Podcast
Questions and Answers
Which element does NOT qualify as a transition metal?
Which element does NOT qualify as a transition metal?
Chromium and copper follow the Aufbau Principle in their electron configurations.
Chromium and copper follow the Aufbau Principle in their electron configurations.
False
What are ligands in the context of transition metals?
What are ligands in the context of transition metals?
Molecules or ions that surround a central metal atom or ion and donate a pair of electrons.
The coordination number is the number of ________ bonds to the central metal atom or ion.
The coordination number is the number of ________ bonds to the central metal atom or ion.
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Match the following transition metals with their potential oxidation states:
Match the following transition metals with their potential oxidation states:
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Which of the following statements about transition metals is true?
Which of the following statements about transition metals is true?
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All ligands are classified as bidentate ligands.
All ligands are classified as bidentate ligands.
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What is a hexadentate ligand and provide an example.
What is a hexadentate ligand and provide an example.
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During catalysis, transition metals can change to various oxidation states by ________ electrons to or from reagents.
During catalysis, transition metals can change to various oxidation states by ________ electrons to or from reagents.
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Which transition metal complex corresponds to a tetrahedral geometry?
Which transition metal complex corresponds to a tetrahedral geometry?
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Study Notes
Transition Metals Overview
- Transition metals have an incomplete d-subshell or can form stable cations with incomplete d-subshell.
- Scandium and zinc are not considered transition metals despite being in the d-block.
Electronic Configuration
- The first five subshells can be abbreviated as [Ar], representing the argon core.
- Exceptions to the Aufbau Principle exist in the first row of d-block elements.
- Chromium has the electron configuration [Ar] 3d⁵ 4s¹.
- Copper has the electron configuration [Ar] 3d¹⁰ 4s¹.
- In ion formation, 4s electrons are removed before 3d electrons.
Properties of Transition Metals
- Transition metals can lose electrons to form positively charged ions, indicated by Roman numerals for oxidation states.
- Example: Iron (Fe) can form Fe²⁺ (Fe(II)) and Fe³⁺ (Fe(III)) ions.
Complex Ions
- Transition metals can form complex ions due to variable oxidation states.
- A complex ion consists of a central metal ion surrounded by ligands (molecules or ions).
- Ligands donate a pair of electrons, acting as Lewis bases (nucleophiles).
- Examples of iron(III) complexes include [Fe(NH₃)₆]³⁺, [Fe(OH)₆]³⁻, and [Fe(H₂O)₆]³⁺.
Color and Catalysis
- Compounds of transition metals are often colored.
- During catalysis, transition metals can change oxidation states, gaining or donating electrons.
Coordination Number and Ligand Types
- Coordination number refers to the number of coordinate bonds around a central metal atom or ion.
- Tetrahedral complexes (e.g., [CuCl₄]²⁻) and square planar complexes (e.g., [Ni(CN)₄]²⁻) have a coordination number of 4.
- Ligands can be multidentate, forming multiple dative bonds; for instance, EDTA⁴⁻ is a hexadentate ligand that forms 6 dative covalent bonds.
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Description
This quiz covers the essential characteristics of transition metals, focusing on their electronic configurations and distinguishing features compared to d-block elements. Test your understanding of concepts like incomplete d-subshells and stable cations. Ideal for students of chemistry looking to deepen their knowledge of metallic elements.
