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Bettel Plus Chang Chemistry > 6. Gases, Liquids, and Solids > Flashcards

6. Gases, Liquids, and Solids Flashcards

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1
Q

Attractive forces that hold matter together…

A

-counteracts kinetic energy
-in the absence of attractive forces, the kinetic energy keeps the particles constantly moving randomly

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2
Q

Kinetic energy increases…

A

with increasing temperature

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3
Q

Gaseous state

A

-at high temperature:
molecules possess high kinetic energy; moves fast, attractive forces weak

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4
Q

Liquid state

A

-at lower temperature:
molecules move more slowly, attractive forces is stronger than gaseous state

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5
Q

Solid state

A

-at even lower temperature:
molecules no longer have velocity to move past each other
-strong attractive forces

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6
Q

Pressure

A

-force per unit area exerted against a surface

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7
Q

Barometer

A

-measure atmospheric pressure
-long glass tube that is completely filled with mercury then inverted into a pool of mercury in a dish
-measure of Mercury rise in tube= cmHg/inHg/mmHg (measure of pressure)

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8
Q

Evangelista Torricelli

A

-torr
-invented barometer

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9
Q

Manometer

A

-measure the pressure of gas in a container
-uses mercury as working fluid due to its very high density (height of liquid volume inversely proportional to liguid density); para small barometers and manometers lng

  1. Open-tube manometer: suited for measuring pressures equal or greater than atmospheric pressure
    Pgas = Pheight + Patm
  2. Closed-tube manometer: measuring pressure below atmospheric (vacuum)
    Pgas = Ph
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10
Q

Boyle’s law
Robert Boyle

A

-for a fixed mass of gas at T=k,
⬆️ V ⬇️ P

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11
Q

Charles’s law
Jacques Alexandre Cesar Charles

A

-for a fixed mass of gas at P=k,
⬆️ V ⬇️ T

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12
Q

Gay-Lussac’s law
Joseph Louis Gay-Lussac

A

-for a fixed mass of gas at V=k,
⬆️P ⬇️T

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13
Q

Avogadro’s law

A

-equal volumes of gases at same temperature and pressure contain equal number of molecules, regardless of their identity

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14
Q

Standard temperature and pressure (STP)

A

-1 bar, 0°C
-all gases at STP or any other combination of T and P contain the same number of molecules at any given volume

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15
Q

Ideal gas

A

-a gas whose physical properties are described accurately by the ideal gas law

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16
Q

Ideal gas condition

A

-Real gases behave most like ideal gases at LOW PRESSURE (1 atm or less) and HIGH TEMPERATURE (300K or higher)

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17
Q

Partial pressure

A

-the pressure that a gas in a mixture of gases would exert if it were alone in the container

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18
Q

Dalton’s law of partial pressure

A

-total pressure is the sum of the partial pressures of each individual gas

PT = Pa + Pb +….

Pi = xi.PT

where xi: mole fraction of gas

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19
Q

Kinetic molecular theory
(Idealized picture of molecules of gases)

A
  1. Gases consist of particles, either atoms or molecules, constantly moving through space in straight lines, random direction, and various speeds
  2. The average kinetic energy of gss particles is proportional to temperature in kelvins
  3. Molecules collide with each other. Each time they collide, they may exchange kinetic energy but the total kinetic energy of the gas sample remains the same
  4. Gas particles have no volume
  5. There are no attractive forces between gas particles
  6. Molecules collide with the walls of the container, and these collisions constitute the pressure of a gas
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20
Q

Ideal gas

A

-at STP, most real gases behave in such a way that an ideal gas would

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21
Q

Condensation

A

-change of a substance from the vapor or gaseous state to the liquid state

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22
Q

Solidification/ Crystallization

A

Change from liquid to solid

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23
Q

London dispersion forces

A

-Fritz London
-extremely weak attractive forces between atoms or molecules caused by electrostatic attraction between temporary induced dipoles
-exist between all molecules
-only forces of attraction in nonpolar molecules

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24
Q

Dipole-dipole interactions

A

-attraction between positive end of a dipole of one one molecule and negative end of another dipole in the same or different molecule

25
Q

Hydrogen bond

A

-a noncovalent force of attraction between the partial positive charge on a hydrogen atom bonded to an atom of high electronegativity (O,N,F) and a partial negative charge on a nearby O,N,F

26
Q

Liquids at molecular level

A

-incompressible
-density of liquids are much greater tgan gases because same mass occupies a smaller volume in liquid form

27
Q

Surface tension

A

-directly related to strength of intermolecular attraction between its molecules
-tendency of fluid surface to shrink into minimum surface area possible

28
Q

Vapor pressure

A

-the pressure of a gas in equilibrium with its liquid form in a closed container

*at equilibrium, the rate of vaporixation equals the rate of liquefaction

29
Q

Boiling point

A

-temperature at which the vapor pressure of a liquid is equal to the pressure of the atmosphere in contact with its surface

30
Q

Normal boiling point

A

Temperature at which a liquid boils under a pressure of 1 atm

31
Q

Factors that affect boiling point

A
  1. Intermolecular forces (esp for molecules having similar molecular weight).
    ⬆️ Intermolecular force, ⬆️ Boiling point
  2. Number of sites for intermolecular interaction, (surface area).
    ⬆️ Surface area ⬆️ Boiling point
  3. Molecular shape
    (i.e. pentane (linear shape) vs 2,2-dimethylpropane (spherical shape); pentane higher b.pt. since larger surface area)
32
Q

