covalent radius

More recent data can be found in Covalent radius.

Fluorine has a relatively small covalent radius, around 60 picometers.

He therefore assumed that the covalent radius of fluorine was half this value, or 73 pm.

The first attempt at trying to find the covalent radius of fluorine was in 1938, by Brockway.

Gold sulfides exist in nature as solid solutions with silver, which has the same covalent radius.

Gillespie has also done extensive work on interpreting the covalent radius of fluorine.

The ionic radius of fluoride is much larger than its covalent radius.

In a bond between two identical atoms half the bond distance is equal to the covalent radius.

Its major weakness is the use of the covalent radius of fluorine that is known as being too large.

For more recent data on covalent radii see Covalent radius.

Covalent radius: half the distance between two atoms of a diatomic compound, singly bonded.

Covalent radius: ?

Since fluorine is a relatively small atom with a large electronegativity, its covalent radius is difficult to evaluate.

The covalent radius is defined as half the bond lengths between two neutral atoms of the same kind connected with a single bond.

The same, self-consistent approach was used to fit tetrahedral covalent radii for 30 elements in 48 crystals with subpicometer accuracy.

Theoreticians have predicted the covalent radius of meitnerium to be 6 to 10 pm larger than that of iridium.

The following table shows empirically measured covalent radii for the elements, as published by J. C. Slater in 1964.

Often the polar covalent bonds are shorter than would be expected on the basis of the sum of covalent radii.

The covalent radius of most atoms is found by taking half the length of a single bond between two similar atoms in a neutral molecule.

In principle, the sum of the two covalent radii should equal the covalent bond length between two atoms.

Covalent radius (Single-, double- and triple-bond radii, up to the superheavy elements.)

The covalent radius, r, is a measure of the size of an atom that forms part of one covalent bond.

Tabulated values of covalent radii are either average or idealized values, which nevertheless show a certain transferability between different situations, that makes them useful.

Calculating the covalent radius for fluorine is more difficult because of its high electronegativity compared to its small atomic radius size.

Therefore, we can use the metallic radius, ionic radius, or covalent radius of each atom in the molecule to determine the bond strength.