Which statement about electrons and orbitals is false?In an atom with many electrons, 3d orbitals are lower in energy than the 4s orbital.There is a non-zero electron density on the nucleus in all s orbitals.Each orbital can hold zero, one or two electrons.The electrons with the same n and I values of their quantum numbers always have the same average separationfrom the nucleus.Orbitals with the same n and I values of their quantum numbers are degenerate.

An atom is made up of nucleus that consist of protons and neutrons.

hich statement about electrons and orbitals is false? In an atom with many electrons, 3d orbitals are lower in energy than the 4s orbital. O There is a non-zero electron density on the nucleus in all s orbitals. O Each orbital can hold zero, one or two electrons. The electrons with the same n and I values of their quantum numbers always have the same average separation from the pusle

hich statement about electrons and orbitals is false? In an atom with many electrons, 3d orbitals are lower in energy than the 4s orbital. O There is a non-zero electron density on the nucleus in all s orbitals. O Each orbital can hold zero, one or two electrons. The electrons with the same n and I values of their quantum numbers always have the same average separation from the pusle

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 96E: In the ground state of element 115, Uup, a. how many electrons have n = 5 as one of their quantum...

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How do 2p orbitals differ from each other? How do 2p and 3p orbitals differ from each other? What is a nodal surface in an atomic orbital? What is wrong with lp, ld, 2d, lf, 2f, and 3f orbitals? Explain what we mean when we say that a 4s electron is more penetrating than a 3d electron.
• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
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?
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
Which of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2
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.
6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.
Although no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could being orbitals. For g orbitals, the value of l is 4. What is the lowest value of n for which g orbitals could exist? What are tile possible values of ml? How many electrons could a set of g orbitals hold?
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.
Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 b. n = 5, ml = + l c. n = 5,ms = +12 d. n = 3, l = 2 e. n = 2, l = 1
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
What are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?