Question
Describe the shape of $2p$ orbitals.
✓
Answer
Shape of $2p$ orbitals:
$i.$ For $p$ orbital$, l = 1.$ For $l = 1, m_l = +1, 0, -1.$ Thus, $p$ orbitals have three orientations.
$ii.$ Each orbital has two lobes on the two sides of a nodal plane passing through the nucleus.
$iii.$ Shape of $2p$ orbitals resembles a dumbbell.
$iv.$ The size and energy of the three $2p$ orbitals are the same. However, their orientations in space are different. The lobes of the three $2p$ orbitals are along the $x, y$ and $z$ axes. Accordingly, the corresponding orbitals are designated as $2p_x, 2p_y$ and $2p_z.$ The size and energy of the orbitals in $p$ subshell increase with the increase of principal quantum number.
Diagram:
$i.$ For $p$ orbital$, l = 1.$ For $l = 1, m_l = +1, 0, -1.$ Thus, $p$ orbitals have three orientations.
$ii.$ Each orbital has two lobes on the two sides of a nodal plane passing through the nucleus.
$iii.$ Shape of $2p$ orbitals resembles a dumbbell.
$iv.$ The size and energy of the three $2p$ orbitals are the same. However, their orientations in space are different. The lobes of the three $2p$ orbitals are along the $x, y$ and $z$ axes. Accordingly, the corresponding orbitals are designated as $2p_x, 2p_y$ and $2p_z.$ The size and energy of the orbitals in $p$ subshell increase with the increase of principal quantum number.
Diagram:
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