307528
The number of spherical nodes in Is orbital is
1 1
2 0
3 4
4 2
Explanation:
The number of spherical or radial nodes in an orbital \( = ({\text{n}} - l - 1)\). 1s orbital \(({\text{n = }}1,l{\text{ = 0}})\) has no spherical node.
CHXI02:STRUCTURE OF ATOM
307529
Assertion : Number of radial and angular nodes for \({\text{3 p}}\) -orbital are 1, 1 respectively. Reason : Number of radial and angular nodes depends only on principal quantum number.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For the 3p-orbital, the number of radial nodes is given by the formula: \(\mathrm{n}-1-1\), which in this case is \(3-1-1\), resulting in 1 radial node. Additionally, the number of angular nodes in a \({\text{3 p}}\) -orbital is equal to the value of the azimuthal quantum number (1), which is 1 . The number of radial and angular nodes in an orbital depends on both the principal quantum number (n) and the azimuthal quantum number (1). So option (3) is correct.
CHXI02:STRUCTURE OF ATOM
307530
Assertion : \({\rm{2}}{{\rm{p}}_{\rm{x}}}{\rm{,2}}{{\rm{p}}_{\rm{y}}}\) and \({\rm{2}}{{\rm{p}}_{\rm{z}}}\) each have one nodal plane. Reason : These orbitals are degenerate orbitals.
1 If both Assertion & Reason are true and reason is the correct explanation of the assertion.
2 If both Assertion & Reason are true but reason is not the correct explanation of the assertion.
3 If Assertion is true statement but Reason is false.
4 Assertion is false but reason is true.
Explanation:
Conceptual Questions
CHXI02:STRUCTURE OF ATOM
307531
The number of nodes in \({\mathrm{3 p}}\) orbital.
1 1
2 2
3 0
4 3
Explanation:
Number of nodes \({\rm{ = n}} - l - {\rm{1 = 3}} - {\rm{1}} - {\rm{1 = }} - {\rm{1}}\)
307528
The number of spherical nodes in Is orbital is
1 1
2 0
3 4
4 2
Explanation:
The number of spherical or radial nodes in an orbital \( = ({\text{n}} - l - 1)\). 1s orbital \(({\text{n = }}1,l{\text{ = 0}})\) has no spherical node.
CHXI02:STRUCTURE OF ATOM
307529
Assertion : Number of radial and angular nodes for \({\text{3 p}}\) -orbital are 1, 1 respectively. Reason : Number of radial and angular nodes depends only on principal quantum number.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For the 3p-orbital, the number of radial nodes is given by the formula: \(\mathrm{n}-1-1\), which in this case is \(3-1-1\), resulting in 1 radial node. Additionally, the number of angular nodes in a \({\text{3 p}}\) -orbital is equal to the value of the azimuthal quantum number (1), which is 1 . The number of radial and angular nodes in an orbital depends on both the principal quantum number (n) and the azimuthal quantum number (1). So option (3) is correct.
CHXI02:STRUCTURE OF ATOM
307530
Assertion : \({\rm{2}}{{\rm{p}}_{\rm{x}}}{\rm{,2}}{{\rm{p}}_{\rm{y}}}\) and \({\rm{2}}{{\rm{p}}_{\rm{z}}}\) each have one nodal plane. Reason : These orbitals are degenerate orbitals.
1 If both Assertion & Reason are true and reason is the correct explanation of the assertion.
2 If both Assertion & Reason are true but reason is not the correct explanation of the assertion.
3 If Assertion is true statement but Reason is false.
4 Assertion is false but reason is true.
Explanation:
Conceptual Questions
CHXI02:STRUCTURE OF ATOM
307531
The number of nodes in \({\mathrm{3 p}}\) orbital.
