Intermolecular interactions: London forces Flashcards

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1
Q

interactions between molecules are described as (2 items)

A
  • ‘non-bonded interactions’

- ‘intermolecular’

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2
Q

London forces are an important

A

non-bonded interaction also known as dispersion forces

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3
Q

London forces are weaker than

A

covalent bonds and polar covalent bonds

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4
Q

on average, diatomic molecules such as nitrogen are non-polar because

A

the electron density is symmetrically distributed throughout the molecule

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5
Q

the electron density in molecules can

A

change over time, generating a dipole as the molecule becomes unsymmetrical in electron density

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6
Q

when the electron density in a molecule changes, London forces arise because

A
  • one molecule gains an unsymmetrical distribution of electron density, with partial charges forming at each end of the molecule
  • this partial charge is called an instantaneous dipole
  • the partial charge of a molecule will affect the electron densities of the molecules on either side of it as their electrons will respond to the partial charges of the instantaneous dipole by either repelling or being attracted to a partial positive charge
  • the resulting dipole is called an induced dipole
  • the two dipoles are arranged so that they interact favourably, and it is this force that is responsible for the London force of attraction between two molecules
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7
Q

the induced dipole will ……………..be aligned……………….

A

ALWAYS be aligned in such a way that the interaction with the instantaneous dipole is FAVOURABLE

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8
Q

the fluctuations that lead to the generation of an instantaneous dipole and the subsequent induced dipole are

A

very rapid processes compared to the rates which the molecules are moving owing to the kinetic and rotational energy they have

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9
Q

the relative speed of the dipole generating processes means that as molecules move around, they will continue to

A

attract each other regardless of the orientation of the two molecules

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10
Q

the attractive force of London forces increases with

A

the increasing number of electrons in the molecule

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11
Q

we can easily see how the increasing number of electrons in a molecule increases the London forces with the study of

A
  • the boiling temperatures of the noble gases (monatomic molecules)
  • as the London force is the only force of attraction between them
  • the boiling temperatures of each member down the group increases
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12
Q

using noble gas boiling temperature as a study of London forces is suitable because

A

London forces are the only force of attraction between the monatomic molecules

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13
Q

the more electrons there are in a molecule, the greater

A

the fluctuation in electron density and the larger the instantaneous and induced dipoles created

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14
Q

London forces also depend on

A

the shape and size of the molecule

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15
Q

the greater the points of contact between the molecules, the greater

A

the overall London force

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16
Q

London forces are always

A

present between molecules