1. Complete the table: Examine the sets of quantum numbers shown below. For each set, indicate (a) whether the set is allowed, and (b) if allowed, indicate the orbital in which the electron resides in the ground state (example: 1s) If allowed, Allowed ? (circle yes or no) m, m, name orbital 1 +1/2 yes no 3. 2 -1 +1/2 yes no +2 -1/2 yes no -2 +1 yes no -2 +1/2 yes no 2. How many d orbitals are possible for n = 6? 3. How many f orbitals are possible for n = 3?

1. Complete the table: Examine the sets of quantum numbers shown below. For each set, indicate (a) whether the set is allowed, and (b) if allowed, indicate the orbital in which the electron resides in the ground state (example: 1s) If allowed, Allowed ? (circle yes or no) m, m, name orbital 1 +1/2 yes no 3. 2 -1 +1/2 yes no +2 -1/2 yes no -2 +1 yes no -2 +1/2 yes no 2. How many d orbitals are possible for n = 6? 3. How many f orbitals are possible for n = 3?

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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101 Chem101 b My Questions | bartleby x + -> app.101edu.co M Apps G M Gmail YouTube Maps a AMAZON Translate O Gflights Case Status Onlin... b Homework Help a... C Get Homework He... > KATAPULK CUBA 23 Agencia Supermar.. Reading List Question 3 of 22 Submit Which of the following is not permitted as a plausible orbital designation according to quantum theory. A) 4f B) 7s C) Зр D) 3f +
A) Identify the subshell (e.g., 1s, 2p, 3d, etc.) in which electrons with the following quantum numbers are found: i) n = 2, l = 1 : ii) n = 4, l = 2 : iii) n = 6, l = 4: B) Select the combinations that are allowed and those that are not? (If allowed write Yes & if not write No) : i) n = 3, l = 3, ml = 0, ms = -1/2: ii) n = 4, l = 3, ml = -1, ms = +1/2: iii) n = 5, l = 2, ml = +3, ms = -1/2: iv) n = 2, l = 1, ml = -2, ms = -1: C) Give the maximum number of electrons in an atom that can have the following quantum numbers: i) n = 5: ii) n = 4, ms = +1/2: iii) n = 3, l = 2:
1. How many f orbitals can have the value n=3? Answer 2. How many electrons in an atom can have the following designations? n=5 and ml=2? Answer W3. hat is the short hand electron configurations for Bi? When writing your answer do not put in any spaces ex: [He]2s22p1.
8. Hund's rule states that a) in the same orbital only 2 electron of opposite spin are possible b) we cannot know the exact position of an electron c) the p orbital must always be filled before the s orbital d) each electron tends to occupy an empty orbital before occupying an orbital which contains another electron 9. Which of the following sets of quantum numbers are impossible? Explain your choice a) (1,0, 0, -½) d) (4,3,-2, +½) b) (3,0,1, +½) e) (3,2,1,1) c) (2,2,1, +½)
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Which of the following set of quantum numbers (ordered n, ℓ, mℓ, ms) are possible for an electron in an atom? Check all that apply.
(Give clear handwritten answer) Give wavelength in manometers of light from hydrogen atom when electron transitions from the n1= 7 to the n2 = 2 orbital?
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Choose the valence orbital diagram (the valence electrons) that represents the ground state of Si. Note: ground state just means "regular" configuration. It does not change anything. A) 1 1 4s 4p B) 1 1 3s 3p C) 1L 1L |1 1 4s 4p D) 1L 1L 1L 1L 4s 4p E) 1L 1L 1 3s 3p
geNSUINortheastern St Content OWLv2 LOnline teaching. Chomistry uestion Lbart| vLAShort Panor: Alcohol/Foo O X Screenshot 2020-11-15 at 10.52... O O Q Q Write the electron configurations for the following species: (Do not use noble gas notation and enter the subshells in the order in which they are filled. Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s²2s².) a. Mg²+ b. Rb+ с. Те2- d. O²- Submit Answer Try Another Version 3 item attempts remaining 10:52