1 1
2 2
3 0
4 3
Explanation:
Number of nodes \({\rm{ = n}} - l - {\rm{1 = 3}} - {\rm{1}} - {\rm{1 = }} - {\rm{1}}\)
307528
The number of spherical nodes in Is orbital is
1 1
2 0
3 4
4 2
Explanation:
The number of spherical or radial nodes in an orbital \( = ({\text{n}} - l - 1)\). 1s orbital \(({\text{n = }}1,l{\text{ = 0}})\) has no spherical node.
CHXI02:STRUCTURE OF ATOM
307529
Assertion : Number of radial and angular nodes for \({\text{3 p}}\) -orbital are 1, 1 respectively. Reason : Number of radial and angular nodes depends only on principal quantum number.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For the 3p-orbital, the number of radial nodes is given by the formula: \(\mathrm{n}-1-1\), which in this case is \(3-1-1\), resulting in 1 radial node. Additionally, the number of angular nodes in a \({\text{3 p}}\) -orbital is equal to the value of the azimuthal quantum number (1), which is 1 . The number of radial and angular nodes in an orbital depends on both the principal quantum number (n) and the azimuthal quantum number (1). So option (3) is correct.
CHXI02:STRUCTURE OF ATOM
307530
Assertion : \({\rm{2}}{{\rm{p}}_{\rm{x}}}{\rm{,2}}{{\rm{p}}_{\rm{y}}}\) and \({\rm{2}}{{\rm{p}}_{\rm{z}}}\) each have one nodal plane. Reason : These orbitals are degenerate orbitals.
1 If both Assertion & Reason are true and reason is the correct explanation of the assertion.
2 If both Assertion & Reason are true but reason is not the correct explanation of the assertion.
3 If Assertion is true statement but Reason is false.
4 Assertion is false but reason is true.
Explanation:
Conceptual Questions
CHXI02:STRUCTURE OF ATOM
307531
The number of nodes in \({\mathrm{3 p}}\) orbital.
1 1
2 2
3 0
4 3
Explanation:
Number of nodes \({\rm{ = n}} - l - {\rm{1 = 3}} - {\rm{1}} - {\rm{1 = }} - {\rm{1}}\)
307528
The number of spherical nodes in Is orbital is
1 1
2 0
3 4
4 2
Explanation:
The number of spherical or radial nodes in an orbital \( = ({\text{n}} - l - 1)\). 1s orbital \(({\text{n = }}1,l{\text{ = 0}})\) has no spherical node.
CHXI02:STRUCTURE OF ATOM
307529
Assertion : Number of radial and angular nodes for \({\text{3 p}}\) -orbital are 1, 1 respectively. Reason : Number of radial and angular nodes depends only on principal quantum number.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
For the 3p-orbital, the number of radial nodes is given by the formula: \(\mathrm{n}-1-1\), which in this case is \(3-1-1\), resulting in 1 radial node. Additionally, the number of angular nodes in a \({\text{3 p}}\) -orbital is equal to the value of the azimuthal quantum number (1), which is 1 . The number of radial and angular nodes in an orbital depends on both the principal quantum number (n) and the azimuthal quantum number (1). So option (3) is correct.
CHXI02:STRUCTURE OF ATOM
307530
Assertion : \({\rm{2}}{{\rm{p}}_{\rm{x}}}{\rm{,2}}{{\rm{p}}_{\rm{y}}}\) and \({\rm{2}}{{\rm{p}}_{\rm{z}}}\) each have one nodal plane. Reason : These orbitals are degenerate orbitals.
1 If both Assertion & Reason are true and reason is the correct explanation of the assertion.
2 If both Assertion & Reason are true but reason is not the correct explanation of the assertion.
3 If Assertion is true statement but Reason is false.
4 Assertion is false but reason is true.
Explanation:
Conceptual Questions
CHXI02:STRUCTURE OF ATOM
307531
The number of nodes in \({\mathrm{3 p}}\) orbital.
1 1
2 2
3 0
4 3
Explanation:
Number of nodes \({\rm{ = n}} - l - {\rm{1 = 3}} - {\rm{1}} - {\rm{1 = }} - {\rm{1}}\)
