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SIUE Organic Chem
Kevins Lecture, Physics & chem applied anesthesia
| Question | Answer |
|---|---|
| protons | carry positive charge, located in the nucleus |
| What distinguishes the characteristics of an atom | the # of protons |
| Neutrons | are neutral, also located in the nucleus |
| Atomic Number | number of protons |
| Atomic Weight | # protons + # neutrons |
| Electrons | carry negative charge, located outside the nucleus |
| Electron Orbit | 2 in first orbit, 8 in each additional orbit |
| Atoms attempt to have ____ electrons in their orbit | 8 |
| Objects with like charges | repel eachother |
| ojects with opposite charges | attract |
| isotopes | Atoms have same number of protons and electrons, but have different number of NEUTRONS. Same characteristics, different atomic weight |
| The outtermost and most reactive electrons of an atom | Valence shell |
| Valence shell is a measure of | the # of chemical bonds formed by atoms of a given element |
| group number of letter A on periodic table = | # of valence electrons |
| O2 is group 6 on periodic table so it wants to form | 8-6 = 2, 2 bonds |
| Hydrogen is group A1 on periodic table so it wants to form | 1 bond, wants to rid that one electron to have 0 |
| Carbon is group A4 on periodic table so it wants to form | 4 bonds. 8-4 = 4. |
| Quantom Mechanical Model is used to | find the probable location of an electron in an atom |
| Quantom number "n" is | size; describes average distance of the orbital from the nucleus & the energy of the electron in an atom. Can be any positive whole number. |
| A larger number for "n" in quantom model means | more energy and larger orbital |
| Quantom number "l" describes | The shape of the orbital; positive whole number froom 0 to n-1. |
| Simple names of "l" quantom number | s orbital = 0, p orbital =1, d orbital = 2, f orbital =3 |
| Quantom number "m" describes | how orbitals are oriented in space, 3D. |
| Quantom number "s" describes | The direction that the electron is spinning. Only two values are used +1/2 & -1/2. |
| Hybrid orbitals | new set of obritbals could be created by mixing s, p, and or d atomic orbitals on an atom |
| When bonds are formed | reactions occur, and molecules are held together |
| in a chemical reaction | atoms are neither created or destroyed |
| exothermic reactions | release heat |
| endothermic reactions | absorb heat |
| Ionic bonds | complete transfer of an electron, requiring lots of energy, forming a cation and anion, atoms with significantly different electromagnitivity |
| cation | + form |
| anion | - form |
| Ionic bonds are used to form | simple salts NaCL |
| Covalent bonds | share electrons, requiring less energy than ionic bonds, occurs by overlap of individual atomic orbitals Ex: HCL, most covalent bonds demonstrated polarization |
| In covalent bonds electrons in each atom | tend to become attracted to the positive nucleus of the other atom |
| Symmetrical Covalent bond | "pure covalent bond", having a net neutral charge |
| Hydrogen bonds | bond between two 1 s atomic orbitials. Electrons are attracted to the positive nuclues in other atom. Continue to come together until the nuclei become to repel eachother. |
| Sigma bond | formed by head on overlap of atomic orbitals, bonding densitiy is concentrated in the middel making it the strongest type of covalent bond |
| Strongest type of covalent bond | Sigma |
| Pi bonds | sideways or parrallel overlap, usuall from P orbials |
| Single bonds always are | sigma bonds |
| double bonds have | 1 sigma, and one pi bond |
| triple bonds have | 1 sigma and 2 pi bonds |
| Organic chem is the | study of carbons or other carbon molecules |
| Carbon is unique because | it can form bonds with other carbons, as well as stable covalent bonds with other nonmetal compounds, there are more carbon compounds than any other compounds combined, tetravalent, 4 electrons in outer shell, 4 bonds |
| Strongest bonds in nature are | CARBON bonds |
| Organic Molecule characteristics | Insoluble, like oil. Have low melting and boiling points due to the weak intermolecular forces |
| Because the bonding of carbons is so versatile, they exhibit | isomerism |
| Isomers | different compounds with same molecular formula, via by which atom is bonded to which, or how atoms are arranged in 3-dimensional space |
| Isomers | organic compounds have similar chemical form, but different structures, same atomic weight, different physical characteristics |
