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Mod. 2 - Water
Biochemistry Module 2
| Question | Answer |
|---|---|
| what is the most amazing molecule in the world of biochemisty | water |
| what is an aqueous solution | the basic solution for life. it is a solution that is water based and all the solvents therein |
| what is an example of an aqueous solution that is needed for life. | cytosol (cytoplasm) |
| what are some important important reactions (necessary for life) that occur in the cytoplasm | DNA/Protein,/Carbohydrate/lipid building and breakdown |
| describe the water molecule | only non-metal elements, two covalent bonds with two pairs of unbound electrons (gives the molecule its structure) |
| because oxygen has four sets of valentce electrons, it would be considered to have ______________________________ | sp3 hybridization |
| the bent shape and polarization or the water molecule arises from | the difference in electronegativity between the hydrogen and oxygen molecules. |
| what is a dipole arrow | an arrow used to notate which element in a molecule has the higher electron density |
| draw the dipole arrows for a water molecule | see picture |
| what is the importance of using dipole arrows in a water molecule | the dipole arrows show oxygen's ability to attract electrons from both the hydrogens it is bonded to in the molecule |
| give examples of other polar molecules | glucose and acetic acid (do to the OH and COOH ions, respectively) |
| give examples of non polar molecules | cooking oil and bees wax |
| the polarization of waters allows for the dissolving of (polar/non-polar molecules) | water only dissolves other polar molecules |
| give an examples of molecules that would dissolve in water | glucose, acetic acid, and sodium chloride |
| other than polarity, what else helps with the dissolving nature of a molecule | the size of the molecule being dissolved |
| water (which is polar) is unable to dissolve what types of molecule | water cannot dissolve non-polar molecules |
| what are some examples of molecules that water cannot dissolve | water cannot dissolve cooking oil or bees wax |
| what is autoionization | the molecule's ability to react to itself and form ions |
| show the autoionization that water performs | H2O + H2O ==> H3O+ + OH- |
| an important aspect of water is that it can autoionize (not/and) has solvent properties | water can autoionize AND has solvent properties |
| list all the important properties of water | - autoionize - solvent - high melting point - high boiling point, - high heat of vaporization |
| waters higher than normal melting and boiling points indicate what? | the substances stronger than normal intermolecular forces |
| what is heat of vaporization | the heat at which a substance changes from a liquid to a gas |
| the unique structural and physical properties of water result from | the non-covalent attractions |
| what is the melting point of water | 0 degrees C |
| what is the boiling point of water | 100 degrees C |
| what is the heat of vaporization of water | 540 degrees C |
| what is the melting point of hydrogen sulfide (H2S) | -82 degrees C |
| what is the boiling point of hydrogen sulfide (H2S) | -60 degrees C |
| what is the heat of vaporization of hydrogen sulfide (H2S) | 69 degrees C |
| what is the melting point of hexane | -95 degrees C |
| what is the boiling point of hexane | 69 degrees C |
| what is the heat of vaporization of hexane | 88 degrees C |
| what is the melting point of carbon tetrachloride | -23 degrees C |
| what is the boiling point of carbon tetrachloride | 77 degrees C |
| what is the Heat of Vaporization of carbon tetrachloride | 47 degrees C |
| what are non-covalent forces | they are the attractive/repulsive forces between two molecules and it is based on the sharing of electrons/polarity of the molecule. |
| most of the non-covalent forces discussed are (attractive/repulsive) | attractive |
| what are some examples of attractive non-covalent forces | - water beading up on a waxed care - water and oil separating - bugs walking on water - fat soluble vitamins dissolving in a plasma membrane |
| in polarized molecules, there is an attractive force between the areas of the molecules that have | opposing/opposite partial charges (i.e. the partially negative O and the partially positive H) |
| _________________ determines how a molecule will orient self | non-covalent forces in polar molecules |
| list the three types of non covalent forces | 1) dipole - dipole forces 2) hydrogen bonding 3) London dispersion forces |
| what are dipole-dipole forces | molecular forces that are more similar to magnets |
| put a molecule with dipole dipole forces in a liquid what would happen | the molecules would align themselves so that the + and - forces attract each other |
