To learn the restrictions on each quantum number. Quantum numbers can be thought

Question

To learn the restrictions on each quantum number.

Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers.

The principal quantum number n corresponds to the shell in which the electron is located. Thus ncan therefore be any integer. For example, an electron in the 2p subshell has a principal quantum number of n=2 because 2p is in the second shell.

The azimuthal or angular momentum quantum number corresponds to the subshell in which the electron is located. s subshells are coded as 0, psubshells as 1, d as 2, and f as 3. For example, an electron in the 2p subshell has =1. As a rule, can have integer values ranging from 0 to n1.

The magnetic quantum number m corresponds to the orbital in which the electron is located. Instead of 2px, 2py, and 2pz, the three 2p orbitals can be labeled 1, 0, and 1, but not necessarily respectively. As a rule, m can have integer values ranging from to +.

The spin quantum number ms corresponds to the spin of the electron in the orbital. A value of 1/2means an "up" spin, whereas 1/2 means a "down" spin.

Part A

What is the only possible value of m for an electron in an s orbital?

Express your answer numerically.

Part B

What are the possible values of m for an electron in a d orbital?

Express your answer numerically with sequential values separated by commas.

SubmitHintsMy AnswersGive UpReview Part

Part C

Which of the following set of quantum numbers (ordered n, , m, ms) are possible for an electron in an atom?

Check all that apply.

Check all that apply.

3, 2, 0, -1/2 5, 3, 4, 1/2 3, 2, 2, -1/2 2, 1, 0, 1 5, 2, 1, -1/2 4, 3, -4, -1/2 -2, 1, 0, -1/2 2, 2, 2, 1/2

Explanation / Answer

What is the only possible value of m for an electron in an s orbital?

s orbital has a "l" value of 0

therefore

since mL = +/- 0,1,2,3, ... up to "l"

so..

l = 0, so mL = 0 ONLY

What are the possible values of m for an electron in a d orbital?

if "d"

then

l = 0,1,2,3,4

s,p,d,f...

l = 2

so ml = 0,1,2,-1,-2 = 5 values

Which of the following set of quantum numbers (ordered n, , m, ms) are possible for an electron in an atom?

5, 3, 4, 1/2 not posible, since ml > l, which is not possible

2, 1, 0, 1 not possible since spin is either 1/2 or -12

4, 3, -4, -1/2 not possible since absolute value of ml is greater than l

-2, 1, 0, -1/2 not possible since n can't be negative

2, 2, 2, 1/2 not possible since l = n-1 alwas, so l = 1

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.