CHEM 1100 Book Notes PDF

. 5 : The Atmosphere 3 as Natural Protection in Ozone layer : designated region Stratosphere w/ max. Ozone concentration ·...

. 5 : The Atmosphere 3 as Natural Protection in Ozone layer : designated region Stratosphere w/ max. Ozone concentration · Ozone has an odor - can smell it during a severe lightning storm Ozone forms both naturally AND as a result of human activity Due to high reactivity ozone does not persist for long periods · , How is Ozone formed ? · Energy + 302 - > 2 03 ↳ This equation helps explain why ozone is formed from oxygen in the presence of a high-energy electrical discharge Ozone is rare in the troposphere , region of the atmosphere closest to Earth's surface · Somewhere between 20-100 Ozone Molecules (20-100 ppb) Stratosphere : farther away from Earth's surface · mostly where Ozone filters some types of ou light from the Sun · about 90 % of Ozone is found here. 6 : How Does Ozone Decompose In UV Light ? · 3 · Ozone protects us from damaging solar radiation by interactions of matter and energy from the Sun electron Valence - Valence electrons : electrons in the outermost shells · involved in covalent bonding · D ! Lewis Structures: structures drawn for molecules bonds and lone pairs D involving Valence electrons Single bond Triple bond in each coresections 2 > 2e - > be- Group - Double bond 2 345678 > He - - 1 Octet Rule : every atom Shares 8 e -. 7 : How Safe Is Our Protective Ozone 3 Layer ? Covalent Bond : Electrons in a covalent bond are common property to both atoms that make up the bond - - covalent bond involves the Sharing of e between 2 Atoms - Involves the attraction between the nucleus of each atom and the e-of the Other Longest Bond SingleCovalent Double Covalent ↓ TripleCovalent Shortest Bond Steady State: Stratospheric Ozone is formed and decomposed by a natural cycle Ozon Destruction : Series of reactions involving water vapor and its breakdown products Free Radicals : highly interactive Chemical Species with one or more unpaired e highly reactive H20 and N , O cause ozone to break down naturally in the Stratosphere Concentration of Stratospheric Ozone at the equator is lower at the poles Factors that cause an ↑in Ozone Production : · UV radiation intensity increased · Sun directly overhead · Earth near the Sun No and OH : Radicals responsible for Ozone depletion Chapter 4 1 :. Carbon Everywhere Carbon Cycle : Carbon containing substances cycle through nature Carbon reservoirs ↳ in atmosphere Rocks that Earth's crust is the largest reservior · make up · Uptake of CO , from the atmosphere occurs at the surface of the olean through Photosynthesis · deposition from rainwater · dissolving the gas directly into the ocean sur face Plants and Animals : another reservoir where Catoms Combine with O It a n d , , · Carbon reservoirs : - usually Contain carbon in the form of one of its compounds · exchange forms of (with each other Greenhouse Effect : · natural process · atmospheric gases on Earth trap 80 % of the IR produced by the Earth warming the Planet · the greenhouse effect causes the average temperature than Predicted on Earth to be higher considering its distance from the Sun Anthropogenic Influence : human sources such as industry , transportation , mining , and agriculture · IR radiation can excite both bending and stretching vibrations The wavelengths of IR radiation absorbed depends on the structure of the molecules · IR radiation causes the bonds in a molecule to vibrate in various ways Exam #2 Study Notes earth comfortable and survivable · The greenhouse effect-> keep's the surface large portion Light from sun reaches , in Earth's atmosphere category of passes get collected More GG there are , more heat will be trapped good no evil maintaing - no CO2 · too much will damage Include. Ot F-gases (CFC) atoms are held together loosely enough to when they vibrate , they will absorb heat vibrations let off radiation which gets , absorbed by GG keeps heat trapped near the Earth's surface  Final Study Guide Unit 1 Matter All ↓ "Kinds of light" Pure Substance mixture - heterogenous 11 1 diff Composition. homogenous throughout element mixture compound : PureSubstance wh 2 or more elements x - mixture : Variable ratio , Substance w/ 2 or more elements V Allotrope : same element different substance ↓ visible light Isotopes : same element , different # of neutrons Ion : same element , different e · 118 elements Photons: tiny "packets" of light Conservation of atoms/mass : total mass at start-total mass at end Wave-particle duality : light can have properties of both depending on experiment the same ↳ # of atoms