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Chemistry > Phases > Flashcards

Phases Flashcards

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1
Q

Liquid vs gas

A

Less volume more intermolecular interaction, so expands and contracts only slightly with temp change, move in Brownian motion, fast moving molecules with high KE escape into gas = liquid cools

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2
Q

Viscosity

A

Friction or resistance to motion between liquid molecules, ^attraction ^viscosity IMF, hydrogen bonds=higher viscosity=stronger (water), lower = alcohol, gasoline

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3
Q

Surface tension

A

Molecules at surface of liquid experience attractive forces downwards/inwards/sideways along surface. Molecules at center=uniformly distributed forces. IMBALANCE=surface tension. ^suface tension ^ability to support objects on surface

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4
Q

Capillary action

A

Attraction of surface of liquid to surface of solid, against gravity. Continues until weight of the liquid balances the gravitational force (paper chromatography, meniscus)

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5
Q

Phase equilibrium

A

Equal rate of evaporation and condensation

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6
Q

Dynamic equilibrium

A

Closed system, opposing charges @ equal rates. High temp=more molecules at gaseous phase, but rate of evap and consensation equal (equilibrium vapor pressure)

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7
Q

Boiling point

A

Liquid vapor pressure=atmospheric pressure

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8
Q

Critical temperature

A

Temperature above where a liquid can’t exist above it despite pressure (far right on chart)

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9
Q

Critical pressure

A

Minimum pressure required to liquid gas at critical temperature (far top chart)

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10
Q

Crystalline solids

A

3D like brick wall, regular structure, repeating pattern

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11
Q

Amorphous solid

A

Random structure

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12
Q

Polycrystalline solid

A

Aggregate of regularly structured small crystals in a random fashion

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13
Q

Solid diffusion

A

Particles vibrate/may diffuse through (Gold on lead) NOT in strong ionic bonds (NaCl) or covalent bonds in network solids (diamond)

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14
Q

Sublimation

A

Solid>vapor (carbon dioxide and iodine, high VP)

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15
Q

Melting point

A

Vapor pressure of solid=VP liquid, heat of fusion (depends on nature of bonds)

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16
Q

Heavy water

A

Deuterium D (isotope of hydrogen), one proton and 1 NEUTRON rather than just 1 proton
Tritium, one proton 2 NEUTRONS
(Use in nuclear energy)

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17
Q

Hydrogen peroxide

A

Bleaching and oxidizing agent H2O2

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18
Q

Solution

A

Homogeneous, one substance dissolved in another

19
Q

Aqueous solution

A

Transparent, transition metals have color (salts), pass through filter paper…separate through distillation

20
Q

Solubility

A

g solute/100 mL or g H2O, temperature dependent

21
Q

Solvation

A

Solvent surrounds/separated split (molecule ion attraction, water+solute=hydration)

22
Q

Saturated

A

On the line, rate of dissolving=rate of recrystallization equilibrium

23
Q

Unsaturated

A

Below line, less solute

24
Q

Supersaturated

A

Above line, more solute

25
Q

Concentrated

A

g solute>g H2O

26
Q

Dilute

A

g solute

27
Q

Increase temperature of solid or liquid…

A

Increase solubility, little effect on pressure

28
Q

Increase temperature of a gas

A

Increased entropy caused decreased solubility in water

Henry’s law=solubility increases pressure increases

29
Q

What substances are soluble?

A

Nitrates, acetates, bicarbonates, chlorates, sodium, potassium, ammonium, and chlorides (except silver, Mercury(I), and lead), and sulfates (except lead, barium, strontium, and calcium)

30
Q

What substances are insoluble?

A

Carbonates, phosphates, silicates, sulfides (except sodium, potassium, and ammonium) and hydroxides (except in sodium, potassium, ammonium, calcium, barium, and strontium)

31
Q

Factors affecting rate of solution making

A

Pulverizing (inc surface area), stirring, heating

32
Q

Solute a dissolve in solvents with…

A

Similar! Ionic and polar dissolve in polar, nonpolar dissolve in nonpolar

33
Q

Sugars, alcohols and glycerols

A

Are polar molecules that do not ionize in aqueous solutions since they have molecule solute particles

34
Q

Ammonia and acetic acid

A

Are polar molecules that partially ionize in aqueous solutions because they have a mixture of molecules and ion solute particles

35
Q

Hydrogen chloride and hydrogen iodide

A

Are polar molecules that completely ionize in aqueous solution because they have ions as solute particles

36
Q

Alloy

A

Homogeneous mixture of metals or carbon

37
Q

Solid in liquid

A

Endothermic, ^Temperature ^H ^S G-

38
Q

Gas in liquid

A

Exothermic, attraction solute-solvent, vTemperature vH vS ^pressure for G- (cold soda has more carbonation)

39
Q

Henry’s law

A

Mass of a gas in a liquid is directly proportional to pressure applied above ^mass ^pressure

40
Q

Colloids

A

Mixture of 2 phases: dispersed and continuous (solution particles

41
Q

The Tyndall effect

A

Colloids scatter beams of light

42
Q

Brownian motion

A

Zigzag/scattering motion of soloists under microscope ; can’t see true solution

43
Q

Suspensions

A

Cloudy

44
Q

For a double reaction to go to completion…

A

An insoluble precipitate is formed OR a no ionizing substance is formed OR a gas is formed

Chemistry (10 decks)

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