Principles of General, Organic, Biologi...2nd EditionJanice Gorzynski Smith Dr. Publisher: McGraw-Hill EducationISBN: 9780073511191
Principles of General, Organic, Biologi...
Solutions for Principles of General, Organic, Biological Chemistry
Browse All Chapters of This Textbook
Chapter 1 - Matter And MeasurementChapter 1.1 - Chemistry—the Science Of Everyday ExperienceChapter 1.2 - States Of MatterChapter 1.3 - Classification Of MatterChapter 1.4 - MeasurementChapter 1.5 - Significant FiguresChapter 1.6 - Scientific NotationChapter 1.7 - Problem Solving Using Conversion FactorsChapter 1.8 - Focus On Health & Medicine: Problem Solving Using Clinical Conversion FactorsChapter 1.9 - Temperature
Chapter 1.10 - Density And Specific GravityChapter 2 - Atoms And The Periodic TableChapter 2.1 - ElementsChapter 2.2 - Structure Of The AtomChapter 2.3 - IsotopesChapter 2.4 - The Periodic TableChapter 2.5 - Electronic StructureChapter 2.6 - Electronic ConfigurationsChapter 2.7 - Valence ElectronsChapter 2.8 - Periodic TrendsChapter 3 - Ionic And Covalent CompoundsChapter 3.1 - Introduction To BondingChapter 3.2 - IonsChapter 3.3 - Ionic CompoundsChapter 3.4 - Naming Ionic CompoundsChapter 3.5 - Physical Properties Of Ionic CompoundsChapter 3.6 - Polyatomic IonsChapter 3.7 - Covalent BondingChapter 3.8 - Lewis StructuresChapter 3.9 - Naming Covalent CompoundsChapter 3.10 - Molecular ShapeChapter 3.11 - Electronegativity And Bond PolarityChapter 3.12 - Polarity Of MoleculesChapter 4 - Energy And MatterChapter 4.1 - EnergyChapter 4.2 - The Three States Of MatterChapter 4.3 - Intermolecular ForcesChapter 4.4 - Boiling Point And Melting PointChapter 4.5 - Specific HeatChapter 4.6 - Energy And Phase ChangesChapter 4.7 - Heating And Cooling CurvesChapter 5 - Chemical ReactionsChapter 5.1 - Introduction To Chemical ReactionsChapter 5.2 - Balancing Chemical EquationsChapter 5.3 - The Mole And Avogadro’s NumberChapter 5.4 - Mass To Mole ConversionsChapter 5.5 - Mole Calculations In Chemical EquationsChapter 5.6 - Mass Calculations In Chemical EquationsChapter 5.7 - Oxidation And ReductionChapter 5.8 - Energy Changes In ReactionsChapter 5.9 - Reaction RatesChapter 5.10 - EquilibriumChapter 6 - GasesChapter 6.1 - Gases And PressureChapter 6.2 - Boyle’s Law Relating Gas Pressure And VolumeChapter 6.3 - Charles’s Law Relating Gas Volume And TemperatureChapter 6.4 - Gay–lussac’s Law Relating Gas Pressure And TemperatureChapter 6.5 - The Combined Gas LawChapter 6.6 - Avogadro’s Law Relating Gas Volume And MolesChapter 6.7 - The Ideal Gas LawChapter 6.8 - Dalton’s Law And Partial PressuresChapter 6.9 - Focus On The Environment: Ozone And Carbon Dioxide In The AtmosphereChapter 7 - SolutionsChapter 7.1 - MixturesChapter 7.2 - Electrolytes And NonelectrolytesChapter 7.3 - Solubility—general FeaturesChapter 7.4 - Solubility—effects Of Temperature And PressureChapter 7.5 - Concentration Units—percent ConcentrationChapter 7.6 - Concentration Units—molarityChapter 7.7 - DilutionChapter 7.8 - Osmosis And DialysisChapter 8 - Acids And BasesChapter 8.1 - Introduction To Acids And BasesChapter 8.2 - The Reaction Of A Brønsted–lowry Acid With A Brønsted–lowry BaseChapter 8.3 - Acid And Base StrengthChapter 8.4 - Dissociation Of WaterChapter 8.5 - The Ph ScaleChapter 8.6 - Common Acid–base ReactionsChapter 8.7 - TitrationChapter 8.8 - BuffersChapter 9 - Nuclear ChemistryChapter 9.1 - IntroductionChapter 9.2 - Nuclear ReactionsChapter 9.3 - Half-lifeChapter 9.4 - Detecting And Measuring RadioactivityChapter 9.5 - Focus On