Transition metals - basics
- Created by: Agata
- Created on: 09-05-16 17:24
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- 3.5.4 - Transition Metals
- A transition metal is a metal that can form one or more stable ions with incomplete (partially filled) d-subshell
- It's the incomplete d-subshell that causes the special chemical properties of transition metals. D-block elements without an incomplete d-subshell don't have these properties
- SCANDIUM & ZINC
- Sc and Zn are NOT transition metals as their stable ions don't have partially filled d-subshell
- Scandium only forms one ion Sc^3+, which has an empty d-subshell.
- Sc Electronic configuration: [Ar]3d^1 4s^2
- When it loses 3 electrons to form its ion, the ion has electronic configuration of [Ar]
- Sc Electronic configuration: [Ar]3d^1 4s^2
- Zinc only forms one ion, Zn^2+, which has a full d-subshell
- Zn electronic configuration: [Ar]3d^10 4s^2
- When it loses 2 electrons, both are removed from 4s subshell - electronic configuration of the ion [Ar]3d^10
- Zn electronic configuration: [Ar]3d^10 4s^2
- Scandium only forms one ion Sc^3+, which has an empty d-subshell.
- Sc and Zn are NOT transition metals as their stable ions don't have partially filled d-subshell
- TRANSITION METAL IONS
- Transition metal atoms form POSITIVE IONS. When this happens the S electrons are removed FIRST, then the D electrons.
- To write the electronic configuration of transition metal ion follow these steps:
- 1) Write down the electronic configuration of the element.
- 2) Work out how many electrons have been removed to make the ion.
- 3) Remove that number of electrons from the electronic configuration taking them out of the S-orbital FIRST and then the d-orbitals
- 2) Work out how many electrons have been removed to make the ion.
- 1) Write down the electronic configuration of the element.
- To write the electronic configuration of transition metal ion follow these steps:
- Transition metal atoms form POSITIVE IONS. When this happens the S electrons are removed FIRST, then the D electrons.
- ELECTRONIC CONFIGURAT-IONS
- 2 Rules: 1) Electrons fill up the lowest energy subshells first. 2)Electrons fill orbitals singly before they start sharing.
- Exceptions:
- Chromium has one electron in each orbital of the 3d subshell and just one in the 4s subshell- this gives it more stability.
- Copper has a full 3d subshell and just one electron in the 4s subshell - this gives it more stability
- Exceptions:
- 2 Rules: 1) Electrons fill up the lowest energy subshells first. 2)Electrons fill orbitals singly before they start sharing.
- PHYSICAL PROPERTIES OF TRANSITION METALS
- All have HIGH DENSITY
- All have HIGH MELTING and HIGH BOILING POINTS.
- Their IONIC RADII are more or less the SAME.
- CHEMICAL PROPERTIES OF TRANSITION METALS
- They can FORM COMPLEX IONS
- They form COLOURED IONS
- They're GOOD CATALYSTS
- They can exist in VARIABLE OXIDATION STATES.
- A transition metal is a metal that can form one or more stable ions with incomplete (partially filled) d-subshell
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