4238476
| Question | Answer |
| Functional groups | Structural characteristics can make molecules function similarly, common partnering of atoms that are agents of reactivity |
| Alkane group | Carbon-carbon single bonds, often have hydrogen bonded to a carbon, simplest and least reactive compound |
| Heteroatom | Atoms other than carbon or hydrogen, N,O,Halogens,S |
| Alkene group | Carbon-carbon double bonds, stronger than single but weaker than triple, able to function as bases or nucleophiles |
| Alkyne group | Carbon-carbon triple bond, stronger than double bond, linear geometry, able to function as bases or nucleophiles |
| Arene group | Carbon-carbon ring with alternating double and single bonds |
| Halide group | Elements are abbreviated with an X, include a carbon-halogen bond, F,Cl,Br,I |
| Alcohol group | Carbon-hydroxide bond |
| Ether group | Carbon-oxygen-carbon bond |
| Amine group | Carbon-nitrogen group, primary, secondary, tertiary |
| Nitrile group | Carbon-nitrogen triple bond, cyanide anion or CN- with active organic species |
| Nitro group | Formal charges, nitrogen with four bonds and no lone pairs with +1 charge, oxygen with one bond and three lone pairs with -1 charge, free to resonate so that negative charge can be shared between two oxygen atoms with +1 charge on nitrogen |
| Sulfide/thioether group | Sulfur equivalent of an ether, carbon-sulfur-carbon bond |
| Thiol group | Sulfur equivalent of alcohol, carbon-sulfur-hydrogen bond |
| Carbonyl group | Carbon-oxygen double bond, contains subgroup of molecules |
| Aldehyde group | Carbon-carbonyl-hydrogen |
| Ketone group | Carbon-carbonyl-carbon |
| Carboxylic acid group | Carbon-carbonyl-hydroxide |
| Ester group | Carbon-carbonyl-oxygen-carbon |
| Amide group | Carbon-carbonyl-nitrogen |
| Acid chloride group | Carbon-carbonyl-chlorine |
| Acid anhydride group | Two carboxylic acids minus a water molecule |
| Imine group | Nitrogen equivalent of carbonyl, carbon-nitrogen-double bond |
| Epoxide group | Cyclic ether, carbon-oxygen-carbon |
| Phenol group | Arene ring with hydroxide attached, specifically benzene |
| Aniline group | Arene with amine attached |
| Hydrocarbons | Compounds composed of only carbon and hydrogen |
| Alkanes/saturated hydrocarbons | Hydrocarbons containing only single bonds, lack pi bonds |
| Straight-chain n-alkanes | Simplest structure of alkanes, homologs of H-(CH2)n-H |
| Straight-chain n-alkanes molecular formula | CnH2n+2 |
| Isomers | Compounds that have the same molecular formula but differ in physical and/or chemical properties |
| Constitutional isomers | Isomers that differ in connectivity |
| C1 prefix and condensed structure | Meth, CH4 |
| C2 prefix and condensed structure | Eth, CH3CH3 |
| C3 prefix and condensed structure | Prop, CH3CH2CH3 |
| C4 prefix and condensed structure | But, CH3CH2CH2CH3 |
| C5 prefix and condensed structure | Pent, CH3CH2CH2CH2CH3 |
| C6 prefix and condensed structure | Hex, CH3CH2CH2CH2CH2CH3 |
| C7 prefix and condensed structure | Hept, CH3(CH2)5CH3 |
| C8 prefix and condensed structure | Oct, CH3(CH2)6CH3 |
| C9 prefix and condensed structure | Non, CH3(CH2)7CH3 |
| C10 prefix and condensed structure | Dec, CH3(CH2)8CH3 |
| C11 prefix and condensed structure | Unde, CH3(CH2)9CH3 |
| C12 prefix and condensed structure | Dodec, CH3(CH2)10CH3 |
| Alkyl group | Alkane from which a single hydrogen has been removed, changes from standalone alkane to a substituent of a larger molecule |
| -R | Generic alkyl group |
| Iso group | CH connected to 2 methyl groups |
| Neo group | Central carbon surrounded by multiple methyl groups |
| Primary carbon | 1˚ bonded to one C |
| Secondary carbon | 2˚ bonded to two C |
| Tertiary carbon | 3˚ bonded to three C |
| Quaternary carbon | 4˚ bonded to four C |
| -ium | Denotes positive charge |
| -ide | Denotes negative charge |
| sp3 hybridized atoms | 4 electron dense areas, no double bonded C,O,Halogens |
| Nuclei | Positively charged, define atomic positions as cartesian coordinates |
| Electron cloud/orbital | Region of space that can be occuped by an electron, negatively charged, defines molecule size and shape, 1s orbital has low energy |
| Distribution of charge | Reveals molecule's chemical and physical properties |
| Electrostatic potential map | Represents molecular charge distribution, illustration of 3D electron density surface around ball and stick model or electron cloud, warm colors represent high electron density, cool colors represent low electron density |
| Types of molecular models | Wireframe, ball and stick, space filling |
| Electrostatic potential energy | Coulombic energy that a point positive charge feels as it passes over electron cloud |
| Coulombic energy | High electron dense atoms are electron rich and have low coulombic energy |
