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Related Concept Videos

Electron Configurations02:46

Electron Configurations

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Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest energy available), Pauli exclusion principle (no two electrons can have the same set of four quantum numbers), and Hund’s rule of maximum multiplicity (whenever possible, electrons retain unpaired spins in degenerate orbitals).
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p,...
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Periodic Classification of the Elements04:00

Periodic Classification of the Elements

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The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their electron configurations are added to the table, a periodic recurrence of similar electron configurations in the outer shells of these elements is observed. Because they are in the outer shells of an atom, valence electrons play the most important role in chemical reactions. The outer electrons have the highest energy of the electrons in an atom...
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π Electron Effects on Chemical Shift: Overview01:27

π Electron Effects on Chemical Shift: Overview

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An applied magnetic field causes loosely bound π-electrons in organic molecules to circulate, producing a local or induced diamagnetic field over a large spatial volume. As the molecules tumble in solution, the field generated by π-electrons in spherical substituents results in a zero net field. However, the net field generated by π-electrons in non-spherical substituents is not zero. The effect of this induced field depends on the orientation of the molecule with respect to B0,...
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Electron Configuration of Multielectron Atoms03:26

Electron Configuration of Multielectron Atoms

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The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...
68.1K
Properties of Transition Metals02:58

Properties of Transition Metals

30.7K
Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3–12 are transition elements. The f-block elements, also called inner transition metals (the lanthanides and actinides), also meet this criterion because the d orbital is partially occupied before the f orbitals.
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Electron Orbital Model01:18

Electron Orbital Model

76.5K
Orbitals are the areas outside of the atomic nucleus where electrons are most likely to reside. They are characterized by different energy levels, shapes, and three-dimensional orientations. The location of electrons is described most generally by a shell or principal energy level, then by a subshell within each shell, and finally, by individual orbitals found within the subshells.
The first shell is closest to the nucleus, and it has only one subshell with a single spherical orbital called the...
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Materials with 5d electrons for future technologies.

Lin Gu1, Ce-Wen Nan2, Yeqiang Tan3

  • 1Beijing National Center for Electron Microscopy and Laboratory of Advanced Materials, State Key Laboratory of New Ceramics and Fine Processing, School of Materials Science and Engineering, Tsinghua University, Beijing, China.

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Summary
This summary is machine-generated.

Materials with 5d electrons possess unique properties due to their electronic structures. Understanding these structures aids in designing advanced materials for diverse applications.

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Area of Science:

  • Solid State Physics
  • Materials Science
  • Quantum Chemistry

Background:

  • Materials featuring 5d electrons exhibit remarkable functional and structural characteristics.
  • Understanding the electronic structure of these materials is key to unlocking their potential.

Purpose of the Study:

  • To systematically analyze the intrinsic electronic structures of 5d electron materials.
  • To elucidate the factors governing their unique electronic properties and functions.

Main Methods:

  • Systematic analysis of intrinsic electronic structures.
  • Investigating the interplay of nuclear attraction, relativistic effects, spin-orbit coupling, orbital extension, crystal field splitting, and electron correlation.

Main Results:

  • Detailed analysis of how combined electronic factors dictate the unique electronic structures of 5d materials.
  • Identification of key electronic characteristics responsible for material properties.

Conclusions:

  • The electronic characteristics of 5d electron materials offer significant opportunities for novel material design.
  • These materials hold promise for advancements in information technologies, quantum sciences, catalysis, aerospace, and energy storage.