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Reviewer > CHEM Exam > Flashcards

CHEM Exam Flashcards

1
Q

attractive forces between molecules/particles in the solid or liquid states

A

Intermolecular Forces

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2
Q

weak intermolecular force

A

Van Der Waals

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3
Q

holds atom together in a molecule

A

Intramolecular Forces

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4
Q

strongest polar
one end of dipole attracts oppositely charged end of another
↳between polar molecules opposite polar compound
polar, boiling point

A

Dipole-Dipole Forces

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5
Q

hydrogen + highly electronegative non metal atom H+N/F/O

A

Hydrogen Bonding

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6
Q

explains solubility of ionic compounds in water

A

Ion-Dipole Forces

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7
Q

“Dipole-induced Dipole Attraction”
weakest
same element

A

London-Dispersion

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8
Q

atoms/ion/molecules are ordered in well-defined arrangements
flat surfaces/faces that make definite angles.
I regular shapes

A

Crystalline Solid

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9
Q

-particles have no orderly structure
-blacks well-derived faces/shapes
-mixture of molecules that do not stack together well
-large complicated molecules
-intermolecular forces vary at strength
-soften over a temperature range
-does not melt at a specific temperature

A

Amorphous Solid

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10
Q

Examples of Crystalline Solids

A

Quartz
Mica
Calcium Fluoride
Snowflakes
Bismuth
Calcite
Sugar
Mica
Diamonds
Rock
Silicon Dioxide

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11
Q

Examples of Amorphous Solids

A

Glass
Plastics
Gels
Rubber
Amorphous Metals
pitch
Foams
Thin Film Coatings
silicon Dioxide
*some types of wax (in certain forms)

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12
Q

alloys cooled rapidly to prevent crystal formation
-used in electrical applications; high-strength materials

A

*amorphous metals (metallic glasses)

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13
Q

used in optics & electronics, such as anti-reflective coatings

A

Thin Film Coatings

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14
Q

viscous, tar-like substance

A

Pitch

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15
Q

Definition of amorphous and crystalline

A

Amorphous
lacks crystalline structure

Crystalline
ordered structure and symmetry

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16
Q

Repeating unit of amorphous and crystalline

A

Amorphous
no repeating unit

Crystalline
one repeating unit

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17
Q

Melting point of amorphous and crystalline

A

Amorphous
No sharp melting point

Crystalline
has a sharp melting point

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18
Q

Chemical nature of amorphous and crystalline

A

Amorphous
Anisotropic

Crystalline
Isotropic

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19
Q

-tension of a surface film due to the attraction of the molecules of the surface than another substance
-allows object with high density to float on water without submerging

A

Surface Tension

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20
Q

-“thickness”
-resistance of liquid to deformation/flow/change into another shape

A

Viscosity

21
Q

-pressure exerted by gas in equilibrium with a liquid enclosed at a certain temperature
-tendency of liquid to change into gaseous state

A

Vapor Pressure

22
Q

heat absorbed by a molt of a substance while being converted from liquid to gas

A

Molar Heat of Vaporization

22
Q

-temperature where the liquid turns into gaseous state due to boiling
-Where the vapor pressure and gas above it is equal

A

Boiling Point

23
Q

-bind similar molecules

A

Cohesive Forces

23
Q

energy required to increase the surface area of a liquid by unit amount
*7.29 x 102 J/m² must be supplied to increase surface area of a given amount of water by 1m²

A

Surface tension

24
Q

-bind a substance to a surface

A

Adhesive Forces

24
Q

-rise of liquids up very narrow tubes

A

Capillary action

25
Q

resistance of a liquid to flow
Viscosity (UP) Temperature (DOWN)
Viscosity (UP) Slowly the liquid flows (UP)

A

Viscosity

26
Q

temperature drops, molecules in gas phase come together and form a liquid

A

Condensation

27
Q

liquid to gas

A

Vaporization

28
Q

-temperature drops, particles move more slowly and become fixed in position

A

Freezing

29
Q

solid to liquid

A

Melting

30
Q

-solid CO₂ changes into gas at ordinary condition

A

Sublimation

31
Q

gas into solid

A

Deposition

32
Q

homogeneous mixtures of 2 or more substances

A

Solution

33
Q

dispersed uniformly throughout the solvent

A

Solute

34
Q

pulls solute particles and surrounds/solvates them

A

Solvent

35
Q

substance that when dissolved in water, results in a solution that can conduct electricity

A

Electrolyte

36
Q

substance that results in a solution that does not conduct electricity

A

Non Electrolyte

37
Q

3 interactions in the solution processes

A

SOLVENT-SOLVENT
SOLUTE-SOLUTE
SOLVENT-SOLUTE

38
Q

absorbs heat

A

Endothermic Processes

39
Q

releases heat

A

Exothermic Processes

40
Q

solvent holds maximum amount of solute at a given temperature
dynamic solute is in dynamic equilibrium with solid solute particles

A

Saturated Solution

41
Q

contains less solute than the maximum capacity of solute the solvent can dissolve at a spec. temp.

A

Unsaturated Solution

42
Q

solvent holds more solute man is normally possible at that temperature

A

Supersaturated Solution

43
Q

*Polar substances tend to dissolve in polar solvents and nonpolar
substances tend to dissolve in nonpolar solvents. the more similar the intermolecular attractions, the more likely I substance is to be soluble in another

A

“LIKE DISSOLVES LIKE”

44
Q

separation of mixture into substances into pure components on the basis of their differing solubility

A

Fractional Crystallization

45
Q

Sg=kPg

A

Henry’s Law

46
Q

-depend on concentration of a solution
normal FP lower FP(Freezing ft. Depression) normal BP higher BP(boiling ft. Elevation)

A

Colligative Properties

Reviewer (41 decks)

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