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The Chemistry of Microbiology
2 The Chemistry of Microbiology
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Atoms Matter – anything that takes up space and has mass
Atoms – the smallest chemical units of matter Atomic Structure Electrons – negatively charged subatomic particles circling a nucleus. Nucleus – structure containing neutrons and protons Neutrons – uncharged particles Protons – positively charged particles
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Figure 2.1 An example of a Bohr model of atomic structure.
Electron shells Proton (p + ) Nucleus Neutron (n ) Electron (e – )
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Atoms Atomic Structure Element – composed of a single type of atom
Atomic number – equal to the number of protons in the nucleus Atomic mass (atomic weight) – sum of masses of protons, neutrons, and electrons
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Atoms Isotopes Atoms of a given element that differ in the number of neutrons in their nuclei Stable isotopes and Unstable isotopes Radioactive isotopes Release energy during radioactive decay
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Figure 2.2 Nuclei of the three naturally occurring isotopes of carbon.
Proton Neutron Carbon-12 Carbon-13 Carbon-14 6 Protons 6 Protons 6 Protons 6 Neutrons 7 Neutrons 8 Neutrons
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Figure 2.4 Bohr diagrams of the first 20 elements and their places within the chart known as the periodic table of the elements.
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Chemical Bonds Valence – combining capacity of an atom
Positive if atom has electrons to give up Negative if atom has spaces to fill Stable when outer electron shells contain eight electrons Chemical bonds – atoms combine by sharing or transferring valence electrons Molecule – two or more atoms held together by chemical bonds Compound – a molecule composed of more than one element
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Chemical Bonds Covalent bond – sharing of a pair of electrons by two atoms Electronegativity – attraction of atom for electrons The more electronegative an atom, the greater the pull its nucleus exerts on electrons
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Chemical Bonds Nonpolar covalent bonds
Shared electrons spend equal amounts of time around each nucleus Atoms with similar electronegativities No poles exist Carbon atoms form four nonpolar covalent bonds with other atoms Organic compounds contain carbon and hydrogen atoms
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Figure 2.5c-d Four molecules formed by covalent bonds.
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Chemical Bonds Polar Covalent Bonds
Unequal sharing of electrons due to significantly different electronegativities Most important polar covalent bonds involve hydrogen Allow for hydrogen bonding
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Chemical Bonds Ionic Bonds
Occur when two atoms with different electronegativities come together Atoms have either positive (cation) or negative (anion) charges Cations and anions attract each other and form ionic bonds (no electrons shared) Typically form crystalline ionic compounds known as salts
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Chemical Bonds Hydrogen Bonds
Electrical attraction between partially charged H+ and full or partial negative charge on same or different molecule Weaker than covalent bonds but essential for life Help to stabilize shapes of large molecules
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Chemical Reactions The making or breaking of chemical bonds
Involve reactants and products Biochemistry involves chemical reactions of living things
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Chemical Reactions Decomposition Reactions
Break bonds within larger molecules to form smaller atoms, ions, and molecules Release energy (exothermic) Common type is hydrolysis Ionic components of water are added to products All the decomposition reactions in an organism are called catabolism
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Chemical Reactions Exchange Reactions
Involve breaking and forming covalent bonds Have endothermic and exothermic steps Involve atoms moving from one molecule to another Sum of all chemical reactions in an organism is called metabolism
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Water, Acids, Bases, and Salts
Most abundant substance in organisms and has special characteristics due to two polar covalent bonds Cohesive molecules – surface tension Excellent solvent Remains liquid across wide range of temperatures Can absorb significant amounts of energy without changing temperature Participates in many chemical reactions
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Water, Acids, Bases, and Salts
Acids and Bases Dissociated by water into component cations and anions Acid – dissociates into one or more H+ and one or more anions Base – binds with H+ when dissolved into water; some dissociate into cations and OH– Concentration of H+ in solution expressed using the pH scale Metabolism requires relatively constant balance of acids and bases Buffers prevent drastic changes in internal pH
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Figure The pH scale.
