Chem 240: Ch#02- Representative Carbon Compounds: Functional Groups, Intermolecular Forces

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Hydrocarbon:

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compounds whose molecules contain only carbon and hydrogen atoms

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Alkane

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carbon carbon single bond

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Alkenes:

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carbon carbon double bond

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Alkynes:

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carbon carbon triple bond

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Saturated compounds:

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contain the max # of H's that a carbon compound can possess.

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unsaturated:

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posses fewer than the max # of H atoms.

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determining the # of unsaturations:

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Benzene:

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aromatic compound

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Delocalization:

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The moment of e-s from single to double to single...etc. "stabilizes molecules"

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Polar Covalent Bonds:

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- Strongly influence the physical properties & reactivity of molecules

- present in molecules that contain bonded atoms w/ different electronegativity values.
--------- e-s are not shared equally. The atom with greater electronegativity draws e-s density closer to it.

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Functional Groups:

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defined groups of atoms in a molecule that usually gives rise to the function (reactivity/ physical properties) of the molecule

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Electronegativity:

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the ability of an element to attract e-s that it is sharing in a covalent bond.

- the part of a molecule where most of its chemical reactions occur

- effectively determines the compound's chemical properties.

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Map of Electrostatic Potential (MEP):

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- RED: regions of an e- density surface that are more (-)

---- attract a positively charged species (or repel a negative charge)

- BLUE: less (-) or positive

---- likely to attract e-s from another molecule

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Alkyl Group:

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groups that we ID for naming purposes....

obtained by removing a H atom from an alkane
---- ending in -yl

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Phenyl group:

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Benzene ring attached to some other group of atoms

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Benzyl Group:

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a phenyl group combined with a methylene group (-CH2-)

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Alkyl Halids (Haloalkanes):

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Alcohols:

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are classified into 3 groups: Primary, secondary, and tertiary alcohols. This classification is based on the degree of substitution of the carbon to which the hydroxyl group is directly attached.

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Ether:

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Amine:

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are amines acids or bases? strong or weak?

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are weak bases

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Carbonyl group:

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aldehyde:

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Ketone:

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Carboxylic acid:

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Ester:

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Amide:

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Nitrile:

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Melting point:

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the temp. @ which an equilibrium exists between the well-ordered crystalline state and the more random liquid state.

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Ion-ion forces:

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forces that hold ions together in the crystalline state....
--- the strong electrostatic lattice forces that act between the (+) & (-) ions in the orderly crystalline structure.

---------- requires large amounts of thermo energy to break the orderly structured crystals.

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dipole-dipole forces:

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- are in most organic molecules which have a permanent dipole moment resulting from a nonuniform distribution of the bonding e-s

- cause the molecule to orient themselves so that the (+) end of one molecule is directed toward the (-) end of another.

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Hydrogen bonds:

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- attractions between hydrogen atom bonded to small strongly electronegative atoms (O,N,F), & nonbonding e- pairs on other such electronegative atoms.

- are weaker than ordinary covalent bonds, but much stronger than dipole-dipole interactions.

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Vander Waals Forces:

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dipole forces w/in molecules that cause attractions to other molecules of opp. force.

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polarizability:

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the ability of the e-s to respond to a changing electric field

- depends on how loosely/ tightly the e-s are held.

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Boiling pt. of a liquid:

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the temp. @ which the vapor pressure of the liquid equals the pressure of the atmosphere above it
--- pressure dependent

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Solubilities:

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The dissolution of a solid in a liquid.

the orderly crystal structure of the solid is destroyed
--- results is the formation of the more disorderly arrangement of the molecules (ions) in solution.

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Hydrophobic:

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fearing/ avoiding water

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Hydrophilic:

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loving/ seeking water

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summary of Attractive Electric Forces

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