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Questions and Answers
Which element does NOT qualify as a transition metal?
Chromium and copper follow the Aufbau Principle in their electron configurations.
False
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.
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Match the following transition metals with their potential oxidation states:
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Which of the following statements about transition metals is true?
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All ligands are classified as bidentate ligands.
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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.
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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.
