Chem orbital and subshells

Q: What is the maximum number of electrons in a subshell with quantum number ℓ?

2(2ℓ+1).

Q: How many electrons can fit in an s subshell?

A: 2 (1 orbital × 2).

Q: How many electrons can fit in a p subshell?

A: 6 (3 orbitals × 2).

Q: How many electrons can fit in a d subshell?

A: 10 (5 orbitals × 2).

Q: How many electrons can fit in an f subshell?

A: 14 (7 orbitals × 2).

Q: Where does the s subshell first appear?

A: At n = 1 (1s).

Q: Where does the p subshell first appear?

A: At n = 2 (2p).

Q: Where does the d subshell first appear?

A: At n = 3 (3d).

Q: Where does the f subshell first appear?

A: At n = 4 (4f).

Q: How many orbitals does the s subshell have, and what shape is it?

A: 1 orbital, spherical.

Q: How many orbitals does the p subshell have, and what shape are they?

A: 3 orbitals, dumbbell-shaped.

Q: How many orbitals does the d subshell have, and what shape are they?

A: 5 orbitals, clover-shaped (mostly).

Q: How many orbitals does the f subshell have?

A: 7 orbitals, complex shapes.

Q: Which block of the periodic table corresponds to the s subshell?

A: Groups 1–2 (alkali & alkaline earth metals) + Helium.

Q: Which block of the periodic table corresponds to the p subshell?

A: Groups 13–18 (right side of the table).

Q: Which block of the periodic table corresponds to the d subshell?

A: Transition metals (groups 3–12, middle of the table).

Q: Which block of the periodic table corresponds to the f subshell?

A: Lanthanides & actinides (the “bottom two rows”).