Chemistry
Simple Molecules
Simple molecules are composed of a small number of atoms bonded together. They are typically held together by covalent bonds and include familiar substances like water (H2O) and carbon dioxide (CO2). These molecules are fundamental building blocks in chemistry and play essential roles in various chemical reactions and processes.
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4 Key excerpts on "Simple Molecules"
eBook - ePub- Dov M. Gabbay, Paul Thagard, John Woods(Authors)
- 2011(Publication Date)
- North Holland(Publisher)
Atoms and Molecules in Classical Chemistry and Quantum Mechanics Brian T. Sutcliffe and R. Guy Woolley 1. The Evolution of Classical Molecular Structure This first section gives a brief account of the development of the atomic-molecular conception of chemistry. Although we cannot go into details, an essential backdrop to the whole discussion is the importance throughout human history of the practical chemical arts which have informed the production of the whole range of useful materials and stimulated enquiry into the theoretical aspects of chemical processes. Chemistry is concerned with the composition and properties of matter, and with the transformations of matter that can occur spontaneously or under the action of heat, radiation or other sources of energy. From the results of chemical experiments the chemist singles out 1 a particular class of materials that have characteristic and invariant properties. Such materials are called pure substances and may be of two kinds, viz: compounds and elements. Formally, elements may be defined as substances which have not been converted either by the action of heat, radiation, or chemical reaction with other substances, or small electrical voltages, into any simpler substance. Compounds are formed from the chemical combination of the elements, and have properties that are invariably different from the properties of the constituent elements; they are also homogeneous. These statements derive from Antiquity 2. This characteristic chemical notion of a pure substance is based on an ideal conception of the chemical and physical properties of matter and their changes under specified experimental conditions (pressure, temperature, in inert containers etc.). Physical properties belong to materials in isolation from other materials, and are those properties that can be observed without conversion of the material into other substances, whereas chemical properties refer to the chemical reactions that materials undergo
eBook - PDF- T. W. Graham Solomons, Craig B. Fryhle, Scott A. Snyder(Authors)
- 2022(Publication Date)
- Wiley(Publisher)
1 CHAPTER 1 Chakrapong Worathat/123RF studiovin/Shutterstock The Basics Bonding and Molecular Structure Organic chemistry plays a role in all aspects of our lives, from the reactions that keep us alive, to medicines that fight disease, to materials for new technologies such as high definition tele- visions. If you take the time to understand organic chemistry, you will truly have the power to change society. Indeed, organic chemistry, provides the power to synthesize new drugs, to engineer molecules that can make computer processors run more quickly, to understand why grilled meat can cause cancer and how its effects can be combated, and to design ways to knock the calories out of sugar while still making food taste deliciously sweet. It can explain biochemical processes like aging, neural functioning, and cardiac arrest and show how we can prolong and improve life. It can do almost anything. IN THIS CHAPTER WE WILL CONSIDER: • what kinds of atoms make up organic molecules • the principles that determine how the atoms in organic molecules are bound together • how best to depict organic molecules WHY DO THESE TOPICS MATTER? At the end of the chapter, we will see how some of the unique organic structures that nature has woven together possess amazing properties that we can harness to aid human health. See the online course materials in for additional examples, videos, and practice. 2 CHAPTER 1 The Basics Organic chemistry is the chemistry of compounds that contain the element carbon. If a compound does not contain the element carbon, it is said to be inorganic. Look for a moment at the periodic table. More than a hundred elements are listed there.
eBook - ePub- Mukesh Doble, Anil Kumar Kruthiventi, Vilas Ganjanan Gaikar(Authors)
- 2004(Publication Date)
- CRC Press(Publisher)
Thus, if more than two atoms combine, we get an electron cloud distributed aross all the nuclei of the atoms. The shape of this electron cloud is distinct and unique to a molecule. That is, say, methane—all of methane molecules have the same electron cloud distribution, but the electron cloud distribution of methyl chloride is different from methane, as shown in Fig. 2.1. In fact it is this unique electron cloud distribution over a molecule that determines its reactivity. 2.1.3 Concept of Chemical Bonding These notes are designed to give a quick guide to bonding—there is a lot more to this subject than is covered here. The forces that hold atoms together within chemical compounds, the chemical bonds, are electrical in nature. Chemical bonds form to lower the energy of the system, the components of the system becomes more stable through the formation of the bonds. This is true even for noncovalent interactions (hydrogen bond, van der Waals interaction, electrostatic interaction, etc.), which are far more important among biomolecules and supramolecular aggregates. These bonding and noncovalent interactions are Nature’s way of attaining greater stability. The development of a sound chemical bonding theory started with the idea put forth by G.N.Lewis in 1916, that bonding results from a sharing of electron pair between two atoms. Two major bonding interactions are common in Organic chemistry: one in which the two atoms constituting the bond share the two electrons, a covalent bond (Fig. 2.2), and the other in which one of the atoms constituting the bond takes both the electrons and attains a negative charge while the other atom loosing an electron attains a positive charge (“sharing” is unequal), an ionic bond (Fig
Available until 31 Dec |Learn more30-Second Chemistry
The 50 most elemental concepts in chemistry, each explained in half a minute.
- Nivaldo Tro(Author)
- 2020(Publication Date)
- Ivy Press(Publisher)
Our Earth contains about 91 different naturally occurring elements, each one with its own distinctive properties. However, certain groups of elements share similarities. The periodic law and the corresponding periodic table allow us to organize the known elements in ways that help us make sense of their properties.INSIDE THE ATOM BONDING ATOMS TOGETHER THE UNIQUENESS PRINCIPLERELATED TOPICS
See also1830–95 German chemist who made significant contributions to the periodic table3-SECOND BIOGRAPHIES
JULIUS LOTHAR MEYERDMITRI MENDELEEV 1834–1907Russian chemistry professor who formulated the periodic law and constructed one of the first periodic tablesMendeleev formulated one of the first periodic tables, which organizes elements according to atomic number and chemical properties.30-SECOND TEXT
Nivaldo TroBONDING ATOMS TOGETHER
the 30-second chemistryAtoms bond together by either sharing (covalent bonding) or transferring (ionic bonding) the electrons in their highest-energy orbitals to form compounds. Sharing of electrons typically occurs between two or more non-metals, resulting in a molecular compound, so called because it is composed of distinct molecules (groups of atoms bonded together). Transfer of electrons typically occurs from a metal to a non-metal and results in an ionic compound. Ionic compounds do not contain distinct molecules, but rather exist as an array of ions (charged particles) with alternating positive and negative charge. Water is a good example of a molecular compound. We represent a compound with a chemical formula, which tells us the elements present in the compound and the relative number of atoms of each one. For example, the formula for water is H2 O, which means that a water molecule is composed of two hydrogen atoms and one oxygen atom, and the formula for sucrose (table sugar) is C12 H22 O11
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