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chem final
| Question | Answer |
|---|---|
| ketone endings | -one |
| alkene endings | -ene |
| aldehyde endings | -al |
| alkyne endings | -yne |
| carb. acid endings | -oic acid |
| alcohol endings | -ol |
| ether endings | -ether |
| thiol endings | -thiol |
| ester endings | -oate |
| amide endings | -amide |
| aromatic endings | -benzene or prefix phenyl |
| amine endings | -amine |
| how do you round addition or subtraction equations | fewest decimal places |
| how do round multiplication or division equations | fewest sig figs |
| how many sig figs do each of these numbers have 40.00 0.003 810 200. | 4 1 2 3 |
| 1l ?mL | 1l 1000mL |
| 1m ?cm | 1m 100cm |
| 1kg ?g | 1kg 1000g |
| 1g ?mg | 1g 1000mg |
| 1cm ?mm | 1cm 10mm |
| milli=10^? | 10^-3 |
| micro=10^? | 10^-6 |
| kilo=10^? | 10^3 |
| centi=10^? | 10^-2 |
| nano=10^? | 10^-9 |
| in what order is the density triangle set up | mass on top, density left bottom, volume right bottom |
| which way do periods and groups run along the periodic table | groups vertical down the table, periods horizontal across the table |
| what is an atomic number | the number of protons that appear in that element |
| what is a mass number | number of particles in the nucleus. sum of protons and neutrons |
| number of protons and electrons are ___ | the same |
| how do you find the number of neutrons | subtract the mass number and the atomic number |
| what is the definition of an isotope | same number of protons but different number of neutrons |
| what is in group 1A (1) of the periodic table | alkali metals |
| what is in group 2A(2) of the periodic table | the alkaline earth metals |
| what is in group 7A (17) of the periodic table | halogens |
| what is in group 8A (18) of the periodic table | noble gases |
| where are valence electrons found | the outermost energy level |
| how do you know the number of valence electrons | group number (skip transition metals) |
| how many numbers are allowed in each ring | 2,8,8,1 |
| how do you find atomic size | decreases going up the periods, decreases going across the groups (l to r) |
| how do you find ionization energy | increases across the groups (l to r) decreases going down the periods |
| how do you find electronegavity | increases across the groups (l to r) decreases going down the periods |
| what are the characteristics of an ionic bond | ions formed by metals and nonmetals bond between ions formed by transferring electrons high melting point solid at room temperature |
| what are the characteristics of a covalent bond | two nonmetals or a nonmetal-metalloid sharing electrons bond formed when non-metals share 1 or more pairs of electrons |
| ionic compounds formula concept and how do you correct... Ba^+2 Cl^- Ca^+2 N^-3 Al^+3 O^-2 | positive ion listed first total positive = total negative BaCl^2 Ca^3N^2 Al^+3 O^3 |
| write the formula for sodium chloride and calcium iodide | NaCl, CaI2 |
| write the formula for ammonium chloride, and sodium bicarbonate | (NH4)Cl, NaHCO3 |
| write the formula for ammonium | NH4^+ |
| write the formula for acetate | C2H3O2^- |
| write the formula for bicarbonate | HCO3^- |
| write the formula for hydroxide | OH^- |
| write the formula for nitrate | NO3^- |
| write the formula for phosephate | PO4^3- |
| write the formula for sulfate | SO4^2- |
| what is the electronegavity spectrum | 0.0-0.4-nonpolar covalent 0.5-1.8-polar covalent 1.9-3.3-ionic |
| name the following CaO and Al2S3 | calcium oxide, dialuminum trisulfide |
| what is a cation and an anion | cation-pos. charge because of the loss of V.E anion-neg. charge because of the gain of V.E |
| how do you determine the charge of ions using the octet rule. example- LiS | find a common denominator using the charges. Li2S |
| what is the equation for solubility ?+?=? | solute + solvent= solution |
| how does temp effect solubility | solubility increases with temp for solids solubility decreases as temp increases for gases |
| how does pressure effect solubility | at high pressures, more gas molecules dissolve in the liquid |
| how does polarity effect solubility | like dissolves like. polar dissolves polar. nonpolar dissolves nonpolar |
| usually soluble if it contains | Li^+, Na^+, K^+, Rb^+, Cs^+, NH4^+, NO3^-, C2H3O2^-, Cl^-, Br^-, I^- |
| what is the (m/m) formula | g of solute ___________________________ x 100 g of solute + g of solvent |