| give some examples of different molecules that have dipole-dipole forces | glucose, acetone, and hydochloride |
| what is the strongest class of intermolecular forces | dipole-dipole forces |
| what is the reason that acetone is a liquid at room temp rather than a gas | dipole-dipole forces are the reason that acetone is a liquid at room temperature |
| what is the strongest dipole-dipole interaction | hydrogen bonds |
| what are the two parts that are needs to form a hydrogen bond | 1) hydrogen atom is a donor (hydrogen donor) 2) specific hydrogen acceptor must be present ( |
| what is a hydrogen donor | a Oxygen, Florine, or Nitrogen that is covalently bonded to Hydrogen |
| what is an electron acceptor | an oxygen, florine, or nitrogen that has a pair of unbonded electrons |
| name the three elements that (when bonded to hydrogen) are capable of creating hydrogen bonds | nitrogen, oxygen, and flouride |
| draw a hydrogen bond between two ammonia molecules | see picture |
| draw a hydrogen bond between an ammonia and water molecule | see picture |
| draw a hydrogen bond between water and methanol molecules | see picture |
| what water freezes it from ______________________ (number) bonds | four (technically: 3.7 bonds) |
| what are the two most important properties of hydrogen bonds | the molecules that have high boiling points and high melting points |
| what are the weakest form of non-covalent forces in molecules | London dispersion forces |
| what are London Dispersion Forces | they are temporary and transient creation and dispersion of polar forces based on where the electrons are congregating in a molecule |
| how does London Dispersion forces affect substances | it can influence the arrangement of molecules near by, causing them to rearrange to maximize their molecular attraction |
| the repeated forming and breaking of London Dispersion Forces can cause | molecules to break down and no longer have any polarity |
| what types of atoms/molecules have greater London Dispersion forces | larger atoms/molecules |
| how do london forces affect the physical properties of molecules | they can lead to higher boiling and melting points |
| Flouride and chlorine have small london forces and as a result they are ________________ (physical property) at room temp. While iodine has large london forces and is ___________________ (physical property) at room temp | flouride and chloride are gas at room temp. iodine is solid at room temp |
| what is the physical state of Bromide at room temp | liquid |
| what is the estimated force of london forces | <1 kCal |
| what is the estimated force of dipole-dipole forces | 0.5-2.0 kCal |
| what is the estimated force of hydrogen bonds | 12-16 kCal |
| the estimated bond of a OH ion is 400(+) kCal, why is it so high | OH are covalently bonded, the others are not covalent bonds |
| compare and contrast covalent bonds with non-covalent bonds/forces | covalent bonds: electron is shared and they are more stable non-covalent bonds: attraction is between the opposite poles, forces are weaker |
| what is an important applied use for non-covalent bond | allows for a drug to bind to a protein on a cell over and over again |
| hydrophilic | polar molecules that are soluble in water |
| hydrophobic | non-polar molecules that are not soluble in water, these molecules have weak london forces and are repelled by or repels water |
| in water, how do phospholipids align themselves | the molecule aligns themselves with polar regions packed together and non-polar regions packed together |
| what is the hydrophobic effect | the arrangement that phospholipids take in order to minimize interactions with water |
| clathrate | the cage-like structure that water molecules make around the the hydrophobic portion of a phospholipid |
| what is the driving force for the arrangement of phospholipids in water | hydrogen bonds in water |
| why are sea monkeys brought it up in this module | because sea monkeys can go into "hibernation" mode when they are dried out. Then they reanimate when they are from hydrated. |
| name three ways humans can get water | 1) drinking water 2) from food 3) metabolic reactions |
| name three ways that water is lost in humans | 1) urine 2) feces 3) sweat |
| about how much water does a human drink on a daily basis | 900 mL |
| about how much water does a human lose through urine | 1050 mL |
| approximately how much water does a human lose in feces | 100 mL |
| approx. how much water is lost in sweat | 850 mL |
| about how much water does the human intake from food | 800 mL |
| approx. how much water does a human intake from metabolism | 300 mL |
| how much total water does the human intake (from water, food, and metabolism) | 2000 mL intake |
| how much total water does the human loose (from urine, feces, or sweat) | 2000 mL output |
