Chapter 4

Front 1

Solution

Back 1

Any homogenous mixture of 2 (or more) substances

Front 2

Solvent

Back 2

The substance in a solution that is present in the larger amount (moles)

Front 3

Solute

Back 3

The substance(s) in a solution that is present in the smaller amount (moles)

Front 4

Why do we dissolve in liquid solvent?

Back 4

To enable particles to move about, encounter one another, and react

Front 5

Aqueous solution

Back 5

A solution for which water is the solvent

Front 6

Water is a solvent for _____ & _____ substances

Back 6

ionic, polar

Front 7

Electrolyte

Back 7

Substances that when dissolved in water causes the resulting solution to conduct an electric current (far better than water alone)

Front 8

Nonelectrolyte

Back 8

Substances that when dissolved in water cause the resulting solution to not conduct an electric current (or, no better than does pure water)

Front 9

Ionic compounds _____ into charged particles (ions) when they dissolve in water

Back 9

Dissociate

Front 10

Hydration

Back 10

Ions surrounded by water molecules

Front 11

Ionization

Back 11

non-ionic compounds that form ions when dissolved in water

Front 12

The presence of mobile ions in a solution allow it to _____ and these substances are _____

Back 12

conduct an electrical current, electrolytes

Front 13

An electric current passing through the electrolyte solution is due to the motion of the....

Back 13

ions

Front 14

Nonelectrolytes neither...

Back 14

Ionize nor dissociate into ions in solution

Front 15

Strong Electrolytes

Back 15

Electrolytes that are completely converted into separate ions in aqueous solution (100% of the compound is used to produce ions -- it has all become ions and there really isn't any of the solute compound in the solution)

Front 16

Weak Electrolytes

Back 16

Only some of the substance will have been converted into separate ions at any given moment. The remaining portion have not yet ionized or have been formed by ions that have re-combined (ie. an equilibrium exists between the molecular form and the ionized form of the solute)

Front 17

Equilibrium

Back 17

2 opposing processes that cancel each other's effects (never stops)

Front 18

For equal amounts of dissolved electrolyte, a solution of a strong electrolyte will carry a ______ current than will a solution of a weak electrolyte because _____

Back 18

greater, more ions are present in the solution of the strong electrolyte

Front 19

Chemical Equilibrium

Back 19

The effects of the forward and reverse actions cancel each other, resulting in a constant amount of un-ionized compound and constant amounts of ions

Front 20

Concentration

Back 20

How much solute is present in a given quantity of a solution

Front 21

Molarity / Molar concentration

Back 21

Moles of solute/liters of solution

Front 22

Dilution

Back 22

When we add solvent to a solution to obtain a less concentrated (more dilute) solution

Front 23

During dilution, when we add solvent we are not changing...

Back 23

The number of moles of solute

Front 24

Acid Properties

Back 24

Sour taste
Litmus turns from blue to red
React with some metals to yield H2(g)
React with carbonates to yield CO2(g)

Front 25

Base Properties

Back 25

Bitter taste
Feel slippery
Litmus turns from red to blue

Front 26

Acid

Back 26

A substance that produces H+ when dissolved in water

Front 27

Base

Back 27

A substance that produces OH- when dissolved in water

Front 28

Most acids possess _____ atoms and have a tendency to ______ them as ____ ions

Back 28

Hydrogen, release, H+

Front 29

H+

Back 29

Proton

Front 30

When a hydrogen ion (proton_ is released into aqueous solution, it combines with a water molecule to form ______

Back 30

the hydronium ion (H3O+)

Front 31

Strong acid

Back 31

If an acid ionizes to completion in water

Front 32

Weak acid

Back 32

If an acid ionizing in water reaches equilibrium before all of it has reacted

Front 33

A base must either contain ______ or be able to release them in aqueous solution or it must react with water to produce _______

Back 33

Hydroxide ions (OH-)

Front 34

Strong base

Back 34

If a base ionizes in water to completion (ie. if all of the base reacts)

Front 35

Most strong bases are...

Back 35

Metal hydroxides

Front 36

Most weak bases...

Back 36

Do not contain the hydroxide ion but produce it by reaction with water

Front 37

Neutralization reaction

Back 37

An acid and a base will reach with each other to form a salt and, usually, water

Front 38

All salts are....

Back 38

Strong electrolytes

Front 39

The products of a neutralization reaction do not have to be...

Back 39

Neutral (the salt produced may have acidic or basic properties)

Front 40

Total ionic equation

Back 40

Write all strong electrolytes as their component ions

Front 41

Spectator Ions

Back 41

Ions that undergo no chemical changes and whose presence do not directly affect the reaction

Front 42

Net ionic equation

Back 42

Cancel out spectator ions

Front 43

Titration

Back 43

A solution of accurately known concentration is added gradually to another solution of unknown concentration until the reaction between the 2 solutions is complete

Front 44

Equivalence point

Back 44

When the acid and base have completely neutralized each other (ie. they have annihilated each other, not necessarily neutral)

Front 45

When a chemical formula appears between square brackets ([])...

Back 45

It represents the molar concentration of that substance

Front 46

Even if only one is a strong electrolyte...

Back 46

It will go to completion

Front 47

Metathesis reactions

Back 47

Reactions in which any ions are exchanged

Front 48

Acid base reaction is the exchange of _______

Back 48

A hydrogen ion (H+)

Front 49

Acids react with some metals to form...

Back 49

Hydrogen gas

Front 50

Precipitate

Back 50

An insoluble solid that separates from a reaction

Front 51

Precipitation reaction

Back 51

When 2 aqueous ionic compounds are mixed and some of the ions in the combined mixture form an insoluble solid(s)

Front 52

To determine whether a particular pair of ions will lead to an insoluble combination, we use a set of.....

Back 52

Solubility rules

Front 53

Precipitation is a sub-class of

Back 53

Metathesis

Front 54

We ____ write weak electrolytes as separate aqueous ions

Back 54

Do not

Front 55

Chemical change

Back 55

Species that existed before the reaction have been consumed and new species have come into existence

Front 56

Oxidation-Reduction/Redox Reactions

Back 56

Chemical reaction involving the exchange of electrons

Front 57

Metals only react by....

Back 57

Redox

Front 58

____ will lose electrons and _____ will gain electrons in a redox reaction

Back 58

Metals, Nonmetals

Front 59

Oxidation Reaction

Back 59

The half-reaction in which electrons are lost

Front 60

Reduction Reaction

Back 60

The half-reaction in which electrons are gained

Front 61

The reducing agent gets...

Back 61

Oxidized

Front 62

Oxidation number/state

Back 62

Can be thought of as the charge that an atom would have if the electrons were transferred completely (rather than just being redistributed among uncharged species)

Front 63

Activity Series

Back 63

The relative ease of oxidation for a collection of substances

Front 64

An activity series allows us to predict...

Back 64

Whether a redox reaction will take place or not

Front 65

Things that are easily oxidized (and whose atoms give of their electrons readily) are located...

Back 65

On the top of the activity series list

Front 66

Elements whose cation strongly attract electrons are located....

Back 66

Near the bottom of the list of the activity series

Front 67

Any ____ on the list will be _____ in the presence of any ____ that appears below it on the list

Back 67

Metal, oxidized, ion

Front 68

For this activity series, the electron acceptor in a redox reaction will always be a _____

Back 68

Cation (because metal atoms do not readily accept electrons