Chemistry - The Molecular Science, Chap. 11

Front 1

Clausius–Clapeyron relation (Vapor Pressure)

Back 1

Front 2

The cubic lattice types in which crystals have been known to crystallize are

Back 2

simple cubic
face centered cubic
body centered cubic

Front 3

number of atoms in a face centered cubic unit cell

Back 3

4

Front 4

number of atoms in a body centered cubic unit cell

Back 4

2

Front 5

number of atoms in a simple cubic unit cell

Back 5

1

Front 6

Viscosity

Back 6

Resistance of liquid to flow

Front 7

Surface tension

Back 7

The energy required to expand a liquid surface

Front 8

Volatility (of a liquid)

Back 8

The tendency of a liquid to vaporize (increases as temperature increases)

Front 9

Vapor Pressure

Back 9

A state of dynamic equilibrium in which molecules enter and leave the liquid at equal rates.
OR
The pressure of a vapor in equilibrium with its non-vapor phases

Front 10

Boiling

Back 10

When the vapor pressure equals the atmospheric pressure

Front 11

Relative Humidity Formula

Back 11

Vapor Pressure of atmosphere divided by equilibrium partial pressure of water vapor at the relevant temperature

Front 12

Relative Humidity

Back 12

Vapor pressure of of water in the atmosphere

Front 13

Vaporization

Back 13

liquid -> vapor

Front 14

Condensation

Back 14

vapor -> liquid

Front 15

ΔHºvap or ΔvH - Definition

Back 15

Enthalpy of vaporization - Energy required to transform a given quantity of a substance into a gas.
Equals -ΔHºcondensation

Front 16

ΔHºsublimation - Definition

Back 16

Enthalpy of sublimation - Energy required to transform a given quantity of a substance into a gas.
Equals -ΔHºdeposition

Front 17

ΔHºfusion - Definition

Back 17

Enthalpy of fusion - Energy required to transform a given quantity of a substance into a liquid.
Equals -ΔHºcrystallization

Front 18

Fusion

Back 18

Solid -> liquid

Front 19

Crystallization

Back 19

liquid -> solid

Front 20

Sublimation

Back 20

solid -> gas

Front 21

Deposition

Back 21

gas -> solid

Front 22

Triple point

Back 22

The point in a phase diagram at which all 3 phases of matter are at equilibrium

Front 23

Phase Diagram

Back 23

chart used to show conditions at which thermodynamically-distinct phases can occur at equilibrium. Every pure substance that exists in all three phases has a distinct phase diagram

Front 24

Types of solids

Back 24

Ionic
Metallic
Molecular
Network
Amorphous

Front 25

Ionic solid - Structural Units

Back 25

positive & negative ions; no discrete molecules

Front 26

Ionic sold - Forces holding units together

Back 26

Ionic bonding

Front 27

Ionic solid - Typical properties

Back 27

Hard, brittle; high melting point, poor electrical conductor as solid, good as molten liquid; often water soluble

Front 28

Metallic solid - Structural Units

Back 28

Metal atoms

Front 29

Metallic sold - Forces holding units together

Back 29

Metallic bonding

Front 30

Metallic solid - Typical properties

Back 30

Malleable; ductile; good conductor

Front 31

Molecular solid - Structural Units

Back 31

Molecules with covalent bonds

Front 32

Molecular sold - Forces holding units together

Back 32

London Forces, dipole-dipole forces & hydrogen bonds

Front 33

Molecular solid - Typical properties

Back 33

low melting & boiling point; soft; poor electrical conductor

Front 34

Network solid - Structural Units

Back 34

Atoms held in infinite one-, two- or three-dimensional network

Front 35

Network sold - Forces holding units together

Back 35

Covalent bonds

Front 36

Network solid - Typical properties

Back 36

hardness and melting points decrease with # of bonds in network; poor electrical conductor

Front 37

Amorphous solid - Structural Units

Back 37

Covalently bonded networks of atoms or collections of large molecules

Front 38

Amorphous sold - Forces holding units together

Back 38

Covalent bonds

Front 39

Amorphous solid - Typical properties

Back 39

Noncrystalline; wide temperature range for melting; poor electrical conductor

Front 40

Crystal lattice

Back 40

The orderly, repeating arrangement of ions, molecules or atoms that shows the position of each particle

Front 41

Unit cell

Back 41

A small part of a lattice that, when repeated, reproduces the entire crystal structure

Front 42

Simple cubic edge - formula

Back 42

edge = 2 * atomic radius

Front 43

face-centered cubic edge - formula

Back 43

edge = 4 * atomic radius / sqrt(2)

Front 44

face-centered cubic edge - formula

Back 44

edge = 4 * atomic radius / sqrt(3)