Chem 102 Exam 1 study guide PDF

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Chapter 9.1-9.3 1. Define what it means to be an “organic” compound. a. Chemistry of compounds containing Carbon b. 95% of all compounds c. Naturally derived from a natural source 2. Describe and draw the bonding patterns of carbon. How many bonds can Carbon form? What does it frequently bond with? a. Can form rings, chains and branches b. Forms 4 bonds (tetrahedral 109.5-degree angle) c. Frequently bonds with: H, O, N, S 3. What are hydrocarbons? a. Compounds that contain only H and C 4. What’re the prefixes for the number of Cs 1-10? a. b. c. d. e.

Meth Eth Prop But Pent

f. g. h. i. j.

Hex Hept Oct Non Dec

5. What are alkanes? Basic formula for molecular formula? Know their properties. a. Alkanes are single bonded hydrocarbons b. Cn H2n c. Suffix: -ane d. Simplest = CH4 = methane e. Properties i. 1-4 Cs = gas ii. 5-16 Cs = liquid iii. 18+ Cs = solid iv. Insoluble in water v. Burn; produce heat and energy vi. Odorless 6. Define and classify alkenes and alkynes. What are alkenes? What are alkynes? Basic formula? Properties. a. Alkenes i. Double bonded hydrocarbons ii. Cn H2n iii. Suffix = -ene iv. Simplest = C2H4 = ethene/ethylene b. Alkynes i. Triple bonded hydrocarbons ii. Cn H2n-2 iii. Suffix = -yne iv. Simplest = C2H2 = ethyne/acetylene c. Properties of both i. Unsaturated fats ii. Burn easily iii. More reactive than alkanes iv. Similar phase properties to alkanes

7. What are cyclic molecules? a. Usually single bonded b. Carbons in cyclic molecules form a ring c. Simplest = C3H6 = cyclopropane d. Naming = cyclo + prop, but, pent, hex …. 8. Given a structural formula, write the molecular formula of a hydrocarbon. Identify, define, and draw isomers (structural and geometric). a. Structural Isomers = same molecular formula, diff structural formula b. Geometric isomers = same molecular formula, diff arrangement around double bond i. Cis = methyl groups are on the same side of the double bond ii. Trans = methyl groups are on diff sides of the double bond c. More Cs = more isomers d. Alkanes i. 1-3 Cs have only 1 isomer ii. Butane has 2 iii. Pentane has 3 iv. Hexane has 5 v. Heptane has 9 9. Interpret and draw chemical skeletal structures. a. Skelton structure = a way to fraw molecules w/o the carbons and hydrogens b. Each point/corner = a carbon c. Lines connecting = degree of bonding d. Hydrogens are implied 10. Identify and describe aromatic and halogenated hydrocarbons. a. Aromatic hydrocarbons i. Equally share electrons ii. EX: benzene ring iii. Have an aroma b. Halogenated hydrocarbons i. Halogens (F, Cl, Br, I, At) are frequently substituted w/H to give diff properties ii. Chlorinated 1. CH3Cl (methyl chloride) = starting material in RX, industrial chem 2. CH2Cl2 (dichloromethane) = solvent, paint remover 3. CHCl3 (trichloromethane) = chloroform, anesthetic 4. CCl4 (tetrachloromethane) = dry cleaning 5. CH2=CHCl = vinyl chloride, PVC iii. Chlorofluorocarbons (CFCs) 1. CFCl3, CF2Cl2, CF2ClCF2Cl = used in propellants/aerosols that can deplete ozone Chapter 9.4-9.8 1. Define functional group. a. A group of atoms attached to a hydrocarbon that gives the compound special properties b. EX: double/triple bonds, halogenated hydrocarbons are also functional groups 2. Name and identify common alkyl- groups. a. Alkyl = an alkane w/1 H removed b. Suffix = -yl c. Naming = meth, eth, prop, but…etc + -yl

3. Classify molecules as ethers, alcohols, or phenols. a. Alcohols i. Have a hydroxyl group (-OH) ii. Suffix = -ol iii. The number before name shows where the -OH is connected iv. Ethanol 1. Made for beverages and fuel by fermentation of grain/starchy materials 2. Can be made through RX of ethylene w/H2O for industrial use v. Toxicity 1. Methanol metabolizes into formaldehyde (very toxic) 2. Ethanol is less toxic but still consumed; doesn’t make as bad byproducts when metabolized 3. Isopropyl (rubbing alcohol) is highly toxic vi. Multifunctional alcohols 1. Ethylene glycol = antifreeze/coolant 2. Propylene glycol = antifreeze 3. Glycerol = lotions, food additives, reactable to make dynamite b. Phenols i. Hydroxyl group is attached to an aromatic ring (such as benzene) c. Ethers i. 2 alkyl groups bonded to same Oxygen ii. ROR or ROR’ iii. Diethyl ether (C4H10O) = anesthetic, causes nausea/vomiting iv. Ethers slowly react with oxygen to make peroxides that can explode v. Ethylene oxide used to make ethylene glycol (antifreeze) 4. Define and differentiate between aldehydes and ketones. Draw simple aldehydes and ketones given their names. a. Aldehydes i. Aldehydes are attached to =O and -H ii. R-CHO iii. Suffix = -al iv. Common aldehydes 1. Formaldehyde (methanal) = natural byproduct of metabolism 2. Acetaldehyde (ethanal) b. Ketones i. Ketones are attached to =O ii. R-CO-R iii. Suffix = -one iv. Common ketones 1. Simples = C3H6O = propanone/acetone 5. Name and draw carboxylic acids. What are esters? a. Carboxylic acids i. Suffix = – e from alkane + oic acid ii. COOH can only go on the ends iii. Simplest = methanoic acid (CH2O2) used in insect stings 1. Ethanoic acid (CH3COOH)

