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chem S.Horvath > states of matter > Flashcards

states of matter Flashcards

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1
Q

what holds molecules rigidly in place in solids

A

intermolecular forces

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2
Q

liquids volume and shape

A

definite volume, no definite shape

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3
Q

molecules in liquids

A

very close together, but can flow past each other

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4
Q

intermolecular forces on liquids

A

strong enough to hold molecules in a condensed phase. not strong enough to prevent molecules from sliding past each other

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5
Q

gases shape/volume

A

no definite shape/volume

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6
Q

intermolecular forces in gases

A

essentially zero between gases and molecules

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7
Q

ionic bonds

A

results from coulombic attraction between oppositely charged ions

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8
Q

ionic compounds are almost always

A

solids

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9
Q

covalent bonds result from

A

sharing one or more pairs of electrons

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10
Q

octet rule

A

states that atoms want to be a noble gas. or at least have a noble gas configuration - species with the same electron configuration are termed isoelectric - this is achieved by giving each atom access to 8 electrons

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11
Q

species with the same electron configurations are termed

A

isoelectric

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12
Q

??octet rule is achieved by giving each atom access to

A

8 electrons

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13
Q

kinetic molecular theory of matter

A

attempts to describe all the states of matter and the conversion between them

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14
Q

valence bond theory

A

a covalent bond results from the overlap of two electron clouds. this allows the electron on 1 atom to spend time around atom 2’s nucleus and vice versa

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15
Q

VSEPR theory

A

valence shell electron pair theory. atoms are bound into molecules by electrons. electrons repel each other. therefore the groups bonded to a central atom try to get as far apart from each other as possible. the goal is to minimize electron pair repulsion around a given central atom

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16
Q

electronegativity

A

the tendency of an atom in a molecule to attract shared electrons to itself.

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17
Q

what is most electronegative element

A

fluorine - the closer an atom is to fluorine, the more electronegative it is

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18
Q

intermolecular forces

A

attractive forces between molecules or atoms or ions

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19
Q

London forces are created by

A

instantaneous dipoles

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20
Q

london forces get stronger with

A

larger atoms/ molecules

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21
Q

london forces are much weaker than

A

dipole-dipole or H-bonding

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22
Q

hydrogen bonding strength

A

generally stronger than dipolar attractins

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23
Q

hydrogen bonding is

A

the attraction between a hydrogen bonded directly to an O, N, or F and another electronegative atom

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24
Q

ion dipole attraction

A

the attraction between an ionic charge and a polar molecule

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25
Q

ion dipole attraction allows

A

ionic solids to dissolve in water

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26
Q

hydrogen bodies in a negative way cause

A

atelectasis

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27
Q

like desolves

A

like

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28
Q

more intermolecular forces does what to boiling and melting points

A

higher

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29
Q

substances with greater intermolecular attraction have greater

A

surface tensions

30
Q

a molecule near the surface of a droplet will experience

A

net inward force

31
Q

surface tension will allow an object having a greater density than a liquid to

A

float in the liquid

32
Q

LaPlace’s law

A

when the liquid is in contact with another surface, this curling creates a pressure difference which is described by La Place’s law.

33
Q

LaPlace’s law can be used to explain

A

why the surface tension on a blood vessel wall will depend on the radius of the vessel.

34
Q

the tension on the surface of the blood vessel is ____ proportional to the radius of the vessel

A

directly

35
Q

wall tension is proportionate to

A

radius (laPlace’s law)

36
Q

as the radius increases, wall tension

A

increases

37
Q

soap makeup

A

polar (hydrophilic) head and non-polar (hydrophobic, greasy) tail

38
Q

monolayers

A

the greasy tails stick out of the surface of water, which breaks down the surface tension of water

39
Q

micelles

A

tails can dissolve in each other forming a sphere. this creates a non-polar microenvironment in the water

40
Q

vapor pressures

A

the most energetic molecules in a liquid have sufficient kinetic energy to escape from the surface of a liquid into the gas phase, and once the molecules are free as gases, they exert a pressure.

41
Q

as temp increases, vapor pressures

A

increase. calusius-clapeyron equation

42
Q

the process of evaportion in a closed container will proceed until

A

there are as many molecules returning to the liquid as there are escaping. (saturated vapor pressure)

43
Q

the temp at which the vapor pressure is equal to the atmospheric pressure is

A

boiling point

44
Q

dynamic equilibrium

A

when there is a balance between vaporization and condensation

45
Q

aneurysm application to laplace?

A

they are approximately spherical, so the tension on the wall of the aneurysm rises as the radius is divided by two. so, while not a good diagnosis, they represent a physical means for lowering the tension on a blood vessel

46
Q

capillary being smaller will withstand pressure better than

A

larger artery or vein

47
Q

volatility

A

the tendency of liquid to evaporate

48
Q

volatility

A

the tendency of liquid to evaporate

49
Q

solid to liquid

A

melting

50
Q

liquid to solid

A

freezing

51
Q

liquid to gas

A

vaporization

52
Q

gas to liquid

A

condensation

53
Q

solid to gas

A

sublimation

54
Q

gas to solid

A

deposition

55
Q

what does temp do to vapor pressure

A

increases

56
Q

vaporization is an _____ process

A

endothermic

57
Q

the unit of energy for vaporization (Hvap) represents

A

the energy needed to break intermolecular forces and allow molecules to escape into the gas phase

58
Q

fusion

A

endothermic - solid to liquid

59
Q

760

A

atmospheric pressure

60
Q

phase diagrams show

A

combined effects of temp and pressure on the state of matter

61
Q

which gas has the highest vapor pressure

A

desflurane 669

62
Q

vapor pressure of isoflurane

A

239

63
Q

vapor pressure of sevoflurane

A

157

64
Q

triple point of phase diagram of water

A

the single temp and pressure combination where all three phases an exist in equilibrium with each other

65
Q

critical point

A

when temp and pressure exceed critical point, system becomes a supercritical fluid… have the flow properties of gases but densities similar to liquids and no surface tension

66
Q

as diameter of a tube decreases, speed

A

increases

67
Q

if an object sinks, boyount force is

A

smaller

68
Q

if an object floats, boyount force is

A

larger

69
Q

as the speed of a fluid increases, the pressure exerted by the fluid

A

decreases (bernoulli effect)

70
Q

bernoulli effect

A

as the speed of a fluid increases, the pressure exerted by the fluid decreases

71
Q

venturi flowmeter is explained by

A

bernoulli effect

chem S.Horvath (11 decks)

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