Chapter 10

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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
    • Image Upload 1
    • Has 180 Degree angles.
    • 2 bonding pairs, 0 lone pairs.
  4. Trigonal Planar
    • Image Upload 2
    • Has 120 Degree angles.
    • 3 bonding pairs, 0 lone pairs.
  5. Tetrahedral
    • Image Upload 3
    • Has 109.5 Degree angles.
    • 4 bonding pairs, 0 lone pairs.
  6. Trigonal Bipyramidal
    • Image Upload 4
    • Has 90 & 120 Degree angles.
    • 5 bonding pairs, 0 lones pairs.
  7. Octahedral
    • Image Upload 5
    • Has 90 Degree angles.
    • 6 bonding pairs, 0 lone pairs.
  8. Image Upload 6
    • Electron Geometry: Trigonal Planar
    • Molecular Geometry: BENT
    • Angels: 120 degrees
    • 2 bonding pairs, 1 lone pair
  9. Image Upload 7
    • Electron Geometry: Tetrahedral
    • Molecular geometry: BENT
    • Angles: 109.5, 104.5 degrees
    • 2 bonding pairs, 2 bonding pairs
  10. Image Upload 8
    • Electron Geometry: Tetrahedral
    • Molecular Geometry: TRIGONAL PYRAMIDAL
    • Angles: 107 degrees
    • 3 bonding pairs, 1 lone pair
  11. Image Upload 9
    • Electron Geomoetry: Trigonal Bipyramidal
    • Molecular Geometry: SEE-SAW
    • Angles:90 degrees
    • 4 Bonding Pairs, 1 Lones pairs
  12. Image Upload 10
    • Electron Geomoetry: Trigonal Bypryamidal
    • Molecular Geometry: T-SHAPE
    • Angles: 90 degrees
    • 3 Bonding Pairs, 2 Lones pairs
  13. Image Upload 11
    • Electron Geomoetry: Trigonal Bipyramidal
    • Molecular Geometry: Linear
    • Angles: 90 degrees
    • 2 Bonding Pairs, 3 Lone pairs
  14. Image Upload 12
    • Electron Geomoetry: Ocatahedral
    • Molecular Geometry:SQUARE PYRAMIDAL
    • Angles: 90
    • 5 Bonding Pairs, 1 Lone pairs
  15. Image Upload 13
    • Electron Geomoetry: Octahedral
    • Molecular Geometry: SQUARE PLANAR
    • Angles: 90
    • 4 Bonding Pairs, 2 Lone pairs
  16. 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.Image Upload 14
  17. 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. waterImage Upload 15
    • T-shaped molecules, eg. IF3
    • See-Saw molecules, eg. SF4Image Upload 16
    • Pyramidal molecules (trigonal pyramidal, square pyramidal, etc) [NOT bi-pyramidal], eg. NF3, BrF5Image Upload 17
  18. 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).
  19. Image Upload 18
    • S Oribital
    • Shape of a sphere.
  20. Image Upload 19
    • p Oribital
    • Shape of a figure eight.
  21. Image Upload 20
    • d Orbital
    • Shape of 2 dumbells
  22. Image Upload 21
    • f Orbitals
    • Shapr of 6 Cloves
  23. sp HYBRID Orbital.
    • sp Hyrbid Orbitals are usually formed with linear electron geometry.
    • Image Upload 22
  24. sp2 HYBRID Orbital.
    • sp2 Hybrid Orbital has a Trigonal planar Electron geometry
    • Image Upload 23
  25. sp3 HYBRID Orbital.
    • Has tetrahedral electron geometry
    • Image Upload 24
  26. sp3d HYRBRID Orbital.
    Has Trigonal Bipyramidal electron geometry
  27. sp3d2 HYBRID Orbital.
    Has Octahedral electron geometry
  28. Isomers
    • Cis: Same side
    • Trans: Across
    • Image Upload 25
  29. Pie Bonds always come from __ Orbital.
    p
  30. _______ Bonds are allowed free movement, while ___ Bonds do not allow movement.
    Single, Pie
  31. ____ bonding is lower than ____ bonding.
    Pie, Sigma
  32. 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
  33. The addition of 2 Atomic Orbitals and gives favorable overlapping is called...
    Bonding
  34. The subtraction of 2 atomic orbitals is called...
    Antibonding
  35. Homonuclear Diatomics are for O2, F2, Ne.
    Image Upload 26
  36. Determines # of bonds, like single, double and triple.
    Image Upload 27
  37. If no bonds are formed and bond order is equal to 0, then the element is said to be...
    Diatomic
  38. The state of an atom or ion that contains unpaired electrons and is, therefore, attracted by an extrenal magnetic feild.
    Paramagnetic
  39. The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelledby an external magnetic field.
    Diamagnetic
  40. Heteronuclear Diatomics
    • diatomic molecules composed of two different elements.
    • Image Upload 28
  41. FOr heteronuclear diatomics, The most electronegative atom withh attain the extra electron. The lower the energy, the more....
    Electronegative
Author:
aarnback
ID:
23391
Card Set:
Chapter 10
Updated:
2010-06-13 23:52:05
Tags:
VSEPR Theory
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Description:
Chemistry (CHM111)
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