General Chem Ii Che-155 Ch 11, 12, 14

Front 1

The term for changing a solid or liquid to vapor. (ch 11)

Back 1

vaporization

Front 2

Changing a substance from one state to another.
Ex. Gas to Liq (ch 11)

Back 2

phase transition

Front 3

The term for changing a solid to the liquid state.
Ex: Snow to water (ch. 11)

Back 3

melting or fusion

Front 4

The term for changing a liquid to the solid state.
Ex: water to ice

Back 4

Freezing

Front 5

The term for changing a solid directly to vapor. ch11

Back 5

sublimation

Front 6

The term for changing a gas to either the liquid or solid state.

Back 6

Condensation (liquid) Deposition (solid)

Front 7

The term for the phase transition when a gas changes to the liquid state.

Back 7

liquefaction

Front 8

The term for the partial pressure of the vapor over the liquid, measured at equilibrium at a given temperature.

Back 8

vapor pressure

Front 9

The temperature at which the vapor pressure of a liquid equals the pressure exerted on the liquid. (Atmospheric pressure unless the vessel containing the liquid is closed).

Back 9

Boiling point

Front 10

The temperature at which a pure liquid changes to a crystalline solid, or freezes.

Back 10

Freezing point

Front 11

Temperature at which a crystalline solid changes to a liquid, or melts.

Back 11

Melting Point

Front 12

The heat needed for the melting point of a solid.

Back 12

Heat of fusion (enthalpy of fusion)

Front 13

The heat needed for the vaporization of a liquid.

Back 13

Heat of Vaporization (enthalpy of vaporization)

Front 14

A graphical representation showing the conditions in which different phases of substances are stable. ch11

Back 14

Phase Diagram

Front 15

The point on a phase diagram representing the temp and pressure at which three phases of a substance coexist in equilibrium. ch11

Back 15

Triple Point

Front 16

The temperature above which the liquid state of a substance no longer exists regardless of pressure.ch11

Back 16

Critical temperature

Front 17

The minimum pressure that must be applied to a gas at the critical temperature to liquefy it.

Back 17

Critical pressure

Front 18

The energy required to increase the surface area of a liquid by a unit amount. ch11

Back 18

Surface Tension

Front 19

The resistance to flow that is exhibited by all liquids and gases. ch11

Back 19

Viscosity

Front 20

The forces of interaction between molecules. ch11

Back 20

Intermolecular forces

Front 21

A general term for those intermolecular forces that include dipole and London forces.

Back 21

Van Der Waals forces

Front 22

An attractive intermolecular force resulting from the tendency of polar molecules to align themselves such that the positive end of one molecule is near the negative end of another. ch11

Back 22

Dipole force

Front 23

The weak attractive forces between molecules that occur because of the varying positions of the electrons during their motion about nuclei.

Back 23

London forces

Front 24

A weak to moderate attractive force that exists between a hydrogen atom covalently bonded to either O, N or F atoms.

Back 24

Hydrogen bonding

Front 25

A solid that consists of atoms or molecules held together by intermolecular forces.

Back 25

Molecular solid

Front 26

A solid that consists of positive cores of atoms held together by a surrounding "sea" of electrons.

Back 26

Metallic Solid

Front 27

A solid that consists of cations and anions held together by the electrical attraction of opposite charges.

Back 27

Ionic solid

Front 28

A solid that consists of atoms held together in large networks or chains by covalent bonds.

Back 28

Covalent network

Front 29

Can be shaped by hammering.

Back 29

Malleable

Front 30

A solid composed of one or more crystals; each crystal has a well-defined ordered structure in three dimensions.

Back 30

Crystalline solid

Front 31

A solid with a disordered structure; it lacks the well-defined arrangement of basic units (atoms, molecules, or ions) found in a crystal.

Back 31

Amorphous solid

Front 32

The geometric arrangement of lattice points of a crystal, in which we choose one lattice point at the same location within each of the basic units of the crystal.

Back 32

Crystal Lattice

Front 33

The smalles boxlike unit (each box having faces that are parallelograms) from which you can imagine constructing a crystal by stacking the units in three dimensions.

Back 33

Unit cell

Front 34

A cubic unit cell in which there are lattice points only at the corners.

Back 34

Simple (or primitive)cubic unit cell

Front 35

A cubic unit cell in which there is a lattice point at the center of the cubic cell in addition to those at the corners.

Back 35

Body centered cubic unit cell

Front 36

A cubic unit cell in which there are lattice points at the centers of each face of the unit cell in addition to those at the corners.

Back 36

Face-centered cubic unit cell

Front 37

A crystal structure composed of close-packed atoms (or other units) with the stacking ABABABA..

Back 37

Hexagonal close-packed structure

Front 38

A crystal structure composed of close-packed atoms (or other units) with the stacking ABCABCA.

Back 38

Cubic close-packed structure (FCC)

Front 39

The number of nearest neighbor atoms of an atom.

Back 39

coordination number

Front 40

low solute concentration

Back 40

dilute