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2nd Semester > Intermolecular forces > Flashcards

Intermolecular forces Flashcards

1
Q

These are electrostatic interactions between
permanently or transiently (temporarily) charged
chemical species.

A

Intermolecular Forces

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2
Q

They refer only to attractive interactions, which hold
molecules and ions together in condensed phases
(liquid and solid).

A

Intermolecular Forces

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3
Q

Intermolecular Forces govern many of the bulk physicals
properties of substances and mixtures, such as
______________________

A

melting point, boiling point, and surface tension.

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4
Q

These forces govern many of the bulk physical
properties of substances and mixtures, such as
melting point, boiling point, and surface tension.

A

Intermolecular Forces

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5
Q

TYPES OF INTERMOLECULAR FORCES?

A
  1. London Dispersion Forces (Van der Waals)
  2. Dipole to Dipole Forces (Van der Waals)
  3. Ion – Dipole Forces
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6
Q

ION-ION FORCES, also known as __________

A

IONIC BONDING.

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7
Q

These forces arise from the electrostatic attraction between two ions with opposite charges.

A

IONIC BONDING.

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8
Q

Ionic Bonding Arises from what?

A

the electrostatic attraction between two ions with opposite charges.

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9
Q

Intermolecular forces only refers to?

A

Attractive Interactions

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10
Q

Attractive interactions does what?

A

hold molecules and ions together in condensed phases

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11
Q

They are not technically considered intermolecular forces, but are a helpful starting point for understanding the true IMFs (intermolecular forces).

A

Ionic Bonding

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12
Q

They are not technically considered intermolecular forces but are a helpful starting point for understanding the true IMFs (intermolecular forces).

A

Ionic Bonding

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13
Q

Ionic Bonds are not technically?

A

Intermolecular Forces

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14
Q

Are also generally stronger than the IMFs, which is why most
pure salts are solids except at extremely high temperatures.

A

Ionic bonds

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15
Q

pure salts are solids except at?

A

extremely high temperatures.

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16
Q

Table salt has a melting point of?

A

800 degrees Celcius

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17
Q

WEAKEST intermolecular forces

A

London Dispersion Forces

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18
Q

✓ The more electrons a molecule has, the stronger the what?

A

London dispersion
forces are.

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19
Q

The breaking of London dispersion forces doesn’t require that much what?

A

Energy

20
Q

All molecules experience London Dispersion Forces (LDFs).true or false?

A

True

21
Q

Are the only IMFs that exist between noble gases and
molecules that are non-polar.

A

Dispersion Forces

22
Q

These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.

A

Dipole to Dipole Forces

23
Q

These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.

A

Dipole to Dipole Forces

24
Q

Are the STRONGEST
the intermolecular force of attraction.

A

DIPOLE-DIPOLE INTERACTIONS

25
Q

a special kind of dipole-dipole interaction that occurs specifically between a
hydrogen atom bonded to either an OXYGEN, NITROGEN, OR FLUORINE ATOM.

A

Hydrogen Bonding

26
Q

Is a relatively strong force of attraction between molecules, and
considerable energy is required to break hydrogen bonds.

A

Hydrogen Bonding

27
Q

Are responsible for holding nucleotide bases together in DNA and RNA.

A

hydrogen bonds

28
Q

Attraction between an ion and a polar molecule.

A

Ion

29
Q

Ions are very similar to ionic bonds, but
tend to be weaker because polar molecules only possess _________________, which generates less electrostatic attraction.

A

partial
electric charge

30
Q

Because of these forces, polar solvents are better able to dissolve
____________ such as NaCl, compared with nonpolar solvents.

A

ionic solids

31
Q

Are better able to dissolve
ionic solids

A

polar solvents

32
Q

Because of these forces, polar solvents are better able to dissolve
ionic solids such as NaCl, compared with nonpolar solvents.

A

Ion

33
Q

there is no what?

A

permanent dipole on the molecule.

34
Q

Can induce a dipole in the neighbouring
molecule, which then interacts with the original transient dipole.

A

Transient dipole

35
Q

PROPERTIES OF SUBSTANCES AFFECTED BY
INTERMOLECULAR FORCES (IMFs)

A
  1. VISCOSITY
  2. SURFACE TENSION
  3. BOILING POINT
  4. MELTING POINT
  5. SOLUBILITY
36
Q

This is a measure of its resistance to flow of a liquid.

A

VISCOSITY

37
Q

The more structurally complex are the molecules in a liquid and __________________, the more difficult it is for them to move past each
other and the________________

A

the stronger the IMFs between them, greater is the viscosity of the liquid.

38
Q

This is the energy required to increase the surface area of a
liquid, or the force required to increase the length of a liquid surface by a given amount.

A

SURFACE TENSION

39
Q

Surface tension results from the ____________ between molecules
at the surface of a liquid, and it causes the surface of a liquid to
behave like a stretched rubber membrane.

A

Cohesive forces

40
Q

Force attracting water
molecules to each other.

A

Cohesion

41
Q

capillary action—when a liquid flows within a
porous material due to the attraction of the liquid molecules to the
the surface of the material and to other liquid molecules.

A

Capillary Action

42
Q

can also
occur when one
end of a small
diameter tube is
immersed in a
liquid.

A

Capillary Action

43
Q

is the temperature at which the vapor pressure
becomes equal to the pressure exerted on the surface of the liquid.

A

Boiling Point

44
Q

as bonds become more
polarized, the charges on the atoms become _______, which leads to
_____________, which leads to___________________

A

greater, greater intermolecular attractions, higher boiling and
melting points.

45
Q

The rule “______________” is applied on the concept of
SOLUBILITY of molecules.

A

like dissolves like

46
Q

Polar solutes dissolve in _____________

A

Polar solvent

47
Q

nonpolar solutes dissolve in __________.

A

nonpolar solvents

2nd Semester (48 decks)

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