Health & Medicine: Medical Uses Of RadioisotopesChapter 9.6 - Nuclear Fission And Nuclear FusionChapter 10 - Introduction To Organic MoleculesChapter 10.1 - Introduction To Organic ChemistryChapter 10.2 - Characteristic Features Of Organic CompoundsChapter 10.3 - Drawing Organic MoleculesChapter 10.4 - Functional GroupsChapter 10.5 - AlkanesChapter 10.6 - Alkane NomenclatureChapter 10.7 - CycloalkanesChapter 10.9 - Physical PropertiesChapter 10.10 - Focus On The Environment: CombustionChapter 11 - Unsaturated HydrocarbonsChapter 11.1 - Alkenes And AlkynesChapter 11.2 - Nomenclature Of Alkenes And AlkynesChapter 11.3 - Cis–trans IsomersChapter 11.5 - Reactions Of AlkenesChapter 11.6 - Focus On Health & Medicine: Margarine Or Butter?Chapter 11.7 - Polymers—the Fabric Of Modern SocietyChapter 11.9 - Nomenclature Of Benzene DerivativesChapter 11.10 - Focus On Health & Medicine: Sunscreens And AntioxidantsChapter 12 - Organic Compounds That Contain Oxygen, Halogen, Or SulfurChapter 12.1 - IntroductionChapter 12.2 - Structure And Properties Of AlcoholsChapter 12.3 - Structure And Properties Of EthersChapter 12.5 - Reactions Of AlcoholsChapter 12.6 - Alkyl HalidesChapter 12.7 - ThiolsChapter 12.8 - Structure And Properties Of Aldehydes And KetonesChapter 12.9 - Focus On Health & Medicine: Interesting Aldehydes And KetonesChapter 12.10 - Oxidation Of AldehydesChapter 12.11 - Looking Glass Chemistry—molecules And Their Mirror ImagesChapter 13 - Carboxylic Acids, Esters, Amines, And AmidesChapter 13.1 - IntroductionChapter 13.2 - Nomenclature Of Carboxylic Acids And EstersChapter 13.3 - Physical Properties Of Carboxylic Acids And EstersChapter 13.4 - Interesting Carboxylic Acids In Consumer Products And MedicinesChapter 13.5 - The Acidity Of Carboxylic AcidsChapter 13.6 - Reactions Involving Carboxylic Acids And EstersChapter 13.7 - AminesChapter 13.8 - Amines As BasesChapter 13.9 - AmidesChapter 13.10 - Interesting Amines And AmidesChapter 14 - CarbohydratesChapter 14.1 - IntroductionChapter 14.2 - MonosaccharidesChapter 14.3 - The Cyclic Forms Of MonosaccharidesChapter 14.4 - Reactions Of MonosaccharidesChapter 14.5 - DisaccharidesChapter 14.6 - PolysaccharidesChapter 15 - LipidsChapter 15.1 - Introduction To LipidsChapter 15.2 - Fatty AcidsChapter 15.3 - WaxesChapter 15.4 - Triacylglycerols—fats And OilsChapter 15.5 - Hydrolysis Of TriacylglycerolsChapter 15.6 - PhospholipidsChapter 15.7 - Cell MembranesChapter 15.8 - Focus On Health & Medicine: Cholesterol, The Most Prominent SteroidChapter 15.9 - Steroid HormonesChapter 15.10 - Focus On Health & Medicine: Fat-soluble VitaminsChapter 16 - Amino Acids, Proteins, And EnzymesChapter 16.2 - Amino AcidsChapter 16.3 - Acid–base Behavior Of Amino AcidsChapter 16.4 - PeptidesChapter 16.5 - Focus On The Human Body: Biologically Active PeptidesChapter 16.6 - ProteinsChapter 16.7 - Focus On The Human Body: Common ProteinsChapter 16.8 - Protein Hydrolysis And DenaturationChapter 16.9 - EnzymesChapter 16.10 - Focus On Health & Medicine: Using Enzymes To Diagnose And Treat DiseasesChapter 17 - Nucleic Acids And Protein SynthesisChapter 17.1 - Nucleosides And NucleotidesChapter 17.2 - Nucleic AcidsChapter 17.3 - The Dna Double HelixChapter 17.4 - ReplicationChapter 17.6 - TranscriptionChapter 17.11 - Focus On Health & Medicine: VirusesChapter 18 - Energy And MetabolismChapter 18.1 - An Overview Of MetabolismChapter 18.2 - Atp And Energy ProductionChapter 18.3 - Coenzymes In MetabolismChapter 18.4 - GlycolysisChapter 18.5 - The Fate Of PyruvateChapter 18.6 - The Citric Acid Cycle
