Reduction & Oxidation – Flashcards
Unlock all answers in this set
Unlock answersDefine:
Electrolyte |
A solute which produces ions when dissolved in H2O. (The resulting aqueous solution of solute conducts electricity) |
Define:
Strong Electrolyte |
| A solute which dissociates/ionizes 100% in aqueous solutions. |
Define:
Weak Electrolyte |
A solute which dissociates/ionizes less than 100% in aqueous solution.
Typically much less than 100%. |
| When writing a reaction for a strong electrolyte what type of symbol do use? |
Single headed arrow
→ |
| When writing a reaction for a weak electrolyte what type of symbol do use? |
Double headed arrow
↔ or → ← |
Define:
Non-Electrolyte |
A solute which does not produce ions when dissolved in H2O. (Aqueous solution does not conduct electricity) |
Define:
Dissociation |
| The process of a solid ionic compound separating into ions when dissolved in H2O. |
Define:
Ionization |
The process of a covalent compound separate into ions when dissolved in H2O.
(Not all covalent compounds ionize) |
| What is a covalent compound? |
| A non-metal bonded to another non-metal. |
| What is an Ionic compound? |
metal - nonmetal metal - polyatomic ion nonmetal - polyatomic ion polyatomic ion1 - polyatomic ion2 |
| Strong Electrolytes contain: |
Strong acids (covalent) Strong bases (ionic) Most water soluable salts (ionic) |
| Weak Electrolytes contain: |
Weak acids (covalent) Weak bases (covalent) Water insoluble salts (ionic) Water |
Define:
Salt |
| An ionic compound which consists of a cation other than H+ and an anion other than OH-. |
| How many types of reactions are there for electrolytes? |
Three... Molecular Reaction Total Ionic Reaction Net Ionic Reaction |
| What are the characteristics of a Molecular Reaction? |
All reactants and products are shown as "intact" compounds(undissociated or unionized).
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) |
| What are the characteristics of a Total Ionic Reaction? |
All soluble reactants and products are in their dissociated/ionized form (written as ions).
Ag+(aq) + NO3-(aq) + Na+(aq)+ Cl-(aq) → AgCl(s) + Na+(aq) +NO3-(aq) |
| What are the characteristics of a Net Ionic Reaction? |
Total ionic reaction with all "spectator ions" removed.
Ag+(aq) + NO3-(aq) + Na+(aq)+ Cl-(aq)→ AgCl(s) + Na+(aq) +NO3-(aq)
Ag+(aq) + Cl-(aq) → AgCl(s) |
Define:
Oxidation |
The loss of 1 or more electrons from a substance.
Na → Na+ + e- |
Define:
Reduction |
The gain of 1 or more electrons.
F + e- → F- |
nemonic:
LEO the lion goes GER |
Loss of Electron = Oxidation
Gain of Electron = Reduction |
Define:
Oxidizing Agent |
| The substance that is reduced(i.e. gains electrons). |
Define:
Reducing Agent |
| The substance that is oxidized (i.e. loses electrons). |
| Q: How do you determine which substances have been oxidized and reduced? |
By the Oxidation State.
Oxidation State is a method of bookkeeping to identify what atoms have been oxidized and reduced. |
Define:
Oxidation State |
| The charge of an atom invilved in a chemical bond if electrons were not shared between the bonded atome but instead were completely transferredto the more electronegative atom. |
T or F
Oxidation(loss of electron/s) = increase in Oxidation state |
| True |
T or F
Oxidation(loss of electron/s) = decrease in Oxidation state |
False
it = increase in oxidation state |
T or F
Reduction(gain of electron/s) = a decrease on oxidation state |
| True |
T or F
Reduction(gain of electron/s) = a increase on oxidation state |
False
it = decrease in oxidation state |
T or F
You only need reduction to occur in a reaction. |
False
Both oxidation and reduction must occur in a reaction. |
Define:
Acid |
| A species which produces H+ (hydrogen ion) in aqueous solution. |
Define:
Base |
| A species which produces OH- (hydroxide ion) in aqueous solution. |
T or F
H and H3O+ are used interchangeably. |
| True. |
Bronsted/Lowery definition of:
Acid |
| Species which can donate a hydrogen proton (H+) |
Bronsted/Lowery definition of a:
Base |
| Species which can accept a hydrogen proton(H+) |
Define:
pH scale |
A numerical scale describing molar concentration of H3O+ of an aqueous solution. pH = -log[H3O+] pH is unitless p = -log |
| For an aqueous solution what is the range of the pH scale? |
| 0-14 |
| What is the pH range of an Acidic solution? |
| pH = [ 0.00 to 7.00 ) |
| What is the pH range of a Base solution? |
| pH = ( 7.00 to 14.00 ] |
| What is the pH range for a Neutral solution? |
| pH = Acidic < 7.00 > Base |
Define:
Solution |
A homogeneous mixture consisting of a solute and a solvent.
solute + solvent = solution solute dissolves in a solvent typically solvent(qty) > solute(qty) |
Define:
Concentration |
An expression relating to the amount of solute present in some amount of solvent or solution.
amount = mass, mole, or volume |
How is Molarity (M) expressed?
hint: it's not M = mole/liter [image] |
moles of solute liter of solution ; or ; mol liter |
Define: ; Titration |
| A procedure in which one substance(titrant) is aded to another substance(analyte) until a complete reaction has occurred. |
Define: ; Equivalence Point |
| The point in the titration at which just enough titrant has been delivered to the receiving flask to completely react with the analyte originally placed in the receiving flask. |
Define: ; Equivalence Point Volume |
| Volume of titrant needed to reach the equivalence point. |
