3p orbital has -

1. Two spherical nodes

2. Two non-spherical nodes

3. One spherical and one non-spherical node

4. One spherical and two non-spherical nodes

The correct order of the total number of nodes of atomic orbitals is: 

1.  4f > 6s > 5d

2.  6s > 5d > 4f

3.  4f > 5d > 6s

4.  5d > 4f > 6s

Correct statement among the following is: 

1.  Number of angular nodes = n - l - 1

2.  Number of radial nodes = l

3.  Total number of nodes = n -1

4.  All of the above

Which orbital has the maximum number of total nodes?
1.  5s

2.  5p

3.  5d

4.  All have the same number of nodes.

Orbitals having two spherical nodes are: 

Given below are two statements:

In a subshell, if the number of radial nodes is two times the number of angular nodes, then the minimum possible value of the principal quantum number (n) is: 

[angular nodes are non-zero)

Orbital having 3 angular nodes and 3 total nodes is:

Assertion: The number of radials and angular nodes for 3p orbital is 1, 1 respectively.

Reason: The number of radials and angular nodes depends only on the principal quantum number.

1. both assertion and reason are true and the reason is the correct explanation of assertion.

2. both assertion and reason are true but the reason is not the correct explanation of
assertion.

3. assertion is true but the reason is false

4. both assertion and reason are false

The number of radial nodes of 3s and 2p-orbitals are respectively:

(1) 2,0

(2) 0,2

(3) 1,2 

(4) 2,1