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28 Cards in this Set
- Front
- Back
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why intermolecular forces important
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control melting/boiling point, energy needed for phase change, solubility and structure
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dipole/dipole
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when the positive end of one molecule is attracted to the negative end of another, the more polar the stronger the bond is, ex HCl
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hydrogen bond
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a really strong dipole/dipole bond, always has F,O, or N (highly electronegative atoms) ex. h20
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LDF
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instantaneous dipole bond, when one end of an molecule becomes slightly more negative than the other and bonds to another slightly more postive end of another molecule (ex He2 and NeonXenon
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ion-dipole interactions
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interactions with the charged ends of polar molecules to give ion-dipole interactions
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van der waals forces
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dipole dipole, hydrogen, and ldf bonds
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is it possible for there to be mulitiple kinds of intermolecular bonds holding a substance together?
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yes :)
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strength order of van der waals forces
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ldf<dipole dipole<hydrogen
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strength order of all intermolecular bonds
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ion dipole>dipole dipole (incl. hydrogen)>dipole/induced dipole ldf
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if there is a lone pair with three bonds the angles are _______
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<120
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AX2
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linear
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AX3
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triangular planar
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AX4
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tetrahedron (4 bonds)
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AX5
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triangular bipyrimidal
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AX6
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tetrahedron
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AX2
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linear
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AX3
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triangular planar
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AX4
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tetrahedron (4 bonds)
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AX5
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triangular bipyrimidal
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AX6
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tetrahedron
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bond angle of 2 bonds
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180
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bond angle of 3 bonds
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120
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bond angle of 4 bonds
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109.5
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inTERmolecular bonding
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bonding WITHIN a molecule
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inTRAmolecular bonding
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bonding BETWEEN two or more molecules that already have intermolecular bonds
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monoatomic ions
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ions with only one atom (ex Ca 2+, Mg 2+)
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polyatomic ions
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ions with multiple atoms (SO4 2-, NO3 -)
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LDFs ________ with size because of a _______ number of electrons in _______atoms
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increase, larger, bigger
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