Phases

Question 1

Liquid vs gas

Answer 1

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

Question 2

Viscosity

Answer 2

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

Question 3

Surface tension

Answer 3

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

Question 4

Capillary action

Answer 4

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

Question 5

Phase equilibrium

Answer 5

Equal rate of evaporation and condensation

Question 6

Dynamic equilibrium

Answer 6

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

Question 7

Boiling point

Answer 7

Liquid vapor pressure=atmospheric pressure

Question 8

Critical temperature

Answer 8

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

Question 9

Critical pressure

Answer 9

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

Question 10

Crystalline solids

Answer 10

3D like brick wall, regular structure, repeating pattern

Question 11

Amorphous solid

Answer 11

Random structure

Question 12

Polycrystalline solid

Answer 12

Aggregate of regularly structured small crystals in a random fashion

Question 13

Solid diffusion

Answer 13

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

Question 14

Sublimation

Answer 14

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

Question 15

Melting point

Answer 15

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

Question 16

Heavy water

Answer 16

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

Question 17

Hydrogen peroxide

Answer 17

Bleaching and oxidizing agent H2O2

Question 18

Solution

Answer 18

Homogeneous, one substance dissolved in another

Question 19

Aqueous solution

Answer 19

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

Question 20

Solubility

Answer 20

g solute/100 mL or g H2O, temperature dependent

Question 21

Solvation

Answer 21

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

Question 22

Saturated

Answer 22

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

Question 23

Unsaturated

Answer 23

Below line, less solute

Question 24

Supersaturated

Answer 24

Above line, more solute

Question 25

Concentrated

Answer 25

g solute>g H2O

Question 26

Dilute

Answer 26

g solute

Question 27

Increase temperature of solid or liquid...

Answer 27

Increase solubility, little effect on pressure

Question 28

Increase temperature of a gas

Answer 28

Increased entropy caused decreased solubility in water | Henry's law=solubility increases pressure increases

Question 29

What substances are soluble?

Answer 29

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

Question 30

What substances are insoluble?

Answer 30

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

Question 31

Factors affecting rate of solution making

Answer 31

Pulverizing (inc surface area), stirring, heating

Question 32

Solute a dissolve in solvents with...

Answer 32

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

Question 33

Sugars, alcohols and glycerols

Answer 33

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

Question 34

Ammonia and acetic acid

Answer 34

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

Question 35

Hydrogen chloride and hydrogen iodide

Answer 35

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

Question 36

Alloy

Answer 36

Homogeneous mixture of metals or carbon

Question 37

Solid in liquid

Answer 37

Endothermic, ^Temperature ^H ^S G-

Question 38

Gas in liquid

Answer 38

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

Question 39

Henry's law

Answer 39

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

Question 40

Colloids

Answer 40

Mixture of 2 phases: dispersed and continuous (solution particles

Question 41

The Tyndall effect

Answer 41

Colloids scatter beams of light

Question 42

Brownian motion

Answer 42

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

Question 43

Suspensions

Answer 43

Cloudy

Question 44

For a double reaction to go to completion...

Answer 44

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