The Resource Chemistry for the biosciences : the essential concepts, Jonathan Crowe, Tony Bradshaw

Chemistry for the biosciences : the essential concepts, Jonathan Crowe, Tony Bradshaw

Label
Chemistry for the biosciences : the essential concepts
Title
Chemistry for the biosciences
Title remainder
the essential concepts
Statement of responsibility
Jonathan Crowe, Tony Bradshaw
Creator
Contributor
Subject
Genre
Language
  • eng
  • eng
Summary
Chemistry pervades our life, giving shape and character to the world around us. It moulds our climate, fuels our transport, gives food its taste and smell. Most of all, chemistry powers life itself.Chemistry for the Biosciences leads students through the essential concepts that are central to understanding biological systems, using everyday examples and analogies to build their confidence in an often daunting subject. Placing an emphasis on clear, straightforward explanations, it fosters understanding as opposed to rote learning; by using relevant biological examples throughout, it illustrates
Cataloging source
MiAaPQ
http://library.link/vocab/creatorName
Crowe, Jonathan
Dewey number
541.02457
Illustrations
illustrations
Index
index present
Language note
English
LC call number
QD415
LC item number
.C769 2010
Literary form
non fiction
Nature of contents
  • dictionaries
  • bibliography
http://library.link/vocab/relatedWorkOrContributorName
Bradshaw, Tony
http://library.link/vocab/subjectName
  • Biochemistry
  • Chemistry
Label
Chemistry for the biosciences : the essential concepts, Jonathan Crowe, Tony Bradshaw
Instantiates
Publication
Copyright
Note
Description based upon print version of record
Bibliography note
Includes bibliographical references and index
Carrier category
online resource
Carrier category code
  • cr
Content category
text
Content type code
  • txt
Contents
  • Cover; Periodic table of the elements; Contents; Acknowledgements; Welcome to the book; 1 Introduction: why biologists need chemistry; 1.1 Science: revealing our world; I'm a biologist: what has chemistry to do with me?; 1.2 The essential concepts; 1.3 The language of chemistry; Units: making sense of numbers; Symbols; 2 Atoms: the foundations of life; 2.1 The chemical elements; 2.2 Atomic composition; Protons, electrons, and electrical charge; Identifying the composition of an atom: atomic number and mass number; The formation of ions; Isotopes: varying the number of neutrons
  • Relative abundances and atomic weightProtons and chemical identity; 2.3 Atomic structure; Atomic orbitals; 2.4 The energy of atoms; Orbitals and energy levels; Filling up orbitals-the building-up principle; The filling of subshells; Moving between orbitals: electron excitation; Energy levels and quantization; 2.5 Valence shells and valence electrons; Valence electrons and the underlying logic of the periodic table; The variety of life: not so varied after all?; 3 Compounds and chemical bonding: bringing atoms together; 3.1 The formation of compounds
  • The chemical bond: bridging the gap between atomsWhich electron configuration is most stable?; 3.2 Valence shells and Lewis dot symbols; Non-bonding pairs of electrons; 3.3 Bond formation: redistributing valence electrons; 3.4 The ionic bond: transferring electrons; Ionic bonding and full shells: how many electrons are transferred?; 3.5 The chemical formula; 3.6 The covalent bond: sharing electrons; Covalent compounds and electrical charge; The molecular formula: identifying the components of a covalent compound; Covalent bonding and the distribution of electrons; Molecular orbitals
  • 3.7 The formation of multiple bondsSigma and pi orbitals; Valency: how many bonds can an atom form?; Sharing one pair of electrons: the single bond; Sharing two pairs of electrons: the double bond; Sharing three pairs of electrons: the triple bond; Satisfying valency with multiple bonds; Hypervalency: going beyond the octet rule; 3.8 Dative bonding: covalent bonding with a twist; Dative bonds in biological systems; 3.9 Aromatic compounds and conjugated bonds; 3.10 Polyatomic compounds; 3.11 Ionic versus covalent bonding; Electronegativity: how easily can electrons be transferred?
  • Ionic and covalent bonding in nature: which is most prevalent?3.12 Blurring the boundaries: polarized bonds; How strongly is a bond polarized?; Non-polar covalent bonds; 4 Molecular interactions: holding it all together; 4.1 Chemical bonding versus non-covalent forces; Intramolecular versus intermolecular forces; The significance of molecular interactions; 4.2 Electrostatic forces: the foundations of molecular interactions; Polar bonds in non-polar molecules; 4.3 The van der Waals interaction; Dispersion forces; Permanent dipolar interactions; Steric repulsion
