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CHEM 0310: CHAPTER 1
alkanes |
Contain only C and H Only single bonds
saturated compounds
ex. butane
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haloalkanes
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organic compounds possessing polar carbon-halogen bonds as their functional groups
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Alcohols |
Carbon atom bonded to the oxygen of a hydroxyl group (-OH)
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Ether |
Oxygen with two single bonds to carbon
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Thiols |
Sulfur with one bond to hydrogen and one to carbon.
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alkenes
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double bonded carbons
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Alkynes |
At least one triple bond CΞC
CnH2n-2
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aromatic compounds
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contain a benzene ring of six carbons atoms
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Aldehydes
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at end of carbon skeleton c double bonded to o and single bond to h
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Ketones |
C double bonded to O and singly bonded to 2 carbon skeleton groups
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Carboxylic Acid
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C bonded with double bond with O bonded to an alchohol and another carbon group.
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Anhydrides
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functional group is a two carbonyl groups bonded to the same oxygen
RC=OOC=OR'
to name drop "acid" and add word anhydride to parent C=O.
example: acetic acid
acetic anhydride
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Esters |
C double bonded to O and single bonded to another O
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amide
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C double bonded to O and single bonded to a N
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Nitrile |
C triple bond with N
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Amine |
N bonded to 2 h and carbon group
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Chlorination
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substitution of hydrogen atoms of an organic compound by chlorine atoms
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Substitution Reaction
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Reaction in which an atom or group of atoms is replaced by another atom or group of atoms
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Elimination reaction
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A chemical reaction in which a double bond is formed when atoms in a molecule are removed
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Hydrogen Atom
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Contains one proton and one electron
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Proton |
Positive charge, H
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A hydride ion is
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a negative hydrogen with two electrons
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ionization potential
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the energy it takes to remove an electron from the atom
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electron affinity
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the energy released when a single electron is added to an isolated atom
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carbon normally has ___ bonds
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4
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nitrogen normally has ___ bonds
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3
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oxygen normally has ___ bonds
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2 |
Electronegativity increases ____ to _____, ______ to _________.
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left, right, bottom, top
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if they have the same electronegativity then they will form
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perfectly covalent bonds
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trigonal planar shape
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sp2 = 3 bonds,
bond angle 180
Bonding -3
nonbonding -0
120 degrees.
E.g. BF3
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Trigonal Pyramidal
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3 bonds, 1 lone pair
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formal charge calculation
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=number valence electrons-bonding-number of lone pair
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Guidelines for resonance contribution of canonical structures
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Major contributors should:
1) Structures w/max octets
2) Charges on atoms should match relative EN
3) Structures w/less separation of opposite charge
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Hybrid Orbital: sp
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Involves 2 electron groups. A hybrid between one s and p orbital.
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sp2 hybrid orbital
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1/3 of an s orbital
2/3 of an p orbital
120 degrees
trigonal planar
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SP3 hybrid orbital
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composition - 1 s and 3 p orbitals = 4 sp3 orbitals
tetrahedral - 109.5o
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π bonds are
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sideway parallel overlap of pure p orbitals
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The most stable form of an element according to MO theory
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has a greater net bondiing
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note "R" "S" and placement of dash wedge
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HCl addition (carbocation intermediate)
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