INTERMOLECULAR FORCES Flashcards

1
Q

T/F The fundamental
difference between states
of matter is the strength of
the intermolecular forces
of attraction.

A

T

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2
Q

they are referred to as the condensed phases

A

solids and liquids

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3
Q

tendency of an electron cloud to distort

A

polarizability

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4
Q

T/F If something is easier
to polarize, it has a
high boiling point.

A

F

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5
Q

Polar molecules have a more positive and a more negative end–a dipole (two poles, δ + and δ).

A

dipole-dipole interactions

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6
Q

strongest intermolecular force

A

hydrogen bonding

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7
Q

The dipole–dipole interactions experienced when H is bonded to N, O, or F are unusually strong.

A

hydrogen bond

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8
Q

interactions found in solutions of ions

A

ion-dipole interactions

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9
Q

resistance of a liquid to flow

A

viscosity

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9
Q

T/F Viscosity decreases with stronger
intermolecular forces and increases
with higher temperature.

A

F

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10
Q

Water acts as if it
has a “skin” on it
due to extra inward
forces on its
surface.

A

surface tension

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11
Q

Intermolecular forces that bind similar
molecules to one another

A

cohesive forces

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12
Q

Intermolecular forces that bind a
substance to a surface

A

adhesive forces

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13
Q

rise of liquids up narrow tubes

A

capillary actions

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14
Q

T/F Water has stronger
adhesive forces with glass;
mercury has stronger
cohesive forces with itself.

A

T

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15
Q

conversion from one state of matter to another

A

phase change

16
Q

the energy required to change a solid at its melting point to a liquid.

A

heat of fusion

17
Q

the energy required to change a liquid at its boiling point to a gas

A

heat of vaporization

18
Q

the energy required to change a solid directly to a gas

A

heat of sublimation

19
Q

a plot of temperature vs heat added

A

heating curve

20
Q

T/F gases solidify when pressure is applied

A

F

21
Q

The temperature beyond which a gas cannot be compressed

A

critical temperature

22
Q

the pressure needed to compress the liquid at critical temperature

A

critical pressure

23
Q

The normal boiling
point is the temperature at which
its vapor pressure

A

760 torr

24
Q

a graph of pressure vs. temperature for a substance.

A

phase diagram

25
Q

substances that do not go directly from the
solid state to the liquid state.

A

liquid crystals

26
Q

type of liquid crystals where molecules
are only ordered in
one dimension, along the long axis.

A

nematic liquid crystals

27
Q

type of liquid crystals where molecules are
ordered in two dimensions, along the long axis
and in layers.

A

smectic liquid crystals

28
Q

type of liquid crystals where nematic-like
crystals are layered at angles to each other.

A

cholesteryic liquid crystals

29
Q

T/F The stronger the Van der Waals forces, the
more energy is needed to break these forces
and the higher the boiling point.

A

T

30
Q

T/F As with boiling points, the melting points
of the alkanes increase with a decrease
in the number of carbon atoms.

A

F

31
Q

they have higher melting and boiling points than corresponding alkanes

A

alkylhalides

32
Q

they have boiling points similar to that of corresponding Aldehydes and Ketones

A

esters

33
Q

they have boiling points relatively higher than corresponding alcohols

A

carboxylic acids