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The van der Waals radius (r(vdw)) is def...

The van der Waals radius `(r_(vdw))` is defined as the half-distance between the nuclei of two atoms of neighboring molecules in the____state.

A

gaseous

B

Iiquid

C

plasme

D

solid

Text Solution

Verified by Experts

The correct Answer is:
D
van der Waals radius is defined in the solid state provided the force of attraction is due only to van der Waals forces.
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An atom is assumed to tbe spherical in shape and thus, the size of atom is generally given in terms of radius of the sphere and is called atomic radius. It is usually defined as the distance between the centre of the nucleus and outermost shell where electron are present. The exact measure of atomic radius is not easy due to following reasons: (i) The atom does not have well defined boundary. the probability of finding the electron is never zero even at large distance from the nucleus. (ii) It is not possible to get an isolated atom. the electron density around an atom is affected by the presence of neighbouring atoms, i.e., the size of the atom changes in going from one set of environement to another. (iii) the size of an atom is very small, of the order of about 1.2 Å,i.e., 1.2xx10^(-10)m . An estimate of the size of the atom can, however, be made by knowing the distance betweent he atoms in the combined state. the distance between the atoms, i.e., bond length are generally measured by the application of techniques such as X-ray differaction, electron diffraction, infrared spectroscopy, nuclear magnetic resonance spectroscopy, etc. However, bond lengths change with different type of bonding. Three types of radius are commonly used, i.e., (a) Covalent radius " " (b) crystals radius " " (c) Vander waal's radius Choose incorrect option regarding atomic radius

An atom is assumed to tbe spherical in shape and thus, the size of atom is generally given in terms of radius of the sphere and is called atomic radius. It is usually defined as the distance between the centre of the nucleus and outermost shell where electron are present. The exact measure of atomic radius is not easy due to following reasons: (i) The atom does not have well defined boundary. the probability of finding the electron is never zero even at large distance from the nucleus. (ii) It is not possible to get an isolated atom. the electron density around an atom is affected by the presence of neighbouring atoms, i.e., the size of the atom changes in going from one set of environement to another. (iii) the size of an atom is very small, of the order of about 1.2 Å,i.e., 1.2xx10^(-10)m . An estimate of the size of the atom can, however, be made by knowing the distance betweent he atoms in the combined state. the distance between the atoms, i.e., bond length are generally measured by the application of techniques such as X-ray differaction, electron diffraction, infrared spectroscopy, nuclear magnetic resonance spectroscopy, etc. However, bond lengths change with different type of bonding. Three types of radius are commonly used, i.e., (a) Covalent radius " " (b) crystals radius " " (c) Vander waal's radius Choose incorrect option regarding atomic size

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It is not possible to measure the atomic radius prectsely since the electron cloub surrouding the atom does not have a sharp boundary. One practial approach to estimate the size of an atom of a non-metallic element is to measure the distance between two atoms when they are bound togther by a signle bond in a covalent molecule and then dividing by two. For metals we define the term "matellic radius" which is taken as half the internuclear distance separating the metal cores in the metallic crystal. Then van der waal's radius represents the over all size of the atoms which includes its valence shell in a non bonded situation. It is the half of the distance between two similar atoms in separate molecules in a solid. The atomis radius decreases across a period and increases down the group. Same trends are observed in case of ionic radius. Ionic radius of the species having same number of electrons depends on the number of protons in their nuclei. Sometimes, atomic and ionic radii give unexpected trends due to poor shielding of nuclear charge by d -and f- orbital electrons. Now answer the following three questions: Select the INCORRECT option regarding atomic//ionic sizes:

R SHARMA-CLASSIFICATION OF ELEMENTS AND PERIODICITY IN ELEMENTS-Follow-up Test
  1. The covalent radius (r(cov)) is defined as the half-distance between t...

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  2. There is no real boundary to an atom because the electrons can be defi...

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  3. The van der Waals radius (r(vdw)) is defined as the half-distance betw...

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  4. The concept of van der Waals radius is confined to

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  5. Metallic radius is usually not defined forelements.

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  6. Atomic radii can be measured by

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  7. Which of the following radius is not described for the element chlorin...

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  8. The magnitude of the does not depend upon the packing of the particles...

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  9. The internuclear distance between adjacent chlorine atoms of the two n...

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  10. Which of the noble gases can be described in terms of either covalent ...

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  11. Which of the following statements is not correct?

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  12. Which of the following radius is the largest?

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  13. Which of the followinf has the smallest atomic radius?

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  14. Which of the following pairs of elements have similar atpmic radii?

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  15. Which of the following has the largest atomic radius?

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  16. Which of the following statements is not correct?

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  17. Which of the following has the smallest ionic radius?

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  18. Sizes of the seond and third row transition elements are almost the sa...

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  19. which of the following has largest radius ?

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  20. Which of the following species will have the largest size?

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