From Wikipedia, the free encyclopedia
A compound is a
composed of many identical
(or ) composed of
from more than one
held together by .
There are four types of compounds, depending on how the constituent atoms are held together:
held together by
held together by
held together by
held together by .
compounds have a unique numerical identifier assigned by the
(CAS): its .
is a way of expressing information about the proportions of atoms that constitute a particular chemical compound, using the standard abbreviations for the chemical elements, and
to indicate the number of atoms involved. For example,
is composed of two
atoms bonded to one
atom: the chemical formula is H2O.
A compound can be converted to a different chemical composition by interaction with a second chemical compound via a . In this process, bonds between atoms are broken in both of the interacting compounds, and then bonds are reformed so that new associations are made between atoms. Schematically, this reaction could be described as AB + CD -& AD + CB, where A, B, C, and D a and AB, AD, CD, and CB are each unique compounds.
bonded to an identical chemical element is not a chemical compound since only one element, not two different elements, is involved. Examples are the
(H2) and the
Any substance consisting of two or more different types of
() in a fixed proportion of its atoms (i.e., ) can be termed a chemical compound; the concept is most readily understood when considering pure .:15
It follows from their being composed of fixed proportions of two or more types of atoms that chemical compounds can be converted, via , into compounds or substances each having fewer atoms. The ratio of each element in the compound is expressed in a ratio in its chemical formula. In the case of , the proportions may be reproducible with regard to their preparation, and give fixed proportions of their component elements, but proportions that are not integral [e.g., for , PdHx (0.02 & x & 0.58)]. Chemical compounds have a unique and defined
held together in a defined spatial arrangement by . Chemical compounds can be
compounds held together by ,
held together by ,
held together by , or the subset of
that are held together by . Pure
are generally not considered chemical compounds, failing the two or more atom requirement, though they often consist of molecules composed of multiple atoms (such as in the
H2, or the
S8, etc.).
There is varying and sometimes inconsistent nomenclature differentiating substances, which include truly non-stoichiometric examples, from chemical compounds, which require the fixed ratios. Many solid chemical substances—for example many —are chemical substances, but do not have simple formulae reflecting chemically bonding of elements to one ano even so, these
substances are often called "". It may be argued that they are related to, rather than being chemical compounds, insofar as the variability in their compositions is often due to either the presence of foreign elements trapped within the crystal structure of an otherwise known true chemical compound, or due to perturbations in structure relative to the known compound that arise because of an excess of deficit of the constituent elements at pla such non-stoichiometric substances form most of the
of the Earth. Other compounds regarded as chemically identical may have varying amounts of heavy or light
of the constituent elements, which changes the ratio of elements by mass slightly.
Compounds are held together through a variety of different types of bonding and forces. The differences in the types of bonds in compounds differ based on the types of elements present in the compound.
are the weakest force of all . They are temporary attractive forces that form when the
in two adjacent atoms are positioned so that they create a temporary . Additionally, London dispersion forces are responsible for condensing
substances to liquids, and to further freeze to a solid state dependent on how low the temperature of the environment is.
A , also known as a molecular bond, involves the sharing of electrons between two atoms. Primarily, this type of bond occurs between elements that fall close to each other on the , yet it is observed between some metals and nonmetals. This is due to the mechanism of this type of bond. Elements that fall close to each other on the periodic table tend to have similar , which means they have a similar affinity for electrons. Since neither element has a stronger affinity to donate or gain electrons, it causes the elements to share electrons so both elements have a more stable .
occurs when
are completely transferred between elements. Opposite to covalent bonding, this chemical bond creates two oppositely charged ions. The metals in ionic bonding usually lose their valence electrons, becoming a positively charged . The nonmetal will gain the electrons from the metal, making the nonmetal a negatively charged . As outlined, ionic bonds occur between an electron donor, usually a metal, and an electron acceptor, which tends to be a nonmetal.
occurs when a hydrogen atom bonded to an electronegative atom forms an
connection with another electronegative atom through interacting dipoles or charges.
Whitten, Kenneth W.; Davis, Raymond E.; Peck, M. Larry (2000), General Chemistry (6th ed.), Fort Worth, TX: Saunders College Publishing/Harcourt College Publishers,  
Brown, Theodore L.; LeMay, H. E Bursten, Bruce E.; Murphy, Catherine J.; Woodward, Patrick (2009),
(11th ed.), Upper Saddle River, NJ: Pearson/Prentice Hall, pp. 5–6,  ,
from the original on
Hill, John W.; Petrucci, Ralph H.; McCreary, Terry W.; Perry, Scott S. (2005),
(4th ed.), Upper Saddle River, NJ: Pearson/Prentice Hall, p. 6,  ,
from the original on
Wilbraham, A Matta, M Staley, D Waterman, Edward (2002), Chemistry (1st ed.), Upper Saddle River, NJ: Pearson/Prentice Hall, p. 36,  
. ScienceDaily.
from the original on .
Manchester, F. D.; San-Martin, A.; Pitre, J. M. (1994). "The H-Pd (hydrogen-palladium) System". Journal of Phase Equilibria. 15: 62. :.
; Jones, Loretta (2004). Chemical Principles: The Quest for Insight.
. www.chem.purdue.edu.
from the original on .
. Chemistry LibreTexts. .
from the original on .
Chemistry, International Union of Pure and Applied. . goldbook.iupac.org. :.
from the original on .
. chemistry.elmhurst.edu.
from the original on .
. www.chem.purdue.edu.
from the original on .
. www.chemguide.co.uk.
from the original on .