must stay Equations Automobiles and trucks.... V = C= unE = hux = 2. emit VOCs and NO X creates smog nanometer : 109m = Inm if you react wh OH-> makes NO , a brownish gas · add sunlight - > forms Os Types of UV Light · all of this then reacts With VOCs > produce more smog UV-A - UV-B IIV-C heat colorless gas Smog : 02 + N - No + 0 320-400 nm 100-290 n m 290 - 320 nm VOCs (Where brown Stuff from) comes creates NO , (brown gas) highestv and E lowest in Mixture Compound Element ↑ The Ozone 800 · 6 Ozone layer : blocks all UV-C and most UU-B from hitting Earth's surface Ozone maps : Oz occurs mostly in urban areas , levels PEAK in late afternoon · air is a mixture i lots of Voc production Ozone alerts occur mostly in the summer compounds are to elements as words are to letters Exhaust produces : NOz So NO +O ~OtE On VOCs smog · Parts per million (PPM) : 10-m Parts Per billion (PPB) : 10-am Tropospheric Ozone : breathed by humans · , secondary pollutant primary would be VOCs/NOL , health Particulate Matter : PM 2.. is much more dangerous than 5 PM , because hazard it is 4x smaller the more jagged more dangerous) , Stratospheric Ozone : UV radiation field, necessary for life Sources : natural volcanic eruptions I wildfires ↳ good up high (Stratospheric Os) , bad nearby Itropospheric Os) Enthropogenic: Powerplants vehicles , wood smoke Only UV has enough v) (Shorter & , higher E , higher · , energy to break Chemical bonds damages biological tissue (mainly UV-B be it penetrates Catalytic Converter deepest) - Co + 12 0 > - CO, and 2NO - > N2 + O Ozone Formation Ozone Destruction wavelength (1) : distance between two crests O not 0 + 0 Oz Unaton 02 + & frequency (2) : # Of crests moving per second 0 + a - 03 X + 03 - 20 As U ,# and u 22 - 03 + 0 203t0 - 20  Unit 2 Ozone hole : severe thinning - less On less protection Chlorflourocarbons (CFCs) : used as propelant in a resols + cht , C , Cl , F · in Stratosphere , CFCs react with UV Photon producing a free radical C which is highly reactive with one or more unpaired electron and is used in the destruction of Ozone · x + 03 - 0 + 0 · (0 + 0 - - - x + 0 [UstO -20 Montreal Protocol : ban of Ozone - depleating substances to heal ozone layers Lewis Structure : each shells #of valence e = the # of elements in row · Remember how to draw , and steps Wavelengths of photon required to break double bond are shorter with higher energy ↳ O , easier than Os CO2 has warming effect on Earth due to greenhouse effect (f Other GHGs which are necessary for life) · 50 % Of UV emitted absorbed into Earth · 23 % into atmosphere where O-O bonds break 37 % absorbed into atmosphere by GHGS · 9 + 6 % emitted · as IR GHGs : CHylmethane) CO2 H O N20 , ,. , ↓ best at trapping heat a summetric f bending Stretching Of - GHGs (molecular geometry) allow for 12 to vibrate them Greenhouse effect: Solar radiation to f remitted as UU Earth which interacts with CO2 molecule in atmosphere to excite it so that it reemits IR radiation back to Earth · more GHGs--higher surface temp (they trap heat through molecular vibrations) CO stays in the atmosphere for double bonds (harder to break) long time because of the 2 amt of reflected light Albedo Effect : amt of incoming light artic mechanism : melting icef snow - Ocean less reflective to warming effect indirect f are sols : can block some direct radiation , absolute cooling effect on Planet (promote cloud formation) Ice cores : drill out ice cylinder , deeper you go = farther back in time + can measure CO2 from air bubbles calculations · molecular weights for each atom... add up all atomic masses · g to atoms (0) (6 0xatoms) = -at i s 9...  massecure (( · - -g = · stoichiometry (how manu g of B in A) Ag. (m). (m = gB · unreactive elements don't need to get another e- to complete octet rule , so generally unreactive melanin : protects against UU Inatural defensive mechanism) The Steady State of Ozone · O3 destroyed as quickly as its produced so the amount stays relatively the same Carbon Cucle · moving from resivoir to resivoir through processes such as Photosynthesis combustion sedimentation , , MolecularShapes Natural Aresul Sources : dust storms , Ocean spray forest fires , negative radioactive Factorsthat impact Earth's forcings : have cooling effects (aresuls) positive forcings : have a Warming effect (GHGs) 7 incoming and ongoing radiation Consequences ofC limate Change · ocean acidification ↳ oceans have absorbed -30% Of CO2 emissions · not and cold extremes extreme cold less likely · sea levels rise  Unit 3 determines Functional Groups · polarity makes molecules more polar Climate Change : CO2 Os H20 CHy N · , , , ,. 