| what some examples of the colligative properties in water | adding salt to ice to lower the melting point, osmotic pressure (creating osmotic pressure) |
| define colligative properties | the collective properties of water and it's solutes |
| for water, liquid is (more/less) dense than solid water. Therefore for allowing ice to float on water | liquid is MORE dense than solid; allowing ice to float in water |
| what is heat capacity | the amount of heat that is absorbed by a substance |
| water on its own, tastes rather bitter. to make it taste better, what needs to be added to water | salts (Magnesium Sulfate and Calcium Cloride) |
| what are some examples of the attractive properties of water | water droplets on a penny, coaster stuck on glass |
| what is Coulumbs law | Law of Attraction (F=k((Q1Q2)/r^2)), where: F - electric fource k - Coulumb's constant Q1 and Q2 - the charges r - distance between Q1 and Q2 |
| bottom line with columns law and how it relates to non-covalent attraction | the closer the atoms are to one another, the more attracted they will be |
| (t/f) water can only form hydrogen bonds with other water molecules | false: water can form hydrogen bonds with other molecule such as ammonia |
| what does aqueous chemistry study | what happens once ions are dissolved in water and what are the reactions that take place in an aqueous solution |
| what is Hydronium | H3O+ or just H+ |
| what is Hydroxide | OH- |
| write the chemical equation that shows the autoionization of CH3COOH (acetic acid) | CH3COOH <----> CH3COO- + H+ |
| what are some examples of other molecules that can self ionize (autoionization) other than water | 1) vinegar (acetic acid) 2) Phosphoric Acid 3) Carbon dioxide 4) Histidine |
| in regards to pH, what happens when adding an acid to water | the pH lowers |
| what is the equation for equilibrium constant | K(eq) = Concentration of the products/concentration of the reactants ( [products]/[reactants] ) |
| regarding equilibrium: list three essential concepts | 1) forward and reverse reactions are occurring 2) reactions continue at equilibrium (rate of forward and reverse occur at the same time) 3) there is no net change (concentrations are the same) |
| why is H2O no included in the equilibrium constant of water | water is a pure liquid |
| what is the numerical value for the constant of water | 1.0*10^-14 |
| why are pure liquids and pure solids left out of the equilibrium contant | because their concentrations do not change |
| what is the pH formula | pH = - log [H+] |
| what is the formula for finding [H+] from pH | [pH] = -10^-pH |
| (t/f) the pH of aqueous solutions influences other compounds | true: pH of aqueous solutions can influence other compounds |
| define equilibrium | when the rates of the forward and reverse reactions are the same |
| define equilibrium constant | K(eq) = [products]/[reactants] |
| what is the equilibrium constant for the following equation: aA + bB <-----> cC + dD | K(eq) = (([C]^c)([D]^d))/(([A]^a)([B]^b)) |
| What is the unit for the equilibrium constant (K(eq)) | there is no unit for the equilibrium constant |
| the equiilibrium constant for water is considered a __________________, because the only things contributing to this constant are the ions | ion product |
| what it the [H+] value of an acidic solution | 10^0 10^-1 10^-2 10^-3 10^-4 10^-5 10^-6 |
| what it the [H+] value of a basic solution | 10^-8 10^-9 10^-10 10^-11 10^-12 10^-13 10^-14 |
| what it the [H+] value of a neutral solution | 10^-7 |
| what it the pH of an acidic solution | 0 1 2 3 4 5 6 |
| what it the pH of a neutral solution | 7 |
| what it the pH of a basic solution | 8 9 10 11 12 13 14 |
| what it the [OH-] value of an acidic solution | 10^-14 10^-13 10^-12 10^-11 10^-10 10^-9 10^-8 |
| what it the [OH-] value of a neutral solution | 10^-7 |
| what it the [OH-] value of a basic solution | 10^-6 10^-5 10^-4 10^-3 10^-2 10^-1 10^0 |
| what is the physiological pH? | 7.4 |
| how is the pH of a lysosome different from that of the rest of the cytosol | the pH inside a lysosome is 5.0, concentration of [H+] is nearly 100X greater than other organelles |
| name three types of compounds that can dissolve in water | 1) ionic (salt) compounds 2) polar molecules 3) molecules that have hydrogen bonds |
| name some ionic compounds would dissolve completely in water | 1) NaCl 2) NaCO3 3) KCl |
| name some polar molecules that will dissolve in water | 1) HCl 2) Acetone 3) other ketones |
| name some examples of molecules that have hydrogen bonds that can dissolve in water | 1) acetic acid (vinegar) 2) sugars |
| what is(are) the product(s) when Carbonate (CO3^2-) is put in water | HCO3- + OH- |
| in the following reaction; the product produces an acid or a base? and would therefore increase or decrease pH? CO3^2- + H2O <====> HCO3- + OH- | the carbonate reaction creates a base and INCREASES the pH of the solution |