b. Esters i. ii. iii. iv.

Smell sweet Formed from carboxylic acid (loses -OH) and alcohol (loses H)  H2O + ester RCOOR’ Naming 1. Start from alcohol side (right side), count # of C and add -yl 2. Then (left side) Count # of C (including the C=O) and add -ate 6. Recognize and classify amines and amides. a. Amine i. Contain nitrogen, carbon and hydrogen ii. Amines are derived from ammonia (NH3) by replacing H with alkyl groups iii. N can make 3 bonds iv. RNH2 v. RNR’H vi. RNR’R’’ vii. Simplest = CH3NH2 = methylamine viii. (C2H7N) has 2 structural isomers: Ethylamine and dimethylamine b. Amide i. Contain nitrogen directly bonded to a carbonyl group ii. Basic amide group can be written like 1. RCONH2 2. RCONHR’ 3. RCONR’R’’ 7. Be able to draw a carbonyl and carboxyl group and which functional group contain them. a. Carbonyl (C=O) i. Ketones, aldehydes, carboxylic acids, esters, amides b. Carboxyl (COOH) i. Only carboxylic acids c. Hydroxyl (-OH) i. Alcohols, phenols, carbox acids Chapter 10.1-10.5 1. Define polymer and monomer. a. Monomer = monomers are the building blocks for polymers b. Polymer = large molecule made of repeating monomers c. Polymerization = the process of making a polymer 2. Explain that polymers can be naturally occurring or synthetic. a. Natural polymers are derived from glucose i. Glucose (C6H12O6) polymers 1. H2O lost when making polymers of glucose 2. []n where n = # of smallest repeating unit ii. Starch = iii. Glycogen = more branching (liver, muscles) broken down into monomers later for energy iv. Cellulose = plants/trees help make cellular structure like the cell wall 1. Uses H-bonds v. Proteins = made from amino acid monomers 1. Carboxyl acid and amine ends form H2O and result in a dipeptide

3. 4.

5.

6.

7.

b. Synthetic polymers i. Made in labs ii. Have a wide variety of uses iii. Polyethylene (PE) = most common and usually starting base of synthetic polymers 1. Long chain of ethylene/ethene (C2H4) 2. Branching and H of polymers will have diff properties a. High density = closely packed and form crystalline structure i. Rigid, used for bottle caps, toys, milk cartons b. Linear low-density PE = bubble wrap c. Low density w/branching = plastic bags/containers d. Lower density = ice/frozen bags Write the condensed structural formula for polyethylene. a. [C2H4]n Define thermoplastic and thermosetting polymers. a. Thermoplastic = can be reshaped when heated and/or pressured b. Thermosetting = can’t be softened or reshaped (can’t be recycled) Explain what happens during an addition polymerization vs. a condensation polymerization. a. Addition polymerization = all atoms are incorporated into the polymer i. Monomers usually have double bonds b. Condensation polymerization = some atoms are lost i. H2O is a common byproduct Describe the monomer and polymer of common addition polymerizations (polypropylene, polystyrene, PVC, and Teflon). a. Polypropylene i. CH2CH2(CH3)CH2CH2(CH3) ii. A methyl group branches off every other C iii. Uses: food packaging, luggage, appliances 1. Tough plastic resists moisture, oils and solvents b. Polystyrene i. CH2C(benzene ring)H ii. Benzene ring replace a H in polyethylene iii. Uses: Toys and household products c. PVC i. Start with ethylene and replace 1 H with Cl ii. CH2C(Cl)H--CH2C(Cl)H iii. Forms tough thermoplastic iv. Monomer (vinyl chloride) is a carcinogen d. Teflon i. Made from tetrafluoroethylene ii. Chemical and heat resistant, and nonflammable when polymerized iii. CF2-CF2-CF2 Identify the monomer used to make rubber and explain the process of vulcanization. a. Natural rubber is made from isoprene CH2=C(CH3)-CH=CH2 b. Polyisoprene [CH2-C(CH3)=CH-CH2]n c. Isoprene for synthetic rubber come from petroleum refineries d. Vulcanization = allows for cross link formation and stronger material by adding sulfur

