What is the only possible value of m_l for an electron in an s orbital? To learn

Question

What is the only possible value of m_l for an electron in an s orbital? 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 n can 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 l corresponds to the subshell in which the electron is located, s subshells are coded as 0, p subshells as 1, d as 2, and f as 3. For example, an electron in the 2p subshell has t = 1. As a rule, l can have integer values ranging from 0 to n - 1. What are the possible values of to/for an electron in a d orbital? The magnetic quantum number mi corresponds to the orbital in which the electron is located. Instead of 2p_x, 2p_y, and 2p_z, the three 2p orbitals can be labeled -1,0, and 1, but not necessarily respectively. As a rule, m_l can have integer values ranging from -l to +l. The spin quantum number m_s corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas -1/2 means a "down" spin. Which of the following set of quantum numbers (ordered n, l, ml, m_s) are possible for an electron in an atom?

Explanation / Answer

1) The only possible value of MQN(ml) in 's' orbital is 0

2) In a 'd' subshell, there are 5 orbitals and thus the possible values of MQN(ml) are -2,-1,0,1,2

3) The correct options are :-

a) 4,2,-1,-1/2

b) 5,3,0,1/2

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

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