Only number 1 1. Complete the table below: Give the maximum number of electrons in an atom that can have each set ofquantum numbers. Then specify the orbital(s) in which the electrons with these quantum numbers would beTound. If a set of quantum numbers is not allowed, write not allowed in the spaces. Justify your answers.Quantum NumbersMaximum ElectronsOrbital(s) (include n values)n = 2, 1 = 1, m = 0n= 3, 1=2n = 4, m = -12. Give one set of allowed quantum numbers to correctly describe an electron in a 3d orbital. Compare withyour group, did you all come up with the same answers? Can there be more than one answer here? Why orwhy not? Explain.n =1 == lu3. As a group discuss how electrons are filled in energy-level diagrams using the following rules: AufbauPrinciple, Pauli Exclusion Principle, and Hund's. Then fill in the energy level diagram here for the groundstate electrons in a neutral arsenic (As) atom.4. Now take your diagram and translate it into anelectron configuration for arsenic.4d4p--3d4.s3p--3s|5. Now write three new diagrams (each group membercan choose one) for arsenic that each violate one of2p-2s-Tunlain why yourEnergy

Quantum numbers are defined as a set of four numbers (n, l, ml,ms) with the help of which we can get…

1. Complete the table below: Give the maximumm number of electrons in an atom that can have each set of quantum numbers. Then specify the orbital(s) in which the electrons with these quantum numbers would be Tound. If a set of quantum numbers is not allowed, write not allowed in the spaces. Justify your answers. Quantum Numbers Maximum Electrons Orbital(s) (include n values) n= 2, 1 = 1, m = 0 n= 3, 1=2 n = 4, m =-1

1. Complete the table below: Give the maximumm number of electrons in an atom that can have each set of quantum numbers. Then specify the orbital(s) in which the electrons with these quantum numbers would be Tound. If a set of quantum numbers is not allowed, write not allowed in the spaces. Justify your answers. Quantum Numbers Maximum Electrons Orbital(s) (include n values) n= 2, 1 = 1, m = 0 n= 3, 1=2 n = 4, m =-1

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 105E: One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of...

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Similar questions

Construct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?
• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. Briefly explain your answers.
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
Write a complete set of quantum numbers (n, , m) that quantum theory allows for each of the following orbitals: (a) 2p, (b) 3d, and (c) 4f.
Use the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?
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.
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 experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?
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?
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
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When none is the correct answer, explain your reasoning. (a) n = 3, = 0, m = +1 (b) n = 5, = 1, (c) n = 7, = 5, (d) n = 4, = 2, m = 2