How are s orbitals different from p orbitals?

S orbitals and p orbitals are both types of atomic orbitals, which are regions of space around an atomic nucleus where electrons are likely to be found. However, they have several key differences:

Shape:

S orbitals are spherically symmetric and have a spherical shape.
P orbitals are dumbbell-shaped and have two lobes with a node (region of zero electron probability) at the nucleus.
Orientation:

S orbitals do not have any orientation. They are spherically symmetrical around the nucleus.
P orbitals come in three different orientations along the x, y, and z axes. These are often labeled as
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p
x
​
,
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p
y
​
, and
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p
z
​
orbitals.
Energy:

S orbitals generally have lower energy than p orbitals when considering the same principal quantum number (n).
Number of electrons:

Each energy level (n) can contain one s orbital with a maximum of 2 electrons (spin-paired).
Each energy level (n) can contain three p orbitals (
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p
x
​
,
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p
y
​
, and
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p
z
​
), accommodating a total of 6 electrons.
Penetration:

S orbitals have higher electron density near the nucleus compared to p orbitals.
P orbitals have regions of high electron density both near the nucleus and farther away.
These differences are important in understanding atomic structure, chemical bonding, and the shapes of molecules.