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

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What are the possible values of m? for an electron in a d 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 e 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 e = 1. As a rule, e can have integer values ranging from 0 to n - 1. The magnetic quantum number me 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_e can have integer values ranging from -e to +e The spin quantum number m* 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. What are the possible values of me for an electron in a of orbital? Express your answer numerically with sequential values separated by commas. Which of the following set of quantum numbers (ordered n. e. me. m_s) are possible for an electron in an atom? Check all that apply.

Explanation / Answer

This would be -l to +l. For d orbital l = 2 therefore ml = -2, -1, 0, +1, +2

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