15.1.1 Electronic Configuration

• What is the key characteristic that distinguishes transition metals from other elements?

  Partially filled d subshells
• The general electronic configuration for transition metals involves the d orbitals being filled.
• Scandium (Sc) is a transition metal because it has a partially filled d subshell in its atom.
• Why is Zinc (Zn) not considered a transition metal?

  Its d subshell is fully filled
• Scandium (Sc) forms Sc3+ with the electronic configuration [Ar], indicating the loss of 4s electrons.
• The ion configuration of scandium (Sc3+) is [Ar].
• Zinc (Zn) has an atomic configuration of [Ar] 3d10 4s2 and is not a transition metal because its d subshell is fully filled.
• Transition metals are defined as elements with partially filled d subshells in any of their ions.
• Zinc (Zn) is considered a transition metal because it has a fully filled d subshell.

  False
• What distinguishes transition metals from other elements in terms of their electronic configuration?

  Partially filled d subshells
• Match the element with its atomic configuration:

  Scandium (Sc) ↔️ [Ar] 3d1 4s2

  Zinc (Zn) ↔️ [Ar] 3d10 4s2
• Order the steps for determining if an element is a transition metal:

  1️⃣ Check if the element has a partially filled d subshell in any of its ions

  2️⃣ Determine the electronic configuration of the element

  3️⃣ Compare the ion configuration with the atomic configuration
• The general electronic configuration of transition metals is (n - 1)d^{1 - 10} ns^{1 - 2}
• The d orbitals are filled after the ns orbitals in transition metals.
• In which block of the periodic table are transition metals located?

  d-block
• Unlike s-block and p-block elements, transition metals exhibit multiple oxidation states due to the partially filled d orbitals.
• Iron (Fe) has an electronic configuration of [Ar] 3d6 4s2.
• What is the electronic configuration of Copper (Cu)?

  [Ar] 3d10 4s1
• The general electronic configuration of transition metals is $(n - 1)d^{1 - 10} ns^{1 - 2}$, where $n$ represents the period number.
• The (n - 1)d^{1 - 10}</latex> term in the electronic configuration represents partially filled d orbitals.
• Order the filling of orbitals in transition metals.

  1️⃣ $(n - 1)d$ orbitals

  2️⃣ $ns$ orbitals
• What is the actual electronic configuration of Chromium (Cr)?

  [Ar] 3d5 4s1
• Exceptions to the filling order of d and s orbitals occur due to extra stability from half-filled or fully filled d subshells.
• Between which groups is the d-block of the periodic table located?

  Groups2 and 13
• What is the defining characteristic of transition metals in terms of their electronic configuration?

  Partially filled d subshells
• Scandium (Sc) is a transition metal because it has a partially filled d subshell in its atom.
• Why is Zinc (Zn) not considered a transition metal?

  Its d subshell is fully filled
• The ion configuration of Scandium (Sc) in Sc3+ is [Ar].
• Zinc (Zn) has an ion configuration of [Ar] in Zn2+.

  False
• What defines transition metals in terms of their electronic configuration?

  Partially filled d subshells
• Zinc (Zn) is a transition metal because its d subshell is fully filled.

  False
• Transition metals are defined as elements that have partially filled d subshells in any of their ions.
• Where are transition metals located on the periodic table?

  d-block
• Match the transition metal with its electronic configuration:

  Iron (Fe) ↔️ [Ar] $3d^{6} 4s^{2}$

  Copper (Cu) ↔️ [Ar] $3d^{10} 4s^{1}$
• Unlike s-block and p-block elements, transition metals exhibit multiple oxidation states due to their partially filled d orbitals.
• In transition metals, the (n-1)d orbitals fill before the ns orbitals.
• Which element is an exception to the general filling order of transition metals with the configuration [Ar] $3d^{5} 4s^{1}$?


  Chromium (Cr)
• The exceptions to the general electronic configuration of transition metals occur because of the extra stability gained from a half-filled or fully filled d subshell.
• The actual electronic configuration of Chromium (Cr) is [Ar] $3d^{5} 4s^{1}$