How many orbitals in an atom can have each of the following designations?

Question

a) 5f number=?

b)4p number=?

c) 5d number=?

d) n=2 number=?

Answer 1

If l is the index of the subshell, the number of orbitals are 2l+1 . The number of sjell has no importance for that question

so a) 5f l=3 there are 3*2+1=7 orbitals 5f

b) 4p l=1 there are 3 orbitals 4p

c) 5d l=2 there are 5 orbitals 5d

d) n=2 l can have two values for l=0 you have one orbital
for l=1 you have 3 orbitals . So you have 4 orbitals

Answer 2

If i'm know-how your question wisely; In an s sublevel, there is only a million orbital. it is not correct no count if that's 1s or 4s. So, 4s could have a million orbital. In a p sublevel, there are 3 orbitals. lower back, it won't count if that's 2p or 5p. For the quantum numbers; The imperative quantum type is n, that's akin to the ability point, so it is going to continually be an integer > or = a million. The azumithal quantum type, l, is the type of orbitals, and is comparable to n-a million. The magnetic quantum type, m, shows the spatial orientation of the orbitals, and that's -l to +l. finally is spin quantum type, z, and designates an electron in an orbital. it's going to be the two +a million/2 or -a million/2. So, to reply to the 2nd component of your question; The 2s sublevel could have n = 2, l =a million, and m = -a million, 0, and +a million. type of orbitals = l = a million. The 6g sublevel could have n=6, l=5, m = -5, -4, -3, -2, -a million, 0 , a million, 2, 3, 4, and 5. type of orbitals = l = 5.