CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313154
The correct order of size would be
1 \({\rm{Ni < Pd}} \simeq {\rm{Pt}}\)
2 \({\rm{Pd < Pt < Ni}}\)
3 \({\rm{Pt > Ni > Pd}}\)
4 \({\rm{Pd > Pt > Ni}}\)
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313155
The correct order of atomic radii of \({\text{C, N, P, S}}\) following the order:
1 \({\text{N < C < P < S}}\)
2 \({\text{C < N < S < P}}\)
3 \({\text{C < N < P < S}}\)
4 \({\text{N < C < S < P}}\)
Explanation:
Along the period, atomic radii decreases and down the group increases. \(\mathrm{C}, \mathrm{N}\) are smaller and in that ' \(\mathrm{C}\) ' is bigger than ' \(\mathrm{N}\) '. S,P are bigger and in that ' \(\mathrm{P}\) ' is bigger than ' \(\mathrm{S}\) '.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313156
Covalent radii of atoms varies in range of 72 pm to 133 pm from F to I while that of noble gases He to Xe varies from 120pm to 220pm. This is because in case of noble gases
1 covalent radius is very large
2 van der Waal radius is considered
3 metallic radii is considered
4 None of these
Explanation:
In case of halogens covalent radius is considered this bond is formed by overlapping of electron clouds; while noble gases remain monoatomic, in this case only way to obtain radius is through vander Waal radii.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313157
Select correct statement about radius of an atom.
1 Values of vander Waals' radii are larger than those of covalent radii because the van der Waals' forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
2 The metallic radii are smaller than the vander Waals' radii, since the bonding forces in the metallic crystal lattice are much stronger than the van der Waals' forces.
3 Both are correct
4 None is correct
Explanation:
Radius of an atom follows the following order: vander Waals' radii \(>\) Metallic radii \(>\) Covalent radii So, both the statements are correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313158
The covalent and van der Waals radii of hydrogen respectively are
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313154
The correct order of size would be
1 \({\rm{Ni < Pd}} \simeq {\rm{Pt}}\)
2 \({\rm{Pd < Pt < Ni}}\)
3 \({\rm{Pt > Ni > Pd}}\)
4 \({\rm{Pd > Pt > Ni}}\)
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313155
The correct order of atomic radii of \({\text{C, N, P, S}}\) following the order:
1 \({\text{N < C < P < S}}\)
2 \({\text{C < N < S < P}}\)
3 \({\text{C < N < P < S}}\)
4 \({\text{N < C < S < P}}\)
Explanation:
Along the period, atomic radii decreases and down the group increases. \(\mathrm{C}, \mathrm{N}\) are smaller and in that ' \(\mathrm{C}\) ' is bigger than ' \(\mathrm{N}\) '. S,P are bigger and in that ' \(\mathrm{P}\) ' is bigger than ' \(\mathrm{S}\) '.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313156
Covalent radii of atoms varies in range of 72 pm to 133 pm from F to I while that of noble gases He to Xe varies from 120pm to 220pm. This is because in case of noble gases
1 covalent radius is very large
2 van der Waal radius is considered
3 metallic radii is considered
4 None of these
Explanation:
In case of halogens covalent radius is considered this bond is formed by overlapping of electron clouds; while noble gases remain monoatomic, in this case only way to obtain radius is through vander Waal radii.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313157
Select correct statement about radius of an atom.
1 Values of vander Waals' radii are larger than those of covalent radii because the van der Waals' forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
2 The metallic radii are smaller than the vander Waals' radii, since the bonding forces in the metallic crystal lattice are much stronger than the van der Waals' forces.
3 Both are correct
4 None is correct
Explanation:
Radius of an atom follows the following order: vander Waals' radii \(>\) Metallic radii \(>\) Covalent radii So, both the statements are correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313158
The covalent and van der Waals radii of hydrogen respectively are
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313154
The correct order of size would be
1 \({\rm{Ni < Pd}} \simeq {\rm{Pt}}\)
2 \({\rm{Pd < Pt < Ni}}\)
3 \({\rm{Pt > Ni > Pd}}\)
4 \({\rm{Pd > Pt > Ni}}\)
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313155
The correct order of atomic radii of \({\text{C, N, P, S}}\) following the order:
1 \({\text{N < C < P < S}}\)
2 \({\text{C < N < S < P}}\)
3 \({\text{C < N < P < S}}\)
4 \({\text{N < C < S < P}}\)
Explanation:
Along the period, atomic radii decreases and down the group increases. \(\mathrm{C}, \mathrm{N}\) are smaller and in that ' \(\mathrm{C}\) ' is bigger than ' \(\mathrm{N}\) '. S,P are bigger and in that ' \(\mathrm{P}\) ' is bigger than ' \(\mathrm{S}\) '.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313156
Covalent radii of atoms varies in range of 72 pm to 133 pm from F to I while that of noble gases He to Xe varies from 120pm to 220pm. This is because in case of noble gases
1 covalent radius is very large
2 van der Waal radius is considered
3 metallic radii is considered
4 None of these
Explanation:
In case of halogens covalent radius is considered this bond is formed by overlapping of electron clouds; while noble gases remain monoatomic, in this case only way to obtain radius is through vander Waal radii.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313157
Select correct statement about radius of an atom.