  • Balancing attraction and repulsion: the van der Waals interaction
Dimensions
unknown
Edition
2nd ed.
Extent
1 online resource (705 p.)
Form of item
online
Isbn
9780191665875
Media category
computer
Media type code
  • c
Specific material designation
remote
System control number
  • (CKB)2550000001176001
  • (EBL)1591381
  • (SSID)ssj0001082691
  • (PQKBManifestationID)12416440
  • (PQKBTitleCode)TC0001082691
  • (PQKBWorkID)11100795
  • (PQKB)11776224
  • (MiAaPQ)EBC1591381
  • (EXLCZ)992550000001176001
Label
Chemistry for the biosciences : the essential concepts, Jonathan Crowe, Tony Bradshaw
Publication
Copyright
Note
Description based upon print version of record
Bibliography note
Includes bibliographical references and index
Carrier category
online resource
Carrier category code
  • cr
Content category
text
Content type code
  • txt
Contents
  • Cover; Periodic table of the elements; Contents; Acknowledgements; Welcome to the book; 1 Introduction: why biologists need chemistry; 1.1 Science: revealing our world; I'm a biologist: what has chemistry to do with me?; 1.2 The essential concepts; 1.3 The language of chemistry; Units: making sense of numbers; Symbols; 2 Atoms: the foundations of life; 2.1 The chemical elements; 2.2 Atomic composition; Protons, electrons, and electrical charge; Identifying the composition of an atom: atomic number and mass number; The formation of ions; Isotopes: varying the number of neutrons
  • Relative abundances and atomic weightProtons and chemical identity; 2.3 Atomic structure; Atomic orbitals; 2.4 The energy of atoms; Orbitals and energy levels; Filling up orbitals-the building-up principle; The filling of subshells; Moving between orbitals: electron excitation; Energy levels and quantization; 2.5 Valence shells and valence electrons; Valence electrons and the underlying logic of the periodic table; The variety of life: not so varied after all?; 3 Compounds and chemical bonding: bringing atoms together; 3.1 The formation of compounds
  • The chemical bond: bridging the gap between atomsWhich electron configuration is most stable?; 3.2 Valence shells and Lewis dot symbols; Non-bonding pairs of electrons; 3.3 Bond formation: redistributing valence electrons; 3.4 The ionic bond: transferring electrons; Ionic bonding and full shells: how many electrons are transferred?; 3.5 The chemical formula; 3.6 The covalent bond: sharing electrons; Covalent compounds and electrical charge; The molecular formula: identifying the components of a covalent compound; Covalent bonding and the distribution of electrons; Molecular orbitals
  • 3.7 The formation of multiple bondsSigma and pi orbitals; Valency: how many bonds can an atom form?; Sharing one pair of electrons: the single bond; Sharing two pairs of electrons: the double bond; Sharing three pairs of electrons: the triple bond; Satisfying valency with multiple bonds; Hypervalency: going beyond the octet rule; 3.8 Dative bonding: covalent bonding with a twist; Dative bonds in biological systems; 3.9 Aromatic compounds and conjugated bonds; 3.10 Polyatomic compounds; 3.11 Ionic versus covalent bonding; Electronegativity: how easily can electrons be transferred?
  • Ionic and covalent bonding in nature: which is most prevalent?3.12 Blurring the boundaries: polarized bonds; How strongly is a bond polarized?; Non-polar covalent bonds; 4 Molecular interactions: holding it all together; 4.1 Chemical bonding versus non-covalent forces; Intramolecular versus intermolecular forces; The significance of molecular interactions; 4.2 Electrostatic forces: the foundations of molecular interactions; Polar bonds in non-polar molecules; 4.3 The van der Waals interaction; Dispersion forces; Permanent dipolar interactions; Steric repulsion
  • Balancing attraction and repulsion: the van der Waals interaction
Dimensions
unknown
Edition
2nd ed.
Extent
1 online resource (705 p.)
Form of item
online
Isbn
9780191665875
Media category
computer
Media type code
  • c
Specific material designation
remote
System control number
  • (CKB)2550000001176001
  • (EBL)1591381
  • (SSID)ssj0001082691
  • (PQKBManifestationID)12416440
  • (PQKBTitleCode)TC0001082691
  • (PQKBWorkID)11100795
  • (PQKB)11776224
  • (MiAaPQ)EBC1591381
  • (EXLCZ)992550000001176001

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