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For an atom in its elemental form, the oxidation number is always ___
0
For any monatomic ion, the oxidation number equals the ___ on the ion
Charge
Nonmetals usually have ___ oxidation numbers, but not always
Negative
The oxidation number of oxygen is usually ___ in both ionic and molecular compounds
-2
In peroxides, which contain the O2^2- ion, oxygen has an oxidation number of ___
-1
The oxidation number of hydrogen is ___ when bonded to nonmetals and ___ when bonded to metals
+1, -1
The oxidation number of fluorine is ___ in all compounds.
-1
The halogens have an oxidation number of ___ in most binary compounds. Exception: when halogens are combined with oxygen, as in oxyanions, they have ___ oxidation states
-1, positive
General pattern for redox reactions
A + BX ---> AX +B
Other names for redox / oxidation-reduction reactions
Single-replacement, displacement
A list of metals arranged in order of decreasing ease of oxidation; also includes hydrogen.
Activity Series
In the activity series, the elements at the ___ are the most easily oxidized; referred to as active metals.
Top
In the activity series, the elements at the ___ have the lowest reactivity; referred to as noble metals.
Bottom
Any metals on the activity list can oxidize a metal listed ___ it.
Below
The amount of solute dissolved in a given quantity of solvent or quantity of solution
Concentration
Molarity is the number of ___ of solute in a ___ of solution
Moles, liter
When an ___ compound dissolves, the relative ___ of the ions introduced in the solution depend on the ___ formula of the compound.
Ionic, concentrations, chemical
___ contains three quantities -- molarity, moles ___, liters ___. So if we know any two of these we can calculate the third.
Molarity, solute, solution
Solutions that are used routinely in the laboratory are often purchased or prepared in concentrated form, called ___ ___.
Stock solutions
When a ___ is added to dilute a solution, the number of moles of ___ remains unchanged.
Solvent, solute
When a ___ is added to dilute a solution, the number of moles of ___ remains unchanged.
Solvent, solute
To calculate the volume needed to make a diluted solution, we use the equation ...
MconcVconc = MdilVdil
The process of reacting a solution of unknown concentration with one of known concentration
Titration
___ can be conducted with acid-base, precipitation, or redox reactions
Titrations
In order to titrate, you need a way to determine when the ___ ___ has been reached
Equivalence point
To determine the equivalence point for acid-base titrations, dyes known as acid-base ___ are used.
Indicators
The ___ change signals the ___ point, which usually coincides very nearly with the equivalence point.
Color, end
A homogenous mixture of two or more substances
Solution
The substance present in the greatest quantity
Solvent
The other substances present in the solution
Solute
Water itself is a poor conductor of ___, but the presence of ___ causes aqueous solutions to become good conductors
Electricity, ions
___ carry electrical charge from one ___ to the other, completing the electrical circuit
Ions, electrode
A substance whose aqueous solutions contain ions
Electrolyte
A substance that does not form ions in solutions
Nonelectrolyte
What compounds are considered electrolytes?
All covalent/ molecular compounds except for acids
___ is a very effective solvent for ionic compounds due to its polar nature. The partially positive H is attracted to the ___, and the partially negative O is attracted to the ___
Water, anion, cation
When the ions become surrounded by H2O molecules, the ions are said to be
Solvated
When a ___ compound dissolves in water, such as CH3OH, the solution usually contains intact ___ dispersed throughout the solution. Without any ____ particles, the solution is unable to conduct electricity.
Molecular, molecules, charged
Solutes that exist in solution completely or nearly completely as ions: consist of all soluble ionic compounds and a few molecular compounds
Strong electrolyte
Solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions
Weak electrolyte
Chemists use a ___ arrow for weak electrolytes and a ___ arrow for strong electrolytes.
Single, double
Reactions that result in the formation of an insoluble product are known as ___ reactions
Precipitation
Precipitation reactions occur when certain pairs of ____ charged ions attract each other so strongly that they form an insoluble ionic ___.
Oppositely, solid
7 strong acids are
HCl, HClO3, HClO4, HI, HBr, HNO3, H2SO4
Double-replacement reactions follow the general formula:
AX + BY ---> AY + BX
An equation written with all soluble strong electrolytes shown as ions
Complete ionic equation
Ions that appear in identical forms among both the reactants and products of a complete ionic equation. They are present but play no direct role in the reaction.
Spectator ions
When spectator ions are omitted we are left with the
Net ionic equation
In a net ionic equation, ___ should be conserved. If every ion is a ___ then no reaction occurs!
Charge, spectator
___ reactions are when H^+ and OH^- ions come together to form H2O
Neutralization
Reactions where electrons are transferred between reactants.
Oxidation-reduction or redox reactions
The conversion of a metal into a metal compound by a reaction between the metal and some other substance in its environment.
Corrosion
When an atom, ion, or molecule has become more positively charged, we say that it has been ___.
oxidized
When an atom, ion, or molecule has become more negatively charged, we say that it has been ___.
Reduced
The loss of electrons
Oxidation
The gain of electrons
Reduction
The oxidation of one substance is always accompanied by the ___ of another as ___ are transferred between them
Reduction, electrons
Oxidation occurs when there is an ___ in oxidation number; reduction occurs when there is a ___ in oxidation number
Increase, decrease
Note 
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