Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers n = 1, l = 1, me = 0 n = 4, = 2, me = 2 n = 2, 1, me = -1 n = 3, 2, me = -3 n = 5,l = 3, me = 1 4f 3s 2d 4p 5f not allowed Answer Bank 3d 4s 2p 5d 3p 4d 1p 1s 5s 5p 2s 3f

Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers n = 1, l = 1, me = 0 n = 4, = 2, me = 2 n = 2, 1, me = -1 n = 3, 2, me = -3 n = 5,l = 3, me = 1 4f 3s 2d 4p 5f not allowed Answer Bank 3d 4s 2p 5d 3p 4d 1p 1s 5s 5p 2s 3f

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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Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number ({), the magnetic quantum number (mp), and the spin quantum number (m,) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. n = 4, l = 0, me = 1, m, = – n = 6, l = 6, me 1, mş = - п%3D 3, е %3D 2, те — — 1, m, — + n = 3, l = -2, mẹ = -1, m, = - 2 n = 5, l = 1, me = 0, m, = + O n = 2, € = 0, mẹ = 0, mş = –1
Which of the following combinations of quantum numbers is not allowed? O n = 4,1 = 2, m = 0, m, = 1/2 On = 2,1 = 1, m¡ = -1, mg 1/2 On = 3, 1 = 0, m¡ = 0, m, = -1/2 O n = 1,1 = 1, m = 0, m, = 1/2 O n = 4, 1 = 3, m¡ = -2, m, = -1/2
Which statement is true for the 2p orbitals of a C atom (atomic number = 6)? They are lower in energy than 2s orbital. The angular quantum number is 1-2. The allowed magnetic quantum numbers are: 0, 1, 2 The principal quantum number is n = 2.
Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number (e), the magnetic quantum number (m,), and the spin quantum number (m,) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. n = 2, l = 1, mę = -1, mş = 1 n = 3, l = 1, mę = 1, mş = - Un = 2, l = 2, mẹ = 0, ms = - n = 5, l = 3, mẹ = -3, ms = - n = 4, l = 2, mẹ = 3, m, = + %3D O n = 3, l = -1, mẹ = 1, m, = -
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Enter full electron configurations for each of the following ions. P3− Express your answer in complete form, in order of increasing orbital. For example, 1s22s2 would be entered as 1s^22s^2.
Which is not a valid set of quantum numbers for an electron in an atom? On= 3,1=2, mj= -1, mg = -1/2 On=2,1= 1, mj= 1, mg = +1/2 On= 4,1= 4, mj=-1, mg=+1/2 On= 5,1=3, m = -2, m, = -1/2