Term
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Definition
| Force that holds two atoms together |
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Term
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Definition
| Energy required to break a bond |
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Term
| Types of electrons does bonding require the behavior of |
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Definition
| Valence electrons (outermost s+p levels) |
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Term
Ionic Bonding
delta X > 1.7 |
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Definition
Involves mixture of (usually) metal and nonmetal
Nonmentals alomst at full valance, therefore want to pull e-
Highest- Fluorine
Lowest- Francium/Cesium
Make a large group of ions...resulting crystal is very sturdy and strong (electrostatic attractions holding it together) |
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Term
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Definition
| Tendancy of bonded atoms to pull electrons toward itself |
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Term
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Definition
| Tendancy of bonded atoms to pull electrons toward itself |
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Term
Covalent Bonding
delta x < .5 or 50 |
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Definition
Generally occurs w/ two nonmetals
E- on one atom will start to be attracted to nucleus(proton) of other, v.e- lowers energy (attracted forces tend to lower energy of a system)
Potential energy goes up when nuclei gets too close together forming repulsion
chemical potential energy stored in bond
difference between 0 and lowest energy point ...but because difference in small to 0, don't take e- from eachother |
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Term
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Definition
Bond is a covalent bond (due to difference in X), but is one in which the electrons are unequally shared
drawing different for covalent bonds |
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Term
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Definition
1. write skeleton structure of the mlcl
2. find total v. e-, including any charges present
3. connect atomos w/ a single bond (a line which stands for 2e-)
4. fill up octets of outside atom w/ remaining e-
5. a) any extra e- go on center atom, even if has octet
b) if run out of e-; meed to multiple bond |
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Term
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Definition
Can find shape of the ion/mlcl formed
shape tells us to dictate how mlcl/ion interacts with other stuff
V = Valence
S = Shell
E = Electron
P = Pair
R = Repulsion |
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Term
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Definition
Sum of the # of atoms attached and # of nonbinding (lone) pairs of electrons on the atom
Tells # orbitals need, which tells you # of old orbitals you used up |
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Term
| All atoms positioning themselves to be as far apart as possible |
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Definition
Because surrounded by e- density and lone pairs of e- around a central atom
minimize the repulsion forces between regions of e- density and lone pairs e- more repulsive than atoms (more pushing power) |
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Term
Coord. # : 2
Lone Pairs : 0 |
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Definition
Electron Geo. = linear
Molecular Geo. = linear
(180 degrees)
Ex: BeF2 |
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Term
Coord. # : 3
Lone Pairs : 0 |
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Definition
Electron Geo. = trig. planar
Molecular Geo. = trig. planar
(120 degrees)
Ex: BF3 |
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Term
Coord. # : 3
Lone Pairs : 1 |
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Definition
Electron Geo. = trig. planar
Molecular Geo. = v-shaped/bnt
( <120 degrees)
Ex: BF2 - |
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Term
Coord. # : 4
Lone Pairs: 0 |
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Definition
Electron Geo. = tetrahedral
Molecular Geo. = tetrahedral
(109.5 degrees)
Ex: CF4 |
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Term
Coord. # : 4
Lone Pairs: 1 |
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Definition
Electron Geo. = tetrahedral
Molecular Geo.=trig. pyramid.
(<109.5 degrees)
Ex: CF3- |
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Term
Coord. # : 4
Lone Pairs: 2 |
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Definition
Electron Geo. = tetrahedral
Molecular Geo. = v-shaped/bnt
(<109.5 degrees)
Ex: CF2 2- |
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Term
Coord. # : 5
Lone Pairs: 0 |
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Definition
Electron Geo. = trig. bipyram
Molecular Geo.= trig. bipyram
(120 + 90 degrees)
Ex: SbF5 |
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Term
Coord. # : 5
Lone Pairs: 1 |
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Definition
Electron Geo. = trig. bipyram
Molecular Geo. = see-saw
(<120,<90 degrees)
Ex: SbF4 - |
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Term
Coord. # : 5
Lone Pairs: 2
Ex: SbF3 2- |
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Definition
Electron Geo. = trig. bipyram
Molecular Geo. = t-shaped
(<90 degrees) |
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Term
Coord. # : 5
Lone Pairs: 2
Ex: SbF3 2- |
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Definition
Electron Geo. = trig. bipyram
Molecular Geo. = t-shaped
(<90 degrees) |
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Term
Coord. # : 5
Lone Pairs: 3 |
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Definition
Electron Geo. = trig. bipyram
Molecular Geo. = linear
(180 degrees)
Ex: SbF2 3- |
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Term
Coord. # : 6
Lone Pairs: 0 |
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Definition
Electron Geo. = octahedral
Molecular Geo. = octahedral
(90 degrees)
Ex: TeF6 |
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Term
Coord. # : 6
Lone Pairs: 1 |
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Definition
Electron Geo. = octahedral
Molecular Geo. = sq. pyramid.
( degrees)
Ex: TeF5 - |
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Term
Coord. # : 6
Lone Pairs: 2 |
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Definition
Electron Geo. = octahedral
Molecular Geo. = sq. planar
(<90 degrees)
Ex: Tef4 2- |
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Term
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Definition
Behavior of an atom that's involved in bonding
When they bond, often create new orbitals specifically for bonding (covalent)
Each coordination # has corresponding hybrid., which produces own unique shape |
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Term
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Definition
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Term
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Definition
Hybrid: sp2
Shape: trigonal planar |
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Term
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Definition
Hybrid: sp3
Shape: tetrahedral |
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Term
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Definition
Hybrid: sp3d
Shape: trigonal bipyramidal |
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