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flashcards! > Ap Chem Ch. 10-11 > Flashcards

Ap Chem Ch. 10-11 Flashcards

0
Q

Force(massXacceleration) acting on an object per unit area.

A

Pressure-

                   P=f/a
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1
Q

4 properties of gases:

A
  • expand to fill their containers
  • highly compressible
  • always mix homogeneous with other gases
  • only occupy a small fraction of the actual volume of their container
  • extremely low densities
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2
Q

Weight of air per unit of area

A

Atmospheric pressure

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3
Q

Pascals-SI units

A

1 Pa= 1 N/m^2

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4
Q

Bar

A

1 bar= 10^5 Pa= 100 kPa

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5
Q

Difference in the heights measured in mm(h) of two connected columns of mercury

A

mm Hg , torr

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6
Q

Normal atmospheric pressure at sea level

A

Standard pressure

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7
Q

Convertions for standard pressure

A

1 atm = 760 torr = 760 mm Hg = 101.325 kPa

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8
Q

Volume is _________ proportional to Pressure.

A

Inversly

  P1V2=P2V2
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9
Q

Voulme is ___________ proportional to temperature

A

Directly

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10
Q

The volume of a gas at constant temperature and pressure is _________ proportional to the number of moles of the gas.

A

Directly

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11
Q

Pressure is ________ proportional to kelvin temperature.

A

Directly

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12
Q

Charles’ law

A

V1 V2
➖ = ➖
T2 T2

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13
Q

Boyle’s law

A

P1V2=P2V2

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14
Q

Gay-lussac’ law

A

P1 P2
➖ = ➖
T2 T2

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15
Q

The product of the pressure and volume of a fixed quantity of gas is ______ proportional to the kelvin temperature.

A

Directly

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16
Q

Conbined gas law

A

P1V1 P2V2
➖➖ = ➖➖
T1 T2

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17
Q

Ideal gas law:

A

PV=nRT

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18
Q

Constants for R( ideal gas constant)

A

.08206 L(atm) / mol( k)

  1. 314 L(kPa) / mol(k)
  2. 36 L(mm Hg) / mol(k)
  3. 314 J / mol(k)
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19
Q

Solving for the volume of 1 MOL at standard temperature and pressure (STP) gives 22.41 L / mol

A

Standard molar volume

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20
Q

Molar mass form of ideal gas law

A

M= mRT
——
PV

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21
Q

Density form of the idal gas law

A

D= MP
—–
RT

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22
Q

In which cases would you know you have to use Gas stoichiometry ?

A
  • they have to be at constant pressure and temperature

* look for an equation

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23
Q

The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone.

A

Dalton’s law of partial pressures

P(total)= P1+P2+P3…

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24
Q

Gases consist of large numbers of molecules that are in continuous, random ______.

A

Motion

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25
Q

The speed of a molecule possessing AVERAGE KINETIC ENERGY.

A

Root-mean-square speed

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26
Q

The escape of gas molecules through a tiny hole into an evacuated space.

A

Effusion

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27
Q

The spread of one substance throughout a space or throughout a second substance.

A

Diffusion

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28
Q

Which diffuse faster, lighter molecules or heavier molecules??

A

Lighter molecules

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29
Q

Distance between collisions

A

Mean free path

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30
Q

Root-mean-square speed equation

A

______
u= | 3rT
—-
M

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31
Q

Properties of solids

A
  • Definite shape and volume
  • ordered arrangement
  • fixed positions
  • virtually incompressible
  • Diffusion occurs extreamly slowly
  • close together
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32
Q

Properties of liquids

A
  • Definite volume, but takes shape of container
  • disorder
  • virtually incompressible
  • Flows readily
  • diffusion occurs slowly
  • particles close together
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33
Q

The state a substance is in at a particular temperature and pressure depends on the balance of 2 antagonistic entities:

A
  • The kinetic energy of the particles

- the strength of the attractions between particles

34
Q

Attractions BETWEEN molecules.

Weaker!

A

Intermolecular forces

35
Q

Attraction WITHIN molecules

Stronger!

A

Intramolecular forces

36
Q

However intermolecular forces are able to control physical properties such as:

A
  • boiling point
  • melting point
  • vapor pressures
  • viscosities
37
Q

The intermolecular forces that exist between NEUTRAL molecules.

