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organic chem exam 1
| Question | Answer |
|---|---|
| Berzelius | the inventor! the guy who defined organic chemistry Vitalism 1806-1810…? |
| vitalism | compounds derived from living organisms can not be synthetically made |
| Wöhler | 1828 disproved vitalism did this ^ via the urea experiment - he was able to make urea from simple inorganic materials - urea is a compound in living organisms that we make |
| Kékelé | 1850s all about the STRUCTURE of organic compounds told us that carbon must have 4 bonds for example |
| Perkin | gave the commercial edge to organic chem showed people chemistry can be used for commercial/market development made the mauve dye and people started buying it |
| Kathleen Lonsdale | discovered/created x ray crystallography |
| x ray crystallography | allows us to see the true structures (of organic compounds?) |
| taxol | used in fighting Ovarian and breast cancer x ray crystallography allowed us to see its structure |
| defined energies | we can say electrons of an atom are bound to defined regions in space, as determined by their wave like properties |
| atomic number | number of protons establishes chemical identity aka identity of the ATOM |
| atomic mass | the sum of the protons and neutrons present |
| isotopes | systems where they have the same number of protons (same chemical identity) but different number of neutrons (different atomic masses) |
| mass spectrometer | how we determine atomic mass of an element - take a molecule and make a solution of it - inject it in the device, it becomes ionized - ionized molecule goes through a magnetic field - the way it behaves is based on its molecular weight |
| how can mass spectrometry used? | forensic - if we don’t know what something is, we can test it and find molecular weight & compare that to known compound molecular weights - ex: aspirin vs fentanyl (look the same, diff molecular weights) food analysis - to make sure pesticides gone |
| valence electrons | outermost electrons responsible for the chemical reactivity of an atom these are the ones that bonds can be broken, made, can be played around with |
| inner core electrons | non valence electrons don’t participate in chemical rxns |
| quantum model of the atom | electrons have particle wave duality electrons occupy regions of space known as orbitals (we cant figure out where they are but we can find out the probability of where they’ll be via___?) heisenberg uncertainty principle schrödinger developed it |
| wavefunction | gives the probability of finding an electron in a certain position 3D MATHEMATICAL description of these systems |
| Hami Honian Operator | H tells us what an orbital looks like how big is the orbital and what shape? takes into account KE and PE associated with an electron |
| pi bond | happens above and below the plane |
| sigma bond | happens…on the plane? the basic one |
| what are the two theories about bonding | valence bond theory molecular orbital theory |
| electronegativity | ability of atom to attract electrons toward itself in a chemical bond |
| methyl groups | CH3 terminal |
| methylene groups | CH2 2 branches /\ |
| methine groups | CH 3 branches |
| quaternary carbon | C X full! |
| polar protocol molecule | has a permanant dipole moment and contains an H atom (proton with a highly distorted chemical bond) attatched to a strongly electronegative atom (O, N, F) |
| formal charge | calculated volume of electron density around an atom, based on its valence electrons |
| electrophile | electron deficient/poor LOVES electrons cause it doesnt have them,,,cant get enough + charge |
| nucleophile | electron rich - charge |
| artificial charge | when formal charge leads you to believe it is electron deficient, but its octet is full because of the way it is bonding a way formal charges can be misleading |
| if something is a nucleophile, | it must have a lone pair |
| to be an electrophile/nucleophile, | you must be able to accept and give electrons electrophiles must have room to accept nucleophiles must have lone pair electrons to give off |
| the more resonance structures a substance has | the more stable is is |
| are individual resonance forms real | nope not blinking between cranberry and orange |
| carbocations | the more stuff around it the more stable it is (the more substituted it is) they’re electron deficient, so always drawing electrons from neighbors the more neighbors, the less need to react with outside stuff any compound with a positively charged C |
| Brønsted Lowry Acid | something that has an extra H+ (an extra proton) to give off HCl, HI, HBr, HNO3 just need an H present the H is usually polarized so its easy to take off (delta +) |
| Brønsted Lowry Base | something capable of removing a H+ usually must have an active lone pair; capable of reaching out and creating new bond OH-, H2O, NH3 |
| with brønsted lowry acids and bases how do you determine | have to draw their lewis structures usually to see if theres a lone pair, or an H (can see H from formula usually) |
| how to tell strength of acid | Kia value that gives us a whole picture lewis structures can be misleading/doesnt give the full picture doesnt tell us strength |
| negative pKa | strong acid |
| positive pKa | weak acid |
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