Term
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Definition
unpaired e- in shells
effected (attracted) by magnetic fields |
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Term
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Definition
paired e- in shells
uneffected by magnetic fields |
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Term
| change in energy and electrons |
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Definition
| smaller energy change when unpaired e- are in shells |
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Term
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Definition
mining of metals
depends on reduction potential
gold, silver, platinum are mined as is |
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Term
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Definition
| get metal into usable form |
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Term
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Definition
metal sulfide ores concentrated
differences in oil in waters effect on gangue and metal
more polar floats |
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Term
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Definition
| heat and air oxidized metal as SLAG |
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Term
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Definition
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Definition
| molecules with same molecular formula but different chemical structures |
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Term
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Definition
linkage isomers
geometric isomers
optical isomers |
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Term
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Definition
ligands approach the metal ion from different directions
affect d orbitals in different ways |
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Term
| Metal complexes and color |
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Definition
| metal complexes are colored because metals EMIT LIGHT AS ELECTRONS RAISE TO HIGHER ENERGY LEVELS |
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Term
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Definition
have vacant d orbitals - accept shares in e- pairs
Group 20 Multiple charges possible (cations)
LEWIS ACIDS |
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Definition
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Definition
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Term
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Definition
| small amounts of chromium in a coordination complex absorb green light |
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Term
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Definition
number of donor atoms an acceptor metal is bonded
(# of ligands) |
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Term
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Definition
metal ligand bonding is ionic by having ligand and d electron repulsion
Have same energy
different ligands create different field strength |
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Term
| how is nuclei re-arranged in a metal |
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Definition
e- conductivity
malleablity and ductility |
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Term
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Definition
| bonds to a central metal atom and donates lone pair of electrons |
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Term
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Definition
| separate materials by density |
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Term
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Definition
| hydrocarbon containing a double bond per molecule |
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Term
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Definition
| hydrocarbon containing a triple bond |
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Term
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Definition
| hydrocarbon containing a single bond |
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Term
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Definition
Cl-, F- Br-, I-
Cannot be oxidized
Only reduced once |
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Definition
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Definition
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Definition
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Definition
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Term
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Definition
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Term
| Which group does not react with acid? |
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Definition
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Term
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Definition
form 2+ or 3+ most of time
Ex. Fe 2+ |
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Term
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Definition
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| What is a good reduction agent for metals? |
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Definition
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Term
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Definition
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Term
| Coordination # 2 Hybrization |
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Definition
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Term
| Coordination # 3 Hybrization |
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Definition
sp2
trigonal planar or bent |
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Term
| Coordination # 4 Hybrization |
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Definition
sp3
tetrahedral
trigonal pyramidal |
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Term
| Coordination # 4 Hybrization alt. |
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Definition
sp3d
square pyramidal
trigonal bipyramid |
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Term
| Coordination # 6 hybrization |
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Definition
sp3d2
octahedral
square pyyramidal |
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Term
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Definition
| Molecules that are the same formula but have different structures |
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Term
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Definition
Two molecules that have the same strucutures
cis/trans |
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Term
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Definition
| If you have to take a model to pieces to convert it into another one, then you've got isomers. If you merely have to twist it a bit, then you haven't! |
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Term
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Definition
| atoms across from each other from the double bond |
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Term
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Definition
| atoms on same side of double bond |
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Term
| Why does sulfur element have S8? |
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Definition
| has a larger distance between sulfur atoms giving poor p-orbital overlap and no pi- bonds |
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Term
| When can nitrogen oxide not be formed? |
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Definition
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Term
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Definition
obtaining the free metal from an ore
Chemical or electrolysis |
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Term
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Definition
| A rod containing the desired pure metal & impurities is passed through a series of heating coils and cooled again. (impurities are moved to end of rod and cut off) |
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Term
| Why does copper turn green? |
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Definition
| copper is oxidized by air, then acid rain (H2SO4) causes green |
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Term
| Example of Bidentate ligands |
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Definition
glycinate ion
oxalate ion
ethylenediamine (en) |
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Term
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Definition
(claw) formed by ligands multi-point attachment to a metal
holds metal ions together preventing oxidation |
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Term
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Definition
| isomers that give different ions in a solution |
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Term
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Definition
| isomers with different metal-ligand bonds |
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Term
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Definition
electrons move from ground state to higher state
must have d-orbitals partially and unequally filled
metal absorbs energy as light as electrons drop |
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Term
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Definition
| same electron amount in each shell |
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Term
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Definition
have vacant d orbitals
LEWIS ACID - ACCEPT E- |
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Term
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Definition
have same molecular mass
different properties (e.g. boiling point) |
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Term
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Definition
| covalent bond is a pair of electrons of opposite spin that are shared by two atoms from orbital overlap |
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Term
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Definition
used to create purified metal
impurities are turned into SLAG |
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Term
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Definition
1/2 bonding- filled
1/2 antibonding- empty
delocalized valence electrons occupy MO energy levels
valency band |
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Term
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Definition
material that is like a metal and an insulator
a few electrons can jump the gap and conduct (group 4 elements) |
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Term
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Definition
| increasing conductivity of a semiconductor by adding small amount of impurities |
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Term
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Definition
| Permits electron flow only one way |
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Term
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Definition
| inorganic nonmetallic non molecular solids |
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