Book Details
Serious Science with an Approach Built for Today's Students. This one-semester Principles of General, Organic, and Biological Chemistry textbook is written with the same student-focused, direct writing style that has been so successful in the Smith: Organic Chemistry and two-semester General, Organic, and Biological Chemistry texts. Janice Smith draws on her extensive teaching background to deliver a student-friendly format - with limited use of text paragraphs, through concisely written bulleted lists and highly detailed, well-labeled "teaching" illustrations - that provides need-to-know information in a succinct style for today's students.
Sample Solutions for this Textbook
We offer sample solutions for Principles of General, Organic, Biological Chemistry homework problems. See examples below:
Chapter 1, Problem 1.31UKCChapter 1, Problem 1.52APThe given quantity is 1,234 g. The number of significant figures in the number 1,234 g is four. The...The given quantity is 0.001 25 m. The number of significant figures in the number 0.001 25 m is...Chapter 1, Problem 1.67APChapter 1, Problem 1.70APGiven, The temperature in degree Celsius is 53oC. Celsius can be converted to Fahrenheit using the...Chapter 2, Problem 2.33UKCGiven, The element symbol is C. The mass number is 12. The atomic number of carbon is 6. Atomic...
Given, The atomic number is 10. The mass number is 20. An element with atomic number 10 is Neon....Chapter 2, Problem 2.59APGiven, The atomic number of Tin is 50. Atomic number of an element=The number of protons Thus the...Given, The atomic number is 13. The mass number is 27. The number of proton is, Atomic number of an...Given, The mass number of silver is 115. The atomic number of silver is 47. The number of proton is,...Chapter 3, Problem 3.33UKCThe cation is Na+. Bromide (Br-): Sodium reacts with bromide (derived from bromine) to form sodium...The cation is K+. Iodide (I-): Potassium reacts with iodide (derived from iodine) to form potassium...When potassium cation (K+) reacts with bisulfate ion (HSO4-), the compound formed is potassium...Chapter 3, Problem 3.66APWhen barium cation (Ba2+) reacts with cyanide ion (CN-), the compound formed is bariumcyanide...When iron (III) cation (Fe3+) reacts with cyanide ion (CN-), the compound formed is iron (III)...Chapter 4, Problem 4.29UKCGiven, The mass of water is 50 g. The temperature at initial (T1) is 15oC. The temperature at final...The amount of energy needed to melt ice: Given, The mass of ice melt is 45 g. The specific heat of...The amount of energy needed to heat water: Given, The mass of water is 150 g. The specific heat of...Chapter 5, Problem 5.39UKCThe formula weight of C18H30O2 is calculated as, 30 H atoms×1.008 amu = 30.24 amu18 C atoms×12.01...The formula weight of NaNO2 is calculated as, 1Na atoms × 22.99 amu = 22.99 amu1 N atoms×14.01amu =...Given, Moles of C2H2 are 2.5 moles. The balanced chemical equation is, 2 C2H2+5 O2→Δ4 CO2+2 H2O The...Given, Moles of Na are 3.0 moles. The balanced chemical equation is, 2 Na(s)+2 H2O(l)→Δ2...The formula weight of sucrose is calculated as, 12 C atoms × 12.01 amu = 144.12 amu22 H atoms×1.008...The formula weight of diethyl ether is calculated as, 4 C atoms × 12.01 amu = 48.04 amu10 H...The pressure on the pressure gauge used by the scuba divers is 2600psi.Given, The pressure of the gas at initial state (P1) is 2.5 atm. The volume of the gas at initial...Given, The volume of the gas at initial state (V1) is 10 ml. The temperature of the gas at