Question

define and explain the terms crystal radius, covalent radius and van der waal's radius with suitable examples.

Answer 1

The covalent radius, r, is a measure of the size of an atomthat forms part of one covalent bond. It is usually measured either in picometres (pm) or angstroms (Å), with 1 Å = 100 pm.

In principle, the sum of the two covalent radii should equal the covalent bond length between two atoms, R(AB) = r(A) + r(B). Moreover, different radii can be introduced for single, double and triple bonds (r, r and r below), in a purely operational sense. These relationships are certainly not exact because the size of an atom is not constant but depends on its chemical environment. For heteroatomic A–B bonds, ionic terms may enter. Often the polar covalent bonds are shorter than would be expected on the basis of the sum of covalent radii. Tabulated values of covalent radii are either average or idealized values, which nevertheless show a certain transferability between different situations, which makes them useful.

The bond lengths R(AB) are measured by X-ray diffraction (more rarely, neutron diffraction on molecular crystals). Rotational spectroscopy can also give extremely accurate values of bond lengths. For homonuclear A–A bonds, Linus Pauling took the covalent radius to be half the single-bond length in the element, e.g. R(H–H, in H) = 74.14 pm so r(H) = 37.07 pm: in practice, it is usual to obtain an average value from a variety of covalent compounds, although the difference is usually small. Sanderson has published a recent set of non-polar covalent radii for the main-group elements,[1] but the availability of large collections of bond lengths, which are more transferable, from the Cambridge Crystallographic Database[2] [3] has rendered covalent radii obsolete in many situations.

Table of covalent radii

The values in the table below are based on a statistical analysis of more than 228,000 experimental bond lengths from the Cambridge Structural Database.[4] The numbers in parentheses are the estimated standard deviations for the last digit. This fit pre-fixes the radii for C, N and O.

A different approach is to make a self-consistent fit for all elements in a smaller set of molecules. This was done separately for single,[5] double,[6] and triple bonds[7] up to superheavy elements. Both experimental and computational data were used. The single-bond results are often similar to those of Cordero et al.[4] When they are different, the coordination numbers used can be different. This is notably the case for most (d and f) transition metals. Normally one expects that r > r > r. Deviations may occur for weak multiple bonds, if the differences of the ligand are larger than the differences of R in the data used. Note that elements up to E118 have now been experimentally produced and that there are chemical studies on an increasing number of them. The same, self-consistent approach was used to fit tetrahedral covalent radii for 30 elements in 48 crystals with subpicometer accuracy.[8]

Covalent radii in pm from analysis of the Cambridge Structural Database, which contains about 426,000 crystal structures[4]H He1 231(5) 28LiBe BCNOFNe34 5678910128(7)96(3) 84(3)sp376(1) sp273(2) sp  69(1)71(1)66(2)57(3)58

Answer 2

Answer:

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Explanation:

Covalent radius: Covalent bond radius refers to half of the distance two singly bonded atom of the same element. (Homonuclear X−X bond)

Van der Waals Radius: It is defined as half of the internuclear separation of two non- bonded atoms of the same element on their closest possible approach.

Ionic radius: It is a radius of an atom's ion in ionic structure. It is denoted by R ion.

The covalent and van der Waals radii decrease with increase in atomic number as we move from left to right in a period.

The atomic radius abruptly increases as we move from halogens to an inert gas.