| what is the formula for molarity | mol of solute _________________ L of solution |
| what is the (m/v) formula | g of solute ________________ x 100 mL of solution |
| dilution formula | C1V1=C2V2 |
| what is an Eq | the amount of moles of an ion that provides 1 mole of electrical charge (+ or -) |
| ? Eq = ? mEq | 1 eq = 1000 mEq |
| characteristics of weak electrolytes | do not produce ions dissolve as molecules in water no electric current |
| characteristics of strong electrolytes | dissociate completely in water produces + and - ions |
| what is the equation for formula mass | 1.66 x 10^-24 |
| how do you find molar mass | adding the weights of the elements on the periodic table multiplied by how many of them there are |
| what is LeChateliers principle | when equilibrium is disturbed the rates of the forward or reverse reaction change to relieve stress and re-establish equilibrium |
| 6 characteristics of Arrhenius bases | produces hydroxide ions (OH^-) in water they are electrolytes because they prduce OH^- taste bitter or chalky feels soapy and slippry turns red litmus paper blue (phenolphthalein pink) named as hydroxides (example NaOH is sodium hydroxide) |
| 5 characteristics of Arrhenius acids | produce H+ in H2O electrolytes sour taste turns blue litmus paper red corrodes some metals |
| Bronsted Lowry theory | BAAD base accepts acid donates |
| KW= ?+? | [H3O^+] x [OH^-] |
| KW= [H3O^+] x [OH^-]= | 1.0x10^-14 |
| if [H3O^+] and [OH^-] are equal than... if [H3O^+] is greater than... if [OH^-] is greater than... | its neutral, its acidic, its basic |
| pH + POH=? | 14 |
| [H3O] + [OH] = ? | 1x10^-14 |
| -log [OH] = | POH |
| -log [H3O] = | pH |
| 10^-pH= | [H3O] |
| 10^-POH= | [OH] |
| what are hydrocarbons | insoluble, nonpolar, with low density organic compounds with only hydrogen and carbon |
| what are unsaturated hydrocarbons | alkenes, alkynes, aromatic |
| what are saturated hydrocarbons | alkanes |
| what are structural isomers | same molecular formula with atoms bonded in a different order |
| cis-trans isomers have (the same or the different) physical and chemical properties | different |
| what is combustion | alkanes are converted to carbon dioxide + water with the release of heat energy |
| what happens during the hydration of an alkene | the double bond breaks and the alkene reacts with H2O to make an alchohol |
| what happens during the hydrogenation of an alkene | Hydrogen atoms are added to the carbon atoms of a double or triple bond |
| how to tell if its a 1,2, or 3 alcohol | how many C groups are attached on the hydroxyl |
| what is alcohols structure and solubility | polar. 1-3 carbons soluble 4=slightly 5=no |
| what is aldehydes and ketones solubility | 1-4 carbons are soluble 5=kinda 6=no |
| oxidation and reduction definition and how they interact with 1,2 and 3 alcohols | OIL RIG oxidation is losing electrons. reduction is gaining electrons 1 alc ->aldehyde->carb. acid 2 alc-> ketone-> can't 3 alc -> can't |
| the dehydration of alcohols produce.. | an alkene and water. loss of H and OH |
| how many carbons are monosaccharides | 3-7 carbons |
| what is amylose connected by and what kind of chain is it | a-D glucose joined by 1-4-glycosidic bonds. straight chained |
| what is amylopectin and what kind of chain is it | a-1-4 glycosidic bonds and a-1-6-glycosidic bonds. branched chain polysaccharide |
| what is cellulose and what kind of chain is it | B-1-4 glycosidic bonds. indigestible by humans. unbranched chains |
| common name of methanoic acid | formic acid |
| common name of ethanoic acid | acetic acid |
| common name for propanoic acid | propionic acid |
| common name for butanoic acid | butyric acid |
| salt name for methanoic acid- | sodium formate |
| salt name for ethanoic acid | acetate or sodium ethanoate |
| salt name for propanoic acid | sodium propionate |
| salt name for butanoic acid | magnesium bromide |
| solubility of carb. acids | 1-5 carbons are very soluble |
| how is an ester made | carb acid + alcohol |
| how do you determine the 1,2 and 3 of amine | how many carbons are attached to the N group |
| what is amines solubility rules | 6 or fewer are soluble (only primary and secondary) tertiary amines are insoluble |
| what are lipids | water-insoluble biological molecules |
| what are fatty acids and where are they found | 12-18 C long unbranched chain with a carb. acid at the end. found in your food, essential because it comes from your diet |
