Chemistry Ch. 4-6

Front 1

Solution

Back 1

A homogeneous misture in which the molecules or ions of the components freely intermingle

Front 2

Solvent

Back 2

The medium into which the solutes are mixed or dissolved

Front 3

Aqueous Solutions

Back 3

A solution in which the solute is dissolved in water

Front 4

Solute

Back 4

Any substance dissolved in the solvent

Front 5

Concentration

Back 5

The ratio of the amount of solute either to the amount of solvent or to the amount of solution

Front 6

Percentage Composition

Back 6

The amount of solute per amount of solution- solute to solution ratio

Front 7

Dilute Solution

Back 7

When the ratio of solute to solvent is small

Front 8

Concentrated Solution

Back 8

When the ratio of solute to solvent is large

Front 9

Solution

Back 9

A homogeneous mixture in which the molecules or ions of the components freely intermingle

Front 10

Solvent

Back 10

The medium into which the solutes are dissolved

Front 11

Aqueous Solutions

Back 11

Solutions in which the solute is dissolved in water

Front 12

Solute

Back 12

Any substance that is dissolved in the solvent

Front 13

Concentration

Back 13

The ratio of the amount of solute either to the amount of solvent or to the amount of solution

Front 14

Percentage Concentration

Back 14

A solute to solution ratio

Front 15

Dilute Solution

Back 15

When the ratio of solute to solvent is small

Front 16

Concentrated Solution

Back 16

When the ratio of solute to solvent is large

Front 17

Saturated Solution

Back 17

When the amount of solute that can dissolve in a given amount of solvent reaches its limit at a given temperature

Front 18

Solubility

Back 18

The amount required to give a saturated solution

Front 19

Unsaturated Solution

Back 19

A solution having less solute than required for saturation

Front 20

Supersaturated Solution

Back 20

When a solution actually contains more solute than required for saturation; are unstable

Front 21

Precipitate

Back 21

A solid that forms in a solution

Front 22

Precipitation Reaction

Back 22

A chemical reaction that produces a precipitate

Front 23

Electrolytes

Back 23

Electrically conducting aqueous solutions

Front 24

Dissociation

Back 24

When an ionic compound dissolves in water and the ions separate from each other and enter the solution as more or less independent particles that are surrounded by molecules of the solvent

Front 25

Strong Electrolytes

Back 25

Strong conductors of electricity; salts

Front 26

Nonelectrolytes

Back 26

Aqueous solutions of most molecular compounds; do not conduct electricity

Front 27

Hydrated

Back 27

When a particle is surrounded by water molecules in the solution

Front 28

Molecular Equation

Back 28

When all the formulas are written with the ions together, as if the substances in solution consist of neutral molecules

Front 29

Ionic Equation

Back 29

When the formulas are written so that the formulas of all soluble strong electrolytes are dissociated

Front 30

Spectator Ions

Back 30

Ions that do not actually take part in a reaction

Front 31

Net Ionic Equation

Back 31

Same as the ionic equation; however, the spectator ions are eliminated

Front 32

Material Balance

Back 32

One of the criteria for balanced ionic and net ionic equations; there must be the same number of atoms of each kind on both sides of the arrow

Front 33

Electrical Balance

Back 33

One of the criteria for balanced ionic and net ionic equations; the net electrical charge on the left must equal the net electrical charge on the right (although this charge does not necessarily have to be zero)

Front 34

Acids

Back 34

Have a tart or sour taste; a substance that reacts with water to produce the hydronium ion

Front 35

Bases

Back 35

Have a somewhat bitter taste and have a soapy feel; substances that produce hydroxide ions in water

Front 36

Salt

Back 36

Any ionic compound that doesn't contain either a hydroxide ion or an oxide ion

Front 37

Ionization Reaction

Back 37

Ions form where none existed before

Front 38

Monoprotic Acids

Back 38

The molecules HCl and HC2H3O2; capable of furnishing only on H+ per molecule of acid

Front 39

Polyprotic Acids

Back 39

Can furnish more than one H+ per molecule

Front 40

Diprotic Acid

Back 40

Has two successive steps to ionize

Front 41

Triprotic Acids

Back 41

Have three successive steps to ionize

Front 42

Acidic Anhydrates

Back 42

Oxides that react to form molecular acids containing hyrdrogen, which are then able to undergo reaction with water to yield a hydronium ion; anhydrate means without water

Front 43

Basic Anhydrates

Back 43

Soluble metal oxides; react with water to form the hydroxide ion as one of the products

Front 44

Strong Acids

Back 44

Strong electrolytes

Front 45

Chemical Equilibrium or Dynamic Equilibrium

Back 45

When two opposing reactions occur at the same rate

Front 46

Position of Equilibrium

Back 46

The extent to which the forward reaction proceeds toward completion

Front 47

Binary Acids

Back 47

The binary compounds of hydrogen with many of the nonmetals; in aqueous solutions

Front 48

Oxoacids

Back 48

Acids that contain hydrogen, oxygen, and another element

Front 49

Molar concentration/Molarity

Back 49

The number of moles of solute per liter of solution

Front 50

Qualitative Analysis

Back 50

When it is determined which substances are present in a sample without measuring their amounts

Front 51

Quantitative Analysis

Back 51

The goal is to measure the amounts of the various substances in a sample

Front 52

Oxidation-Reduction Reactions
(Redox Reactions)

Back 52

Electron transfer reactions

Front 53

Oxidation

Back 53

The loss of electrons by one reactant

Front 54

Reduction

Back 54

The gain of electrons

Front 55

Oxidizing Agent

Back 55

The substance that accepts the electrons

Front 56

Reducing Agent

Back 56

The substance that supplies the electrons

Front 57

Skeleton Equation

Back 57

Shows only the ions (or sometimes molecules, too) involved in the redox changes.

