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47 Cards in this Set
- Front
- Back
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Transition metals |
Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn |
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Oxidation states |
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Paramagnetic |
Unpaired electrons |
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Diamegnetic |
Paired electrons |
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Repersentive |
Main group, transition, non-transition |
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The transition metal rules |
The 3d orbital begins to fill after the 4S orbital is complet |
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For complex ions |
The 4s will loose electrons first then the 3d |
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Across the periodic table trends |
Atomic size decreases at first then remains constant Electro negativity and the ionization energies also increase |
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Within a group |
The atomic size increases from 4-5 but not 5-6 |
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Metallic behavior |
The lower the oxidation state of the transition metal, the more metallic its behavior |
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Ionic bonding |
Is more prevalent for the lower oxidation states, wheres covalent bonding occurs more frequently for higher oxidation state |
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Metals oxides become |
Less basic (more acidic) as the oxidation state increases |
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A metal atom in a positive oxidation state |
Has a greater attraction for bonded electrons = a greater effective electronegativity or valance - state electronegativity, then in the zero oxidation state |
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Color |
Preamegnetic =color bc its unpaired electrons |
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Coordination number |
The number of atoms or ions immediately surrounding a central atom in a complex or crystal The number of bonds formed be a metal ions to ligand in complex ion varies form 2 to 8 or 4 to 6 bonds |
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Coordination number 2 |
Linear |
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Coordination number 4 |
Square planer or tetrahedral (depends on the the charge) |
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Coordination number 6 |
Octahedral |
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Types of ligands |
Monodentate: one bond to a metal Bidentate: two bonds to a metal Polydentate: more than two bonds to a metal |
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Naming coordination [CO(NH3)5Cl]Cl2 |
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Coordination compoud |
Consist of a complex ion and a counter ion |
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Parts of a complex compound |
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Metal- ligand bonding is entirely ionic |
Strong-feild (low spin) large splitting of d orbital Weak -feild (high spin) small splitting of d orbital |
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When the geometry and the ligands are held constant, this splitting decreases in the following order |
Pt4+>Ir3+>Rh3+>CO3+>Cr3+>Fe2+>CO2+>Ni2+>Mn2+ |
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Low spin |
Diamegnetic = no color |
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High spin |
Paramagnetic --> Huns rule = color |
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When the geometry and the metal are held constant, the splitting of the d orbitals increases in the following order |
I<Br<[NCS]<Cl<F<OH<H2O<NH3<en<CN<CO |
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Strong ligand |
Not hunds = big ^E |
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^E= hc/~ |
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Square planer complex |
Rh(I) Ir(I) Pd(II) Pt(II) Au(III) |
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The ways color can change |
Metal charge Ligand |
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Red |
Absorbance 700-620 We see Green |
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Orange |
Absorbance 620-580 We see blue |
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Yellow |
Absorbance 580-560 We see purple |
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Green |
Absorbance 560-490 We see Red |
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Blue |
Absorbance 490-430 We see orange |
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Purple |
Absorbance 430-380 We see yellow |
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CFT |
Symmetry of ligands around a central metal/ion and how this anisotropic |
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The d orbital split into two levels |
Eg ( two upper levels) and t2g (3 lower levels) For octahedral the energies are higher (0.6^°) while t2g is lower (0.4^°) |
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Tetrahedral splitting constant (^t), which is less than (^°) for the same ligand |
Normally high spin ^t= 0.44^° |
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The splitting energy (from highest to lowest orbital) is ^sp and tends to be larger then ^° |
^sp = 1.74 ^° |
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d10 electrons |
Colorless |
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Anionic ligands |
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Neutral Ligands |
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Prefex |
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