Chem 101: Chapter 4 (Aqueous Rxns And Solution Stoichiometry)

Front 1

Aqueous Solutions

Back 1

solutions in which water is the dissolving medium

Front 2

Solvent

Back 2

Substance in the largest quantity

Front 3

Solutes

Back 3

Other components (not largest in quantity)

Front 4

Electrolyte

Back 4

Any substance whose aqueous solution contains ions, conducts electricity

Front 5

Nonelectrolyte

Back 5

Any substance that forms a solution containing no ions

Front 6

Strong electrolytes

Back 6

complete dissociation, present as ALL ions

Front 7

Weak electrolytes

Back 7

incomplete dissociation, present as partly ions, partly molecules

Front 8

Solvation

Back 8

Ions become surrounded by H20 molecules (solvated), stabilizing the ions in solution and prevents cations and anions from recombining

Front 9

What are soluble ionic compounds?

Back 9

Strong electrolytes

Front 10

Precipitation Reaction

Back 10

Reactions resulting in the formation of an insoluble solid, forming precipitates

Front 11

Exchange / Metathesis Reactions

Back 11

Cations and Anions exchange partners

Front 12

Molecular Equations

Back 12

Shows chemical formulas of reactants and products without indicating ionic character [ Pb(NO3)2 + 2KI --> PbI2 + 2KNO3 ]

Front 13

Complete Ionic Equations

Back 13

Shows ions (strong electrolytes) [ Pb+2 + 2 NO3- + 2 K+ + 2- --> PbI2 + 2K+ + 2NO3- ]

Front 14

Spectator Ions

Back 14

Ions present as products and reactants, but play no role, maintain same form

Front 15

Net Ionic Equation

Back 15

Complete Ionic Equation - Spectator Ions

Front 16

Acids

Back 16

Proton donors [H+]

Front 17

Bases

Back 17

Proton acceptors, give [OH-]

Front 18

Strong Acids and Strong Bases

Back 18

are strong electrolytes

Front 19

Weak Acids and Weak Bases

Back 19

are weak electrolytes

Front 20

Neutralization Reactions

Back 20

acid + metal hydroxide --> salt + H20 (+gas)

Front 21

Oxidation

Back 21

loss of electrons

Front 22

Reduction

Back 22

gain of electrons

Front 23

Oxidation Number

Back 23

increase = oxidation, decrease = reduction

Front 24

Oxidation: Elemental Form

Back 24

oxidation # = 0

Front 25

Oxidation: Monatomic Ion

Back 25

oxidation # = ion charge (S-2 = 2, K+ = 1), matches groups

Front 26

Oxidation: Nonmetals

Back 26

usually negative, Oxygen = -2 in ionic / molecular compounds, Oxygen in peroxides, = -1, Hydrogen is +1 when bonded to nonmetals, and -1 when bonded to metals, Fluorine is -1 in all compounds, Other Halogens are -1 unless with Oxygen --> positive

Front 27

Oxidation: Sum

Back 27

Sum of a neutral compound = 0

Front 28

Displacement of a RXN

Back 28

A + BX --> AX + B metal + acid or metal salt, produces salt and hydrogen gas

Front 29

Activity Series

Back 29

a list of metals in decreasing ease of oxidation (top-easy to oxidize)

Front 30

Concentration

Back 30

moles solute / liter solution

Front 31

Dilution

Back 31

adding more solvent, doesn't change moles of solute, changes concentration, MV = MV

Front 32

Standard Solution

Back 32

known solution

Front 33

Tritations

Back 33

acid-base, precipitation, oxidation-reduction types, figuring out concentration of unknown solution using a standard solution

Front 34

Equivalence Point

Back 34

the point at which stoichiometrically equivalent quantities are brought together in a neutralization reaction

Front 35

To determine equivalence point

Back 35

Acid-base: indicators added to unknown solution, end points should coincide with equivalence points