# calculate the total number of angular nodes and radial nodes present in 3p orbital

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## Question 26 Calculate the total number of angular nodes and radical nodes and radical nodes present in 3p orbital.

Question 26 Calculate the total number of angular nodes and radical nodes and radical nodes present in 3p orbital.

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Question 26 Calculate the total number of angular nodes and radical nodes and radical nodes present in 3p orbital.

Question Question 26

Calculate the total number of angular nodes and radical nodes and radical nodes present in 3p orbital.

Open in App Solution

For 3p - orbital, principal quantum number, n = 3 and azimuthal number l = 1

Number of angular nodes = l = 1

Number of radial nodes = n - l - 1 = 3 - 1 - 1 = 1

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SIMILAR QUESTIONS

**Q.**The correct number of angular node(s) and radial node(s) in the 3p orbital is:

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**Q.**Number of radial and angular nodes in

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**Q.**The correct number of angular node(s) and radial node(s) in the 3p orbital is:

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## Calculate the total number of angular nodes and radial nodes present in 3p

For 3p orbital, n =3, l =1 Number of angular nodes = l =1 Number of radial nodes = n -l -1 =3 -1 =1

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Calculate the total number of angular nodes and radial nodes present in 3p- orbital.

Updated On: 27-06-2022

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Text Solution Open Answer in App Solution For 3p orbital, n=3,l=1 n=3,l=1

Number of angular nodes

=l=1 =l=1

Number of radial nodes

=n−l−1=3−1=1 =n-l-1=3-1=1

Answer

Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams.

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Calculate the total number of angular nodes and radical nodes present in 3p orbital.

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## Calculate the total number of angular nodes and radial nodes present in 3p orbital.

Calculate the total number of angular nodes and radial nodes present in 3p orbital.

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Calculate the total number of angular nodes and radial nodes present in 3p orbital.

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### SOLUTION

The number of radial nodes is given by n – l – 1,where n is principal quantum number, l is azimuthal quantum number.

The number of angular nodes is given by n – l, where n is principal quantum number, l is azimuthal quantum number.

Here n = 3 and l = 1

Thus, angular nodes = 3 – 1 = 2 and radial node = 3 – 1 – 1 = 1.

Concept: Quantum Mechanical Model of Atom

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Chapter 2: Structure of Atom - Multiple Choice Questions (Type - I) [Page 19]

Q 26 Q 25 Q 27.(i).(a)

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NCERT Chemistry Exemplar Class 11

Chapter 2 Structure of Atom

Multiple Choice Questions (Type - I) | Q 26 | Page 19

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Quantum Mechanical Model of Atom

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