Chem Chp 4
Color of CuO
black
acids that yield two H⁺ per molecule of acid
diprotic acids
If every ion in a complete ionic equation is a spectator, ______
no reaction occurs
Essentially all water-soluble ionic compounds are _____
strong electrolytes
Color of BaCO₃
white
Color of CaCO₃
white
Color of PbCl₂
white
Color of TiO₂
white
color of As₂O₃
white
Color of PbI₂
yellow
Loss of electrons by a substance
oxidation
Color of AgCl
white
Color of sulfur
yellow
____ represents the ionization of weak electrolytes, and ____ represents the ionization of strong electrolytes
⇌, →
Formula of limestone
CaCO₃
What dissolved species are present in NaClO₄?
K⁺(aq) and ClO₄⁻(aq)
NH₃ is a _____ and ____
weak electrolyte, weak base
The oxidation number of hydrogen bonded to nonmetals
+1
The oxidation number of hydrogen bonded to metals
-1
The oxidation number of oxygen is usually ____, except in peroxides where it is ____ and compounds with ____.
-2, -1, fluorine
Oxidation number of an atom in its elemental form
0
Sum of the oxidation numbers of all atoms in a neutral compound.
0
Number of hydrogens in acetic acid (CH₃COOH) that are ionized and which part of the acid they belong to
1, COOH group
What dissolved species are present in KCN?
K⁺(aq) and CN⁻(aq)
Carbonates and bicarbonates react with acids to form ___. The reaction first gives ____ acid, which is unstable. If present in solution in sufficient concentrations, it ____ into ___ and ___, the latter which escapes as a ____.
CO₂(g), carbonic, decomposes, H₂O(l), CO₂(g), gas
Products of reaction between copper and nitric acid.
Cu(NO₃)₂(aq), NO₂(g), H₂O(l)
If a substance is an acid it begins with __ or contains a ________
H, COOH group
Three electrolytes that are molecular compounds in gas phase but ionize completely when dissolved in water
HI HBr HI
Name the 7 common strong acids.
Hydrobromic, hydrochloric, hydriodic, perchloric, chloric, nitric, sulfuric
Protons in aqueous solutions are solvated, so we write _____
H⁺(aq)
Many sulfides react with acids to form _____, the substance that gives rotten eggs their foul odor.
H₂S(g)
Ammonia reacts with water to produce
NH₄⁺ and OH⁻
Oxides (O²⁻) are usually ____ except for _____ which are soluble, and ____ which is slightly soluble
Na₂O, SrO, K₂O, BaO, CaO
How do you dilute a concentrated acid or base, and why?
The acid or base should be added to water and then further diluted by adding more water. Adding water directly to a concentrated acid or base can cause spattering because of the intense heat generated.
How is a solution of a specific molarity prepared?
The solute is measured and then transferred to a volumetric flask of the desired size. Enough solvent is added to fill the flask about half full, and the mixture is shaken to dissolve all of the solute. Once the solute is dissolved, solvent is added exactly to the mark of the volumetric flask and mixing is repeated.
Only metals _______ in the activity series are able to react with acids to form ____.
above hydrogen, H₂(g)
Substances that ionize in aqueous solution to form H⁺(aq)
acids
The most important of the aqueous solutions of molecular substances that contain ions.
acids
alkali and alkaline metals are ____ metals
active
Metals at the top of the activity series; react readily to form compounds.
active metals
A list of metals arranged in order of decreasing ease of oxidation.
activity series
All common ionic compounds of ___ ___ ___and ___ are soluble in water.
alkali metal cations, NH₄⁺
Name the common strong bases
alkali metal hydroxides hydroxides of Ca²⁺, Sr²⁺, Ba²⁺
The oxidation number of flourine is
always -1.
