[Year 2] DM
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Where are the d-block elements in the periodic table?
In the middle between s-block and p-block.
What is a transition element?
• A d-block element… • that can form at least one stable ion… • with a partially filled d-orbital.
How many electrons can a d-orbital hold?
Up to 10 electrons
Which elements in period four are not transitioned element but are in the d-block? Why?
• Scandium (Sc) and Zinc (Zn) - as they do not form a stable ion with a partially filled d-orbital.
How do electrons fill a d-orbital?
Singularly firsts. Then they double up. • because electrons repel eachother
Write the shorthand electron configuration of the transition elements in period 4 Period 4 d-blocks: Sc Ti V Cr Mn Fe Co Ni Cu Zn
Ti: 3d |↑ |↑ | | | | 4s |↑↓| Config = [Ar] 3d² 4s² V: 3d |↑ |↑ |↑ | | | 4s |↑↓| Config = [Ar] 3d³ 4s² Cr: 3d |↑ |↑ |↑ |↑ |↑ | 4s |↑ | Config = [Ar] 3d⁵ 4s¹ (as filling all with 1 is most stable) Mn: 3d |↑ |↑ |↑ |↑ |↑ | 4s |↑↓| Config = [Ar] 3d⁵ 4s² Fe: 3d |↑↓|↑ |↑ |↑ |↑ | 4s |↑↓| Config = [Ar] 3d⁶ 4s² Co: 3d |↑↓|↑↓|↑ |↑ |↑ | 4s |↑↓| Config = [Ar] 3d⁷ 4s² Ni: 3d |↑↓|↑↓|↑↓|↑ |↑ | 4s |↑↓| Config = [Ar] 3d⁸ 4s² Cu: 3d |↑↓|↑↓|↑↓|↑↓|↑↓| 4s |↑ | Config = [Ar] 3d¹⁰ 4s¹ (as a full 3d orbital is more stable)
Show why Scandium is not a transition metal.
Scandium’s electron configuration is as followed… 3d |↑ | | | | | 4s |↑↓| It only forms one stable ion, Sc³⁺, which has the configuration… 3d | | | | | | 4s | | Because of its empty d-orbital, it cannot be a transition element.
Show why Zinc is not a transition metal.
Zinc’s electron configuration is as followed… 3d |↑↓|↑↓|↑↓|↑↓|↑↓| 4s |↑↓| It only forms one stable ion, Zn²⁺, which has the configuration… 3d |↑↓|↑↓|↑↓|↑↓|↑↓| 4s | | Because of its full d-orbital, it cannot be a transition element.
What is the electron configuration of Fe ions and Cu ions?
Fe²⁺ : [Ar] 3d⁶ Fe³⁺ : [Ar] 3d⁵ Cu⁺: [Ar] 3d¹⁰ Cu²⁺: [Ar] 3d⁹
What are the properties of transition metals?
• Variable oxidation states. • Form coloured ions in solution. • able to form complex ions.
What colour are Fe ions in solution?
Fe²⁺ = light green Fe³⁺ = yellow
What colour are Cu ions in solution?
Cu²⁺ = Blue Cu⁺ is unstable in solution, so will disproportionate into Cu²⁺ and Cu readily… 2Cu⁺ → Cu²⁺ + Cu
What is a complex ion?
• Where a central transition metal ion… • is surrounded by ligands… • bonded by dative covalent bonds.
How do you show a complex ion?
• Central ion. • With dative covalent bond arrows from ligands to it. • In square brackets. • With a charge.
What is a ligand?
Ions, atoms, or molecules that have at least one lone pair of electrons.
What are examples of monodentate ligands?
Water: H₂O፡ Ammonia: ፡NH₃ Cyanide: ፡CN⁻ Chloride: ፡Cl⁻
What are examples of bidentate ligands?
Ethanedioate: ⁻፡OOC=COO፡⁻ Ethylenediamine (diamino ethane): H₂N̈C₂H₄N̈H₂
What are examples of polydentate ligands?
EDTA⁴⁻ 6 lone pairs
What factors affect the shape of a complex ion?
• Size of ligands - Coordination number
What is the coordination number?
The number of coordinate bonds in a complex. not number of ligands as ligands can have multiple coordinate (dative) bonds
Which ligands are small? How many can fit around a central metal ion? What shape do these form?
Water: H₂O፡ Ammonia: ፡NH₃ Cyanide: ፡CN⁻ • 6 can fit around one central ion. • This forms an octahedral shape.
Which ligands are medium? How many can fit around a central metal ion?
Chloride: ፡Cl⁻ 4 can fit around one central ion. - This forms tetrahedral shapes and square planar for Pt[(NH₃)₂(Cl)₂)]₍ₐᵩ₎ (cis platin, an anti-cancer drug).
Which ligands are large?
Ethanedioate: ⁻፡OOC=COO፡⁻ Ethylenediamine (diamino ethane): H₂N̈C₂H₄N̈H₂ Normally 3 can fit around one ion.
What happens to the d-orbital when a ligands bond?
The d-orbital splits. Before: 3d |↑↓|↑↓|↑ |↑ |↑ | After: |↑ |↑ | (this energy gap is ΔE) |↑↓|↑↓|↑ | This is known as the ground state