Chemistry - Solids, Liquids, and Mixtures

vaporization

phase transition from a liquid or a solid state into a gas or vapor

viscosity

resistance to being poured

volatile

substance’s tendency to vaporize or turn into a gas or vapor at normal temperatures and pressures

deposition

phase transition → gas into a solid

cohesion

attraction of molecules to the same substance

adhesion

ability of liquids to stick to a surface

capillary action

flow of a liquid through narrow spaces, driven by surface tension and interaction between adhesive and cohesive forces (ex: liquid through paper towels/thin tubes)

surface tension

when liquids pull their particles close together to form a barrier

allotrope

different structural forms of the same element in the same physical state

characteristics of liquids

particles are relatively close, inter molecular forces are present, non-compressable, definite volume; no shape

fluidity

the ability for liquids to take the shape of their containers, flow easily, and form at minimal effortand can move past one another.

emulsion

substances that don’t mix well

emulsifier

agent added to mixtures that will dissolve the suspended particlesand stabilize the emulsion, preventing separation.

sublimation

transition from a solid to a gas

evaporation

liquid turns to gas below boiling point

What is this graph called?

vapor pressure curve

What is this graph called?

phase diagram

What point is the red dot on?

triple point

What point is the red dot on?

critical point

What phase occurs in the red zone?

solid phase

What phase occurs in the blue zone?

liquid phase

What phase occurs in the yellow zone?

gas phase

characteristics of solids

definite volume, definite shape, particles are packed closely, non compressible, high density

What are crystalline solids? (crystals)

solids where particles are arranged in geometric patterns

What are the five categories of crystalline solids?

atomic, molecular, covalent, ionic, metallic

What are examples of covalent crystals?

diamonds, graphite, Buckminster fullerance

unit cell

basic geometric pattern

crystal lattice

bunch of unit cells

What are examples of ionic crystals?

table salt, lithium fluoride, magnesium oxide

What are examples of metallic crystals?

gold, aluminum, silver

What are amorphous solids?

anything not a crystal

What is the sea of electrons?

electrons surrounding the nucleus, but are not connected to

Examples of amorphous solids

desk, floor, dirt

malleable

put into sheets

ductile

drawn into wires

Characteristics of heterogeneous mixtures

not well blended, not same throughout

Examples of heterogeneous mixtures

vegetable soup, tossed salad, mixed nuts

Characteristics of homogeneous mixtures

well blended, same throughout

What is another name for something being the same throughout?

solution

colloid

group of mixtures

solvent

substance that does the dissolving

solute

substance that is dissolved

What is the universal solvent?

water

What is an aqueous solution?

water solvent mixture

What is a miscible mix?

liquid-liquid mix

immiscible

two liquids that don’t mix

insoluable

solute does not dissolve well

Tyndall Effect

shine light into colloid → light scatters

Examples of colloids

smoke, cream cheese, whipped cream

percent by mass formula

mass solute/ mass solution x 100

percent by volume formula

volume solute/volume solution x 100

molarity formula

mole solute/ liter of solution

What is Brownian motion?

random zig zag movement of particles in a liquid, caused by constant collisions with surrounding molecules