Molecular forces Flashcards

1
Q

covalent bond

A

atoms share electrons

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2
Q

non-covalent bond

A

different types of interactions lead to bond formation

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3
Q

weakness of non-covalent bond

A

inheritance - DNA strands separate
compartment - bilayers etc
signalling - proteins and ligands

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4
Q

ionic

A

for from permanent gain/ lose of e- forming permanent charge
e.g. Na+ and Cl-

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5
Q

Quantitively description of ionic bond

A

E{coulomb} = q1q2 / kcr

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6
Q

r

A

distance between q1 and q2 (charges)

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7
Q

dipole interaction

A

have no net charge - partial charges such as water

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8
Q

quanititive dipole interaction equation

A

E{dipole, charge} = q (vector) cos* / kcr(2)

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9
Q

interaction energy between dipole and charge

A

falls with 1/r(2)

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10
Q

dipole dipole equation

A

E{dip, dip} = (2(vector1 , vector2) / kcr(3)) f(angles)

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11
Q

interaction energy between dipole and dipole

A

falls with 1/r(3)

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12
Q

dispersion forces

A

neutral molecules with out partial charges can have temporary charges

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13
Q

how dispersion forces are formed

A

by short lived uneven electron distribution

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14
Q

induced induced equation

A

E{ind, ind} = -const / r(6)

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15
Q

energy interaction between induced and induced

A

1/r(6)

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16
Q

dispersion forces being universal

A

all molecules being attracted to each other

17
Q

Pauli exclusion principle

A

Quantum mechanics dictates no more than 2 electrons than occupy same orbital so can only get as close as electron distribution allows without overlapping

18
Q

VdW potential

A

where energy if minimal - specifies optimal distance between 2 atoms

19
Q

combining energy in VdW potential due to….

A

VdW radius with dispersion energy

20
Q

hydrogen bond requirements

A

2 electronegative atoms (N, O, F)

21
Q

H donor

A

H bond to electronegative

22
Q

H bond accepter

A

H can only bond with non-bonding pair of electrons on another electronegative atom

23
Q

examples in DNA

A

alpha helices - H bond between CO and NH

beta sheet - H bond between CO and NH - antiparallel strands - at angle (weaker)

24
Q

dipole-dipole attraction

A

dominating H bond interaction - electrostatic

25
Q

angular dependence

A

best of donor and acceptor in straight line - 180 degrees

26
Q

d{0} on graph

A

optimal distance

27
Q

How H bonds vary

A

dependent on donor and acceptor atoms

28
Q

Hydrophobic effect

A

non-polar molecules don’t mix well with polar molecules

29
Q

perturbation

A

effect increases as non-polar molecules affects polar solvent

30
Q

minimize free energy

A

more favourable when non-polar molecules cluster together

31
Q

non-polar molecules clustering

A

minimises perturbation of solvent

driven by maximizing entropy

32
Q

perturbation of polar solvent example

A

water - tetrahedron therefore has 6 options of H bond with neighbouring O atoms

33
Q

When adding hydrophobic group at the corner of tetrahedron

A

to decrease entropy of system

single C atom halves no. microstates

34
Q

packing together the hydrophobic group

A

causes less water perturbation

35
Q

hydrophobic effect driven

A

lipid assembly in to vesicles

bilayer sheets, liposome, micelle

36
Q

protein folding of hydrophobic effect

A

burying majority of amino acid with hydrophobic side chains in the core of protein