1D questions

[John Liang 2I]

11d. " How many orbitals are in subshells with l equal to (a) 0;
(b) 2; (c) 1; (d) 3?

How does one differentiate between the definitions of shell, subshell, and orbital?

[Jamie Lee 1H]

Shells encompass both orbitals and subshells and are represented by value of n- principle quantum number. Subshells are within a shell and are represented by s, p, d, and f. Orbitals are within the subshell such as px, py, pz.
L value of 0= s
L value of 1= p
L value of 2= d
L value of 3= d

[Osvaldo SanchezF -1H]

Well a shell can be determined by the period on the periodic table. It tells you have many outer blocks of electrons it contains such as shell 1 contains 2 electrons and shell 2 contains 8 electrons. A sub shell is just the type of orbital where the electrons lie such as the S, P and D sub shells. The number of orbitals of a sub shell is just how many pairs of electrons each sub shell can contain such as the S-sub shell just has one orbital, the P-sub shell has 3 orbitals and the D-sub shell has 5 orbitals.

[Claire Stoecklein 1E]

A shell corresponds to the principle quantum number, a sub shell to the orbital angular momentum quantum number, and an orbital to the magnetic.

[preyasikumar_2L]

11d. " How many orbitals are in subshells with l equal to
(a) l = 0 --> s --> 1 orbital
(b) l = 2 --> d --> 5 orbitals
(c) l = 1 --> p --> 3 orbitals
(d) l = 3 --> f --> 7 orbitals

N = shell number, you can figure that out by what period (row) the element is in (EX: Na has 3 shells, n = 3. it's in the 3rd period of the table)
Subshell = type of shell, such as s, p, d, or f
Orbital = pairing of electrons and their orientation within a subshell, such as p_x, p_y, p_z