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Properties of Transition Metals02:58

Properties of Transition Metals

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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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Valence Bond Theory

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Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
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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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Metal-Ligand Bonds

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The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
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Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
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Coordination Compounds and Nomenclature

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In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
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Heavier group 14-transition metal π-complex congeners.

Terrance J Hadlington1

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This review explores heavier group 14 element π-complexes, revealing unique bonding with less π-bonding and more polarization compared to traditional organometallic chemistry.

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Area of Science:

  • Organometallic Chemistry
  • Main Group Chemistry

Background:

  • Transition metal π-complexes are fundamental in organometallic chemistry.
  • Research on heavier group 14 elements (Si, Ge, Sn, Pb) has expanded significantly.
  • Heavier congeners of classical π-complexes are now accessible.

Purpose of the Study:

  • To review the synthesis and bonding of heavier group 14 element π-complexes.
  • To highlight differences in bonding compared to lighter elements.
  • To identify future research directions in this field.

Main Methods:

  • Literature review of organometallic complexes.
  • Analysis of electronic structures and bonding characteristics.
  • Comparison of reactivity and stability.

Main Results:

  • Heavier group 14 π-complexes exhibit distinct electronic properties.
  • Bonding involves reduced π-character and increased polarization.
  • These complexes offer new avenues for synthetic applications.

Conclusions:

  • The chemistry of heavier group 14 π-complexes presents unique bonding paradigms.
  • Further exploration promises novel reactivity and applications.
  • This field offers exciting prospects for future organometallic research.