A

Van Der Waals forces

38
Q

Examples of van der waals forces from weakest to strongest

A
  1. London didpersion forces
  2. Dipole-Dipole interactions
  3. Hydrogen bonding
39
Q

Other electrostatic attractions, polar molecule to ion attraction.
These are important in solutions of ions

A

Ion-Dipole

40
Q

Other electrostatic attractions, ion to ion bonding

A

Ionic Bonding

41
Q

Molecules that have permanent _______ are attracted to each other.

A

Dipoles

42
Q

The ______ end of one dipole is attracted to the _____ of the other and vice-versa.

A

Positive

Negative

43
Q

The more polar the molecule, the _______ is its melting point.

A

Higher

44
Q

Attractions between an instantaneous dipole( uneven dispersion of electrons ) and an induced dipole.
-these forces are present in all molecules, whether they are polar or nonpolar

A

London dispersion forces.

45
Q

The ease in which an electron colud can be deformed

A

Polarizability

46
Q

The _______ of a molecule affects the strength of dispersion forces.

A

Shape

47
Q

Larger atoms have larger electron clouds which are easier to _________.

A

Polarize

48
Q

If two molecules are of comparable size, __________ interactions are probably the dominating force.

A

Dipole-dipole

49
Q

If one molecule is much larger than another, _______ forces will likely determine its physical properties.

A

dispersion

50
Q

Dipole-dipole interactions where H is bonded to N,O, or F

A

Hydrogen bonding

51
Q

Hydrogen bonding arises in part from the high _____________ of nitrogen, oxygen ,and fluorine.

A

Electronegativity

52
Q

Hydrogen bonding also arises when hydrogen is bonded to the very electronegative elements, the hydrogen nucleous is _____.

A

Exposed

53
Q

Resistance of a liquid to flow.

A

Vsicosity

54
Q

As intermolecular forces increases, viscosity _______.

A

Increases

55
Q

Increase in temperature will _______ surface tension

A

Decrease

56
Q

The greater the intermolecular forces, the ________ the surface tension.

A

Greater

57
Q

Intermolecular forces that bond similar molecules to one another.

A

Cohesive forces

58
Q

Intermolecular forces between a substance and a different surface

A

Adhesive forces

59
Q

The greateradhesive forces allow water to be drawn up the narrow tube.

A

Capillary action

60
Q

Energy required to change a solid at it’s melting point to a liquid.

A

Heat of fusion

61
Q

Energy required to change a liquid at it’s boiling point to a gas

A

Heat of vaporization

62
Q

Why is vaporization larger than fusion?

A

Breaks intermolecular forces completely

63
Q

The stronger __________ the more energy you have to take to change states.

A

Intermolecular forces

64
Q

Energy needed to vaporize 1 mole of a liquid.

A

Molar heat of vaporization

= 40.7 kJ/ mol

65
Q

Energy that must be removed to condense 1 mole of a gas

A

Molar heat of condensation.

=-40.7 kJ/mol

66
Q

Energy needed to melt 1 mole of a substance.

A

Molar heat of fusion

= 6.01 kJ/mol

67
Q

Energy that must be removed to freeze 1 mole of a substance.

A

Molar heat of solidification

=-6.01 kJ/mol

68
Q

What does adding heat to a system at the melting and boiling points result in?

A

Results in pulling the molecules farther apart from each other.

69
Q

Kinetic energy is spent as ________ in state changes.

A

Potential energy

70
Q

If kinetic energy is constant while changing states, so is _______

A

Temperature

71
Q

What equation is used to calculate state changes when KE and temp. Are constant.

A

q= (

72
Q

Energy while in a single state equation

A

q= (m)(c)(

73
Q

Highest temperature that a liquid phase can form.

A

Critical Temperature

74
Q

Pressure needed to cause liquefaction at the critical temperature.

A

Critical pressure

75
Q

Weaker forces ➡️ ________ critical points

A

Lower

76
Q

As more molecules escape the liquid, the pressure they exert _______.

A

Increases

77
Q

In a closed system, the liquid and vapor reach a state in ehich liquid molecules evaporate and vapor molecules condense at the same rate.

A

Dynamic equilibrium

78
Q

The temperature of a liquid at which it’s vapor pressure equals atmospheric pressure.

A

The boiling point

79
Q

The temperature at which a substance vapor pressure is 760 torr.

A

Normal boiling point

80
Q

The point in which all three states are in equilibrium

A

Triple point

81
Q

Above critical temperature and critical pressure the liquid and vapor are indistinguishable from each other.

A

Critical point

82
Q

Solids in which particles are in highly ordered arrangement

A

Crystalline

83
Q

Solids in which there is no particular order in the arrangement of particles.

A

Amorphus

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