1 Values of vander Waals' radii are larger than those of covalent radii because the van der Waals' forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
2 The metallic radii are smaller than the vander Waals' radii, since the bonding forces in the metallic crystal lattice are much stronger than the van der Waals' forces.
3 Both are correct
4 None is correct
Explanation:
Radius of an atom follows the following order: vander Waals' radii \(>\) Metallic radii \(>\) Covalent radii So, both the statements are correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313158
The covalent and van der Waals radii of hydrogen respectively are
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313154
The correct order of size would be
1 \({\rm{Ni < Pd}} \simeq {\rm{Pt}}\)
2 \({\rm{Pd < Pt < Ni}}\)
3 \({\rm{Pt > Ni > Pd}}\)
4 \({\rm{Pd > Pt > Ni}}\)
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313155
The correct order of atomic radii of \({\text{C, N, P, S}}\) following the order:
1 \({\text{N < C < P < S}}\)
2 \({\text{C < N < S < P}}\)
3 \({\text{C < N < P < S}}\)
4 \({\text{N < C < S < P}}\)
Explanation:
Along the period, atomic radii decreases and down the group increases. \(\mathrm{C}, \mathrm{N}\) are smaller and in that ' \(\mathrm{C}\) ' is bigger than ' \(\mathrm{N}\) '. S,P are bigger and in that ' \(\mathrm{P}\) ' is bigger than ' \(\mathrm{S}\) '.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313156
Covalent radii of atoms varies in range of 72 pm to 133 pm from F to I while that of noble gases He to Xe varies from 120pm to 220pm. This is because in case of noble gases
1 covalent radius is very large
2 van der Waal radius is considered
3 metallic radii is considered
4 None of these
Explanation:
In case of halogens covalent radius is considered this bond is formed by overlapping of electron clouds; while noble gases remain monoatomic, in this case only way to obtain radius is through vander Waal radii.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313157
Select correct statement about radius of an atom.
1 Values of vander Waals' radii are larger than those of covalent radii because the van der Waals' forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
2 The metallic radii are smaller than the vander Waals' radii, since the bonding forces in the metallic crystal lattice are much stronger than the van der Waals' forces.
3 Both are correct
4 None is correct
Explanation:
Radius of an atom follows the following order: vander Waals' radii \(>\) Metallic radii \(>\) Covalent radii So, both the statements are correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313158
The covalent and van der Waals radii of hydrogen respectively are
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313154
The correct order of size would be
1 \({\rm{Ni < Pd}} \simeq {\rm{Pt}}\)
2 \({\rm{Pd < Pt < Ni}}\)
3 \({\rm{Pt > Ni > Pd}}\)
4 \({\rm{Pd > Pt > Ni}}\)
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313155
The correct order of atomic radii of \({\text{C, N, P, S}}\) following the order:
1 \({\text{N < C < P < S}}\)
2 \({\text{C < N < S < P}}\)
3 \({\text{C < N < P < S}}\)
4 \({\text{N < C < S < P}}\)
Explanation:
Along the period, atomic radii decreases and down the group increases. \(\mathrm{C}, \mathrm{N}\) are smaller and in that ' \(\mathrm{C}\) ' is bigger than ' \(\mathrm{N}\) '. S,P are bigger and in that ' \(\mathrm{P}\) ' is bigger than ' \(\mathrm{S}\) '.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313156
Covalent radii of atoms varies in range of 72 pm to 133 pm from F to I while that of noble gases He to Xe varies from 120pm to 220pm. This is because in case of noble gases
1 covalent radius is very large
2 van der Waal radius is considered
3 metallic radii is considered
4 None of these
Explanation:
In case of halogens covalent radius is considered this bond is formed by overlapping of electron clouds; while noble gases remain monoatomic, in this case only way to obtain radius is through vander Waal radii.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313157
Select correct statement about radius of an atom.
1 Values of vander Waals' radii are larger than those of covalent radii because the van der Waals' forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
2 The metallic radii are smaller than the vander Waals' radii, since the bonding forces in the metallic crystal lattice are much stronger than the van der Waals' forces.
3 Both are correct
4 None is correct
Explanation:
Radius of an atom follows the following order: vander Waals' radii \(>\) Metallic radii \(>\) Covalent radii So, both the statements are correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313158
The covalent and van der Waals radii of hydrogen respectively are
