OPENING INSIGHT THEME: Materials for Biomedical Engineering 201 CLOSING INSIGHT THEME: Molecular Scale Engineering for Drug. OPENING INSIGHT TOPIC: Cosmic Rays and Carbon Dating 475 CLOSING INSIGHT TOPIC: Modern Medical Imaging Methods 498.
Limiting Reactants 108
INSIGHT INTO Alternative Fuels and Fuel Additives 117
INSIGHT INTO Air Pollution 126
History and Application of the Gas Law 132
Stoichiometry of Reactions Involving Gases 139
Kinetic–Molecular Theory and Ideal Versus Real Gases 141
INSIGHT INTO Gas Sensors 148
INSIGHT INTO Incandescent and Fluorescent Lights 159
The Electromagnetic Spectrum 161
The Quantum Mechanical Model of the Atom 173
The Pauli Exclusion Principle and Electron Configurations 181
Periodic Trends in Atomic Properties 187
INSIGHT INTO Modern Light Sources: LEDs and Lasers 192
INSIGHT INTO Materials for Biomedical Engineering 201
The Ionic Bond 202
Keeping Track of Bonding: Lewis Structures 215
Shapes of Molecules 226
INSIGHT INTO Molecular Scale Engineering for Drug Delivery 234
Intermolecular Forces 256
Condensed Phases—Liquids 261
INSIGHT INTO Energy Use and the World Economy 281
Defining Energy 284
Energy Transformation and Conservation of Energy 286
Heat Capacity and Calorimetry 289
Enthalpy 295
The Second Law of Thermodynamics 326
Free Energy and Chemical Reactions 333
INSIGHT INTO The Economics of Recycling 335
Rate Laws and the Concentration Dependence of Rates 353
Temperature and Kinetics 366
Reaction Mechanisms 373
INSIGHT INTO Tropospheric Ozone 379
Equilibrium Concentrations 405
Solubility Equilibria 415
Free Energy and Chemical Equilibrium 425
INSIGHT INTO Borates and Boric Acid 427
Cell Potentials and Equilibrium 450
Batteries 453
INSIGHT INTO Corrosion Prevention 465
Kinetics of Radioactive Decay 481
Energetics of Nuclear Reactions 487
Transmutation, Fission, and Fusion 489
The Interaction of Radiation and Matter 495
INSIGHT INTO Modern Medical Imaging Methods 498
The Genesis of This Text
Content and Organization
We suspect that many instructors will not choose to include all of the material on equilibrium in Chapter 12, for example. Similarly, we have included more topics in Chapter 8, on summary stages, than we expect most faculty to include in their courses.
Topic Coverage
Therefore, departments or individual instructors must make some additional choices about the content best suited for their own students.
Specifi c Content Coverage
In light of this, we include references to the account role where appropriate through our MathConnections fields. These essays expand on and review mathematical concepts as they relate to the particular topic under study and appear wherever the connections between the topic at hand and mathematics seem particularly strong.
Connections between Chemistry and Engineering
The purpose of including calculus is not to increase the level of material presented, but rather to show the natural connections between the various subjects that students study.
Approach to Problem Solving
In most cases, it is not possible to arrive at a final numerical answer using the information provided, so students are forced to focus on developing a solution rather than just identifying and implementing an algorithm. End-of-chapter exercises include additional problems of this type so that a problem-solving focus can be fully integrated into the course.
Text Features
This feature grew out of the NSF-funded Evaluation of Problem Solving in Chemistry Lessons project. Marginal Notes Marginal notes in the text highlight additional facts, further emphasize points, or indicate related discussion earlier or later in the book.
New in this Edition
Each chapter also contains a number of additional problems that are not tied to any particular section and may incorporate ideas from multiple sections. Answers to all odd numbers are found at the end of the book in Appendix K.
Supplements for the Instructor
The problems for most chapters end with cumulative problems, asking students to synthesize information from the current chapter with what they have learned from previous chapters to form answers.