The most common weak base is ____
ammonia
Ionic hydroxide compounds are all ____
bases
NaOH, KOH, and Ca(OH)₂ are all ____
bases
Substances that accept H⁺ ions and produce OH⁻ when dissolved in water.
bases
State in which the relative numbers of each type of ion or molecule in the reaction are constant over time.
chemical equilibrium
The only common strong bases are the _____
common soluble metal hydroxides
The __________ ionic equation identifies the actual reactants that participate in a reaction.
complete
_______ shows all ______ as ions.
complete ionic equation, soluble strong electrolytes
The concentration of an electrolyte solution can be specified either in terms of the ______ the solution or in terms of the _____ in the solution
compound used to make, ions
Solutions used routinely in laboratory are often purchased or prepared in _____
concentrated form
the amount of solute dissolved in a given quantity of solvent or quantity of solution
concentration
name the noble metals
copper silver mercury platinum gold
One of the most familiar redox reactions is the ____ of metal.
corrosion
adding water to obtain solutions of lower concentration
dilution
Reaction in which the ion in solution is replaced through oxidation of an element.
displacement
An ionic solid _____ into its component ions as it dissolves
dissociates
The conductivity of water originates from _____
dissolved substances
Substance whose aqueous solutions contain ions
electrolyte
Indicator signals the _____ of the titration, which will lie very near the ___ if the indicator was chosen correctly.
end point, equivalence point
moles of solute in concentrated solution ___ moles of solute in dilute solution
equals
point at which stoichiometrically equivalent quantities are brought together
equivalence point
Solubility and electrolyte strength are related (true/false)
false
etymology of "oxidation"
first reactions observed with oxygen
Because solvated ions and their shells of surrounding water molecules are _______, they become _______ throughout the solution.
free to move about, dispersed uniformly
units of solubility
grams per liter
When a weak electrolyte ionizes in solution, we write the reaction using ____, meaning that the reaction is ________
half arrows(⇌), significant in both directions
Cu(OH)₂ decomposes with ___ to form ___
heat, CuO(s) and H₂O(g)
Compounds containing CO₃²⁻ and PO₄³⁻ are ____ except for compounds of __________
insoluble, NH₄⁺ and alkali metal cations
Compounds containing S²⁻ and OH⁻ are ____ except for compounds of _________
insoluble, NH₄⁺, alkali metal cations, Ca²⁺, Sr²⁺, and Ba²⁺
Chromates (CrO₄²⁻) and oxalates (C₂O₄²⁻) are usually _____, except for compounds containing ____.
insoluble, Na⁺, NH₄⁺, K⁺, Mg²⁺
When a molecular compound dissolves in water, the solution usually consists of ____________________
intact molecules dispersed throughout the solution
Molecular substances ____ to form ions in solution.
ionize
The conductivity of NaCl solutions indicate the presence of ___
ions
Any substance with a solubility of _____ is insoluble
less than 0.01 mol/L
Color of Cu(OH)₂
light blue
Apart from listed guidelines, compounds containing sulfur are also soluble with _____
magnesium
The activity series can be used to predict the outcome of reactions between metals and either ____ or ____.
metal salts, acids
When a metal corrodes, each ____ atom ____ electrons to form a ___, which can then combine with an _____ from the _________.
metal, loses, cation, anion, external environment
Ionic compounds can usually be identified by the presence of both ________, except for compounds containing _____
metals and nonmetals, NH₄⁺
Neutralization reactions between acids and metal hydroxides are _____ reactions.
metathesis
Reactions in which cations and anions appear to exchange partners.
metathesis reactions, exchange reactions
Precipitation reactions to the pattern of _____ reactions
metathesis, exchange
first four alkanes in order
methane ethane propane butane
the concentration of a solution as the number of moles of solute in a liter of solution (soln)
molarity
An equation that shows the complete chemical formulas of reactants and products without indicating ionic character.
molecular equation
Acids that yield one H⁺ per molecule of acid
monoprotic acids
Equation that includes only the ions and molecules directly involved in the reaction
net ionic equation
When sucrose dissolves in water, the solution contains only ____ _____ molecules surrounded by ____ molecules
neutral, sucrose, water
Reaction that occurs when a solution of an acid and a solution of a base are mixed.
neutralization
A _____ reaction between an acid and a metal hydroxide produces _____ and a ____.
neutralization, water, salt
Both NaHCO₃(s) and Na₂CO₃(s) are used to ______ spills; either ____ is added until the fizzing caused by ___ formation stops.