Robert Siegfried (2002), From elements to atoms: a history of chemical composition, American Philosophical Society,  
in Wiktionary, the free dictionary.
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出版社: S Softcover reprint of the original 1st ed. 年9月18日)
平装: 223页
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目录
1. Polyester.- 1.1. Introduction.- 1.2. Disperse dyes.- 1.2.1. Aqueous phase transfer.- 1.2.2. Thermodynamics of dyeing.- 1.2.3. Kinetics of dyeing.- 1.2.4. Effect of crystal form of the dye on dye adsorption.- 1.2.5. Effect of particle size and distribution on dye adsorption.- 1.2.6. Effect of dispersing agents on dye adsorption.- 1.2.7. Effect of levelling agents on dye adsorption.- 1.2.8. Effect of temperature on dye adsorption.- 1.2.9. Isomorphism.- 1.2.10. Oligomers.- 1.2.11. Carrier dyeing.- 1.2.12. Solvent-assisted dyeing.- 1.2.13. Solvent dyeing.- 1.2.14. High-temperature dyeing.- 1.2.15. Thermofixation.- 1.2.16. Afterclearing.- 1.3. Azoic colorants.- 1.4. Vat dyes.- References.- 2. Nylon.- 2.1. Introduction.- 2.2. Anionic dyes.- 2.2.1. Barré effects.- 2.2.2. Acid dyes.- 2.2.3. Mordant dyes.- 2.2.4. Direct dyes.- 2.2.5. Reactive dyes.- 2.3. Cationic dyes.- 2.4. Non-ionic dyes.- 2.4.1. Disperse dyes.- 2.4.2. Disperse reactive dyes.- 2.4.3. Azoic colorants.- 2.4.4. Vat dyes.- References.- 3. Acrylic.- 3.1. Introduction.- 3.2. Cationic dyes.- 3.2.1. Thermodynamics of dye adsorption.- 3.2.2. Kinetics of dye adsorption.- 3.2.3. Effect of pH on dye adsorption.- 3.2.4. Effect of electrolyte on dye adsorption.- 3.2.5. Effect of temperature on dye adsorption.- 3.2.6. Effect of water on PAN fibres.- 3.2.7. Carrier dyeing.- 3.2.8. Retarding agents.- 3.2.9. Dye―fibre characteristics.- 3.2.10. Migrating cationic dyes.- 3.2.11. Gel dyeing.- 3.3. Disperse dyes.- 3.3.1. Thermodynamics of dyeing.- 3.3.2. Kinetics of dyeing.- 3.3.3. General considerations.- References.- 4. Microfibres.- 4.1. Introduction.- 4.1.1. General considerations.- 4.1.2. Microfibre production.- 4.2. Polyester microfibres.- 4.2.1. Mass-reduced polyester fibres.- 4.3. Polyamide micro fibres.- References.- Dye Index.
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5.0 颗星，最多 5 颗星Very ACCESSIBLE to the entry-level chemistry student留言者Tyrone Greenbaum -
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I have difficulty with reading comprehension and this book is one of the easiest-to-understand textbooks I've ever had.
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5.0 颗星，最多 5 颗星Useful chemistry textbook留言者Ben G. -
已在美国亚马逊上发表已确认购买Bought this for a chemistry class in college, and it was useful for explaining concepts that my teacher passed over. Lasted for both Chem I and II. Would recommend.5.0 颗星，最多 5 颗星Great condition留言者Skyler Tan -
已在美国亚马逊上发表已确认购买It's a standard chemistry textbook with everything formatted in a easy to learn style. Full of practice problems and examples to go with readings. I bought a used book but the seller could have honestly fooled me into thinking it was new with the condition it came in1.0 颗星，最多 5 颗星This is one of those profs whom I call a ...留言者Anil V -
已在美国亚马逊上发表已确认购买This is one of those profs whom I call a Master scam artist. Comes out with a new version almost every year and gets his colleagues to force kids to buy the latest version instead of using cheaper used copies of this basic 12th grade syllabus in colleges. The book is so badly written that kids can barely solve any of the problems in it. They then have to shell out another $100 to purchase the solutions book. Why can't the solutions to a few problems be included that you don't need an answer sheet. Why can't the solutions be part of OWL ?
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5.0 颗星，最多 5 颗星Just What I needed留言者Ryan G -
已在美国亚马逊上发表已确认购买I won't lie, I've been bumbling my way through chemistry for a semester and a half.
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The explanations are concise but still provide enough detail for me to backtrack when I've made a mistake.I just wish I'd picked this up earlier...
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Chemical PrinciplesPeter R. BergethonChapter
We will now explore the principal methods for the description and calculation of the electronic distribution in molecules. The importance of having knowledge of a biological molecule’s electron distribution cannot be overstated. The electronic distribution in a molecule is responsible for its chemical properties. As we will see, the formation of chemical bonds with the consequent bond strengths, lengths, force constants, and angles defines the shape and reactivity of molecules. The polarity of bonds determines charge distribution and give rise to the dipole moment of a molecule. The interaction of the electronic distribution with photons determines the optical character and spectral properties of molecules and the source of color and photochemistry. Many of the interactional forces on a large scale, including dipole and quadruple interactions, dispersion forces, and hydrogen bonding, all depend on the electronic structure of the molecules. Our appreciation of the chemistry and chemical biology of living organisms is built on an understanding of the electronic structure.Peter R. Bergethon11.Departments of Anatomy & Neurobiology and BiochemistryBoston University School of MedicineBostonUSA
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