CHEMISTRY THE CENTRAL SCIENCE >EBOOK<14th EditionBrown Publisher: PEARSONISBN: 9780136873891
CHEMISTRY THE CENTRAL SCIENCE >EBOOK<
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Chapter 1 - Introduction: Matter, Energy, And MeasurementChapter 1.2 - Classifications Of MatterChapter 1.5 - Units Of MeasurementChapter 1.6 - Uncertainty In MeasurementChapter 1.7 - Dimensional AnalysisChapter 2 - Atoms, Molecules, And IonsChapter 2.3 - The Modern View Of Atomic StructureChapter 2.4 - Atomic WeightsChapter 2.5 - The Periodic TableChapter 2.6 - Molecules And Molecular Compounds
Chapter 2.7 - Ions And Ionic CompoundsChapter 2.8 - Naming Inorganic CompoundsChapter 2.9 - Some Simple Organic CompoundsChapter 3 - Chemical Reactions And Reaction StoichiometryChapter 3.1 - Chemical EquationsChapter 3.2 - Simple Patterns Of Chemical ReactivityChapter 3.3 - Formula WeightsChapter 3.4 - Avogadro's Number And The MoleChapter 3.5 - Empirical Formulas From AnalysesChapter 3.6 - Quantitative Information From Balanced EquationsChapter 3.7 - Limiting ReactantsChapter 4 - Reactions In Aqueous SolutionChapter 4.1 - General Properties Of Aqueous SolutionsChapter 4.2 - Precipitation ReactionsChapter 4.3 - Acids, Bases, And Neutralization ReactionsChapter 4.4 - Oxidation-reduction ReactionsChapter 4.5 - Concentrations Of SolutionsChapter 4.6 - Solutions Stoichiometry And Chemical AnalysisChapter 5 - ThermochemistryChapter 5.2 - The First Law Of ThermodynamicsChapter 5.3 - EnthalpyChapter 5.4 - Enthalpies Of ReactionChapter 5.5 - CalorimetryChapter 5.6 - Hess's LawChapter 5.7 - Enthalpies Of FormationChapter 5.8 - Bond EnthalpiesChapter 5.9 - Foods And FuelsChapter 6 - Electronic Structure Of AtomsChapter 6.1 - The Wave Nature Of LightChapter 6.2 - Quantized Energy And PhotonsChapter 6.3 - Line Spectra And The Bohr ModelChapter 6.4 - The Wave Behavior Of MatterChapter 6.5 - Quantum Mechanics And Atomic OrbitalsChapter 6.8 - Electron ConfigurationsChapter 6.9 - Electron Configurations And The Periodic TableChapter 7 - Periodic Properties Of The ElementsChapter 7.3 - Sizes Of Atoms And IonsChapter 7.4 - Ionization EnergyChapter 7.6 - Metals, Nonmetals, And MetalloidsChapter 7.7 - Trends Of Group 1a And Group 2a MetalsChapter 8 - Basic Concepts Of Chemical BondingChapter 8.2 - Ionic BondingChapter 8.3 - Covalent BondingChapter 8.4 - Bond Polarity And ElectronegativityChapter 8.5 - Drawing Lewis StructuresChapter 8.6 - Resonance StructuresChapter 8.7 - Exceptions Of The Octet RuleChapter 9 - Molecular Geometry And Bonding TheoriesChapter 9.2 - The Vsepr ModelChapter 9.3 - Molecular Shape And Molecular PolarityChapter 9.5 - Hybrid OrbitalsChapter 9.6 - Multiple BondsChapter 9.7 - Molecular OrbitalsChapter 9.8 - Bonding In Period 2 Diatomic MoleculesChapter 10 - GasesChapter 10.2 - PressureChapter 10.3 - The Gas LawsChapter 10.4 - The Ideal-gas EquationChapter 10.5 - Further Applications Of The Ideal-gas EquationChapter 10.6 - Gas Mixtures And Partial PressuresChapter 10.7 - The Kinetic-molecular Theory Of GasesChapter 10.8 - Molecular Effusion And DiffusionChapter 10.9 - Real Gases: Deviations From Ideal BehaviorChapter 11 - Liquids And Intermolecular ForcesChapter 11.2 - Intermolecular ForcesChapter 11.3 - Select Properties Of LiquidsChapter 11.4 - Phase ChangesChapter 11.5 - Vapor PressureChapter 11.6 - Phase DiagramChapter 11.7 - Liquid CrystalsChapter 12 - Solids And Modern MaterialsChapter 12.3 - Metallic SolidsChapter 12.5 - Ionic SolidChapter 12.7 - Covalent-network SolidsChapter 13 - Properties Of SolutionsChapter 13.3 - Factor Affecting SolubilityChapter 13.4 - Expressing Solution ConcentrationChapter 13.5 - Colligative PropertiesChapter 14 - Chemical KineticsChapter 14.2 - Reaction RatesChapter 14.3 - Concentration And Rate LawsChapter 14.4 - The Change Of Concentration With TimeChapter 14.5 - Temperature And RateChapter 14.6 - Reaction MechanismsChapter 15 - Chemical EquilibriumChapter 15.2 - The Equilibrium ConstantChapter 15.3 - Understanding And Working With Equilibrium ConstantChapter 15.4 - Heterogeneous EquilibriumChapter 15.5 - Calculating Equilibrium ConstantsChapter 15.6 - Applications Equilibrium ConstantsChapter 15.7 - Le Chatelier's PrincipleChapter 16 - Acid—base EquilibriumChapter 16.2 - Bronsted-lowery Acids And BasesChapter 16.3 - The Autoionization Of WaterChapter 16.4 - The Ph ScaleChapter 16.5 - Strong Acids And BasesChapter 16.6 - Weak AcidsChapter 16.7 - Weak BasesChapter 16.8 - Relation Between Ka And KbChapter 16.9 - Acid-base Properties Of Salt SolutionChapter 16.10 - Acid-base Behavior And Chemical StructureChapter 17 - Additional Aspects Of Aqueous EquilibriumChapter 17.1 - The Common Ion EffectChapter 17.2 - BuffersChapter 17.3 - Acid-base TitrationsChapter 17.4 - Solubility EquilibriaChapter 17.5 - Factor That Affect SolubilityChapter 17.6 - Precipitation And Separation Of IonsChapter 18 - Chemistry Of The EnvironmentChapter 18.1 - Earth's AtmosphereChapter 18.2 - Human Activities And Earth AtmosphereChapter 19 - Chemical ThermodynamicsChapter 19.1 - Spontaneous ProcessesChapter 19.2 - Entropy And Second Law Of ThermodynamicsChapter 19.3 - The Molecular Interpretation Of Entropy And The Third Law Of ThermodynamicsChapter 19.4 - Entropy Changes In Chemical ReactionsChapter 19.5 - Gibbs Free EnergyChapter 19.6 - Free Energy And TemperatureChapter 19.7 - Free Energy And Equilibrium ConstantChapter 20 - ElectrochemistryChapter 20.1 - Oxidation States And Oxidation-reduction ReactionsChapter 20.2 - Balancing Redox EquationsChapter 20.3 - Voltaic CellsChapter 20.4 - Cell Potentials Under Standard ConditionsChapter 20.5 - Free Energy And Redox ReactionsChapter 20.6 - Cell Potentials Under Nonstandard ConditionsChapter 20.9 - ElectrolysisChapter 21 - Nuclear ChemistryChapter 21.1 - Radioactivity And Nuclear EquationsChapter 21.2 - Patterns Of Nuclear StabilityChapter 21.3 - Nuclear TransmutationsChapter 21.4 - Rates Of Radioactive DecayChapter 21.6 - Energy Changes In Nuclear ReactionsChapter 22 - Chemistry Of The NonmetalsChapter 22.1 - Periodic Trends And Chemical ReactionsChapter 22.3 - Group 8a:the Noble GasesChapter 22.4 - Group 7a:the HalogensChapter 22.7 - NitrogenChapter 22.10 - The Other Group 4a:elements:si,ge,sn And PbChapter 23 - Transition Metals And Coordination ChemistryChapter 23.2 - Transition-metals ComplexesChapter 23.4 - Nomenclature And Isomerism In Coordination ChemistryChapter 23.5 - Color And Magnetism In Coordination ChemistryChapter 23.6 - Crystal-field TheoryChapter 24 - The Chemistry Of Life: Organic And Biological ChemistryChapter 24.2 - Introduction To HydrocarbonsChapter 24.3 - Alkenes,alkynes,and Aromatic HydrocarbonsChapter 24.4 - Organic Functional GroupsChapter 24.7 - Proteins
Sample Solutions for this Textbook
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The figure (i) represents the space filling molecular models of two spheres attached to each other...The sign of the electric charge on the particle is negative in the given diagram. This experiment...Chapter 3, Problem 1EGiven The three salts are named as sodium sulfide, sodium bicarbonate and sodium chloride. The...Chapter 5, Problem 1DEChapter 6, Problem 1DEThe alkali metals such as rubidium and cesium which has lower first ionization energies can be used...The heat of hydrogenation of acetylene is −1299.53 kJ/mol and the fuel value of 3.0 mol acetylene is...The energy absorbed by the given compound is calculated by the formula, Energy=Plank's...
The given unknown gas is a noble gas and the difference in molar masses of noble gases is much...The force of attraction between the hydrogen and an electronegative atom is called hydrogen bonding....Explanation: The given polymer is first dissolved in the buffer solution. The experiment is...According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole...Given The chemical equation for the given hypothetical reaction is, aA+bB→cC+dD The reactants...Explanation: The spectrometer is a device which splits light into the array of separate colors which...If the solution is acidic, it changes blue litmus paper into red and there is no change in color for...Explanation: The concentration of NaOH solution is calculated by considering the small volume of the...Explanation: The chemicals involved in fracking operations are hydrochloric acid, sodium chloride,...The relation between the standard free energy change, standard entropy change and standard enthalpy...GivenThe electrical potential output of the cell is 1.50 V . The external device draws the current...Explanation: Pitchblende is a uranium ore with excess amount of UO2 , on oxidation UO2 leads to the...The physical state of the substance depends upon the size of the substance. The size of the atoms...The reaction of the given coordination compound with the solution of AgNO3 solution gives the...Explanation: The buffer solution of hemoglobin is prepared first. This buffer solution of hemoglobin...
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