Faculty Companion Website
Instructor’s Resource CD-DVD Package
ExamView ® Computerized Testing CD-ROM
Supplements for the Student
Student Solutions Manual and Study Guide
OWL for General Chemistry
Go Chemistry ® for General Chemistry
Acknowledgments
Scott Oliver, State University of New York at Binghamton The late Robert Paine, Rochester Institute of Technology Steve Rathbone, Blinn College. Mike Shaw, Southern Illinois University-Edwardsville Joyce Solochek, Milwaukee School of Engineering Jack Tossell, University of Maryland.
Chemistry and Engineering
About This Text
Aluminum
But you probably wouldn't ask, "Where does the can containing this soda come from, and why is it made of aluminum?" The aluminum can has become so common that it is easy to take for granted. However, some of the early steps can be solved by clever applications of physical properties, and we will consider a few of them as we examine the introductory material in this chapter.
The Study of Chemistry
Corrosion—the breakdown of metals in the presence of air and moisture—is another commonly observed chemical change. In Figure 1.4, we can see that when water boils, the composition of individual molecules is the same in the liquid and gas phases.
The Science of Chemistry
This type of drawing emphasizes the fact that the ore is made up of different types of atoms, while only one type of atom is present in the metal. This formula is slightly more complicated than that of water, and we will look more closely at this type of symbolism in Chapter 2.
Observations in Science
Numbers and Measurements in Chemistry
Three key rules will be required to determine the number of significant figures in the results of calculations. Perform the calculation and express the result to the correct number of significant figures.
Problem Solving in Chemistry and Engineering
We will often include discussions about the relationships we form in the "strategic" part of the example problems. In this way, we can see an industrial process on a large scale while thinking in the microscopic perspective.
Material Selection and Bicycle Frames
Use the Internet to research the origins of energy units erg and calorie, and describe how they exemplify this type of historical development. If the density is 2.70 g/cm3, what is the thickness of the film in inches.
Polymers
The carbon atoms are linked together in a long chain called the backbone of the polymer in the polymer molecule, and there are two hydrogen atoms attached to each carbon. Plastic pipes made of PVC have been widely used in plumbing for many years, so you have Because these molecules are so large,.
Atomic Structure and Mass
But the existence and even relative abundance of isotopes can be proven by careful examination of the masses of atoms. Therefore, the combined total of protons and neutrons is called the mass number of the atom.
Ions
Looking at this expression, when both charges have the same sign (positive or negative), the resulting value for the force is a positive number. As the two equal charges are brought closer together, the term r 2 in the denominator shrinks and the (positive) force increases: the particles repel each other. When the charges have the same sign, the particles will repel each other, so the value of the force is positive.
If the charges have opposite signs, the particles will attract each other and the value of the force will be negative.
Compounds and Chemical Bonds
The number of each atom in the compound is indicated by a subscript to the right of the atom symbol. Water molecules associated with certain compounds called hydrates are indicated separately from the rest of the compound. If the molecular formula is C8H12N4, how many of each type of atom are in a molecule of the compound?
Here, the blue area shows these mobile (or "delocalized") electrons, while the red circles represent the positively charged "cores" of the individual atoms.
The Periodic Table
The shading of the squares in the periodic table represents the density of each element; darker shading indicates higher density. Elements that separate these two parts of the representative groups in the main body of the periodic table are called transition metals. The elements that appear below the rest of the periodic table are called lanthanides (named after the element lanthanum, Z = 57) and actinides (named after the element actinium, Z = 89).
Their general location in the periodic table is towards the left and at the bottom, as seen in the coloring of the periodic table in Figure 2.14.
Inorganic and Organic Chemistry
This huge number of compounds arises from some unusual aspects of the chemistry of carbon itself. Many of the polymer molecules discussed in this chapter contain thousands of carbon atoms. Solution We will first remove the symbols and bonds for all hydrogen atoms because they are all directly bonded to carbon.
In combination, these two facts allow us to fill in all the carbon and hydrogen atoms not explicitly written in a line structure.
