L1: Water: the "universal" solvent

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33 Terms

1

what makes water the “universal” solvent

  1. nearly all biological molecules assume their shapes and functional properties based on their interactions w water

  2. the “solvent” for most biochemical reactions is water, and metabolites depend on water for their transport in vivo

  3. water is catalytically involved in many biochemical reactions

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2

OH- acts as electron -

donor

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3

H+ acts as an electron -

acceptor

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4

in most biochemical reactions

  • when water is a reactant, the reaction is called -

  • when water is product, the reaction is called -

hydrolysis, dehydration/condensation

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5

angular geometry results from - nature of H2O

polar

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6

four hybrid sp3 electron orbitals of oxygen form a -

  • two orbitals represent the - electrons of of oxygen

  • other two orbitals represent the - electrons between O and H

tetrahedron, unshared, shared

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7

oxygen, with its 2 pairs of -, is electronegative and the H atoms carry a net - charge

this creates an -

unshared electrons, positive, electrical dipole

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8

water molecules orient themselves according to their - and hydrogen bonds form between a - H and - O in adjacent water molecules

electric dipole, donor, acceptor

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9

H bonds between adjacent molecules give water its strong - and unique properties (ex. - melting, boiling, vaporizing temperatures)

internal cohesion, high

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10

in ice, each water molecule H bonds with - other water molecules, forming -

this is the reason why water - upon freezing

four, hexagonal lattices, expands

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11

liquid water does not possess the static hexagonal structure of ice but it is still -

strongly cohesive

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12

theoretical and spectroscopic data suggests that liquid water forms between - membered H bonded rings

3-7

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13
<p>water H-bonded to what?</p>

water H-bonded to what?

hydroxyl functional groups

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14
<p>water H-bonded to what?</p>

water H-bonded to what?

carbonyl functional groups

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15
<p>water H-bonded to what?</p>

water H-bonded to what?

carboxylate functional groups

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16
<p>water H-bonded to what?</p>

water H-bonded to what?

amino functional group

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17

water dipole is able to interact with both - and -

anions, cations

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18

when water molecules surround an ion, they - the attractive forces between opposite ions and keep them -, which is why - dissolve readily in water

weaken, apart, salts

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19

the strength of multiple water:ion bonds compensates for the energy used to break - between water molecules

hydrogen bonds

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20

like water, carbon dioxide bonds also form dipoles and can orient themselves via weak - interactions called -

electrostatic, permanent dipoles

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21

dipole of a polar molecule can induce a dipole in an, otherwise, neutral molecule by attracting electrons toward the dipole

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22

higher negative exponent, the higher affinity

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23

weakest VDW form when complementary dipole moments occur in - molecules

non-polar

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24

strength of chemical bonds

covalent » ionic > h bond > polar VDW > non-polar VDW

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25

non-polar/hydrophobic molecules added to water do not -

this is because they are unable to form - or - bonds with water

instead, water molecules form - bonds between themselves around the non-polar solute

dissolve

ionic, hydrogen

hydrogen

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26

clustering of non-polar solutes is driven by the thermodynamic properties of water = -

hydrophobic effect

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27

delta G = -

if delta G is negative, reaction/interaction can occur -

negative delta G means reaction or interaction is energetically -

free energy change

spontaneously

favourable

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28

delta H = - change in making or breaking bonds

generally forming bonds yields - delta H and breaking bonds - delta H

negative delta H favours reaction or interaction by making delta G more -

enthalpy

negative, positive

negative

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29

delta S = change in relative order of reactants and products = -

increase in disorder = - delta S, favours reaction or interaction

- delta S decreases delta G

entropy

positive

positive

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30

increase in - increases delta S, lowers delta G

temperature

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31

it is always unfavourable to have - solutes in water

non-polar

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32

water becomes more - around the non-polar solute → - in entropy

despite reduction in entropy, clustering of non-polar solutes occurs because the same volume of solutes can be “caged” by a - surface area of water

ordered, decrease

smaller

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33

structure of macromolecules is driven by the -

hydrophobic effect

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