Number of nodes in a 3p orbital (n=3, l=1):
A0
B2 (n-1 total nodes; 1 angular + 1 radial)
C3
D1
Answer & Solution
Correct answer: B. 2 (n-1 total nodes; 1 angular + 1 radial)
Total nodes = n - 1 = 2 for n=3. Angular nodes = l = 1 (the planar node through the nucleus). Radial nodes = n - l - 1 = 1. So 1 angular + 1 radial = 2 total nodes.
Related questions
The strength of a bond depends chiefly on the extent of:Sidewise overlapping produces charged clouds shaped like a:In a pi bond, the axes of the overlapping orbitals remain:Head-on overlap along the internuclear axis is also called:A sigma bond is formed by overlap that is:In a molecule such as HF, the covalent bond is:A bond where the electron pair sits exactly between identical nuclei is:The nitrogen bond enthalpy of 946 kJ per mol is one of the: