Microbiology: A Systems Approach, 2 nd ed. Chapter 2: The Chemistry of Biology
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1 Microbiology: A Systems Approach, 2 nd ed. Chapter 2: The Chemistry of Biology
2 2.1 Atoms, Bonds, and Molecules: Fundamental Building Blocks Matter: anything that occupies space and has mass Can be liquid, solid, or gaseous state Building blocks of matter atoms Subatomic particles of atoms protons (p + ), neutrons (n 0 ), and electrons (e ) Protons and neutrons make up the nucleus, electrons surround the nucleus Held together by the attraction of positive protons to negative electrons
3 Figure 2.1
4 Different Types of Atoms: Elements and Their Properties Different numbers of protons, neutrons, and electrons in atoms create different elements Each element has a characteristic atomic structure and predictable chemical behavior Each assigned a distinctive name with an abbreviated shorthand symbol
5 The Major Elements of Life and Their Primary Characteristics Isotopes variant forms of the same element that differ in the number of neutrons Radioactive isotopes used in research and medical applications and in dating fossils and ancient materials Electron orbitals and shells
6 Electron Orbitals and Shells An atom can be envisioned as a central nucleus surrounded by a cloud of electrons Electrons rotate about the nucleus in pathways called orbitals volumes of space in which an electron is likely to be found Electrons occupy energy shells, from lower energy to higher energy as they move away from the nucleus Electrons fill the orbitals and shells in pairs starting with the shell nearest the nucleus Each element, then, has a unuiqe pattern of orbitals and shells
7 Figure 2.2
8 Bonds and Molecules Most elements do not exist naturally in pure form Molecule a distinct chemical substance that results from the combination of two or more atoms (can be two of the same element, such as O 2 ) Compounds molecules that are combinations of two or more different elements (such as CO 2 ) Chemical Bonds When two or more atoms share, donate, or accept electrons Types of bonds formed and to which atoms and element bonds are determined by the atom s valence
9 Figure 2.3
10 Covalent Bonds and Polarity: Molecules with Shared Electrons Covalent bonds between atoms that share electrons (such as H 2 ). The majority of molecules associated with living things are composed of single and double covalent bonds between C, H, O, N, S, and P.
11 Figure 2.4
12 Polar vs. Nonpolar Molecules Some covalent bonds result in a polar molecule an unequal distribution of charge (ex. H 2 O). Polarity is a significant property of many large molecules, influences both reactivity and structure An electrically neutral molecule is nonpolar share electrons equally
13 Figure 2.5
14 Ionic Bonds: Electron Transfer Among Atoms Electrons transferred completely from one atom to another, without sharing, results in an ionic bond (ex. NaCl) Molecules with ionic bonds, when dissolved in a solvent, can separate in to charged particles called ions in a process called ionization Cations positively charged ions Anions negatively charged ions These ionic molecules that dissolve to form ions are called electrolytes
15 Figure 2.6
16 Figure 2.7
17 Hydrogen Bonding Weak bond between a H covalently bonded to one molecule and an O or N atom on the same or different molecule (such as between water molecules) Figure 2.8
18 Chemical Shorthand: Formulas, Models, and Equations Molecular formula gives atomic symbols and the number of elements involved in subscript (H 2 O, C 6 H 12 O 6 ). Molecular formulas might not be unique (glucose, galactose, and fructose, for example) Structural formulas illustrate the relationships of the atoms and the number and types of bonds
19 Figure 2.9
20 Chemical Equations Equations are used to illustrate chemical reactions Reactants Molecules entering the reaction Products the substances left by a reaction
21 Types of Reactions Synthesis: reactants bond together to form an entirely new molecule A + B AB S + O 2 SO 2 2H 2 + O 2 2H 2 O (note that equations must be balanced) Decomposition: bonds on a single reactant molecule are permanently broken to release two or more product molecules AB A + B 2H 2 O 2 2H 2 O + O 2
22 Exchange: The reactants trade places between each other and release products that are combinations of the two AB + XY AX + BY (reversible reaction) Catalysts increase the rate of the reaction
