Question

Question 6 of 25 > Two types of nodes occur in atomic orbitals: spherical (radial) surfaces and planes (angles). Examine the 2s 2p, and 3p orbitals, and then characterize their nodes. outer ball of electron density (wave trough) nucleus inner ball of electron density (wave peak) The 2s orbital has The 2p orbital has T auhital han Which of the statements are true?

Answer 1

Nodes is a point where the probability of finding an electron is zero. There are two type of nodes angular and radial nodes.

Total number of nodes = n-1 (n= principal quantum number)

Number of angular nodes = l ( azimuthal quantum number)

Number of radial nodes = (n-1)-l

1) number of nodes in 2s orbital

​​​​​​Principal quantum number, n = 2

Azimuthal quantum number, l = 0

Therefore , radial nodes = n-1-l = 2-1-0 = 1

Angular nodes = l = 0

2) number of nodes in 2p orbital

n = 2. ,. l = 1

Radial nodes = n-1-l = 2-1-1 = 0

Angular nodes = l = 1

3) number of nodes in 3p orbital

n = 3. ,. l= 1

Radial nodes = n-1-l = 3-1-1= 1

Angular nodes= l = 1

4) number of nodes in 5s orbital

n = 5. l= 0

Radial nodes = n-1-l = 5-1-0= 4

5) number of nodes in 3d orbital

n= 3. l= 2

Radial nodes = n-1-l = 3-1-2= 0

Angular nodes= l = 2

Total nodes = n-1= 3-1= 2