| what is(are) the product(s) when HCl is put in water | H3O+ + Cl- |
| the following reaction; the product produces an acid or a base? and would therefore increase or decrease pH? HCl + H2O ====> H3O+ + Cl- | hydrochloric acid is a strong ACID and DECREASES pH of a solution |
| what is(are) the product(s) when CH3COOH (acetic acid/vinegar) is put in water | H3O+ + CH3COO- |
| the following reaction; the product produces an acid or a base? and would therefore increase or decrease pH? CH3COOH + H2O <====> H3O+ + CH3COO- | acetic acid (vinegar) is acidic and DECREASES the pH of a solution |
| what is the condensed formula for Lactic Acid | CH3CH(OH)COOH |
| where is Lactic Acid produced | lactic acid is produce in cell during anaerobic exercise |
| what is the conjugate base for lactic acid | Acetate (CH3CH(OH)COO-) |
| what is the formula for the equilibrium constant for the following Lactic Acid: CH3CH(OH)COOH + H2O <======> H3O+ + CH3CH(OH)COO- | Ka = ([H3O+][CH3CH(OH)COO-])/[CH3CH(OH)COOH] |
| what is the formula for pKa | pKa = -log[Ka] |
| what is a buffer | a buffer is a chemical that resists changes in pH with small amounts of H+ and Oh- added |
| how is lactic acid a buffer (base added to solution) | when OH- is added to a solution of lactic acid. The lactic acid become acetate (gives off a proton) this proton bonds with the OH- ion to create water |
| how is lactic acid a buffer (acid added to solution) | when a proton (or H3O+) is added to an acetate solution, the acetate accepts the extra proton to create lactic acid and water |
| a buffer capacity depends on: | the acid and its conjugate base |
| what is the importance of a buffering system (specific in life/the cell) | - helps to maintain the pH of the system - helps to protect proteins from pH levels that would otherwise degrade them |
| what is the most important buffering system in the body and where can this be found | the bicarbonate buffering system |
| what is a strong acid | the acidic compound completely dissolves in water |
| what are some examples of strong acids | HCl (hydrochloric acid) and Sulfuric Acid |
| (strong/weak) acids have an arrow going in one direction because the reaction only goes in one directions; while (strong/weak) acids have two arrows because these acids will disassociate and then reassociate in an aqueous solution | STRONG acids has an arrow in one direction, WEAK acids have two arrows |
| (t/f) only strong acids can change the pH of a solution drastically; while weak acids effect the pH of a solution in a minor way | FALSE: both strong and weak acids can change the pH of an aqueous solution drastically |
| (t/f) weak acids are more common in biological systems | TRUE: weak acids and bases are most common in biological systems (cytosol or the blood stream) |
| what influences the metabolic rate/reactions and biological structure | the weak acids/pH of the cytosol or in the blood |
| why are weak acids more common in biological systems | because they only partially ionize in a solution |
| acetic acid is a proton (acceptor/donor) | acetic acid is a proton DONOR |
| what is a proton donor | the donor generates (or gives off) a proton in the product of a reaction (reaction is going forward) |
| what is a proton acceptor | in the REVERSE reaction, the ion (or conjugate base) accepts an electron |
| what is the equilibrium constant for acids. Use the the following equation as an example: HA <=====> A- + H+ | Ka = ([A-][H+])/[HA] |
| what is the acid dissociation constant | Ka |
| what is the purpose of the Ka and pKa measurement | Ka and pKa indicated tendency for weak acids to lose a proton |
| dihydrogen phosphate is a (strong/weak) acid | dihydrogen phosphate is a WEAK acid |
| what is the relationship of strong/weak acids to Ka | Ka is larger for stronger acids and smaller for weaker acids |
| what is the relationship of strong/weak acids to pKa | pKa is smaller for stronger acids and larger for weaker acids |
| what is the Ka and pKa of Trataric acid (H2C4H4O6) | Ka: 1.0*10^-3 pKa: 3.0 |
| what is the Ka and pKa of Formic Acid (HCOOH) | Ka: 1.8*10^-4 pKa: 3.74 |
| what is the Ka and pKa of Acetic Acid (CH3COOH) | Ka: 1.8*10^-5 pKa: 4.82 |
| what is the Ka and pKa of Proprionic Acid (C2H5COOH) | Ka: 1.3*10^-5 pKa: 4.89 |
| what is the Ka and pKa of Dihydrogen Phosphate (H2PO4-) | Ka: 6.2*10^-8 pKa: 7.21 |
| Which is the stronger acid? Formic Acid: Ka= 1.8*10^-4 Dihydrogen Phosphate: Ka= 6.2*10^-8 | Formic acid is the stronger acid because it has a larger Ka |
| which acid is stronger Proprionic Acid: pKa= 4.89 Tartaric Acid: pKa= 3.0 | tartaric acid is the stronger acid because it has a smaller pKa |
| buffers can be produced by | weak acids |
| this is an aqueous solution system that resists a change in pH when small amounts of H+ and OH- are added | a buffer |
