codedas 0, p subshells as 1, d as 2, and fas 3. For example, an electron inthe 2p subshell has l = 1. As a rule, l can have integer valuesranging from 0 to n -1SubmitThe magnetic quantum number mų corresponds to the orbital in whichthe electron is located. Instead of 2pz, 2py, and 2pz, the three 2porbitals can be labeled –1, 0, and 1, but not necessarily respectively.As a rule, me can have integer values ranging from -l to +l.Part BThe spin quantum number m, corresponds to the spin of the electronin the orbital. A value of 1/2 means an "up" spin, whereas -1/2means a "down" spin.What are the possible values of me for an electron in a d orbital?Express your answer numerically with sequential values separated by commas.• View Available Hint(s)Submit

Part A ml is the magnetic quantum number and can have values -l to +l, where l is the azimuthal…

Part A What is the only possible value of mę for an electron in an s orbital? Express your answer numerically. • View Available Hint(s) Submit Part B What are the possible values of me for an electron in a d orbital? Express your answer numerically with sequential values separated by commas. • View Available Hint(s) Submit

Part A What is the only possible value of mę for an electron in an s orbital? Express your answer numerically. • View Available Hint(s) Submit Part B What are the possible values of me for an electron in a d orbital? Express your answer numerically with sequential values separated by commas. • View Available Hint(s) Submit

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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Please answer both question! Make sure its handwritten and legible!!
Select all allowed quantum number combinations that describe orbitals. ) n = 3;1 = 0; m = 0 On = 1;1 = 1; m = 0 ) n = 2; 1 = 1; m = 0 On = 4; 1 = 3; m = -3
Give only typing answer with explanation and conclusion 1. How many degenerate orbitals are in each of the following subshells? (Enter 0 if there are none.) a) n = 6, l = 0 2. Identify the subshell in which electrons with the following quantum numbers are found. (Enter your answers in the format 1s, 2p, etc.) a) n = 6, l = 4 b) n = 2, l = 0 c) n = 4, l = 3
Which values of ?ℓ are possible within the 2s subshell?
Please give typed answer andvwith detailed explanation. Not hand written answer .
Identify the problem in the given set of quantum numbers. Then, suggest a correct value. (ms has been omitted on purpose; the error is not that it is missing.) n = 4, l = 0, ml = 1 I
please explain and then give complete answer
what is the value of ml in the 4d orbital? what is the value of ms in the 4d orbital?
Y Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s²2p should be entered as [He]2s^22p^2. Submit Request Answer Part C Ti Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s²2p² should be entered as [He]2s^22p^2. Submit Request Answer Part D Те Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, He]2s 2p should be entered as [He]2s^22p^2.
1. If the nquantum number of an atomic orbital is equal to 3, what are the possible values of l? What are the possible values of mlif the quantum number l is equal to 2?
List these electron subshells in order of increasing energy. 3p, 3s, 2s, 2p Note for advanced students: you may assume these subshells are all in an atom with many electrons, not a hydrogen atom.
Which principle or rule is violated by the following orbital diagram of an atom in its ground state? Explain your answer. 1s 2s 2p () For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). A V 2エ BIUS Paragraph Arial 10pt AV II II ...