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Related Concept Videos

Atomic Radii and Effective Nuclear Charge03:08

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number and distribution of electrons in their valence shells.
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Covalent Bonds

When two atoms share electrons to complete their valence shells they create a covalent bond. An atom’s electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.A Covalent...
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Overview
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.
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Covalent bonds are formed between two atoms when both have similar tendencies to attract electrons to themselves (i.e., when both atoms have identical or fairly similar ionization energies and electron affinities). Nonmetal atoms frequently form covalent bonds with other nonmetal atoms. For example, the hydrogen molecule, H2, contains a covalent bond between its two hydrogen atoms. When two separate hydrogen atoms with a particular potential energy approach each other, their valence orbitals...
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Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...

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Covalent radii revisited.

Beatriz Cordero1, Verónica Gómez, Ana E Platero-Prats

  • 1Departament de Química Inorgànica and Institut de Química Teòrica i Computacional, Universitat de Barcelona, Martí i Franqués 1-11, 08028, Barcelona, Spain.

Dalton Transactions (Cambridge, England : 2003)
|May 15, 2008
PubMed
Summary

This study introduces a new set of covalent atomic radii derived from crystallographic data, improving accuracy and filling gaps for elements like noble gases. These new radii offer a more consistent understanding of atomic sizes across the periodic table.

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Area of Science:

  • Chemistry
  • Crystallography
  • Physics

Background:

  • Accurate covalent atomic radii are crucial for understanding chemical bonding and molecular structure.
  • Existing covalent radii sets have inconsistencies and gaps, particularly for certain elements and transition metal configurations.

Purpose of the Study:

  • To deduce a new, comprehensive set of covalent atomic radii using crystallographic data.
  • To address inconsistencies and fill gaps in existing covalent radii data.
  • To illustrate periodic trends, including transition metal and lanthanide contractions, and spin-state effects.

Main Methods:

  • Analysis of crystallographic data for elements up to atomic number 96.
  • Deduction of covalent atomic radii based on observed bond lengths in crystal structures.
  • Interpolation of radii for elements lacking structural data, such as noble gases.

Main Results:

  • A new set of covalent atomic radii has been established for most elements up to Z=96.
  • The proposed radii exhibit a well-behaved periodic dependence.
  • The new set resolves inconsistencies and fills gaps in previously available covalent radii data.

Conclusions:

  • The new covalent atomic radii provide a more accurate and complete representation of atomic sizes.
  • This dataset aids in understanding phenomena like transition metal and lanthanide contractions.
  • The findings offer improved insights into covalent bonding across the periodic table.