23 Solutions: Homogeneous Mixtures of Molecules Solution a mixture of one or more solutes uniformly dispersed in a solvent The solute cannot be separated by filtration or settling The rule of solubility like dissolves like Water the most common solvent in natural systems because of its special characteristics Hydrophilic molecules attract water to their surface (polar) Hydrophobic molecules repel water (nonpolar) Amphipathic molecules have both hydrophilic and hydrophobic properties
24 Concentration of Solutions Concentration the amount of solute dissolved in a certain amount of solvent In biological solutions, commonly expressed as molar concentration or molarity (M) One mole dissolved in 1 L One mole is the molecular weight of the compound in grams
25 Figure 2.11
26 Acidity, Alkalinity, and the ph Scale Acidic solutions when a component dissolved in water (acid) releases excess hydrogen ions (H + ) Basic solutions when a component releases excess hydroxide ions (OH ) ph scale measures the acid and base concentrations of solutions Ranges from 0 (most acidic) to 14 (most basic); 7 is neutral ph = log[h + ]
27 Figure 2.12
28
29 Neutralization Reactions Neutralization reactions occur in aqueous solutions containing both acids and bases Give rise to water and other neutral byproducts HCl + NaOH H 2 O + NaCl
30 The Chemistry of Carbon and Organic Compounds Inorganic chemicals usually does not contain both C and H (ex. NaCl, CaCO 3 ) Organic chemicals Carbon compounds with a basic framework of the element carbon bonded to other atoms Most of the chemical reactions and structures of living things involve organic chemicals
31 Carbon the Fundamental Element of Life Valence makes it an ideal atomic building block Forms stable chains containing thousands of C atoms, with bonding sites available Can form linear, branched, or ringed bonds Can form single, double, or triple bonds Most often associates with H, O, N, S, and P
32 Figure 2.13
33 Functional Groups of Organic Compounds Special molecular groups or accessory molecules that bind to organic compounds functional groups Help define the chemical class of certain groups of organic compounds Give organic compounds unique reactive properties Reactions of an organic compound can be predicted by knowing the kind of functional group or groups it carries
34
35 2.2 Macromolecules: Superstructures of Life Biochemistry study of the compounds of life Biochemicals organic compounds produced by (or components of) living things Four main families carbohydrates, lipids, proteins, and nucleic acids Often very large, called macromolecules All macromolecules except for lipids are formed by polymerization Repeating subunits (monomers) are bound in to chains of various lengths (polymers)
36 Carbohydrates Carbohydrates: Sugars and Polysaccharides Most can be represented by the general formula (CH 2 O) n, where n = the number of units of this combination of atoms
37 Figure 2.14
38 Carbohydrates Exist in a variety of configurations Sugar (saccharide) a simple carbohydrate with a sweet taste Monosaccharide contains 3 7 carbons Disaccharide contains two monosaccharides Polysaccharide contains five or more monosaccharides Monosaccharides and disaccharides are specified by combining a prefix that describes a characteristic of the sugar with the suffix ose Hexoses six carbons Pentoses five carbons Fructose for fruit
39 Figure 2.15 The Nature of Carbohydrate Bonds
40 The Functions of Polysacharides Structural support and protection Serve as nutrient and energy stores Cell walls in plants and many microscopic algae from cellulose Figure 2.16a
41 Other Important Polysaccharides Include agar, peptidoglycan, chitin, lipopolysaccharide, glycocalyx, and glycogen Figure 2.16b
42 Lipids: Fats, Phospholipids, and Waxes Lipids a variety of substances that are not soluble in polar substances Will dissolve in nonpolar solvents Main groups of lipids Triglycerides a single molecule of glycerol bound to three fatty acids Includes fats and oils
43 Figure 2.17
44 Phospholipids Contain two fatty acids attached to the glycerol with a phosphate group on the third glycerol binding site Important membrane molecules Phospholipids Figure 2.18
45 Miscellaneous Lipids Steroids complex ringed compounds commonly found in cell membranes and animal hormones Best known cholesterol Waxes esters formed between a long chain alcohol and a saturated fatty acid
46 Figure 2.19
47 Proteins: Shapers of Life Predominant organic molecules Building blocks amino acids 20 different naturally occurring forms Basic skeleton a carbon (the α carbon) linked to an amino group (NH 2 ), a carboxyl group (COOH), a hydrogen atom (H), and a variable R group Peptide bond forms between the amino group on one amino acid and the carboxyl group on another.