Chapter 15 1. Understand the units to describe power and energy. a. Energy = the ability to do work or transfer heat i. Measured in Joules (J) ii. 1 J = .2388 cal iii. Forms 1. Potential = stored energy or energy of position 2. Kinetic = energy in motion b. Power is measured in watts (W) i. 1W= 1J/s 2. What factors increase the rate of reaction? a. Temperature i. More motion increases the likelihood of atoms colliding b. Concentration of reactants i. If you have more product in a space, more of that will form c. Presence of catalysts i. Lowers the activation energy and isn’t consumed in the reaction 3. Classify reactions/processes as endothermic or exothermic. a. Endothermic = absorbs heat/energy to surrounding; requires heat i. EX: melting ice b. Exothermic = releases heat/energy to surroundings; releases heat i. EX: metabolism 4. Discuss implications of first and second law of thermodynamics to energy production and use. a. 1st = energy can’t be destroyed nor created; but can be transformed b. 2nd = energy flows from hotter to cooler objects; universe tends to favor disorder i. Liquid has more order and gas has more disorder 5. List common fuels and how they are used, characteristics, advantages and disadvantages to fuels: coal, natural gas, petroleum, nuclear energy, and various renewable energy sources. a. Coal i. Characteristics 1. Made of C and other minerals 2. More C  more useful, more water (lower grade)  less useful ii. Uses 1. Makes coke = ash left over that’s used to make steel and iron 2. Coal tar can be used to extract chemicals iii. Pros/Cons 1. Hazardous and tedious to obtain/transport 2. Contributes to acid rain when burned b. Natural gas i. Characteristics 1. Mostly methane ii. Uses 1. Chemical production 2. Alternative fuel iii. Pros/cons 1. Clean burning 2. Easy to transport 3. Hydrofracking a. Cons: competition with agriculture, contamination of water; Non-renewable

c. Petroleum i. Characteristics 1. Complex mixture of hydrocarbons 2. Comes from crude oil, through distillation = heating crude oil to varying temperatures to collect molecules 3. Cracking = larger broken down into smaller fractions 4. Gasoline a. Lighter fraction than crude oil b. Straight run gasoline isn’t good for cars i. Knocking = ignites on its own w/o spark plug 5. Octane rating = Measures fuel’s ability to resist knocking a. Isooctane is very resistant (100) b. Heptane isn’t resistant (0) c. If a gasoline has a rating of 90 then IT PERFORMS THE SAME AS a mixture of 90% isooctane and 10% heptane 6. Ethanol, methanol, t-butyl alcohol are common gasoline boosters a. Ethanol is oxidized so less energy from it ii. Uses 1. Fuel iii. Pros/Cons 1. Easiest to transport (pipes) 2. Nonrenewable 3. Pollution when burned 4. Competition w/agriculture (ethanol comes from corn) d. Nuclear energy i. Characteristics 1. Based on nuclear fission = atoms are split into smaller atoms, releasing energy a. More e will be released from the splitting b. Energy is used to heat watermakes steamturns turbinemakes electricity 2. Uranium 235 splits the most easily, but is rare ii. Uses 1. Makes electricity iii. Pros/Cons 1. Has to mined 2. Finite resource (nonrenewable) e. Renewable sources i. Characteristics 1. Hydroelectric, wind, biomass (burning biological material), solar, geothermal ii. Uses 1. Generate electricity, heat, energy iii. Pros/Cons 1. Renewable 2. Take a lot of space or material to generate lots of electricity 3. Haven’t found a good way to store energy 4. Conditions aren’t always favorable

6. Convenient energy a. Based on its state of matter i. Solids = hardest to transport ii. Liquid/gasses = easily trapped or pipped iii. Electricity = most convenient w/wires b. Cleanliness is also a factor i. Burning coal produces pollution where electricity doesn’t c. Electricity can be made from burning fuel/energy i. Water heatedsteam made turns turbinemagnets around copper make an electrical current

Alkyl groups of propanone: isopropyl and propyl

Alcohols of propane: 1-propanol and 2-propanol

Structural isomers of butene: 1-butene and 2-butene

Geometric isomers of butene: cis-2-butene and trans-2-butene

Alkyl groups of butane: butyl and sec-butyl

Alkyl groups of isobutane: isobutyl, tertiary butyl

Tert butyl alcohol/tert. Butanol

1-butanol (1-butyl alcohol) and 2-butanol (sec-butyl alcohol/2-butyl alcohol)

Ethyl oxide

Isopropyl methyl ether

Butyl methyl ether

Propyl ethyl ether

Acetyladehyde (ethenal)

Propanal

Propanone

2-hexanone

2-pentanone, 3-pentanone

Methanoic acid, ethanoic acid, octanoic acid

Methyl ethanante, propyl propanate, ethyl butanate, methyl pentanate

Methylamine, ethylamine

Polyethene/ethene

4-methyl-1pentene

Polypropylene/propene

Methyl vinyl ketone

Vinyl fluoride

Poly vinyl acetate

Polystyrene

Tetrafluoroethylene

Polyisoprene/Isoprene...