| when acids/bases are added to a solution and then they are neutralized by __________________ and ___________________ (respectively) | conjugate bases or weak acids |
| name two metabolic reactions that use buffers | glycolysis and citric acid cycle |
| how are buffers used in the metabolic reactions | these reactions produce protons (H+) buffers in the cell help to neutralize these protons so the pH does not get too high |
| what is the main buffer used by the cell for metabolic reactions | dihydrogen phosphate (H2PO4-) |
| what is the pH of cytosol | 7.4 |
| the buffering range can effectively neutralize a solution within _____________ pH units of its pKa | +/- 1.0 pH |
| if acetic acid has a pKa of 4.82, what is the buffering range of acetic acid | 3.82 to 5.82 |
| (t/f) an innumerable amount of acid/base can be added to a buffer and the pH will change only minimally | FALSE: the buffers can only handle a certain amount of acids/bases added to the solution |
| what is the buffering limit | the amount of an acid/base that can be added to a buffered solution that will be neutralized |
| CO2 is | a product of cell metabolism |
| what is Carbonic acid (H2CO3) | when CO2 combines with water |
| write the chemical equation for the bicarbonate buffer solution | see drawing |
| why is the bicarbonate buffer solution so important | bicarbonate buffer system helps keep blood pH at 7.4 and helps to transport CO2 back to the lungs |
| the bicarbonate buffer system is monitored by | the renal tubular cells in the kidneys, they take up excess HO3- to maintain appropriate levels |
| list the five indicators of a chemical reaction | - light production - heat change (heat exchange) - sound - color change - bubble formation (gas is produced) |
| of all the five indicators of a chemical reaction, which ones are most used in biochemistry | - heat exchange - bubble formation |
| what is thermochemistry | how heat changes in a systemp |
| what are the three major components of thermochemistry | enthalpy, entropy, and gibbs free energy |
| what is enthalpy (H) | the action of heat transfer in a reaction |
| what is entropy (S) | the amount of disorder that was created by a reaction/heat |
| in most reactions, have (positive/negative) enthalpy | most reactions have NEGATIVE enthalpy |
| what is the Gibbs Free energy equation | G = H-TS or deltaG=deltaH-TdeltaS |
| if G (or delta G) is negative ... | spontaneous reaction (striking a match) |
| if G (or delta G) is positive ... | non-spontaneous (water beading up on stainless steele) |
| in a exothermic reaction | heat is leaving the system |
| in a endothermic reaction | heat enter s the system |
| if entropy (S) is positive | the reaction creates more chaos |
| if entropy (S) is negative | there is more order (two molecules coming together to build a bond) |
| a spontaneous reaction is more likely to have a (positive/negative) entropy | spontaneous reactions have POSITIVE entropy |
| the production of ATP (formula below), has a (positive/negative) gibbs free energy this means it is (spontaneous/nonspontaneous): Glucose + Pi ========> Glucose-6-Phosphate | creation of ATP has a POSITIVE Gibbs Free Energy making it non-spontaneous |
| the breaking of ATP to ADP + Pi has a (positive/negative) gibbs free energy | ATP====>ADP + Pi is NEGATIVE gibbs free energy |
| overall, the below reaction is (spontaneous/non-spontaneous) Glucose + ATP ====> Glucose-6-Phosphate + ADP | overall this reaction is spontaneous |
| the creation of luciferin in fireflies produce no heat meaning, what? | the energy released by the metabolic reactions creating luciferin is mostly in the form of light and very little in the form of heat |
| humans are considered warm blooded, why? | the heat comes from all the metabolic reactions |
| in hand warmers, the heat given off is considered. which represents/reflects | enthalpy, reflecting the number of bonds in a system |
| if there are more products than reactants, what does this tell us about entropy | the entropy is considered positive and there is more chaos, randomness, and disorder |
| a solid is changed to a liquid in a reaction, what does this tell us about entropy | the entropy is positive when reactants have more structure than the products |
| if there are more products than reactants, what does this tell us about gibbs free energy | G is negative and will proceed spontaneously |
| what is the equation of a cold pack | Urea(s) + Water(l) =====> Urea(aq) + Water(l) |
| why does a cold pack feel cold | the reaction occurs without energy input leading to a cold feeling |
| if deltaH (enthalpy) is positive, what does that tell us | heat is flowing into the reaction (making cold pack feel cold) |
| what is the role of ATP in a cell | to allow non-spontaneous reactions to occur |
Created by:
kandriot
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