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