Chapter 10

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aarnback
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23391
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Chapter 10
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2010-06-13 19:52:05
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VSEPR Theory
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Chemistry (CHM111)
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  1. 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.
  2. Types of electron geometrys?
    • Linear
    • Trigonal Planar
    • Tetrahedral
    • Trigonal Bipyramidal
    • Octahedral
  3. Linear
    • Has 180 Degree angles.
    • 2 bonding pairs, 0 lone pairs.
  4. Trigonal Planar
    • Has 120 Degree angles.
    • 3 bonding pairs, 0 lone pairs.
  5. Tetrahedral
    • Has 109.5 Degree angles.
    • 4 bonding pairs, 0 lone pairs.
  6. Trigonal Bipyramidal
    • Has 90 & 120 Degree angles.
    • 5 bonding pairs, 0 lones pairs.
  7. 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: SEE-SAW
    • Angles:90 degrees
    • 4 Bonding Pairs, 1 Lones pairs
    • Electron Geomoetry: Trigonal Bypryamidal
    • Molecular Geometry: T-SHAPE
    • 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
  8. 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.
  9. What are polar molecules? Give examples of when molecules are polar.
    A polar molecule is one with a permanent Dipole Moment. A polar molecule must have a slightly positive end opposite a slightly negative one.Molecules that have 'low' symmetry will always have at least a small dipole moment and therefore be referred to as polar. Examples of such low symmetry molecular shapes include:


    • Bent molecules, eg. water
    • T-shaped molecules, eg. IF3
    • See-Saw molecules, eg. SF4
    • Pyramidal molecules (trigonal pyramidal, square pyramidal, etc) [NOT bi-pyramidal], eg. NF3, BrF5
  10. 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
  11. sp HYBRID Orbital.
    • sp Hyrbid Orbitals are usually formed with linear electron geometry.
  12. sp2 HYBRID Orbital.
    • sp2 Hybrid Orbital has a Trigonal planar Electron geometry
  13. sp3 HYBRID Orbital.
    • Has tetrahedral electron geometry
  14. sp3d HYRBRID Orbital.
    Has Trigonal Bipyramidal electron geometry
  15. sp3d2 HYBRID Orbital.
    Has Octahedral electron geometry
  16. Isomers
    • Cis: Same side
    • Trans: Across
  17. Pie Bonds always come from __ Orbital.
    p
  18. _______ Bonds are allowed free movement, while ___ Bonds do not allow movement.
    Single, Pie
  19. ____ bonding is lower than ____ bonding.
    Pie, Sigma
  20. 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
  21. The addition of 2 Atomic Orbitals and gives favorable overlapping is called...
    Bonding
  22. The subtraction of 2 atomic orbitals is called...
    Antibonding
  23. Homonuclear Diatomics are for O2, F2, Ne.
  24. Determines # of bonds, like single, double and triple.
  25. If no bonds are formed and bond order is equal to 0, then the element is said to be...
    Diatomic
  26. The state of an atom or ion that contains unpaired electrons and is, therefore, attracted by an extrenal magnetic feild.
    Paramagnetic
  27. The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelledby an external magnetic field.
    Diamagnetic
  28. Heteronuclear Diatomics
    • diatomic molecules composed of two different elements.
  29. FOr heteronuclear diatomics, The most electronegative atom withh attain the extra electron. The lower the energy, the more....
    Electronegative

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