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35 Cards in this Set
- Front
- Back
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hydrocarbons |
compounds only containing carbon atoms |
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Name 3 groups of hydrocarbon compounds |
alkanes, alkenes, alkynes |
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Alkanes |
single bonds between carbon atoms |
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Alkenes |
contain 1+ carbon-carbon double bond |
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Alkynes |
contain 1+ carbon-carbon triple bond |
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Systematic name |
based on chemical structure |
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Generic name |
internationally accepted name |
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Trade name |
assigned by manufacturing company |
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Octet Rule |
main group elements want to have 8 e- around them - atoms will loose, gain or share to achieve 8 |
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electron deficient elements |
elements with les than 8 electrons |
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expended octets |
elements with more than 8 e- |
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radicals |
odd number of e- |
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formal charge |
valence electrons - # of nonbonding electrons - 1/2(# of bonding electrons) |
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Valence Shell Electron Pair Repulsion theory |
electron groups arrange themselves in a way to minimize repulsion |
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Why do lone pairs take up more space around the central atom? |
they cause more repulsion |
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electron geometry |
determined by the number of groups around the central atom |
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Bond angle of linear electron geometry |
180 |
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Bond angle of trigonal planar electron geometry |
120 |
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Bond angle of tetrahedral electron geometry |
109.5 |
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What happens to the bond angles when the central atom has a lone pair? |
The angles around the central atom decrease. |
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If the difference between the electronegative values of 2 atoms in a bond is </= 0.5 then the bond is...? |
polar |
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If a molecule has a net dipole then it is a ____ molecule |
polar |
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No net dipole means that the molecule is ____ |
nonpolar |
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What are the 2 posibilites that make a molecule nonpolar? |
Having all nonpolar bonds in a molecule or all the polar bonds cancel out |
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What are Intermolecular forces? |
nonbonding forces that exist between molecules and influence the physical properties of the substance |
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Name the types of intermolecular forces: |
Ion-ion, dipole-dipole, h-bonding, van der Walls |
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ion-ion |
interactions only between cations and anions (metal and nonmetals) |
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dipole-dipole |
interactions between polar covalent molecules |
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Hydrogen bonding |
between molecules that contain N, O, F |
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van der Waals |
all covalent molecules and are only forces that exist between nonpolar molecules |
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strength of van der Waals interactions depends on: |
polarizability & surface area |
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Polarizability |
determined by the size of electron cloud in a molecule (MW) |
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From weakest to strongest name the IM forces: |
van der Waals, dipole-dipole, H-bonding, ion-ion |
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boiling point |
phase change from a liquid to a gas state the IM forces need to be broken |
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The stronger the force the higher the boiling point, true or false? |
true |
