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# What are the possible values of n and ml for an electron in a 5d orbital ? A) n = 5 and ml = -2, -1, 0, +1, or +2 B) n = 1, 2, 3, 4, or 5 and ml = 2 C) n = 5 and ml = 2 D) n = 1, 2, 3, 4, or 5 and ml = -2, -1, 0, +1, or +2

The answer is **A)**.

The **principal quantum number**, or ##n##, describes the energy lelvel in which the electron can be found, Since you're interested in an electron located in a **5d-orbital**, ##n=5##.

The **angular momentum quantum number**, or ##l##, describes the subshell, or orbital type, in which your electron is located. Since you have a **d-orbital**, ##l=2##.

The value of ##l## will give you the value of the **magnetic quantum number**, or ##m_l##, which describes the orientation of the orbital.

The accepted values for ##m_l## range from ##-l## to ##+l##, which means that you can have **5** d-orbitals in the **fifth energy level**, ##d_(xy)##, ##d_(xz)##, ##d_(yz)##, ##d_(z^2)##, and ##d_(x^2-y^2)##, each described by a magnetic quantum number

##m_l = -2## ##m_l = -1## ##m_l = 0## ##m_l = +1## ##m_l = +2##

As an example, here's how these orbitals would look for the **3d subshell**