| Isomers occur in organic compounds that have | more than 3 carbon atoms |
| constitutional isomers | compounds with same molecular formula, but atoms connected in different arragement. different structure, different physical properties, and different physiological properties |
| 2 kinds of stereoisomers | Diastereomers & enantiomers |
| Stereoisomers | atttached in same sequence, but have different 3-D orientation |
| Diastereomers | NOT mirror images, and include Cis & Trans, and conformational isomers |
| Cis Isomers | functional group is on the same side of the = carbon bond. (kind of diastereomers) |
| Trans | functional group is on the opposite side of the = carbon bond (kind of diastereomers) |
| Conformational Isomer | spin around the carbon-carbon single bond giving rise to an infinite # of 3-D geometries, called rotamers. Not really isomers |
| Enantiomers | kind of steroisomer, is a MIRROR image, optical isomer, cannot be super imposed, rotate in opposite directions, having same physical properties & solubility with different physiological properties |
| Enantiomers rotate in | equal amounts, but in different directions |
| Dextro isomer | r= rectus, or R spin |
| Levo isomer | sinister or L spin |
| Only the ___ form of LSD Is psychoactive | R- or D- form |
| Thalidomide ___ form acts as seditive | S-form or L spin |
| Structure of Organic Molecules 2 parts: | 1.) carbon backbone 2.) one or more functional groups |
| Functional groups | set of atoms within a larger molecule that have a characcteristic structure & chem behavior. Largely defines the chem and physical properties. |
| Hydrocarbon functional groups | containt only H & C atoms, and are very flammable (include alkane, alkene, alkyne, arenes) |
| Alkanes | carbon - carbon single bond. simplest organic molecule. No functional groups. Methane is simplest. Relatively unreactive, and saturated. |
| Alkene | carbon-carbon double bond. Has functional group. Simplest is ethene. unsaturated |
| alkyne | carbon-carbon triple bond. Has functional group. simplest is ethyne. unsaturated |
| Alkyl group | substituent that branches off the main chain, CH3 |
| Quaternary carbon | four alkyl groups, doesn't pass blood-brain barrier well. |
| Aromatics | circular, 6 member carbon ring with 3 double carbon-carbon bonds, also called arenes, functional group is benzene ring, very stable |
| organohalogen compounds | are less flammable, contain one or more halogen atoms fourn in 7A (F, Cl Br, I) |
| Alcohols | R-O-H. OH (hydroxyl group) methanol is simplest |
| Aromatic alcohols are called | phenols |
| Ethers | R-O-R. Funtional group is O2 bridge between 2 alkyl group. |
| Most anesthetic gases are | halogenated ethers (Enflurane, Isoflurane, Sevofluroane) |
| amines | funct group derived from ammonia (NH3) Large number of meds are amines (Ketamine, Dopamine, Epinephrine. MOst have strong base strength and will accept a proton to form its conjugate acid. Called ammonium salts with are much more soluble in water |
| By controlling pH of the medium (amines base to acid) | you can control the solubility of many medications |
| Carbonyl functional groups | See note cards |
| cycolalkanes | NOT aromatic rings. (alkane = single c-c bond only) |
| Rules of Nomenclature | 1.) Define longest carbon chain 2.) Identify/name groups attached to chain 3.) Number chain consect, start end nearest substituent group 4.) designate location of sub group by # & name 5.) Assemle name of groups in alphabetical order |
| Iso prefix | stands for a branched chain akyl group |
| Almost all anesthetic agents are | Organic compounds |
| Nitrous is | inoragnic |
| Halothane is | halogenated hydrocarbon, (an ethane with F, Cl, or Br) |
| Inhalation gases other than halothane are | halogentated ethers |
| Local anesthetics are made from | amides and esters |
| Halogenation of hydrocarbons creates | H atom replaced by a halogen atom (I, Br, Cl, F) to create a highly potent nonflammable gas |
| Enflurane and Isoflurane are | Isomers, same chemical structure & weight, different physical characteristics |
| Ethers | R-O-R most inhalation gases |
| Iso, Des and Sevo are | Methyl ethyl ethers |
| Esters | Local anesthetics, functional group is -COOR, R is akyl group. |
| Natural Epinephrine | exists in L-isomer or L spin having greater beta 1 (cardiac) than beta 2 (pulmonary) activity |
| Racemic Epi | nebulizer has 50/50 of R and L spin. Get more pulm effects with less tachycardia. |
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