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