| how do you know if its an unsaturated or saturated fatty acid | unsaturated- when there's a C-C double bond saturated- when there's not a C-C double bond |
| main structures & function of waxes | 14-30 C long. esters of saturated fatty acids + long chain alcohols they form coatings on leaves and stems to prevent loss of water |
| main structures & function of triacylglycerols | fatty acids are stored as triacylglycerols formed when 3 hydroxyl groups of glycerol react with the carboxyl groups of 3 fatty acids |
| main structures & function of glycerophoslipids | have a polar and non-polar regions. polar head and a hydrocarbon tail most abundant in lipids in cell membranes plays an important role in cellular permeability |
| main structures & function of sphingolipids | a fatty acid is linked to amine group of sphingosine by an amide bond abundant in myelin sheath. increases the speed of nerve impulses + insulates and protects the nerve cell |
| what do sphingolipids contain | a sphingosine, fatty acid, phosphate and amino alcohols |
| fatty acid melting points | unsaturated fatty acids have higher melting points in hydrogenation, the more saturated the higher the melting point |
| describe triacylglycerol hydrogenation | double bonds in unsaturated fatty acids with hydrogen gas to produce C-C single bonds |
| describe triacylglycerol saponification | reaction of a fat with a strong base such as NaOH in the presence of the heat splits triacylglycerols into glycerol + the salts of the fatty acids (soaps) |
| in triacylglycerol saponification: fat (oil) + ? --> glycerol + ? | fat (oil) + strong base --> glycerols + 3 salts of fatty acids |
| what does an amino acid have | an α-carbon that's attcahed to -NH3^+, -COO^- and an H group the fourth component ( the R group differs) |
| how to tell if an amino acid is non-polar, polar uncharged or polar charged | non-polar: the R group is either H, alkyl, or aromatic polar uncharged: the R group is hydroxyl, thiol or amide polar charged: the R group is a carboxylate, or an amine |
| how are peptides written | written from left to right N terminal: the left side, -NH3+ C terminal: the right side -COO- |
| what are the (3) main functions of proteins | structural components such as cartilage, muscles, hair and nails enzymes accelerate biological reactions such as digestion and cellular metabolism transport of oxygen in the bloodstream such as hemoglobin and myoglobin |
| primary structure of protein structure | the sequence of amino acids held together by peptide bonds |
| secondary structure of protein structure | α-helix and β-pleated sheet |
| tertiary structure of protein structure | the overall 3D shape caused by interactions on different parts of the chain. causing it to bend and twist |
| quaternary structure of protein structure | the combination of two or more protein chains to form a functional protein |
| definition of the denaturing of proteins | involves the disruption of bonds in secondary, tertiary and quaternary protein structures |
| what is disrupted in heat denaturation and example | above 50 degrees C disrupted H bonds and hydrophobic interactions between non-polar R groups example: cooking or autoclave |
| what is disrupted in acids & bases and example | disruption of H bonds between polar and R group disruption of salt bridges example: lactic acid from bacteria, denatures milk or cheese and yogurt |
| what is disrupted in organic compounds and example | disrupts hydrophobic interactions example: ethanol and isopropyl alcohol disinfects wounds |
| what is disrupted in heavy metals and example | disrupted Ag^+, Pb^2+, Hg^2+. disrupted disulfide bonds in proteins by forming ionic bonds example: mercury + lead poisoning |
| what is disrupted in agitation and example | disrupts hydrogen bonds + hydrophobic interactions by stretching polypeptide chains+ disrupting stabilizing interactions example: whipped cream |
| what is the definition of enzymes | biological catalysts that lower the activation energy (by increasing the rate of reaction) |
| classes of enzymes vs. types of reactions | oxidoreductases-oxidation reduction transferase- transfer groups of atoms hydrolases-hydrolysis lyases- add or remove atoms to or from a double bond isomerases- rearrange atoms ligases-use ATP to combine small molecules |
| definition of a substrate | an active site; the compound or compounds whose reaction an enzyme catalyzes |
| the three types of inhibitors | non-competitive, competitive, and irreversible |