| Valency | Number of bonds an element forms, carbon is tetravalent, nitrogen is trivalent, oxygen is divalent, hydrogen and halogens are monovalent |
| Lewis structures | Count valence electrons on columns of periodic table, connect all bonds |
| Electronegativity | Ability of an atom to attract electrons, <0.5 is equal or covalent, 0.5-1.7 is unqual or polar covalent, >1.7 does not share and is ionic - the result of the force of attraction between two oppositely charged ions, atom with higher electronegativity is sigma- or electron rich, atom with lower electronegativity is sigma+ or electron poor, greater electronegative pair is more ionic |
| Induction | WIthdrawal of electrons toward oxygen, causes partial positive and partial negative charges |
| Single bonds | sp3 hybridized, one sigma bond, longest, weakest, steric number 4 |
| Double bonds | sp2 hybridized, one sigma bond, one pi bond, shorter, weaker, steric number 3 |
| Triple bonds | sp hybridized, one sigma bond, two pi bonds (overlapping p orbitals), shortest, strongest, steric number 2 |
| Steric number | Total pi bonds plus lone pairs, number of electron pairs repelling each other whether bonding or nonbonding |
| Intermolecular forces | Attractive forces between individual molecules, electrostatic, can be dipole dipole interaction or hydrogen bonding or fleeting dipole diple interaction, higher boiling point is less branched |
| IUPAC nomeclature | Choose longest carbon chain with most substituents |
| Straight chain substituents | Receive generic alkyl group names |
| Complex substituents | Treat as a miniparent, put everything in parentheses, longest carbon chain numbered starting from parent chain unless you can make substituents smaller numbers, numbered substituent followed by mini parent, EX: (2-methylbutyl), alphabetical substituents should come first |
| Bicyclic | Two fused rings, label carbons from bridgehead along longest path to shortest, EX. 6-methylbicyclo[3.2.1]octane |
| Conformation | Variety of possible 3D shapes adopted from rotation about carbon-carbon single bonds |
| Dihedral/torsional angle | Angle of bonds in a conformation anywhere from 0˚-180˚ |
| Staggered conformation | Lowest energy |
| Eclipsed conformation | Highest energy |
| Anti conformation | Confirmation with lowest energy |
| Gauche interaction | Type of steric interaction, different from torsional strain, when two electron clouds are repelling each other/trying to occupy the same region of space, conformations with least gauche interactions are lowest in energy |
| Homolytic bond cleavage | Generates uncharged radicals, uses fish hook arrows, energy required to break a covalent bond is bond dissociation energy |
| Heterolytic bond cleavage | Generates charged ions, uses a two headed arrow |
| Isopropyl | (1-methylethyl) |
| sec-Butyl | (1-methylpropyl) |
| Isobutyl | (2-methylpropyl) |
| tert-Butyl | (1,1-dimethylethyl) |
| Isopentyl/isoamyl | (3-methylbutyl) |
| Neopentyl | (2,2-dimethylpropyl) |
| Ethane conformation | 12 kJ/mol diference, all staggered are degenerate, all eclipsed are degenerate, each eclipsing hydrogen pair is 4 kJ/mol |
| Torsional strain | Difference in energy between staggered and eclipsed conformations |
| Propane conformations | 14 kJ/mol diference, all staggered are degenerate, all eclipsed are degenerate, each eclipsing hydrogen pair is 4 kJ/mol, hydrogen-methyl group is 6 kJ/mol |
| Butane conformations | Not degenerate, eclipsed confomation at dihedral angle 0˚ is higher in energy, staggered conformation at dihedral angle 180˚ is lower in energy, eclipsing methyl groups cost 11 kJ/mol |
| Cyclohexane conformations | Both conformations possess very little angle strain (close to 109.5˚), chair conformation has no torsional strain, boat conformation has two torsional strains from flagpole interactions, boat conformation can alleviate torsional strain by forming a twist boat |
| Exothermic | Negative heat of reaction dH˚, decreased in energy/gave energy to surroundings, starting materials to products |
| Endothermic | Positive heat of reaction dH˚, increased in energy/gained energy from surroundings, products to starting materials |
| Kinetics | Dependent on rate of reaction |
| Thermodynamics | Dependent on equilibrium concentrations of reactants and products |
| Ionic/polar reactions | Involve ions as reactants,products,or most commonly intermediates, one reactant has a site of high electron density and other reactant has a site of low electron density |
| Nucleophile | Electron rich center, has ability to react with a positive or partial positive charge, capable of donating a pair of electrons |
| Electrophile | Electron deficient center, has ability to react with negative or partial negative charged, capable of accepting a pair of electrons |
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