Chem 111 (3Rd Q 2Nd Sem 1St Term)

Front 1

Kinetic

Back 1

Came from greek kinesis which means movement

Front 2

Kinetic theory (Kinetic Molecular Theory in Gases)

Back 2

Always associated in describing gas as particles in random motion

Front 3

Kinetic molecular theory in liquids and solids

Back 3

Explains attraction which forms sllid and liquid phases

Front 4

Intermolecular force

Back 4

Attractive force between molecules

Front 5

Intermolecular and intramolecular forces

Back 5

2 forces involved in liquid and solid molecules

Front 6

Intramolecular forces

Back 6

Holding atoms together (to molecules)

Front 7

Intermolecular forces

Back 7

Generally much weaker than intramolecular forces (bonds)

Front 8

Ion-dipole forces

Back 8

Bond between ion and polar molecule

Front 9

Dipole-dipole forces

Back 9

Attractive forces between polar molecules

-between neighboring molecules with permanent dipoles

Front 10

Hydrogen bond

Back 10

Special dipole dipole interaction between hydrogen atom in polar N-H, O-H, or F-H bond and on electronegativity O, N, or F atom

Front 11

Dispersion forces

Back 11

Induced-dipole / van der waals forces / London forces

Front 12

Polarity

Back 12

Results in uneven partial distribution of a molecule between various atom groups

Front 13

Dipole moment

Back 13

Direceion of the polar bond of a molecule

Front 14

Polar molecules

Back 14

Asymmetric, en diff 0.5-1.7, net dipole moment, diatomic molecules of different elements, molecules with O, N, or OH at one end

Front 15

Non polar molecules

Back 15

Symmetric, en diff 0-0.4, dipole moments are cancelled out, molecules of elements sharing electrons equally

Front 16

Polarizability

Back 16

Ease with which electron distribution can be distorted

Front 17

Vapor pressuree

Back 17

In a sealed container, some liquid evaporates to establish a pressure in the vapor phase, Vapor pressure: partial pressure of the vapor over the liquid measured at equilibrium and at some temperature. • Dynamic equilibrium

Front 18

Clausius-Clapeyron equation

Back 18

shows how the vapor pressure and temperature are related.

Front 19

Boiling point

Back 19

the temperature at which the vapor pressure of a liquid is equal to the pressure of the external atmosphere.

Front 20

Normal boiling point

Back 20

The temperature at which the vapor pressure of a liquid is equal to atmospheric pressure (1 atm).

Front 21

Heat of vaporization

Back 21

heat needed for the vaporization of a liquid.

Front 22

Heat of fusion

Back 22

heat needed for the melting of a liquid.

Front 23

Surface tension

Back 23

is the amount of energy required to stretch or increase the surface of a liquid by a unit area, it is a force that causes the molecules on the surface of the liquid to be pushed together (contract) and form a layer.

Front 24

Cohesion

Back 24

is the intermolecular attraction between like molecules, responsible for surface tension

Front 25

Adhesion

Back 25

is the intermolecular attraction between unlike molecules

Front 26

Viscosity

Back 26

is a measure of a fluid’s resistance to flow.

Front 27

Fluidity

Back 27

A measure of how molecules move/flow “freely” with one another.

Front 28

Ionic solid

Back 28

ionic bonds hold the solids in a regular three dimensional arrangement

Front 29

Molecular solid

Back 29

solids like ice that are held together by intermolecular forces.

Front 30

Covalent network

Back 30

a solid consists of atoms held together in large networks or chains by covalent networks.

Front 31

Metallic

Back 31

similar to covalent network except with metals. Provides high conductivity.

Front 32

Metal crystals

Back 32

made up of atoms in regular arrays

Front 33

Unit cell

Back 33

the smallest of repeating array of atoms

Front 34

Crystalline solid

Back 34

a well defined arrangement of atoms; this arrangement is often seen on a macroscopic level.

Front 35

Amorphous solid

Back 35

atoms are randomly arranged. No order exists in the solid.