Carbon

A

-five crystalline form
(i.e. diamond and graphite, buckyball, nanotubes, soot; carbon atoms are packed differently)

33
Q

Buckyballs

A

-60 carbon atoms named buckminsterfullerene “buckyball”

-named after Buckminster Fuller for his invention geodesic domes (similar structure as buckyball)

34
Q

Fullerenes

A

-cage like structures containing 72, 80, and even larger atoms

35
Q

Nanotube

A

-new variations of fullerene
-cross section of each tube is only 10^(-9) m
-industrial interest due to optical and electronic property

36
Q

Soot

A

-solidifies directly out of carbon vapor
-amorphous solid

37
Q

Types of Solids
1. Ionic

A
  • ions in a a crystal lattice
    -high melting point
    -NaCl, K2SO4
38
Q

Types of Solids
2. Molecular

A

-molecules in a crystal lattice shape
-low melting point
-ice, aspirin

39
Q

Types of Solids
3. Polymeric

A

-giant molecules
-can be crystalline, semicrystalline, amorphous
-low melting point or cannot be melted
-soft or hard
-rubber, plastic, proteins

40
Q

Types of Solids
4. Network

A

-very large number of atoms connected by covalent bonds
-very hard
-very high melting point or cannot be melted
-diamond, quartz

41
Q

Types of Solids
5. Amorphous

A

-randomly arranged atoms or molecules
-mostly soft, can be made to flow, no melting point
-soot, tar, glass

42
Q

Phase change

A

-change from one physical state to another

43
Q

Heat of fusion/ melting

A

-heat necessary to melt 1.0g of any solid

44
Q

Specific heat

A

-heat required to raise the temperature of 1g of fluud sample

45
Q

Heat of vaporization

A

-amount of heat necessary to vaporize 1.0 g of liquid at its normal boiling point

46
Q

Sublimation

A

-transition from solid state directly to vapor state
-solids usually sublime only at reduced pressures (less than 1 atm)

47
Q

Phase diagram

A

-Pressure (y) against temperature (x)
-solid liquid vapor

48
Q

Triple point

A

All three phases coexist

49
Q

For water:

A

Specific heat of ice
0.48 cal/g °C

Heat of fusion of ice
80 cal/g

Specific heat of liquid water
1.0 cal/g °C

Heat of vaporization
540 cal/g

Specific heat of steam
0.48 cal/g °C

50
Q

Gas vs Vapor

A

•Gas- substance that is normally in gaseous state at ordinary temperatures and pressures

•Vapor- gaseous form of any substance that is a liquid or a solid at normal temperature.

51
Q

Atmospheric pressure

A

-pressure exerted by Earth’s atmosphere

-depends on locations, temperature, and condition

-atmosphere is much denser near the surface of the Earth than at high altitudes;
denser air, greater pressure it exerts

52
Q

Absolute zero

A

-Lowest attainable temperature (theoretically) (-273.15°C)

53
Q

Absolute temperature scale/
Kelvin temperature scale
-William Thomson, Lord Kelvin

A

-absolute zero as starting point

54
Q

Molar mass of unknown substance

A

-bulb of known volume is filled with unknown gas
-temperature and pressure
-total mass of bulb plus gas
-mass of empty bulb
-difference of total mass and mass empty = mass of gas
-density of gas = mass of gas/ volume of bulb

Molar mass = (density.R.T) / P

55
Q

Scuba diving and gas laws

A

•Application of Boyle’s Law
33 ft of seawater = 1 atm pressure
⬆️ Pressure ⬆️ Depth
-divers must ascend slowly to adjust to decreasing pressure
-otherwise, rupture membranes of lungs due to air expansion; OR air embolism (air forced into capillaries, blocking normal blood flow) resulting to lost of consciousness

•Application of partial pressure
-body functions best when
PO2 = 0.20 atm
-when diver submerged, pressure of water on diver is greater than atmospheric pressure
-special valve adjusts pressure air breathed from scuba tank to ensure air pressure = water pressure all times (adjusts oxygen content in air breathed in terms of %volume) -otherwise, body cavities like lungs and sinuses will collpase

56
Q

Gas pressure

A

-result of collissions between molecules and the walls of their containers
-depends on frequency of collission per unit area and how hard molecules hit the wall
⬆️Temperature ⬆️KE of molecules
⬆️Speed of molecules

57
Q

Maxwell speed distribution

A

-at given temperature, distribution curve tells us the number of molecules moving at certain speed

-peak of each curve
MOST PROBABLE SPEED: speed of the largest number of molecules
⬆️ Temp, ⬆️ Most probable speed
(As temp increases, the peak shifts toward right and the curve flattens out, indicating larger number of molecules are moving at greater speed)

58
Q

Root-mean-square speed

A

-average molecular speed at any temperature

•Earth, unlike Jupiter, doesn’t have appreciable amount of Hydrogen/ Helium
-weaker gravitational attraction, smaller escape velocity required
-average speed of He exceeds Ni and O2, so trace amount of He found in atmosphere

59
Q

Diffusion

A

-gradual mixing of molecules of one gas with molecules of another by virtue of their kinetic properties

-region of higher concentration to one of lower concentration

Bettel Plus Chang Chemistry (19 decks)

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