### Quantum Theory and Orbital Question#### Multiple-Choice Question:According to the quantum theory, how many \( (d) \) orbitals are there in the \( n = 4 \) shell?**Options:**- a. 1- b. 3- c. 5- d. 7- e. d orbitals are not allowed in the \( n = 4 \) shell.#### Detailed Explanation:In the context of quantum theory, the principal quantum number \( n \) can have any positive integer value. The \( n = 4 \) shell can have \( s \), \( p \), \( d \), and \( f \) orbitals:- **1** \( s \) orbital - **3** \( p \) orbitals - **5** \( d \) orbitals - **7** \( f \) orbitals Therefore, the correct answer to this question is **c. 5**.This exercise is part of learning the distribution of electrons in atomic orbitals according to quantum mechanical principles.

How many d orbitlas in 4 th shell.

Answered: 8. According to the quantum theory, how…

8. According to the quantum theory, how many (d) orbitals are d. 7 a. 1 b. 3 8.911 c. 5 e. d orbitals are not allowed in the n = 4 shell

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...

See similar textbooks

Similar questions

Which atomic orbital is spherical in shape? Select one: a. 2s b. 4f c. 3d d. 3p
Iron has the following electronic configuration 1s²2s²2p63s²3p64s²3d6. What would be the values for the principal quantum number (n) and the angular momentum quantum number (1) for one of its valence electrons? A b. n = 4, and 1=2 B) c. n = 4, and 1=3 a. n = 3, and 1 = 3 d. n = 3, and I=2
Hello, I am having trouble understanding these two questions about quantum numbers. 1. The principle quantum number for the 3 outermost electrons in Sc are A. 3, 3 and 3.B. 4, 4 and 3.C. 4, 4 and 4.D. 3, 3, and 4.E. 4, 4, and 5. 2. Which of the following set of quantum numbers is possible? A. n =2, l = 0, ml = 1, ms =1/2B. n =3, l = 3, ml = 2, ms =1/2C. n =4, l = 3, ml = 3, ms = –1/2D. n =3, l = 3, ml = 2, ms = –1/2E. n = 2, l = 1, ml = 2, ms = –1/2 Any help is greatly appreciated thank you :)
2. Electrons are in different orbitals outside of the nucleus. As we know, the nucleus is positively charged, and electrons are negatively charged. Take the nickel atom as an example, it has 28 electrons, and all reside in different orbitals. a. What are the complete, condensed, and valence electron configurations of nickel atom? b. There will be some electrons on 3d orbitals. What are the four quantum numbers for each electron in the 3d orbitals?
Suppose that in an alternate universe, the possible values of l are the integer values from 0 to n (instead of 0 to n - 1). Assuming no other differences between this imaginary universe and ours, how many orbitals exist in each level in the alternate universe? a. n = 1 b. n = 2 c. n = 3
Which of the following will be the same for all orbitals in a given subshell? I. the n quantum number II. the l quantum number III. the m quantum number IV. the energy III and IV only O I, Il and IIl only I and II only O Il and IV only I, II, and IV only
Write out a possible set of quantum numbers for an electron in each of the following a. a 3p electron b. a 5p electron c. a valence d-orbital electron of iron
Draw the following orbitals with as much detail as possible and draw the electron probability distribution graph a. 3s b. 2p c. 3d
The following are 2s, 2p, sp, sp?, and sp orbitals, in random order. Which of these orbitals exhibits 33% s character? II II Select one: O a. I O b. I O . II O d. IV O e. V
3. Which of the following represents Hund’s rule?A. No two electrons can have the same set of quantum numbers.B. The electrons are added to lower energy atomic orbitals before higher energy orbitals.C. Unpaired spins are maximized in lowest energy configurations for degenerate orbitals.D. The position and momentum of a particle cannot be known precisely at the same time.
) The element whose atoms in the ground state have three half-filled orbitals isNa. Mg. Si. O. As. Al
) Which combinations ofn and I represent real orbitals, and which do not exist? d. 2d a. 1s b. 2p С. 4s