Question

Which list of transition metals is arranged in the correct order, from lowest to highest number of electrons in the d sublevel?

A. zirconium, rhodium, vanadium, nickel, scandium
B. scandium, vanadium, nickel, zirconium, rhodium
C. rhodium, vanadium, scandium, nickel, zirconium
D. scandium, zirconium, vanadium, nickel, rhodium

Answer 1

Answer:

D. scandium, zirconium, vanadium, nickel, rhodium

Explanation:

Lets have a look into the electronic configuration of these elements.

Ar is for Argon and Kr is for Krypton.

${21} Sc_$ =$[Ar]$ = $4s^{2} 3d^{1}$

${40} Zr_$ =$[Kr]$ =$5s^{2} 4d^{2}$

${23} V_$ =$[Ar]$ =$4s^{2} 3d^{3}$

${28} Ni_$ =$[Ar]$ =$4s^{2} 3d^{8}$

${45} Rh_$ =$[Kr]$ =$4s^{2} 3d^{7}$=$5s^{1} 4d^{8}$

Note:Rhodium is an exception as $5s^{1} 3d^{8}$ is more stable than $5s^{2} 3d^{7}$.

One electron from $5s^{2}$ orbital is being transferred with the $4d^{7}$ orbital electon.

We see that Scandium has one electron in d sublevel.

Zirconium has two electrons in d sublevel.

Vanadium has three electrons in d sublevel.

Nickel and Rhodium has eight electrons in d sublevel.

So from lowest to highest number of electrons are as follows: scandium, zirconium, vanadium, nickel, rhodium

Answer 2

Transition metals from lowest to highest number of electrons in the d sublevel : Scandium, Zirconium, Vanadium, Nickel, Rodium

Further explanation

In an atom there are levels of energy in the shell and sub shell

This energy level is expressed in the form of electron configurations.

Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub-shells in the shell of an atom, namely s, p, d and f. The maximum number of electrons for each sub shell is

• s: 2 electrons

• p: 6 electrons

• d: 10 electrons and

• f: 14 electrons

Charging electrons in the sub shell uses the following sequence:

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.

Determination of electron configurations based on principles:

 Hund's Rule, Aufbau's Principle, and Pauli-exclusion principle.

• 1. Aufbau: Electrons occupy orbitals of the lowest energy level
• 2 Hund: electrons fill orbitals with the same energy level
• 3. Pauli: no electrons have the same 4 quantum numbers

Let's look at each of the electron configurations:

Zirconium: Zr: [Cr] 4d² 5s²: 2 electrons in the d sublevel

Rodium: Rh: Cr 4d⁸ 5s¹: 8 electrons in the d sublevel

Vanadium: V: [Ar] 3d³ 4s²: 3 electrons in the d sublevel

Nickel: Ni: [Ar] 3d⁸ 4s²: 8 electrons in the d sublevel

Scandium: Sc: [Ar] 3d¹ 4s²: 1 electron in the d sublevel

If we look at the number of electrons in the d sublevel above, then the order from lowest to highest:

Scandium, Zirconium, Vanadium, Nickel, Rodium

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