Moore, EdD, teaches chemistry at Stephen F. Austin University in Texas and is the author of Chemistry For Dummies. Richard Langley, PhD, grades the free-response portion of the AP Chemistry Exam. Together with John, he authored Organic Chemistry II For Dummies. Chapter 1: Biochemistry: What. Physics for Beginners 2 Matthew Raspanti been, and still is, intrigued by the fundamental nature of its inquiry. This is shown by the success of dozens of books that have been written since Stephen Hawking’ s 'A Brief History of Time' (1988) became a best seller. In most of the popular books on the market, however, the bulk of the.
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So why do so many of us desperately resist learning chemistry when we're young? Now there's a fun, easy way to learn basic chemistry. Whether you're studying chemistry in school and you're looking for a little help making sense of what's being taught in class, or you're just into learning new things, Chemistry For Dummies gets you rolling with all the basics of matter and energy, atoms and molecules, acids and bases, and much more! Tracks a typical chemistry course, giving you step-by-step lessons you can easily grasp Packed with basic chemistry principles and time-saving tips from chemistry professors Real-world examples provide everyday context for complicated topics Full of modern, relevant examples and updated to mirror current teaching methods and classroom protocols, Chemistry For Dummies puts you on the fast-track to mastering the basics of chemistry. Author by: Arthur Winter, PhDLanguange: enPublisher by: John Wiley & SonsFormat Available: PDF, ePub, MobiTotal Read: 33Total Download: 121File Size: 46,7 MbDescription: A plain-English guide to one of the toughest science courses around Organic chemistry is rated among the most difficult courses that students take and is frequently the cause of washout among pre-med, medical, and nursing students.
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Author by: John T. MooreLanguange: enPublisher by: For DummiesFormat Available: PDF, ePub, MobiTotal Read: 88Total Download: 187File Size: 49,6 MbDescription: We’re all natural born chemists. Every time we cook, clean, take a shower, drive a car, use a solvent, such as fingernail polish remover, or perform any of the countless everyday activities that involve complex chemical reactions we’re doing chemistry. You might even say that we’re all participating in a grand chemistry experiment that started with the first human who mixed pigments to do a cave painting. Why do so many of us desperately resist learning chemistry when we’re young? Maybe it has something to do with the way it’s taught in school. Now there’s a fun, easy way to learn basic chemistry.
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An extension of the successful Organic Chemistry I For Dummies Covers topics in a straightforward and effective manner Explains concepts and terms in a fast and easy-to-understand way Whether you're confused by composites, baffled by biomolecules, or anything in between, Organic Chemistry II For Dummies gives you the help you need — in plain English! Author by: John T. MooreLanguange: enPublisher by: John Wiley & SonsFormat Available: PDF, ePub, MobiTotal Read: 71Total Download: 726File Size: 45,7 MbDescription: Chemistry Essentials For Dummies (146) was previously published as Chemistry Essentials For Dummies (363). While this version features a new Dummies cover and design, the content is the same as the prior release and should not be considered a new or updated product.
Whether studying chemistry as part of a degree requirement or as part of a core curriculum, students will find Chemistry Essentials For Dummies to be an invaluable quick reference guide to the fundamentals of this often challenging course. Chemistry Essentials For Dummies contains content focused on key topics only, with discrete explanations of critical concepts taught in a typical two-semester high school chemistry class or a college level Chemistry I course, from bonds and reactions to acids, bases, and the mole. This guide is also a perfect reference for parents who need to review critical chemistry concepts as they help high school students with homework assignments, as well as for adult learners headed back into the classroom who just need to a refresher of the core concepts. The Essentials For Dummies Series Dummies is proud to present our new series, The Essentials For Dummies. Now students who are prepping for exams, preparing to study new material, or who just need a refresher can have a concise, easy-to-understand review guide that covers an entire course by concentrating solely on the most important concepts.
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Chemical Bonding BasicsIn bonding, atoms lose, gain, or share electrons in order to have the same number of electrons as the noble gas that’s nearest on the periodic table. Ionic, covalent, and metallic bonds are formed by combinations of metals and nonmetals.Metal + nonmetal = ionic bond.Nonmetal + nonmetal = covalent bond.Metal + metal = metallic bondWhen two elements engage in ionic bonding, one or more electrons are transferred from the metal to the nonmetal, forming ions (charged atoms).
The metal, having lost one or more electrons, forms a cation, an ion with a positive charge; the nonmetal, having gained one or more electrons, becomes an anion, an ion with a negative charge. Chemistry Concepts: Energy Levels and OrbitalsA lot of chemistry is explained by the sharing and trading of electrons between atoms. Understanding how electrons are arranged in an atom is a building block of Chem I.Electrons in an atom are contained in specific energy levels (1, 2, 3, and so on) that are different distances from the nucleus. The larger the number of the energy level, the farther it is from the nucleus. Electrons that are in the highest energy level are called valence electrons. Within each energy level is a volume of space where specific electrons are likely to be located.
These spaces, called orbitals, are of different shapes, denoted by a letter (s, p, d, f, g). (In most cases, only the electrons contained in the s and p orbitals are considered valence electrons.) Electrons seek the lowest energy level possible.The following electron-filling pattern indicates how the electrons fill into the energy levels. Knowing this pattern is useful in many aspects of chemistry, including predicting the bonding situation of a particular atom and in the prediction of the geometry of a covalent compound.Electron filling pattern: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f.
Digging the Mole Concept in ChemistryThe mole (abbreviate mol and sometimes called Avogadro ‘ s number) is a conversion number that allows a chemist or chemistry student to move from the microscopic world of atoms, ions, and molecules to the macroscopic world of grams, kilograms, and tons. The mole is used in reaction stoichiometry to predict how much product can be made from a certain amount of reactant or how much reactant is required to produce a certain amount of product.If you know the particles, moles, or grams of a substance, you can calculate the other two measurements by using the following equation:1 mole = 6.022 × 10 23 particles/mol = formula weight expressed in grams. The Basic Chemistry of Acids and BasesA lot of chemistry requires you to understand the difference between acids and bases. An acid is a substance that donates an H + ion to another chemical species called a base. A base is a substance that accepts (combines with) an H + ion.If you need to know the concentration of the H + ion in solution, you can do so by representing the H + molarity, H +. Another way to represent the H + concentration is the pH, which is the negative logarithm of the H + molarity. The following equation shows this mathematical relationship as well as the way to calculate the H + molarity given the pH:pH = –logH +; H + = 10 –pH.pH = 7 is neutral.pH less than 7 is acidic.pH greater than 7 is basic.
The Combined Gas Law and Ideal Gas LawWhen studying the properties of gases, you need to know the relationships between the variables of volume (V), pressure (P), Kelvin temperature (T), and the amount in moles (n) so that you can calculate missing information ( P, V, T, or n) and solve reaction stoichiometry problems. Although the pairs of variables have individual relationships, the two most important and useful gas laws are the combined gas law and the ideal gas law: Combined gas law( P 1 V 1)/ T 1=( P 2 V 2)/ T 2( T must be in Kelvin)Ideal gas lawPV = nR T(R = 0.0821 L atm/K.mol).