48
49 Figure 2.20
50 Protein Structure and Diversity Primary (1 ) structure the type, number, and order of amino acids in the chain Secondary (2 ) structure when various functional groups exposed on the outer surface of the molecule interact by forming hydrogen bonds Coiled configuration αhelix Accordion pattern β pleated sheet Tertiary (3 ) structure created by additional bonds between functional groups Quarternary (4 ) structure more than one polypeptide forms a large, multiunit protein
51 Figure 2.21
52 Protein Shape Each different type of protein develops a unique shape, so it can only react with molecules that fit its particular surface features Ex. enzymes and antibodies Native state the functional three dimensional form of a protein Denatured when the protein s native state has been disrupted
53 The Nucleic Acids: A Cell Computer and Its Programs DNA specially coded genetic program DNA transfers its program to RNA Both are polymers of repeating units called nucleotides Nucleotides composed of three smaller units: a nitrogen base, a pentose sugar, and a phosphate. The nitrogen base can be one of two forms a purine (two rings) or a pyrimidine (one ring) Two types of purines: adenine (A) and guanine (G) Three types of pyrimidines: thymine (T), cytosine (C), and uracil (U) DNA contains all of the nitrogen bases except uracil RNA contains all of the nitrogen bases except thymine The nitrogen base is covalently bonded to ribose in RNA and deoxyribose in DNA Phosphate (PO 4 3 ) covalently bonds the sugars in series
54 Figure 2.22
55 Figure 2.23
56 The Double Helix of DNA Formed by two long polynucleotide strands Linked along their length by hydrogen bonds between complimentary pairs of nitrogen bases Adenine pairs with thymine Cytosine pairs with guanine
57 Figure 2.24
58 RNA: Organizers of Protein Synthesis Also consists of a long chain of nucleotides It is single stranded and contains ribose instead of deoxyribose anduracil instead of thymine Several functional types of RNA formed using the DNA template Messenger RNA (mrna) a copy of a gene that provides the order and type of amino acids in a protein Transfer RNA (trna) a carrier that delivers the correct amino acids for protein assembly Ribosomal RNA (rrna) a major component of ribosomes
59 ATP: The Energy Molecule of Cells Adenosine triphosphate (ATP) a nucleotide containing adenine, ribose, and three phosphates High energy compound that gives off energy when the bond is broken between the outermost phosphates Releases and stores energy for cellular chemical reactions When the terminal phosphate bond is broken to release energy, adenosine diphosphate (ADP) is formed ADP can be converted back to ATP when the third phosphate is restored.
60 Figure 2.25
61 2.3 Cells: Where Chemicals Come to Life The fundamental unit of life cell Fundamental characteristics of cells Tend to be spherical, polygonal, cubical, or cylindrical Their protoplasm is encased in a cell or cytoplasmic membrane Chromosomes containing DNA Ribosomes for protein synthesis
62 Eukaryotic and Prokaryotic Cells Eukaryotic cells Found in animals, plants, fungi, and protists Contain organelles that perform cell functions (such as the nucleus, Golgi apparatus, endoplasmic reticulum, vacuoles, and mitochondria) Prokaryotic cells Only found n bacteria and archae No nucleus or other organelles
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