4. In a hydrogen atom, the 3s, 3p, and 3d orbitals are degenerate. In a multielectron atom, the 3s, 3p, and 3d are not degenerate. First explain what "degenerate orbitals" is referring to. Then, explain why this is so.

4. In a hydrogen atom, the 3s, 3p, and 3d orbitals are degenerate. In a multielectron atom, the 3s, 3p, and 3d are not degenerate. First explain what "degenerate orbitals" is referring to. Then, explain why this is so.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter15: Introduction To Electronic Spectroscopy And Structure

Section: Chapter Questions

Problem 15.22E

See similar textbooks

Related questions

Q: For an He+ ion, do the 2s and 2p orbitals have the sameenergy? If not, which orbital has a lower…

A: He+ has only one electron. So, for a single electron system, energy depends on Principal quantum…

Q: Which of the following sets of quantum numbers is not allowed?

A: There are four sets of quantum number for a particular electron in an atom :- principle quantum…

Q: Consider a 4d orbital. a. What are the allowed values for the n and l quantum numbers for a 4d…

A: Quantum numbers are like address of an electron in an atom There are four quantum numbers…

Q: Give a combination of four quantum numbers that could be assigned to an electron occupying a 5p…

A: The four types of quantum numbers used to locate an electron in an atom are as follows: Principal…

Q: For a hydrogenic atom all orbitals in a given shell are energetically degenerate. What does this…

A: Single-electron atoms : The atoms which has only one electron is categorize into this category.That…

Q: Sketch and clearly label the orbital energy diagrams for As and K using arrows to represent the…

Q: Suppose that the spin quantum number did not exist, and therefore only one electron could occupy…

Q: 6.8 B Using quantum numbers, explain why there is no 2d subshell.

A: ANSWERE IS DISCUSSED BELOW :

Q: Quantum Numbers" (Quantum Mechanical Description and the Electronic Structure of Atoms) Answer the…

A: a) There are four quantum numbers, Principal quantum number (n) Azimuthal quantum number (l)…

Q: Which quantum number distinguishes the different shapes of the orbitals? n (shells) l (subshells)…

A: In quantum theory, there are 4 different quantum numbers Principle quantum number (n) for a number…

Q: Give sets of four quantum numbers for two electrons that are (a) in the same energy shell and…

A: A question based on quantum numbers, which is to be accomplished.

Q: The elements Ge, As, Cd, Te, Al are all used in the manufacture of various semiconductor devices.…

A: Atomic number of germanium is 32.The electronic configuration is [Ar]3d104s24p2.Atomic number of…

Q: (a) The quantum number n describes the. * an atomic orbital and the quantum number e describes its…

Q: Write the 4 quantum numbers for Rhodium’s LAST valence electron.

Q: Suppose you have an h-orbital. What is the smallest value n could be for an h-orbital?

Q: Determine the number of atomic orbitals in subshells with the following values of the orbital…

A: Given : ℓ = 0, 2 and 3.

Q: Consider 3px and 3py orbitals. Which quantum number(s) is (are) the same for thesetwo orbitals?…

A: There are four quantum number for an orbital. 1. Principal Quantum number(n) 2. Azimuthal Quantum…

Q: An orbital in a ground-state gas-phase As atoms has n=3, l=1. How many electrons are in this…

A: The electronic configuration is shown below: As-1s22s22p23s23p63d104s24p3

Q: a. In Atomic orbital theory, we've seen that as we go through the periodic table we see more and…

A: Slater rule for calculating the Zeff for 4s and 3d electrons of vanadium. The rule states that the…

Q: List the following orbitals in order of increasing energy: 2s, 2p, 4s, 1s, 3d, 3p, 4p, 3s

A: Aufbau Principle indicates that electrons are filled in the increasing order of their energy levels.…

Q: Write all subshells (# of subshells) for the principal quatum number n=4. Label the quantum number…

A: Write all subshells (# of subshells) for the principal quatum number n=4

Q: Why do the 4s, 4p, 4d, and 4f orbitals have the same energy in the H atom, but different energies in…

A: Energy of H-atom = -13.6 z2/n2 So, here the energy of the Hydrogen atom only depend on the 'n'…

Q: se quantum numbers to designate the following: All 5p orbitals and all valid electrons in the 2s…

A: Pauli exclusion principle states that every electron placed in any orbital will possess a different…

Q: Match the quantum number with the correct description. Principle energy level 1. n Electron Magnetic…

Q: The following do not represent valid ground-state electronconfigurations for an atom either because…

A: According to Pauli's exclusion principle, no two electrons in an atom can have same values of all…

Q: At what radius (radii) will an electron not be found in the 1s, 2s, 2p and 3s orbitals.