| describe a non-competitive inhibitor and their shape, where they bind, and is it reversible | non-competitive: not similar shape to substrate, binds away from an active site to change shape of enzyme, not reversed by adding more substrate but by a chemical change that removes the inhibitor |
| describe a competitive inhibitor and their shape, where they bind, and is it reversible | competitive: similar shape to substate, competes and binds at active site, and adding more substrate reverses the inhibition |
| describe an irreversible inhibitor and their shape, where they bind, and is it reversible | irreversible: not similar shape to substrate, forms covalent bond with the enzyme, not reversible |
| how is enzyme activity effected by temperature and pH | temperature: enzymes most active at 37 degrees C (in humans) little activity at cold temps becomes denatured at 50 degrees C pH: most active at the pH of 7.4 |
| describe catabolic & anabolic reactions | catabolic: break down large complex molecules to release energy and smaller molecules anabolic reactions: use ATP and small substrates as building blocks to synthesize larger molecules |
| what is glycolysis, where does it take place and how many reactions are there | provide pyruvate for the trichloroacetic acid cycle takes place in the cytoplasm there are 10 reactions |
| main purpose of reactions 1-5 of glycolysis and how many ATP are used | energy investment phase 1 glucose molecule (6C)( is converted into two molecules of glyceraldehyde-3-phosphate (3C) 2 molecules of ATP are used |
| main purpose of reactions 6-10 of glycolysis and how many ATP are used | energy generating phase 2 molecules of glyceraldehyde's-phosphate (3C) are converted into 2 molecules of pyruvate (3C) 4 ATP synthesized, 2 NADH formed with a net yield of 2 ATP/glucose |
| describe how pyruvate is converted under aerobic and anaerobic conditions | aerobic: converted to acetyl-CoA anaerobic: converted to lactate |
| where do the electron transport chain and phosphorylation take place and what is the order of the complexes | in the mitochondria ETC order: complex I, complex II, coenzyme Q, complex III, cytochrome C, complex IV |
| complex I of electron transport chain's donor and acceptor | donor: NADH acceptor: coenzyme Q |
| complex II of electron transport chain's donor and acceptor | donor: FADH2 acceptor: coenzyme Q |
| complex III of electron transport chain's donor and acceptor | donor: coenzyme G H2 acceptor: cytochrome C |
| complex IV of electron transport chain's donor and acceptor | donor: reduced cytochrome C acceptor: O2 |
| where does the citric acid cycle take place and how many reactions are there | mitochondria, 8 reactions |
| what is produced after one round of the citric acid cycle and what are the substrates for the first cycle | 2 CO2, 3 NADH, 1 FADH2, 1GTP substrates: acetyl CoA and oxalacetate |
| which complexs transfers protons from mitochondrial matrix into intermembrane space | complex I, II, and IV |
| what is oxidative phosphorylation | couples the energy from the electron transport to the synthesis of ATP from ADT and phosphate (Pi) |
| fatty acid oxidation: what happens in reaction I | oxidation. hydrogen atoms removed by the FAD from the α and β carbons form a c-c double bond and FADH2 |
| fatty acid oxidation: what happens in reaction II | hydration H-OH adds across the double bond, which forms the -OH adding on the β- carbon |
| fatty acid oxidation: what happens in reaction III | oxidation the secondary hydroxyl group (-OH) on the β carbon is oxidized to yield a ketone while NAD+ is reduced to NADH |
| fatty acid oxidation: what happens in reaction IV | cleavage the C α and β is cleared to yield an acetyl-CoA (2C) and shorter (8C) fatty acyl-CoA |
| when do ketone bodies form (specifics) | ~large amounts of acetyl-CoA accumulate ~2 acetyl-CoA molecules form acetoacetyl-CoA ~acetoacetyl-CoA hydrolysyzes to acetoacetyl-CoA ~acetoacetate reduces to β-hydroxybutyrate OR ~loses Co2 to form acetate |
| when do ketone bodies form (general) and what is formed from ketogensis | if carbohydrates are not available, body fat breaks down for energy in a process that makes ketone bodies ' acetoacetate, β-hydroxybutyrate and acetone are formed |
| how many ATP are formed in one round of the citric acid cycle | 10 ATP |
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paigefigs
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