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Related Concept Videos

Properties of Transition Metals02:58

Properties of Transition Metals

29.4K
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.
29.4K
Periodic Classification of the Elements04:00

Periodic Classification of the Elements

58.3K
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...
58.3K
The Periodic Table03:25

The Periodic Table

106.3K
As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping includes lithium (Li), sodium (Na), and potassium (K). All of these elements are shiny, conduct heat and electricity well, and have similar chemical properties. A second grouping includes calcium (Ca), strontium (Sr), and barium (Ba), which also are shiny, good conductors of heat and electricity, and have chemical properties in common. However,...
106.3K
Ions and Ionic Charges03:27

Ions and Ionic Charges

78.2K
In ordinary chemical reactions, the nucleus — which contains the protons and neutrons of each atom and thus identifies the element — remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons to form electrically charged particles called...
78.2K
Noble Gases02:54

Noble Gases

22.2K

The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name “noble” because they were assumed to be nonreactive since they have filled valence shells. In 1962, Dr. Neil Bartlett at the University of British Columbia proved this assumption to be false.
22.2K
Electron Configuration of Multielectron Atoms03:26

Electron Configuration of Multielectron Atoms

64.0K
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...
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Updated: Jan 9, 2026

Synthesis and Performance Characterizations of Transition Metal Single Atom Catalyst for Electrochemical CO2 Reduction
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Synthesis and Performance Characterizations of Transition Metal Single Atom Catalyst for Electrochemical CO2 Reduction

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Main-group elements as transition metals.

Philip P Power1

  • 1Department of Chemistry, University of California, Davis, California 95616, USA.

Nature
|January 16, 2010
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Summary
This summary is machine-generated.

Recent advances reveal heavier main-group element compounds exhibit unique electronic properties, differing significantly from lighter elements. Their chemistry increasingly parallels transition metals, showing potential in catalysis.

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Area of Science:

  • Inorganic Chemistry
  • Main-Group Element Chemistry

Background:

  • The late 20th and early 21st centuries have seen significant breakthroughs in the chemistry of heavier main-group elements.
  • Newly synthesized compounds reveal distinct electronic properties compared to lighter elements, challenging prior understanding.

Purpose of the Study:

  • To explore the unique structural and bonding characteristics of heavier main-group element compounds.
  • To investigate the parallels between the reactivity of these compounds and transition-metal complexes.

Main Methods:

  • Synthesis of novel heavier main-group element compounds.
  • Characterization of electronic properties and structural features.
  • Reactivity studies with small molecules (e.g., H(2), NH(3), C(2)H(4), CO).

Main Results:

  • Highlighted fundamental differences in electronic properties between heavier and lighter main-group elements.
  • Demonstrated that the chemistry of heavier main-group elements increasingly resembles that of transition-metal complexes.
  • Observed reactions of new compounds with small molecules under mild conditions.

Conclusions:

  • The study provides new structural and bonding insights into heavier main-group elements.
  • Heavier main-group element chemistry shares significant similarities with transition-metal chemistry.
  • These compounds show potential for catalytic applications due to their reactivity.