Draw and explain the shapes of p and d orbitals.
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Answers
Answer:
Atomic orbitals are mathematical functions that describe the wave nature of electrons (or electron pairs) in an atom.
The boundary surface diagram for the s orbital looks like a sphere having the nucleus as its centre which in two dimensions can be seen as a circle.
Hence, we can say that s-orbitals are spherically symmetric having the probability of finding the electron at a given distance equal in all the directions.
The size of the s orbital is also found to increase with the increase in the value of the principal quantum number (n), thus, 4s > 3s> 2s > 1s.
The Shape of s Orbitals
Each p orbital consists of two sections better known as lobes which lie on either side of the plane passing through the nucleus.
The three p orbitals differ in the way the lobes are oriented whereas they are identical in terms of size shape and energy.
As the lobes lie along one of the x, y or z-axis, these three orbitals are given the designations 2px, 2py, and 2pz. Thus, we can say that there are three p orbitals whose axes are mutually perpendicular.
Similar to s orbitals, size, and energy of p orbitals increases with an increase in the principal quantum number (4p > 3p > 2p).
The Shape of p Orbitals
The magnetic orbital quantum number for d orbitals is given as (-2,-1,0, 1,2). Hence, we can say that there are five d-orbitals.
These orbitals are designated as dxy, dyz, dxz, dx2–y 2 and dz2.
Out of these five d orbitals, shapes of the first four d-orbitals are similar to each other, which is different from the dz2 orbital whereas the energy of all five d orbitals is the same.
The Shape of d Orbitals