0 group wh OtN 4 polarity · · IR · R group (Carbon Substitute) ↑ CO ! temperature S =HS0St -NHL CENH · fossil fuel combustion 05 Of + 1st s 1 R Ozone depletion : Os CFCs , O , St CNHz CONItz · UU radiation alconol carboxylic ester amine amide · Oz acid C F C s Cl · molecules with similar structures Shapes , f Polarities , will have similar functions Polar covalent bonds : non-equally shared Pair of e-in · all functional groups add Polarity which they are closer to more electronegative atoms Enzymes : protiens that contain active sight to accelerate/control reactions What is electronegativity ? ↳ active sight binds only to specific reactions) ability to attract electrons to itself Biocatalyst : Speed UP reaction Ex : N, O, E Induced fit : active sight folds around substrate to bind - less more provides eleneg elecneg surface for absorption - causes partial neg (5) + partial positive (St) Aracondic Acid -o aspirin Hydrogen Bonding COX-1 : good Prostagladin · between molecules /intermolecular) COX-2 : Bad Prostagladin (VIOXX) COX-2 · covalent (intramolecular) super-aspirin : only blocks because it doesn't fit in 1 Remember... Isomer : same chemical formula but different chemical structure · Polar dissolves Polar · nonpolar dissolves Polar Propanal (C3Ht - 0) Propanone (C3Hy0) Ex : i It · Polar is water soluble It 0 H I I O nonpolar is not water soluble H CC - C H --- - H H20 properties it if it it it · highest boiling point Polarity Chirality affects how enzyme binds f its solubility · f · highest melting point · high heat of vaporization amino acid : amine f acid functional groups ↳ compounds of similar type Optical isomers : 1 chiral molecule bonded to 4 unique groups as molar mass 4 so does boilingPoint 1 Chiral molecure : not superimposable :! , Ex Bondss... H = 1 bund e ? "- 4 4 % if going around ring is different both ways · have same melting/boiling pointsf solubility bunds 3 3 0 = 2 N = 3 bonds Opiates : Morphine (what makes it so addicting is how it reacts w/ enzymes) Coedine , herion , C = 4 bonds THC : fat soluble t nonpolar because only one polar (-0H) group Synthesizing esters : Chain formed from hydroxyl a acid creating Polyesters - fentynall Stronger than morphine because it can find things to bind to enzyme that morphine can't + it has a much more potent effect because of this  Steroids Difference is the double 4 rings (3 hexagons + / pentagon) · bond on the has decorations around · fat soluble nexago Cholesterol · component of cellular membrane · acts as structural reinforcement polarity important is designing drug molecule · can be fat or water soluble + effects was it binds Unit 4 Triglycerides : how we store fat · I glyceride stitched Wh 3 fatty acids Polyunsaturated Fat : Saturated fatty acid ! Unsaturated Fatty Acid' has onlyI c = c double bond 2 or more C= c double bonds · 2 Hudrogens per C double bond produces bend · multiple bends nonpolar chain consists of · · only C-C single bonds Drawing : Drawing : i · How to draw... & Y a Physical Property Changes : - increasing number of C-cbonds melting pointf molecular weight Partial : Some double bonds are converted C=C double bonds melting point Ican't be packed as fight to a single bonds by addingIt - increasing number of > trans fat) (poly unsat. - Partial Hydrogenation : adds I at high heat wh catalyst , I melting Point Istops separation) 1. ) converts Some C = C bonds to C-C Complete Hydrogenation : all double bonds are.) converts the 2 rest to Cis-trans formation converted to single bonds (polyunsat > - saturated fat) Cis-trans isomers' Straightens chain out so that It's are diagnol - cis - trans (straight) second rate of glucose - glycogen for Short-term Storage I much more branched) Isomers of polyglucose : glycogen - - starch - cellulose Starch : Polar - Ol groups in Spiral Shape make very water soluble - X-links - body can metabolise  DNA · codon : 3 consecutive bases in DNA Sequence : DNA-> RNA- > Protein Fats are more "fattening" than carbs blc they provide more energy when metabolized Photosynthesis COSTS energy Metabolism PLEASES energy 3D Structure of DNA : · double helix · sugar attatched to a phosphate and nucleotide base Backbone of DNA : Phosphate and a Sugar Ideoxyribose) Backbone of protein : amino acids It bonding in DNA... The nucleotide bases create H bonds with other bases It bunding in proteins... The O in the carboxylic acid hydrogen bonds to the I in the amine (amino DNA · exists double strand #NA · has A ,T G C bases, , · single-stranded · contains A , C , G, U contains the sugar deoxyribose Contains the sugar ribose · · Base & I 23 G 27 %. Final Exam Study Guide Order of DNA