A: To find out the radius of an nth orbit in a hydrogen atom we use the formula of Bohr's radius.…

Q: Which statement about the Schrödinger equation is true? A - The Schrödinger equation gives the…

A: The following statements are correct about Schrödinger wave equation:

Q: b) For the principal quantum number, n=3, determine the number of allowed subshells (different…

A: A question based on atomic structure, which is to be accomplished.

Q: In a hydrogen atom, orbitals with the same energy: I) are the same distance from the nucleus. II)…

A: Orbitals having the same energy are called as degenerate orbitals. Principal quantum number is the…

Q: How many distinct Second electron shell, where n- 2?p or bitals exist in the orbitals i

Q: Consider a 3d orbital. a. What are the allowed values for the n and l quantum numbers for a 3d…

A: Here use the concept of Quantum numbers.

Q: 6) Write an acceptable set of the first three quantum numbers for the following electron…

A: Principal quantum number, n is used to determine the energy of electron. Azimuthal quantum number, l…

Q: Explain why an electron behaves in ways that are at least partially indeterminate?

Q: Use the References to access important values if needed for this question. Give the ground-state…

A: (a) C The atomic number of C is 6. Thus, its electron configuration is : 1s22s22p2 or [He]2s22p2

Q: Which of the following represents Hund’s rule? A. No two electrons can have the same set of quantum…

A: HUND'S RULE HAVE VARIOUS FORM,WILL EXPLAIN THEM BY EXAMPLE

Q: According to Hund’s rule, how are degenerate orbitals occupied?

A: The arrangement of electrons in the atomic orbitals according to Aufbau principle, Pauli’s exclusion…

Q: If you have 14 electrons to be distributed at 4p, 4d and 5s, determine the 4 quantum numbers for…

Q: vi) d-orbital can have maximum of............. electrons. ✔ a. 2 b. 6 c. 10 d. 18 alement?

A: Maximum number of electrons held in the d orbitals is 10.There are 5 sub-levels in a d orbital, each…

Q: The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four…

A: Concept is based on Quantum numbers:

Q: Write the electron configurations for the following species: (Do not use noble gas notation and…

Q: Consider a 3d orbital. a. What are the allowed values for the n and l quantum numbers for a 3d…

A: Fill in the blanks by using rule of quantum number --

Q: Fill in the blanks. Write the correct answer in the space provided. a. The number of orbitals with…

A: Given: a. The number of orbitals with the quantum numbers n=5, l=3 and ml = 1 is _________. b. The…

Q: quantum numbers and orbital notation. Explain why these are impossible. a. n=4, =2, m²-3, m,=-½ b.…

A: ->n,l,ml,ms are quantum number then l =0 ( s orbital) l = 1 ( p-orbital ) l = 2 ( d-orbital) l =…

Question

4.
In a hydrogen atom, the 3s, 3p, and 3d orbitals are degenerate. In a multielectron atom,
the 3s, 3p, and 3d are not degenerate. First explain what “degenerate orbitals" is referring to. Then,
explain why this is so.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Suppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.
In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
What major assumption (that was analogous to what had already been demonstrated for electromagnetic radiation) did de Broglie and Schrodinger make about the motion of tiny panicles?
State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. Briefly explain your answers.
What type of electron orbital (i.e., s, p, d, or f) is designated by (a) n=3,l=1,m l =1?(b) n=5,l=0,m l =0? (c) n=6,l=4,m l =4?
The table below is partially completed for subshells A and B, where subshell B is the next subshell higher in energy compared to subshell A. For example, if subshell A is the 4s subshell, then subshell B would be the 3d subshell. Use this criteria and the information provided to complete the table.
What type of electron orbital (i.e., s, p, d, or f) is designated by an electron with quantum numbers (a) n=1,l=0,m l =0(b) n=3,l=2,m l =1? (c) n=4,l=3,m l =3
Heated lithium atoms emit photons of light with an energy of 2.9611019 J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?