There are [Fill in the blank]
orbitals in a 5p subshell. The angular momentum quantum number (l) of these orbitals is [Fill in the blank]
.
(Input numbers only.)

Question

There are [Fill in the blank]
 orbitals in a 5p subshell. The angular momentum quantum number (l) of these orbitals is [Fill in the blank]
.
(Input numbers only.)

BlackTom AI · Accepted Answer

We are dealing with a 5p subshell and need to fill two blanks with the correct numbers.
First, recall that a p subshell corresponds to an angular momentum quantum number l = 1. This immediately identifies the second blank: the l value for p orbitals is 1.
Next, determine how many orbitals reside in a given subshell characterized by l. The number of orbitals in a subshell is given by the magnetic quantum number m_l values, which range from -l to +l in integer steps. Therefore the total number of orbitals in a subshell with a given l is (2l + 1).
For l = 1, (2l + 1) becomes (2×1 + 1) = 3. Hence the first blank should be filled with 3, representing the number of orbitals in the 5p subshell.
In summary: the 5p subshell has 3 orbitals because m_l can be -1, 0, or +1, and the angular momentum quantum number l for p orbitals is 1.

CHEM1012 (L2) Online Quiz #1

There are [Fill in the blank] orbitals in a 5p subshell. The angular momentum quantum number (l) of these orbitals is [Fill in the blank] . (Input numbers only.)

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