Front 36

3 types of cubic cells

Back 36

Simple cubic, body centered cubic, face centered cubic

Front 37

Simple cubic

Back 37

All sides equal, all angles 90°

Front 38

Tetragonal

Back 38

2 sides (a and b) equal, all angles 90°

Front 39

Orthorhombic

Back 39

All sides unequal, all angles 90°

Front 40

Rhombohedral

Back 40

All sides equal, 2 angles 90°

Front 41

Monoclinic

Back 41

All sides unequal, 2 angles 90°

Front 42

Triclinic

Back 42

All sides unequal, no angles 90°

Front 43

Hexagonal

Back 43

2 sides are equal, 2 angles 90° and 1 120°

Front 44

Melting

Back 44

change of a solid to a liquid.

Front 45

Freezing

Back 45

Liquid to solid

Front 46

Vaporization

Back 46

Liquid to gas

Front 47

Sublimation

Back 47

Solid to gas

Front 48

Condensation

Back 48

Gas to liquid

Front 49

Deposition

Back 49

Gas to solid

Front 50

Phase Diagram

Back 50

Graph of pressure-temperature relationship;

describes when 1,2,3 or more phases are present and/or in equilibrium with each other, lines indicate equilibrium state of two phases.

Front 51

Critical temperature

Back 51

Temperature where substance must always be gas, no matter what the pressure is.

Front 52

Triple point

Back 52

Temperature and pressure where all three phases co-exist in equilibrium

Front 53

Critical point

Back 53

point where system is at its critical pressure and temperature

Front 54

Critical pressure

Back 54

vapor pressure at critical temperature

Front 55

Phase diagram

Back 55

summarizes the conditions at which a substance exists as a solid, liquid, or gas

Front 56

Solution

Back 56

•a mixture of two or more substances that is identical throughout

Front 57

Solute

Back 57

is the substance being dissolved

Front 58

Solvent

Back 58

is the medium in which the solute is dissolved

Front 59

Solubility

Back 59

Refers to maximum amount of solute that can be dissolved under specific temperature and pressure conditions

Front 60

Insoluble

Back 60

A substance that cannot dissolve or only to a very limited extent is called

Front 61

Miscibility

Back 61

Ability of a liquid to solute and dissolve to another

Front 62

Factors affecting solubility

Back 62

A. Nature of solute and solvent

B. Effect of Temperature

C. Effect of Pressure

D. Surface Area

E. Stirring

Front 63

Miscible; immiscible

Back 63

Able to mix; unable to mix (liquid)

Front 64

final observable phase

Back 64

Solutions can be classified based on the _

-gaseous solution, liquid solution or solid solution

Front 65

Amount of solute present

Back 65

Solutions can be classified based on the _

-dilute solution, concentrated solution

Front 66

amount of solute dissolved in the given solvent

Back 66

Solutions can also be classified in relation to the __

-unsaturated solution, saturated solution, supersaturated solution

Front 67

Types of solutions

Back 67

Front 68

Concentration of solutions

Back 68

Solutions can be described qualitatively or quantitatively based on the amount of solute relative to a given amount of solvent.

Front 69

Dilute solution

Back 69

contains a relatively small amount of solute

Front 70

Concentrated

Back 70

solution contains a relatively large amount of solute.

Front 71

Unsaturated solution

Back 71

contains less solute than the solvent has the capacity to dissolve at a specific temperature.

Front 72

Saturated solution

Back 72

contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature.

Front 73

Supresaturated solution

Back 73

contains more solute than is present in a saturated solution at a specific temperature.

Front 74

Ways of expressing the concentration of solutions

Back 74

1. Parts per Million & Parts per Billion

2. Percent by Mass & Percent by Volume

3. Mole Fraction

4. Molarity

5. Molality

Front 75

Parts per Million (ppm) & Parts per Billion (ppb) used

Back 75

used when the concentration of solute present is very low

Front 76

Ppm and ppb

Back 76

unit for expressing very dilute concentrations. It is commonly used to express the concentration of pollutants in air or in water

Front 77

Mass/volume percent

Back 77

One way of representing the concentration of an element in a compound or a component in a mixture.

It gives the mass of solute dissolved in a volume of solution, in a percent

Front 78

Mole Fraction

Back 78

is the ratio of the number of moles of one component to the total number of moles in a solution represented by capital X

Front 79

Molarity

Back 79

is the ratio of the number of moles per liter of solution

Front 80

Molality

Back 80

defined as the number of moles of solute per kilogram of solvent