Give the values for n, l, and ml for each orbital in the 2p subshell,

enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. separate values within each set by semicolons. enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. example: "1; 0; -1,1; 1; -1,1; 2; 1" (n; l; ml, n; l; ml, n; l; ml).

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part b

give the values for n, l, and ml for each orbital in the 5d subshell.

enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. separate values within each set by semicolons. enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. example: "1; 0; -1,1; 1; -1,1; 2; 1" (n; l; ml, n; l; ml, n; l; ml).

(2; 1; -1, 2; 1; 0, 2; 1; 1)

(5; 2; -2, 5; 2; -1, 5; 2; 0, 5; 2; 1, 5; 2, 2)

Explanation:

Give the values for n, l, and ml for each orbital in the 2p subshell

Orbitals in 2p subshell belong to shell 2. Thus, the principal quantum number (n) is 2.

Orbitals of the p-type have an angular quantum number (l) of 1.

In the 2p subshell there are 3 orbitals p, distinguishable by the magnetic quantum number (ml). When l = ,1 ml can take the values -1, 0, 1.

The combinations of n, l, ml for these orbitals are (2; 1; -1, 2; 1; 0, 2; 1; 1)

Give the values for n, l, and ml for each orbital in the 5d subshell.

Orbitals in 5d subshell belong to shell 5. Thus, the principal quantum number (n) is 5.

Orbitals of the d-type have an angular quantum number (l) of 2.

In the 2p subshell there are 5 orbitals p, distinguishable by the magnetic quantum number (ml). When l = ,2 ml can take the values -2, -1, 0, 1, 2.

The combinations of n, l, ml for these orbitals are (5; 2; -2, 5; 2; -1, 5; 2; 0, 5; 2; 1, 5; 2, 2)