Front 58

Nonoxidizing Acids

Back 58

Acids that have poor oxidizing abilities

Front 59

Corrosion/Tarnishing

Back 59

When metals react directly with oxygen

Front 60

Energy

Back 60

Something an object has if the object is able to do work

Front 61

Kinetic Energy

Back 61

The energy an object has when it is moving

Front 62

Potential Energy

Back 62

Energy an object has that can be changed to kinetic energy; can be thought of as stored energy

Front 63

Chemical Energy

Back 63

The potential energy of chemicals

Front 64

Law of the Conservation of Energy

Back 64

Energy cannot be created or destroyed; it can only be changed from one form to another

Front 65

Heat (Thermal Energy)

Back 65

Energy that is transferred between objects caused by differences in their temperatures

Front 66

Thermal Equilibrium

Back 66

When a system and its surroundings come to equal temperatures

Front 67

Internal Energy (E)

Back 67

The sum of energies for all of the individual particles in a sample of matter

Front 68

Molecular Kinetic Energy

Back 68

The energy associated with the movement of particles within matter

Front 69

Internal Energy Change

Back 69

The change in internal energy that accompanies both chemical and physical changes

Front 70

Kinetic Molecular Theory

Back 70

Temperature is related to the average kinetic energy of the atoms and molecules of an object

Front 71

State

Back 71

The complete list of properties that specify an object's current condition; includes the object's pressure, temperature, volume, anc chemical compostion (numbers of moles of all substances present)

Front 72

State Function

Back 72

Any property that, like energy, depends only on an object's current state

Front 73

Open System

Back 73

A system that can gain or lose mass and energy across its boundaries

Front 74

Closed System

Back 74

A system that can absorb or release energy, but not mass, across the boundary

Front 75

Isolated System

Back 75

A system that cannot exhange matter or energy with their surroundings

Front 76

Adiabatic

Back 76

Processes that occur within an isolated system

Front 77

Heat Capacity

Back 77

The amount of energy needed to raise the temperature of an object by 1 degree Celsius

Front 78

Specific Heat Capacity

Back 78

The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius

Front 79

Exothermic

Back 79

Any reaction in which heat is a product

Front 80

Endothermic

Back 80

Reactions that consume energy

Front 81

Heat of Reaction

Back 81

The amount of heat absorbed or released in a chemical reaction

Front 82

Calorimetry

Back 82

The science of using a calorimeter for determining heats of reaction

Front 83

Pressure

Back 83

The amount of force acting on a unit of area; the ratio of force to area

Front 84

Atmospheric Pressure

Back 84

The pressure exerted by the mixture of gases in our atmosphere

Front 85

Expansion Work

Back 85

The energy transferred as work when a system expands or contracts against the pressure exerted by the surroundings

Front 86

Heat of Combustion

Back 86

Heat produced by a combustion reaction

Front 87

Heat of Reaction at Constant Volume

Back 87

The heat of reaction measured in a bomb calorimeter

Front 88

Heat of Reaction at Constant Pressure

Back 88

The heat of reaction in an open system

Front 89

Enthalpy

Back 89

The heat content of a system

Front 90

Enthalpy Change

Back 90

The difference in enthalpy between the initial state and the final state form some change

Front 91

Standard Heat of Reaction

Back 91

The value of the enthalpy change fro a reaction occurring under standard conditions and involving the actual numbers of moles specified by the coefficients of the equation

Front 92

Thermochemical Equation

Back 92

An equation that also shows the value of the standard heat of reaction

Front 93

Enthalpy Diagram

Back 93

A graphical construction that shows the energy relationships among the alternative pathways for the same overall reaction

Front 94

Hess's Law of Heat Summation

Back 94

The value of the standard heat of reaction for any reaction that can be written in steps equals the sum of the values of the standard heat of reaction of each of the individual steps

Front 95

Standard Heat of Combustion

Back 95

The amount of heat released when one mole of a fuel substance is completely burned in pure oxygen gas, with all reactants and products brought to 25 degrees Celsius and 1 bar of pressure

Front 96

Standard Enthalpy of Formation (Standard Heat of Formation)

Back 96

The amount of heat absorbed or evolved when specifically one mole of the substance is formed at 25 degrees Celsius and 1 bar from its elements in their standard states

Front 97

Standard State

Back 97

An element is in its standard state when it is at 25 degrees Celsius and 1 bar and in its most stable form and physical state