Which statements are true about the isolated, single p orbital shown below? 8 I. It can hold up to two electrons. II. It can hold up to six electrons. III. An electron in this orbital moves around the edge in a figure eight pattern. IV. An electron of a certain energy is highly likely to be found within the orbital, but we cannot say exactly where. O II and III O II and IV OI and III O I, II, III, and IV are all corect

Which statements are true about the isolated, single p orbital shown below? 8 I. It can hold up to two electrons. II. It can hold up to six electrons. III. An electron in this orbital moves around the edge in a figure eight pattern. IV. An electron of a certain energy is highly likely to be found within the orbital, but we cannot say exactly where. O II and III O II and IV OI and III O I, II, III, and IV are all corect

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section5.5: Quantum Numbers, Energy Levels, And Atomic Orbitals

Problem 5.12E

See similar textbooks

Similar questions

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?
Answer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.
Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1s22s23p1 b. 1s22s22p6 c. 1s22s22p43s1 d. [Ar]4s23d54p1 How many unpaired electrons are present in each of these species?
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
rue or false? The hydrogen atom has a 3 orbital. Explain.
How many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. Ca b.O c. element 117 d. In e. Ar f. Bi
How many valence electrons does each of the following atoms have? rubidium, Z=37 c. aluminum, Z=13 arsenic, Z=33 d. nickel, Z=28
State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. Briefly explain your answers.
What does wave-particle duality mean? What are its implications in our modem view of atomic structure?