initial...Given, The pressure of the gas at initial state (P1) is 3.25 atm. The temperature of the gas at...Given, The pressure of the gas at initial state (P1) is 1.74 atm. The temperature of the gas at...Given, The volume of the gas at initial state (V1) is 4.0 L. The volume of the gas at final state...Given, The volume of the gas at initial state (V1) is 1.1 L. The volume of the gas at final state...Potassium iodide is an ionic compound, hence separation of ions will takes place when they are...Potassium chloride (KCl) consists of K+ and Cl- ions. Potassium has +1 charge, there are 1 Eq of K+...Given, Weight/volume percent of the solution=4.8%(w/v) Volume of the solution=250mL The mass of the...Given, Volume of solution=150mL Molarity of solution=0.25M Milliliters is converted into liters,...Given, Volume of solution=250mL Molarity of solution=0.55M Milliliters is converted into liters,...Given, Mass of the solute=1300μg Mass of the solution=1kg Microgram is converted into grams,...Given, M1=2.5M M2=1.0M V2=25mL The initial volume of the solution is calculated as,...Given, M1=5.0M M2=4.0M V2=45mL The initial volume of the solution is calculated as,...Chapter 8, Problem 8.31UKCAcid loses a proton and forms a conjugate base. Base gains a proton and forms a conjugate acid. The...Acid loses a proton and forms conjugate base. Base accepts a proton and forms conjugate acid. The...Acid loses a proton and forms conjugate base. Base accepts a proton and forms conjugate acid. The...Chapter 8, Problem 8.69APChapter 8, Problem 8.70APChapter 8, Problem 8.71APGiven, [OH−]=10-12MKw=1.0×10-14 The concentration of H3O+ is calculated as,...Chapter 9, Problem 9.23UKCGiven, The mass of Iodine-131 at initial is 64 mg. The half-life of Iodine-131 is 8 d. The time...Given, The mass of Phosphorous-32 at initial is 124 mg. The half-life of Phosphorous-32 is 14 d. The...The ball and stick model is given below, The black ball represents carbon atom, the white ball...Chapter 10, Problem 10.35UKCChapter 10, Problem 10.36UKCThe potassium iodide (KI) compound forms an ionic bond. The elements potassium and iodine have...The structure of an alkane compound having five carbon atoms has to be drawn. The alkane compounds...The number of carbon atoms present in a straight-chain alkane having 20 hydrogen atoms has given...Chapter 10, Problem 10.77APThe structure can be derived from the given IUPAC name 3-ethyl-3-methylhexane. First step, look at...The given compound is anethole. The molecular formula of anethole is C10H12O. The structure can be...Given compound is norepinephrine, In the given drug (i,e) norepinephrine, the CH2 group is not a...Chapter 12, Problem 12.39UKCChapter 12, Problem 12.40UKCStructure of lidocaine is: Lidocaine contains two nitrogen atoms. Among this, one nitrogen atom is...Structure of monosaccharide A is drawn as shown below. The carbonyl group is present on the terminal...Given monosaccharide structure is: This contains a carbonyl group in the terminal carbon atom C1....Given monosaccharide structure is: This contains a carbonyl group in the terminal carbon atom C1....Food B is high in unsaturated triacylglycerols because unsaturated fats are considered as healthy...In ball and stick model different atoms are as follows: Amino acid can be drawn as follows:Chapter 17, Problem 17.26UKCChapter 17, Problem 17.29UKCChapter 17, Problem 17.30UKCChymotrypsin is enzyme that known to break protein into individual amino acids. It is used in small...
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