neutralize acid, salt, CO₂(g)
Interestingly enough, copper does react with _____ acid even though it is below hydrogen on the activity series. The metal is oxidized by the ____ ion, accompanied by the formation of ___.
nitric, nitrate, NO₂(g)
Metals art the bottom of the activity series; very stable and form compounds less readily
noble metals
The products of a neutralization reaction have ____ of the characteristic properties of either the acidic solution or the basic solution.
none
A substance that does not form ions in solution
nonelectrolyte
Any molecular substance that is not an acid or NH₃ is probably a ___
nonelectrolyte
Most molecular compounds are __________ (electrolytes, nonelectrolytes)
nonelectrolytes
Fictional bookkeeping system designed to keep track of the flow of electrons in redox reactions
oxidation numbers
An atom that loses electrons is _____.
oxidized
Metals at the top of the activity series are most easily ____
oxidized
Any metal on the activity series can be ____ by the ions of the metal ____ it.
oxidized, below
Apart from __, an acid's strength can be determined by ______.
pH, electronegativity, atomic radius, charge
Color of AgI
pale yellow
The O atom in H₂O has a ______ charge, and each H atom has a _____ charge.
partial negative, partial positive
Using a photon of sufficient energy to remove an electron
photoionization
Pure water is a ____ (strong, poor) conductor of electricty
poor
insoluble solid formed by a reaction in solution
precipitate
Reactions that result in the formation of an insoluble product
precipitation reactions
Acids are often called ___ donors
proton
Color of AgCrO₄
red
Color of Cu₂O
red
Acids turn litmus paper ___, bases turn it ____.
red, blue
Reactions in which electrons are transferred from one reactant to another.
redox
Gain of electrons by a substance
reduction
hydrated ferrous oxide
rust
Any ionic compound whose cation comes from a base and whose anion comes from an acid.
salt
Many metals undergo displacement reactions with acids to produce ___ and ____.
salts, hydrogen gas
The amount of the substance that can be dissolved in a given quantity of solvent at the given temperature
solubility
chlorates and perchlorates are ______
soluble no exceptions
Compounds containing Cl⁻, Br⁻, and I⁻ are ___ except for compounds of ______
soluble, Ag⁺, Hg₂²⁺, and Pb²⁺
Compounds containing SO₄²⁻are _____ except for compounds of _____
soluble, Sr²⁺, Ba²⁺, Ca²⁺, Hg₂²⁺, and Pb²⁺
Compounds containing NO₃⁻ and CH₃COO⁻ are _____
soluble, no exceptions
The _____ are said to be dissolved in the ______
solutes, solvent
Homogenous mixture of two or more substances
solution
Ions surrounded by H₂O are said to be _____, and we denote this by writing ____ at the end
solvated, (aq)
Acids have a ___ taste, bases have a ___ taste
sour, bitter
Ions that appear in identical forms on both sides of a complete ionic equation and play no direct role in the reaction
spectator ions
How does solvation help?
stabilizes ions in solution and and prevents cations and anions from recombining
reagent solution of known concentration used in titration
standard solution
concentrated form of a solution used in laboratories
stock solution
If a soluble molecular compound is a strong electrolyte, it is a ____
strong acid.
Acids and bases that are strong electrolytes (completely ionized in solution)
strong acids and strong bases
When reactivity depends only on H⁺(aq) concentration, _____ are more reactive than _____.
strong acids, weak acids
All soluble ionic compounds are _______
strong electrolytes
All water-soluble ionic compounds are _____
strong electrolytes
Solutes that exist in solution completely or nearly completely as ions
strong electrolytes
Sum of the oxidation numbers in a polyatomic ion
the charge of the ion
Oxidation number of any monoatomic ion
the ionic charge
combining a solution where the solute concentration is not known with a reagent solution of known concentration
titration
Why is HF not a strong acid?
very high dissociation energy
______ ____ compounds are followed by ___
water-soluble ionic, (aq)
Most acids are ___
weak
Acids and bases that are weak electrolytes (party ionized in solution)
weak acids and weak bases
Solutes that exist in solution mostly in the form of neutral molecules with only a small fraction in the form of ions.
weak electrolytes
