The orbitals represented by the quantum numbers n=3, l=2, m=+2 and n=3, l=2, m=-2  have the same energy

It is true that the set of three quantum numbers n, l, and ml together specify a particular orbital.  So it may be confusing to you that there are some orbitals for which the value of ml is not identified.  If you review your notes, you will find, for example:A 1s orbital corresponds to n = 1, l = 0, and ml = 0.A 2pz orbital corresponds to n = 2, l = 1, and ml = 0.We can also say that the 2px and 2py orbitals both correspond to n = 2, l = 1, BUT we cannot identify a value of ml for each; the two values ml = 1 and -1 belong to both orbitals together but there is no one-to-one correspondence.  (The technical reason for this is that orbitals are not simply functions in real space but rather in "complex space", if you know what complex numbers are (they contain imaginary components, i = √-1).  For purposes of portraying the orbitals in real space, we transform the complex functions into real functions by taking linear combinations.)A 3s orbital corresponds to n = Answer 1 Question 10, l = Answer 2 Question 10, ml = Answer 3 Question 10.A 3px orbital corresponds to n = Answer 4 Question 10, l = Answer 5 Question 10, ml = Answer 6 Question 10.A 3dx2-y2 orbital corresponds to n = Answer 7 Question 10, l = Answer 8 Question 10, ml = Answer 9 Question 10.

Which of the following sets of quantum numbers refers to a 2s orbital?Group of answer choicesn= 1, l = 2, ml = 2, ms = + ½n= 2, l = 1, ml = -1, ms = + ½n= 2, l = 2, ml = 0, ms = + ½n= 1, l = 2, ml = 1, ms = + ½n= 2, l = 0, ml = 0, ms = + ½

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. List if any of these combination(s) has/have the same energy(i) n = 4, l = 2, ml = -2, ms = -1/2(ii) n = 3, l = 2, ml = 1, ms = +1/2(iii) n = 4, l = 1, ml = 0, ms = +1/2(iv) n = 3, l = 2, ml = -2, ms = -111(v) n = 3, l = l, ml = -1, ms = +1/2(vi) n = 4, l = 1, ml = 0, ms = +1/2

Using s,p,d,f notation, give orbital designation for:(a) n = 2, l =1, ml = -1, ms = + ½(b) n = 3, l=2, ml = -2, ms = + ½(c) n = 3, l=1, ml = -1, ms = + ½(d) n = 4, l=0, ml = 0, ms = + ½

The electrons of the same orbitals can be distinguished by(a) Principal quantum number(b) Azimuthal quantum number(c) Spin quantum number(d) Magnetic quantum