Term
| Complex Ion with a CN of 4 |
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Definition
| Tetrahedral or Square Planar |
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Term
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Definition
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Term
| Complex Ion with a CN of 2 |
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Definition
Linear.
Requires sp hybridization. |
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Term
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Definition
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Term
| Metal ion-ligand interaction |
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Definition
| Lewis acid-base interaction. The ligand donates a lone pair of electrons to an empty orbital on the metal ion to form a coordinate covalent bond. |
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Term
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Definition
| Yeilds the minimum number of unpaired electrons (fills up the t2g orbitals before jumping to the eg orbitals) as a result of a large delta-o. aka strong-field case. |
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Term
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Definition
Yeilds the maximum number of unpaired electrons (puts an electron in all orbitals before pairing any) as a result of a small delta-o. aka weak-field case.
Delta-o is less than the energy needed to pair electrons so they stay unpaired as long as possible. |
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Term
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Definition
Goes from small delta-o to large delta-o, therefore high spin to low spin. The ligands are arranged in order of increasing delta-o values, or their ability to produce d-orbital splitting.
I- < Br- < Cl- < F- < OH- < H2O < NH3 < en < CN- |
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Term
| 3d M +2 compounds are ___ spin |
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Definition
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Term
| 3m M +3 compounds are ___ spin |
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Definition
| high spin for delta-o < H20 or NH3 and low spin for higher delta-o |
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Term
| 4d/5d compounds are ___ spin |
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Definition
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Term
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Definition
Positive polyatomic ion.
Polar-covalent bond between a transition metal (Lewis Acid) and a ligand (Lewis Base). |
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Term
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Definition
d0 metals, ligands that form double bonds, and larger ligands.
sp3 hybridization is required.
Always produce high spin. |
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Term
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Definition
| is most common for all transition metals |
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Term
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Definition
most common for d8 metals.
dsp2 hybridization is required. |
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Term
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Definition
Same formula, different ligand arrangement around the metal atom. Type of stereoisomerism. Same bonds, just different spatial arrangements.
Have different physical and chemical properties. |
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Term
| How do transition metals get their color? |
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Definition
| Comes from the absorption of some visible frequencies to provide energy for moving electrons between "d-like" MOs. delta-o = 12-30 k/cm |
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Term
| What is the trend for delta-o for metals? |
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Definition
| delta-o increases down columns and with increasing oxidation state |
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Term
| What is the trend for delta-o for ligands? |
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Definition
| delta-o increases from strong acids like I-, Br- to H2O, NH3 and then ends with CN-, aka the spectrochemical series |
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Term
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Definition
| dxz, dyz, dxy orbitals are nonbonding orbitals. Those which lobes point "in between" the point charges and are thus lower in energy in the octahedral complex than dz^2 and dx^2-y^2. This is the splitting of the d-like MOs that explains the color and magnetism of complex ions for 3d TMs. The splitting leads to delta-o which then determines if it is high spin or low spin. |
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Term
| How do the TMs get their color and magnetism? |
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Definition
| The splitting of the d-like MOs that explains the color and magnetism of complex ions for 3d TMs. The splitting leads to delta-o which then determines if it is high spin or low spin. |
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Term
| TM (Lewis Acid) plus a LIGAND (Lewis Base) is a |
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Definition
| Coordination Compound or Complex, a polar covalent bond in direction M+---L- |
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Term
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Definition
| dz^2, dx^2-y^2 point at the ligands and therefore are bonding and anti-boings sigma MOs. |
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Term
| neutral transition metal + organic ligand = |
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Definition
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Term
| Magnetism is determined by |
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Definition
| the energy needed to pair 2 electrons in the same orbital. Both high-spin and low-spin are possible for d4-7 metals. |
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Term
| Transition metals in the body serve 3 different functions. |
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Definition
1-electron carriers (>1 oxidation state)
2-oxygen carriers (>1 coordination number)
3-catalysts/enzymes (organisms must be carried out near STP, can't have too much variation in delta-H) |
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Term
| Which transition metals are the most abundant? |
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Definition
| 3d are >> than 4d or 5d. Fe is the most abundant 3d element and is used most biologically while Mo is the most abundant 4d/5d. |
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Term
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Definition
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Term
| Brackets [ ] indicate atoms are |
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Definition
| within the covalently-bonded silicate network. Other atoms outside the brackets are ions there to balance the silicate charge. |
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Term
| C forms single bonds with ___. With all bonds single, it is ___ hybridized, a ___ in shape |
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Definition
| C, H, N, O, S, Cl; sp3; tetrahedral |
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Term
| C forms double bonds with ___, is ___ hybridized, and ___ in shape |
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Definition
| C, N, O, S; sp2, trigonal planar |
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Term
| C forms triple bonds with ___, is ___ hybridized, and ___ in shape |
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Definition
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Term
| Which carbon bonds are reactive? |
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Definition
| carbon double and triple bonds. C-C bonds and C-H bonds are unreactive |
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Term
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Definition
saturated hydocarbons; only form single bonds.
Carbon will always be sp3, tetrahedral, so NO alkane is planar.
Unreactive at STP.
Will chlorinate or oxidize at high temp. |
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Term
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Definition
Unsaturated hydrocarbons; have a C=C double bond.
More reactive as it is electron rich.
Trigonal planar, sp2.
If has different groups attached, geometric isomer. |
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Term
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Definition
good solvents for polar and nonpolar molecules.
High bp and water solubility (polarity, h bonding).
Liquids up to C12.
With strong reductants and bases, act like H2O.
With acids, substitution. |
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Term
| Aldehydes (RCH=O) and Ketones (R2C=O) |
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Definition
water-soluble
lengthen C chain, important for building up large molecules |
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Term
| Carboxilic Acid (RC(=O)OH) |
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Definition
weak acids in water
high bp (high polarity, h bond)
can convert to esters (RCo2R') or amides (RCONHR') |
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Term
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Definition
weak acids in water
lower bp than O compounds |
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Term
| Amino Acids [RCH9(NH2)Co2H] |
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Definition
high melting point as solids
conduct electricity as liquids
high dipole moments
not acidic or basic in water
polymerize to give proteins by elimination of H2O, forming a peptide (amide) bond |
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