Chemical Nomenclature
So when one of the charges is specified in the name, the full formula is known. When we encounter such a situation, we indicate the charge of the cation in the name with a Roman numeral in parentheses after the element name. The basic name oxyanion provides an element other than oxygen.
Example Problem 2.6 gives some examples of how to determine the name of an ionic compound.
Polyethylene
2.53 ■ Identify the region of the periodic table where you would expect to find each of the following types of elements. 2.72 ■ Give the formula for each of the following compounds:. a) sulfur dichloride, (b) dinitrogen pentaoxide, (c) silicon tetrachloride, (d) diboron trioxide (commonly called boron oxide). 2.73 ■ Write the molecular formula for each of the following covalent compounds: (a) sulfur hexafluoride, (b) bromine pentafluoride, (c) disulfur dichloride, (d) tetrasulfur tetranitride.
2.76 ■ Give the formula for each of the following ionic compounds: (a) ammonium carbonate, (b) calcium iodide, (c) copper(II) bromide, (d) aluminum phosphate, (e) silver(I) acetate .
Explosions
Close examination of the progress of explosive chemical reactions shows that they accelerate as they proceed. It is no coincidence; the generation of gases is actually very important for the development of the explosion. When a chemical reaction converts a solid explosive into a large number of gaseous molecules, those gases will initially occupy a volume similar to that of the solid.
When considering chemical reactions – including explosions – it is often useful to think in terms of the microscopic, macroscopic and symbolic perspectives introduced in Section 1.2.
Chemical Formulas and Equations
The underlying premise of the chemical equation is that it is a written representation of a chemical reaction. To maintain this condition, we must have the same number of atoms of each element on both sides of the chemical equation (see Figure 3.4). The stoichiometric coefficient multiplies the number of atoms of each element in the formula unit of the compound it precedes.
The coefficient of one before the propane would normally be omitted, but is explicitly stated here for emphasis.).
MathConnections
Aqueous Solutions and Net Ionic Equations
Strong electrolytes dissolve completely, so only individual ions are present in solution, with virtually no intact molecules. We will Figure 3.7 ❚ The pictures show a classroom demonstration in which a pair of copper rods is immersed in different solutions. In the commercial preparation of ammonium nitrate, pure ammonia (NH3) in the gas phase is combined with concentrated aqueous nitric acid (HNO3).
At this point, you're probably wondering, "Which of these equations is correct?" The answer is that all of these forms provide valid descriptions of the reaction, so none are inherently "better" than the others.
- Interpreting Equations and the Mole
- Calculations Using Moles and Molar Masses
- Explosives and Green Chemistry
- Gasoline and Other Fuels
The relationship between the mass of a sample and the number of moles present is the molar mass of the substance in question. Determine the molar mass of each of the following compounds, all of which have been used as explosives: (a) lead azide, PbN6, (b) nitroglycerin, C3H5N3O9, (c) mercury fulminate, Hg(ONC)2. So we need to determine the molar mass of the substance and then use that to do the conversion.
We know that the relationship between these two quantities is the molar mass of the compound, so we can start by calculating that.
CHCH 2 CH3CH2CH2CH2
- Fundamentals of Stoichiometry
- Limiting Reactants
- Theoretical and Percentage Yields
- Solution Stoichiometry
- Alternative Fuels and Fuel Additives
- Air Pollution
- Pressure
- History and Application of the Gas Law
- Partial Pressure
- Stoichiometry of Reactions Involving Gases
- Kinetic–Molecular Theory and Ideal Versus Real Gases
- Gas Sensors
- Incandescent and Fluorescent Lights
- The Electromagnetic Spectrum
- Atomic Spectra
Using the mole ratio from the balanced equation is the only new concept here. We know the number of moles of the first reactant (or molarity and volume) and the volume of the second reactant used. If the temperature is constant throughout this process, what is the new pressure of the gas?
What is the volume of the container and what are the partial pressures of each gas. M is the molar mass of the gas, R is the gas constant, and T is the temperature. In the wave model, both wavelength and frequency correspond to the color of light.
