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For all practical purposes, the size of ...

For all practical purposes, the size of an individual atom cannot be uniquely defined. An indirect approach is required. The size of an atom is determined by its immediate environment, especially its interaction with surrounding atoms. Pertaining to the types of bonding how many types of atomic radii are employed?

A

Two

B

Four

C

Five

D

Three

Text Solution

Verified by Experts

The correct Answer is:
B
Pertaining to four major types of bonding, atomic radii are of the following four types: covalent raidus, van der Walls radius, metallic raidus, and ionic radius.
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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:

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: C^(+), CI^(-), Ca^(2+), S^(2-) ions are isoelectronic. The decreasing order of their size is:

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: Which of the following relations is correct, if considered for the same element.

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

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 The correct order of effective nuclear charge Z_(eff) is

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 Atomic radius of atoms in a period decreases with the increases in Z_(eff) which of the following is incorrect order of atomic radius ?

An atom is assumed to be spherical in shape and thus, the size of atom is generally in term 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 or electrons are present. The exact measure of atomic radius is not easy due to following reasons : (a) The atom does not have well defined boundary. The propability of finding the electron is never zero even at large distance from the nucleus. (b) It is not distances from 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 environment to another. (c ) The size of an atom is very small, of the order of abouit 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 between the atoms in the combined state. The distance between the atoms, i.e., bond lengths are generally measured by the application of techniques such as X-ray diffraction, electron diffraction, infrared spectroscpy, nuclear magnetic resonance spectroscopy, etc. However, bond length change with different type of bonding. Three types of radius are commonly used, i.e., (a) Covalent radius (b) Crystal radius (c ) van der Waal's radius Which of the following set of ions have the same value of screening constant for the valence electron, calculated from Slater's rule?

R SHARMA-CLASSIFICATION OF ELEMENTS AND PERIODICITY IN ELEMENTS-Follow-up Test
  1. Arrange the following elements in the increasing order of metallic cha...

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  2. The electron density in an atom extends far beyond the nucleus. In pra...

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  3. For all practical purposes, the size of an individual atom cannot be u...

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  4. The internuclear distance between any two carbon atoms in diamond is 1...

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  5. The covalent radius (r(cov)) is defined as the half-distance between t...

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

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

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

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  9. Metallic radius is usually not defined forelements.

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  10. Atomic radii can be measured by

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

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

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

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

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  15. Which of the following statements is not correct?

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  16. Which of the following radius is the largest?

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

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

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

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  20. Which of the following statements is not correct?

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