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30 Cards in this Set
- Front
- Back
Chemical bond
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Force that holds two atoms together
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Bond dissociation energy
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Energy required to break a bopnd
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Types of electrons does bonding require the behavior of?
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Valence electrons (outermost s+p levels)
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Ionic Bonding
delta X > 1.7 |
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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Electronegativity
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Tendancy of bonded atoms to pull electrons toward itself
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Lewis dot diagrams
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Diagrams used to represent element in question w/ its correct number of electrons
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Covalent Bonding
delta x < .5 or 50 |
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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Polar Covalent Bonding
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Mixture of an ionic bond and covalent bond
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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Drawing covalent bonds
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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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VSEPR
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Can find shape of the ion/mlcl formed
shape tells us to dictate how mlcl/ion interacts with other stuff |
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Coordination number
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Sum of the # of atomos attached and # of nonbinding (lone) pairs of electros on the atom
Tells # orbitals need, which tells you # of old orbitals you used up V = Valence S = Shell E = Electron P = Pair R = Repulsion |
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All atoms positioning themselves to be as far apart as possible
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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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Coord. # : 2
Lone Pairs : 0 |
Electron Geo. = linear
Molecular Geo. = linear (180 degrees) Ex: BeF2 |
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Coord. # : 3
Lone Pairs : 0 |
Electron Geo. = trig. planar
Molecular Geo. = trig. planar (120 degrees) Ex: BF3 |
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Coord. # : 3
Lone Pairs : 1 |
Electron Geo. = trig. planar
Molecular Geo. = v-shaped/bnt ( <120 degrees) Ex: BF2 - |
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Coord. # : 4
Lone Pairs: 0 |
Electron Geo. = tetrahedral
Molecular Geo. = tetrahedral (109.5 degrees) Ex: CF4 |
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Coord. # : 4
Lone Pairs: 1 |
Electron Geo. = tetrahedral
Molecular Geo.=trig. pyramid. (<109.5 degrees) Ex: CF3- |
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Coord. # : 4
Lone Pairs: 2 |
Electron Geo. = tetrahedral
Molecular Geo. = v-shaped/bnt (<109.5 degrees) Ex: CF2 2- |
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Coord. # : 5
Lone Pairs: 0 |
Electron Geo. = trig. bipyram
Molecular Geo.= trig. bipyram (120 + 90 degrees) Ex: SbF5 |
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Coord. # : 5
Lone Pairs: 1 |
Electron Geo. = trig. bipyram
Molecular Geo. = see-saw (<120,<90 degrees) Ex: SbF4 - |
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Coord. # : 5
Lone Pairs: 2 |
Electron Geo. = trig. bipyram
Molecular Geo. = t-shaped (<90 degrees) Ex: SbF3 2- |
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Coord. # : 5
Lone Pairs: 3 |
Electron Geo. = trig. bipyram
Molecular Geo. = linear (180 degrees) Ex: SbF2 3- |
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Coord. # : 6
Lone Pairs: 0 |
Electron Geo. = octahedral
Molecular Geo. = octahedral (90 degrees) Ex: TeF6 |
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Coord. # : 6
Lone Pairs: 1 |
Electron Geo. = octahedral
Molecular Geo. = sq. pyramid. ( degrees) Ex: TeF5 - |
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Coord. # : 6
Lone Pairs: 2 |
Electron Geo. = octahedral
Molecular Geo. = sq. planar (<90 degrees) Ex: Tef4 2- |
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Hybridization
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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 Certain kind of symmetry- sigma (sigma bond). formed by p orbital having pi symm. so any multpile bonds are called pi bonds. |
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Coord # 2
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Hybrid: sp
Shape: linear |
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Coord # 3
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Hybrid: sp2
Shape: trigonal planar |
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Coord # 4
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Hybrid: sp3
Shape: tetrahedral |
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Coord # 5
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Hybrid: sp3d
Shape: trigonal bipyramidal |