Chem Sat- Liquids Solids And Phase Changes

Front 1

viscosity

Back 1

friction or resistance liquids have when moving past each other

the stronger the attraction between the molecules the more resistance there is so the more viscous it is

ex.
syrup=higher
water=lower

Front 2

surface tension

Back 2

molecules (liquids) have spread out attractions in every direction so liquids act as a film

like how a pin floats on water

Front 3

capillary action

Back 3

liquids attracted to solids will move around on the solid

like liquid going up a straw

liquids tend to be pulled upwards like chromatography paper

Front 4

phase equilibrium

Back 4

when 2 phases balance each other out

ex. eventually the water evaporating and the water condensing will reach an equilibrium and balance each other out

Front 5

dynamic equilibrium

Back 5

when opposing changes (water evaporating and water condensing) occur at equal rates

Front 6

le chatlier principle

Back 6

when a system at equilibrium is stressed it will react to minimize the stress and reach a new equilibrium

Front 7

boiling points

Back 7

when the vapor pressure increases as the temp increases it will reach a boiling point where liquid will convert to gas

Front 8

critical temp.

Back 8

the temperature above where a phase can no longer exist regardless of pressure

Front 9

critical pressure

Back 9

the minimum pressure needed to change phases at the critical temperature

Front 10

solids

include 3 types of crystalline structures

Back 10

most ordered system

crystalline solids- like brick wall
amorphous solids- random structure
polycristalline solids- many crystallines put together

Front 11

sublimation

Back 11

solid--> gas

happens with a very high vapor pressure

Front 12

melting point

Back 12

solid-->liquid

Front 13

heat of fusion

Back 13

heat needed to change phases

Front 14

triple point

Back 14

point on a phase diagram where all three lines meet- where all three phases can exist

Front 15

distillation

Back 15

process of purifying water

removes any substance with a boiling point higher than water by evaporating all the water, letting it condense, then collecting the condensation

separates matter by boiling points

Front 16

aeration

Back 16

purifies water as well

water is sprayed into the air and anything that's not water falls out

Front 17

hard water

Back 17

water with stuff in it like Ca and Cl2

Front 18

composition of water

talk about helpful ratios and stuff

Back 18

H2 and O2 combine to form water in a 1mass:8mass ratio by MASS

so 1 g of H2 and 8 g of O2 makes 9 g of H2O

gaseous H2O exists in VOLUME in 2volume:1volume ratios (H2:O2)

Front 19

heavy water

Back 19

water with an isotope of Hydrogen

Front 20

Molar heat of fusion

Back 20

amount of heat energy required to melt one mole of solid at its melting point

Front 21

molar heat of vaporization

Back 21

heat energy needed to vaporize a mole of liquid at its boiling point

Front 22

Calorimetry problems

Back 22

Quantity of heat needed= m x C

m=mass
c=heat of fusion

Front 23

Anhydrides

Back 23

oxides that react with water to form two classes of compounds (acids and bases)

Front 24

Basic anhydrides

Back 24

ex. Na

Na2O + H2O= 2NaOH

an element that when it's made an oxide and reacted with water it forms excess OH - ions

ALWAYS metal + oxygen like Na2O

Front 25

Acidic anhydrides

Back 25

ex. CO2

CO2 + H2O= H2CO3

any element that when its made an oxide and reacted with water it forms excess H+ ions

ALWAYS nonmental + oxygen like CO2

Front 26

saturated

Back 26

when substances are dissolved in water to the extent that no more will dissolve at that temperature

Front 27

unsaturated

Back 27

solution with less solute than a saturated solution under existing conditions

Front 28

polar things dissolve in

Back 28

polar things

Front 29

nonpolar things dissolve in

Back 29

nonpolar things

Front 30

hydrated ion

Back 30

things dissolve when the entire ion/molecule is surrounded by water molecules- the ion and the water molecules are held together by dipole forces- the entire molecule is a hydrated ion

Front 31

miscible

Back 31

when two liquids mix and dissolve in each other

Front 32

immiscible

Back 32

when 2 liquids don't mix

Front 33

colloid

Back 33

substances microscopically dispersed evenly throughout another colloid

mixtures whose particles are larger than the size of a molecule but smaller than particles that can be seen with the eye

ex. milk, butter, plaster

particles are microscopically visible

Front 34

suspensions

Back 34

heterogenous fluid with solid particles big enough for sedimentation

particles are visible

Front 35

solutions

Back 35

homogenous mixtures where a solute is dissolved in a solvent

particles are NOT visible

HAS MORE SOLVENT and less SOLUTE

Front 36

dilute

Back 36

small amount of solute is dispersed in the solvent

Front 37

concentrated

Back 37

large amount of solute is dissolved in the solvent

Front 38

supersaturated

Back 38

when a solution is cooled enough the solute can't come out of the solvent- then the solution can be packed with more solute than usual because it's cooled

Front 39

Water's heat of vaporization

Back 39

40.79 kj/mol

Front 40

water's heat of fusion

Back 40

6.01 kj/mol

Front 41

%concentration

Back 41

grams of solute/grams of solution x 100

Front 42

Molarity (M)

Back 42

# moles of solute / 1L of solution

Front 43

Molality (m)

Back 43

# moles of solute / 1000 g of solvent

Front 44

mole fraction

Back 44

# moles of solute / moles solute + moles of everything else

Front 45

DILUTION PROBLEMS EQUATION

Back 45

M1V1=M2V2

M= Molarity

V= Volume in L


IMPORTANT: when the question asks how much water needs to be ADDED make sure you solve for final volume and subtract that from the initial volume!!!!

Front 46

colligative properties of solutions

Back 46

properties that depend on the concentration of particles not the type of particle

ex. freezing and boiling points

Front 47

calculating freezing and boiling points

Back 47

how to calculate the degree increase or decrease of a substance's boiling or freezing point

- find MOLALITY of solution
- use MOLALITY to find the number of moles of solute in the solution

BELOW ARE CHANGES BASED ON 1 MOL PER 1000 GRAMS
1) count number of particles (ions its made of up)

ex. NaCl=2 Cu(NO3)2=3

2) for boiling point- multiply by 0.51
3) for freezing point- multiply by -1.86

this gives you the change in boiling or freezing points

Front 48

Hydrate

Back 48

substance that holds a definite proportion of water in its crystal structure

Front 49

efflorescent

Back 49

hydrated crystals that lose water of hydration when exposed to air at ordinary temperatures

Front 50

deliquescent/hydroscopic

Back 50

hydrates that absorb water from the air and become wet

Front 51

water specific heat

Back 51

C= 4.18 J/g
C= 1 cal

Front 52

what happens to the boiling point/freezing point when you add a solute?

Back 52

raises boiling points and lowers freezing points

saltwater boils at higher temperature than pure water