CHEM Exam

Question 1

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

Answer 1

Intermolecular Forces

Question 2

weak intermolecular force

Answer 2

Van Der Waals

Question 3

holds atom together in a molecule

Answer 3

Intramolecular Forces

Question 4

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

Answer 4

Dipole-Dipole Forces

Question 5

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

Answer 5

Hydrogen Bonding

Question 6

explains solubility of ionic compounds in water

Answer 6

Ion-Dipole Forces

Question 7

“Dipole-induced Dipole Attraction”
weakest
same element

Answer 7

London-Dispersion

Question 8

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

Answer 8

Crystalline Solid

Question 9

-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

Answer 9

Amorphous Solid

Question 10

Examples of Crystalline Solids

Answer 10

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

Question 11

Examples of Amorphous Solids

Answer 11

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

Question 12

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

Answer 12

*amorphous metals (metallic glasses)

Question 13

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

Answer 13

Thin Film Coatings

Question 14

viscous, tar-like substance

Answer 14

Pitch

Question 15

Definition of amorphous and crystalline

Answer 15

Amorphous
lacks crystalline structure

Crystalline
ordered structure and symmetry

Question 16

Repeating unit of amorphous and crystalline

Answer 16

Amorphous
no repeating unit

Crystalline
one repeating unit

Question 17

Melting point of amorphous and crystalline

Answer 17

Amorphous
No sharp melting point

Crystalline
has a sharp melting point

Question 18

Chemical nature of amorphous and crystalline

Answer 18

Amorphous
Anisotropic

Crystalline
Isotropic

Question 19

-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

Answer 19

Surface Tension

Question 20

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

Answer 20

Viscosity

Question 21

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

Answer 21

Vapor Pressure

Question 22

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

Answer 22

Molar Heat of Vaporization

Question 22

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

Answer 22

Boiling Point

Question 23

-bind similar molecules

Answer 23

Cohesive Forces

Question 23

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

Answer 23

Surface tension

Question 24

-bind a substance to a surface

Answer 24

Adhesive Forces

Question 24

-rise of liquids up very narrow tubes

Answer 24

Capillary action

Question 25

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

Answer 25

Viscosity

Question 26

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

Answer 26

Condensation

Question 27

liquid to gas

Answer 27

Vaporization

Question 28

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

Answer 28

Freezing

Question 29

solid to liquid

Answer 29

Melting

Question 30

-solid CO₂ changes into gas at ordinary condition

Answer 30

Sublimation

Question 31

gas into solid

Answer 31

Deposition

Question 32

homogeneous mixtures of 2 or more substances

Answer 32

Solution

Question 33

dispersed uniformly throughout the solvent

Answer 33

Solute

Question 34

pulls solute particles and surrounds/solvates them

Answer 34

Solvent

Question 35

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

Answer 35

Electrolyte

Question 36

substance that results in a solution that does not conduct electricity

Answer 36

Non Electrolyte

Question 37

3 interactions in the solution processes

Answer 37

SOLVENT-SOLVENT
SOLUTE-SOLUTE
SOLVENT-SOLUTE

Question 38

absorbs heat

Answer 38

Endothermic Processes

Question 39

releases heat

Answer 39

Exothermic Processes

Question 40

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

Answer 40

Saturated Solution

Question 41

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

Answer 41

Unsaturated Solution

Question 42

solvent holds more solute man is normally possible at that temperature

Answer 42

Supersaturated Solution

Question 43

*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

Answer 43

“LIKE DISSOLVES LIKE”

Question 44

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

Answer 44

Fractional Crystallization

Question 45

Sg=kPg

Answer 45

Henry’s Law

Question 46

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

Answer 46

Colligative Properties