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Phy Pharm LEC > (Prelim) States of Matter > Flashcards

(Prelim) States of Matter Flashcards

1
Q

Manifestations of Intermolecular forces:

A
  • Repulsive and Attractive forces
  • Adhesion –attraction of unlike molecules
  • Cohesion –attraction of like molecules
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2
Q

attraction of like molecules

A

Cohesion

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3
Q

attraction of unlike molecules

A

Adhesion

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4
Q

necessary in order that molecules cohere/adhere

A

Attractive forces

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5
Q

necessary in order that the molecules do not
interpenetrate one another.

A

Repulsive forces

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6
Q

due to the interpenetration of the electronic clouds of molecules and increases exponentially with a decrease in distance between the molecules.

A

Repulsion

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7
Q

At certain equilibrium distance, about ________________, the repulsive and attractive forces are equal

A

3 or 4x10-8 cm (3 or 4angstroms)

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8
Q
  • Attraction between nonpolar
    molecules
  • Weakest
A

London Forces

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9
Q

Attractions occur between nonpolar molecules and ions.

A

Ion-induced dipole forces

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9
Q

Types of Intermolecular Forces

A
  1. Van der Waals Forces
  2. Ion-induced dipole forces
  3. Ion-Dipole Forces
  4. Hydrogen Bonding
  5. Hydrophobic Interactions
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10
Q
  • Orientation Effect
  • Attraction between polar molecules
  • Strongest
A

Keesom Forces

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10
Q

3 Van der Waals Forces

A
  • Keesom Forces
  • Debye Forces
  • London Forces
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11
Q
  • Induction effect
  • Attraction between nonpolar and
    polar molecules
A

Debye Forces

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12
Q

involved in the formation of the iodide
complex

A

Ion-induced dipole forces

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13
Q

These types of interactions account in
part for the solubility of ionic crystalline substances in water

A

Ion-induced dipole forces

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14
Q

Attractions occur between polar
molecules and ions.

A

Ion-Dipole Forces

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14
Q

Because of the small size of hydrogen
atom, it can move in close to the electronegative atom and form an electrostatic type of union known as hydrogen bond or hydrogen bridge.

A

Hydrogen Bonding

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15
Q

It is a special type of dipole-dipole in which hydrogen is bonded to an electronegative element.

A

Hydrogen Bonding

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15
Q

Forces of attraction between non
polar atoms and molecules in water.

A

Hydrophobic Interactions

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16
Q

It can exist as Intramolecular and Intermolecular forces of attraction.

A

Hydrogen Bonding

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17
Q

liquid to solid

A

freezing

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17
Q
  • Strongest
  • Definite
  • Definite
  • Vibration
A

Solid

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17
Q

They cause the nonpolar species to
be driven together and are critical for
the structure and stabilization of
many molecules including proteins
(with non-polar amino acids) and
aggregates of amphiphiles.

A

Hydrophobic Interactions

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18
Q

Phases/States

A

Solid
Liquid
Gas

19
Q
  • Melting/fusion
  • Evaporation
  • Condensation
  • Freezing
  • Sublimation
  • Deposition
A

Physical Changes

19
Q
  • Strong
  • Definite
  • Indefinite
  • Gliding/flowing
A

Liquid

19
Q
  • Weakest
  • Indefinite
  • Indefinite
  • Constant random motion
A

Gas

20
Q

gas to solid

A

deposition

21
Q

solid to liquid

A

melting

22
Q

solid to gas

A

sublimation

23
Q

gas to liquid

A

condensation

24
Q

liquid to gas

A

evaporation

25
Q
  • Higher kinetic energy
  • Held together by weak
    intermolecular forces.
  • Have no regular shape.
  • Compressible
  • Invisible
A

Characteristics of Gases

26
Q

7 Gas Laws

A
  1. Boyle’s Law
  2. Charles’s Law
  3. Gay-Lusaac’s Law
  4. Combined Gas Law
  5. Ideal Gas Law
  6. Avogadro’s Law
  7. Dalton’s Law of Partial Pressure
27
Q

states that the pressure and absolute temperature of a given mass of a gas at constant volume are directly proportional

A

Gay-Lusaac’s Law

28
Q

relates the volume and pressure of a given mass of gas at constant temperature.

A

Boyle’s Law

29
Q

states that the volume and absolute temperature of a given mass of
a gas at constant pressure are directly proportional.

A

Charles’s Law

30
Q

the summary of the relationship of the three gas laws presented earlier.

A

Combined Gas Law

31
Q

infinite volume = non-attracting molecules

A

Ideal Gas Law

32
Q

universal gas constant

A

0.08205 𝑳𝒂𝒕𝒎/𝒎𝒐𝒍𝑲

33
Q

𝑉= n

A

Avogadro’s Law

34
Q

The total pressure (Pt) is the sum of the individual partial pressure of each component in the system.

A

Dalton’s Law of Partial Pressure

34
Q

1 mole =

A

6.02 x 1023

35
Q

The theory was developed to explain the behavior of gases and supported the validity of the gas laws

A

Kinetic Molecular Theory

36
Q

Gases are composed of particles called molecules, the total volume of which is so small as to be negligible in relation to
the volume of the space in which the molecules are confined

A

Kinetic Molecular Theory

37
Q

The particles of the gas do not attract one another but rather move with complete independence

A

Kinetic Molecular Theory

38
Q

The particles exhibit continuous random motion owing the kinetic energy. The average kinetic energy is directly proportional to the absolute temperature of the gas.

A

Kinetic Molecular Theory

38
Q

composed of particles called molecules

A

Gases

39
Q

The molecules exhibit perfect elasticity, that is, there is no net loss of speed after they collide with one another and with the walls of the confining vessel, which latter effect accounts for the gas pressure. Although the net velocity, and therefore the average kinetic energy, does not change in collision, the speed and energy of the individual molecules may differ widely at any instant.

A

Kinetic Molecular Theory

40
Q

have low internal pressures and are not able to over come the powerful cohesive forces of the polar solvent molecules.

A

Nonpolar molecules

40
Q

type of matter with specific properties that make it less rigid than a solid but more rigid than a gas.

A

Liquid State

40
Q

have high internal pressures and serve as solvents only for substances of similar internal pressures

A

Polar liquids

41
Q

maximum temperature, above
which a liquid can no longer
exist

A

Critical Temperature

42
Q

critical temperature of water:__________;
critical pressure: __________

A

374°C or 647°K;
218 atm

43
Q

pressure required to liquefy a gas at its critical temperature, which is also the highest vapor pressure that the liquid can have.

A

Critical Pressure

44
Q
A
45
Q
A
46
Q
A

Phy Pharm LEC (4 decks)

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