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What does VSEPR Stand for? What does it attempt to explain?
Valence Shell Electron Pair Repulsion.
Help predict shape of electron pairs, like bonding and lone pairs, all are negative so they repel eachother.

Types of electron geometrys?
 Linear
 Trigonal Planar
 Tetrahedral
 Trigonal Bipyramidal
 Octahedral

Linear
 Has 180 Degree angles.
 2 bonding pairs, 0 lone pairs.

Trigonal Planar
 Has 120 Degree angles.
 3 bonding pairs, 0 lone pairs.

Tetrahedral
 Has 109.5 Degree angles.
 4 bonding pairs, 0 lone pairs.

Trigonal Bipyramidal
 Has 90 & 120 Degree angles.
 5 bonding pairs, 0 lones pairs.

Octahedral
 Has 90 Degree angles.
 6 bonding pairs, 0 lone pairs.

 Electron Geometry: Trigonal Planar
 Molecular Geometry: BENT
 Angels: 120 degrees
 2 bonding pairs, 1 lone pair

 Electron Geometry: Tetrahedral
 Molecular geometry: BENT
 Angles: 109.5, 104.5 degrees
 2 bonding pairs, 2 bonding pairs

 Electron Geometry: Tetrahedral
 Molecular Geometry: TRIGONAL PYRAMIDAL
 Angles: 107 degrees
 3 bonding pairs, 1 lone pair

 Electron Geomoetry: Trigonal Bipyramidal
 Molecular Geometry: SEESAW
 Angles:90 degrees
 4 Bonding Pairs, 1 Lones pairs

 Electron Geomoetry: Trigonal Bypryamidal
 Molecular Geometry: TSHAPE
 Angles: 90 degrees
 3 Bonding Pairs, 2 Lones pairs

 Electron Geomoetry: Trigonal Bipyramidal
 Molecular Geometry: Linear
 Angles: 90 degrees
 2 Bonding Pairs, 3 Lone pairs

 Electron Geomoetry: Ocatahedral
 Molecular Geometry:SQUARE PYRAMIDAL
 Angles: 90
 5 Bonding Pairs, 1 Lone pairs

 Electron Geomoetry: Octahedral
 Molecular Geometry: SQUARE PLANAR
 Angles: 90
 4 Bonding Pairs, 2 Lone pairs

What is a Dipole Moment?
The electric dipole moment for a pair of opposite charges of magnitude q is defined as the magnitude of the charge times the distance between them and the defined direction is toward the positive charge.

What are polar molecules? Give examples of when molecules are polar.

What is the difference between Intramolecular forces and Intermolecular forces?
The Intermolecular Forces (forces between molecules) are weaker than Intramolecular Forces (The Chemical Bonds within an Individual Molecule).

 S Oribital
 Shape of a sphere.

 p Oribital
 Shape of a figure eight.

 d Orbital
 Shape of 2 dumbells

 f Orbitals
 Shapr of 6 Cloves

sp HYBRID Orbital.
 sp Hyrbid Orbitals are usually formed with linear electron geometry.

sp^{2} HYBRID Orbital.
 sp^{2} Hybrid Orbital has a Trigonal planar Electron geometry

sp^{3} HYBRID Orbital.
 Has tetrahedral electron geometry

sp^{3}d HYRBRID Orbital.
Has Trigonal Bipyramidal electron geometry

sp^{3}d^{2} HYBRID Orbital.
Has Octahedral electron geometry

Isomers
 Cis: Same side
 Trans: Across


Pie Bonds always come from __ Orbital.
p

_______ Bonds are allowed free movement, while ___ Bonds do not allow movement.
Single, Pie

____ bonding is lower than ____ bonding.
Pie, Sigma

Molecular Orbital Theory consists of adding, ________ and subtracting ________ atomic orbitals. This is called the _____.
Bonding, Antinbonding, L.C.A.O.= Linear Combination of Atomic orbitals

The addition of 2 Atomic Orbitals and gives favorable overlapping is called...
Bonding

The subtraction of 2 atomic orbitals is called...
Antibonding

Homonuclear Diatomics are for O_{2, }F_{2,} Ne.

Determines # of bonds, like single, double and triple.

If no bonds are formed and bond order is equal to 0, then the element is said to be...
Diatomic

The state of an atom or ion that contains unpaired electrons and is, therefore, attracted by an extrenal magnetic feild.
Paramagnetic

The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelledby an external magnetic field.
Diamagnetic

Heteronuclear Diatomics
 diatomic molecules composed of two different elements.

FOr heteronuclear diatomics, The most electronegative atom withh attain the extra electron. The lower the energy, the more....
Electronegative

