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Chemistry > Liquids, Solids & Phase Changes > Flashcards

Liquids, Solids & Phase Changes Flashcards

1
Q

Brownian Movement

A

Type of motion

Zigzagging movement of colloidal particles in dispersing medium, as viewed through ultramicroscope

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2
Q

Change of phase (L to G)

A

If a molecule gains enough KE when near surface, it may overcome attractive forces & escape into gas

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3
Q

Viscosity

A

The friction or resistance to motion that exists between the molecules of a liquid when they move past each other

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4
Q

Surface Tension

A

Property resulting from an imbalance of forces at surface of liquid

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5
Q

Capillary Action

A

The attraction of surface of a liquid to surface of a solid

Property related to surface tension

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6
Q

Phase Equilibrium

A

The point in a reversible reaction at which the forward reaction is occurring at same rate as opposing reaction

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7
Q

Dynamic Equilibrium

A

In a closed system, when opposing changes are taking place at equal rates

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8
Q

La Chatelier’s Principle

A

When a system at equilibrium is disturbed by the application of a stress (change in temp., pressure, or conc.), it reacts so as to minimise the stress & attain a new equilibrium position

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9
Q

Equilibrium Vapor Pressure

A

Molecules in vapor that are in equilibrium with liquid at given temperature exert a constant pressure

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10
Q

Boiling Point

A

The temperature at which the liquid’s vapor pressure equals the atmospheric pressure

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11
Q

Critical Temperature

A

The temperature above which the liquid phase of a substance cannot exist

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12
Q

Critical Pressure

A

The minimum pressure required to liquefy a gas at its critical temperature

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13
Q

Crystalline Solids

A

Have a regular structure, in which particles pack in a repeating pattern from one edge of solid to the other

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14
Q

Amorphous Solids

A

Have a random structure, with little if any long-range order

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15
Q

Polycrystalline Solids

A

An aggregate of a large number of small crystals/grains in which structure is regular

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16
Q

Sublimation

A

When heated at certain pressures, some solids vaporize directly without passing through liquid phase

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17
Q

Melting Point

A

The temperature at which atomic/molecular vibrations of a solid become so great that particles break free from fixed position & begin to slide freely over each other in a liquid state

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18
Q

Heat of Fusion

A

Amount of energy required at the melting point temperature to cause the change of phase to occur

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19
Q

Calorimeter

A

An instrument used to measure the amount of heat liberated/absorbed during a change

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20
Q

Molar Heat of Fusion

A

Amount of heat energy required to melt 1 mole of solid at its melting point

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21
Q

Molar Heat of Vaporization

A

Amount of heat energy required to vaporize 1 mole of liquid at its boiling point

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22
Q

Anhydrides

A

Certain oxides that react with water to form 2 classes of compounds - acids & bases

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23
Q

Basic Anhydrides

A

A metallic oxide that forms a base when placed in water

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24
Q

Acidic Anhydrides

A

A nonmetallic oxide that, when placed in water, reacts to form an acid solution

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25
Q

Saturated Solution

A

A solution that contains the maximum amount of solute under existing temperature & pressure

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26
Q

Saturated

A

When substances are dissolved in water to extent that no more will dissolve at that temperature

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27
Q

Solute

A

Substances dissolved

28
Q

Solvent

A

Dissolving medium

29
Q

Unsaturated

A

A solution that contains less solute than a saturated solution, & container will show no undissolved solute

30
Q

Pulverizing

A

Increases surface exposed to solvent

Increase rate of solution making

31
Q

Stirring

A

Bring more solvent that is unsaturated into contact with solute
(Increases rate of solution making)

32
Q

Heating

A

Increases molecular action & gives rise to mixing by convection currents
(Increase rate of solution making)

33
Q

Exothermic (Water solution)

A

Process of going into solution if energy is released in process

34
Q

Endothermic (Water solution)

A

Process of going into solution if energy from water is used to a greater extent than energy is released in freeing the particle

35
Q

Miscible

A

If 2 liquids are mixed & dissolve in each other

36
Q

Immiscible

A

If 2 liquids separate & do not mix

37
Q

Alloy

A

A solid solution made by mixing of 2/more metals, often by melting

38
Q

Liquid

A

Form of matter that has a definite volume & takes the shape of its container

39
Q

Solids

A

Particles are fixed in rather definite positions & maintain definite shapes
Most ordered system

40
Q

Phase Diagram

A

Ties together the effects of temperature & also pressure on the phase changes of a substance

41
Q

Triple Point

A

Only temperature & pressure at which 3 phases of substance can exist in equilibrium with one another in a system containing only the pure substance

42
Q

Distillation

A

Purification of water
Involves the evaporation & condensation of the water molecules
Remove any substance that has a higher boiling point than water

43
Q

Synthesis

A

The formation of a compound by uniting its components

44
Q

Dumas Experiment

A

Showed that hydrogen & oxygen combine to form water in a ratio of 1:8 by mass

45
Q

Heavy Water

A

Contains deuterium (isotope of hydrogen) rather than ordinary hydrogen

46
Q

Hydrogen Peroxide

A

Contains more than usual oxide (per)

H2O2

47
Q

Heat of Vaporization

A

Quantity of heat needed to vaporize 1 gram of liquid at constant temperature & pressure

48
Q

Heat of Fusion

A

The amount of heat required to melt 1 gram of a solid

49
Q

Substance Solubility

A

Need to account amount of solute, solvent & temperature of the solution

50
Q

Equilibrium State

A

When 2 opposing processes (like dissolving & crystallization) equal each other in rate

51
Q

Saturated Solution

A

At equilibrium state, solution is holding the maximum amount of solute that it can contain

52
Q

Unsaturated Solution

A

A solution that contains less solute than saturated solution, container will show no undissolved solute

53
Q

Hydrated Ion

A

Ex; water solutions

Whole group of ions (water molecules that surround ion differ in number for various ions)

54
Q

Dilute

A

Small amount of solute is dispersed in the solvent

55
Q

Concentrated

A

Large amount of solute is dissolved in the solvent

56
Q

Saturated

A

Solution is holding all the solute possible at that temperature

57
Q

Unsaturated

A

More solute can go into solution at that temperature

Solvent has further capacity to hold more solute

58
Q

Supersaturated

A

A solution that contains a greater quantity of solute than is normally possible at a given temperature

59
Q

Molarity

A

Number of moles of a substance dissolved in 1 liter of solution

60
Q

Molality

A

Number of moles of the solute dissolved in 1kg of solvent

61
Q

Mole Fraction

A

Concentration of a component in a solution

62
Q

Colligative Properties

A

Properties that depend primarily on the concentration of particles & not the type of particle

63
Q

Crystal

A

Having a definite molecular or ionic structure

64
Q

Unit Cell

A

Smallest portion of crystal lattice that is repeated throughout the crystal

65
Q

Hydrate

A

A substance that holds a definite proportion of water in its crystal structure

66
Q

Efflorescence

A

The loss by a substance of its water of hydration on exposure to air at ordinary temperature

67
Q

Deliquesence/Hydroscopic

A

The absorption by a substance of water from the air, so that the substance becomes wet

Chemistry (15 decks)

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