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Water, Acids, Bases, and Salts
Compounds that dissociate in water into cations and anions other than H+ and OH– Cations and anions of salts are electrolytes Create electrical differences between inside and outside of cell Transfer electrons from one location to another Form important components of many enzymes
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Organic Macromolecules
Functional Groups Contain carbon and hydrogen atoms Atoms often appear in arrangements called functional groups Macromolecules – large molecules used by all organisms Lipids Carbohydrates Proteins Nucleic acids Monomers – basic building blocks of macromolecules
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Organic Macromolecules
Lipids Not composed of regular subunits Are all hydrophobic Four groups Fats Phospholipids Waxes Steroids
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Organic group Cell Unsaturated fatty acid Hydrophilic (polar)
Figure Phospholipids. Organic group Cell Unsaturated fatty acid Hydrophilic (polar) head Phosphate group Glycerol Symbol Phospholipid bilayer Hydrophobic (nonpolar) tails Double bond Saturated fatty acid Unsaturated fatty acid Phospholipid
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Organic Macromolecules
Lipids Waxes Contain one long-chain fatty acid covalently linked to long-chain alcohol by ester bond Lack hydrophilic head Completely insoluble in water
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Organic Macromolecules
Carbohydrates Organic molecules composed of carbon, hydrogen, and oxygen (CH2O)n Functions Long-term storage of chemical energy Ready energy source Part of backbones of nucleic acids Converted to amino acids Form cell wall Involved in intracellular interactions between animal cells
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Organic Macromolecules
Carbohydrates Types Monosaccharides Disaccharides Polysaccharides
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Figure 2.18 Monosaccharides (simple sugars).
configuration configuration Glucose Acetyl group N-acetylglucosamine
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Figure Disaccharides.
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Figure 2.20 Polysaccharides.
-1,4 bonds Hydrogen bonds Hydrogen bond Cellulose -1,4 bonds Amylose (unbranched) -1,4 bond -1,6 bond -1,6 bond -1,4 bond Glycogen
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Organic Macromolecules
Proteins Mostly composed of carbon, hydrogen, oxygen, nitrogen, and sulfur Functions Structure Enzymatic catalysis Regulation Transportation Defense and offense
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Organic Macromolecules
Proteins Amino acids The monomers that make up proteins Most organisms use only 21 amino acids in protein synthesis Side groups affect how amino acids interact with one another and how a protein interacts with other molecules A covalent peptide bond is formed between amino acids
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Figure 2.24 Levels of protein structure.
Amino acid 1 Peptide bond -pleated sheet Amino acid 2 -helix Hydrogen bond Amino acid 3 Secondary structure Amino acid 4 -pleated sheets Primary structure -helix Tertiary structure Quaternary structure
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Organic Macromolecules
Nucleic Acids DNA and RNA are the genetic material of organisms and viruses RNA also acts as enzyme, binds amino acids, and helps form polypeptides
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Organic Macromolecules
Nucleic Acids Nucleotides and nucleosides Nucleotides Monomers that make up nucleic acids Composed of three parts Phosphate Pentose sugar – deoxyribose or ribose One of five cyclic nitrogenous bases Nucleosides are nucleotides lacking phosphate
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Organic Macromolecules
Nucleic Acids Nucleic acid structure Three H bonds form between C and G Two H bonds form between T and A (DNA) or U and A (RNA) DNA is double stranded in most cells and viruses The two strands are complementary The two strands are antiparallel
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Figure 2.26 General nucleic acid structure.
5' 3' A T Two hydrogen bonds G C Three hydrogen bonds T A 5' end Adenine base C 5' C O G 4' 1' C G Deoxyribose 3' 2' A Phosphate Guanine base Thymine base Sugar- phosphate backbones Cytosine base 3' end 5' 3'
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Organic Macromolecules
Nucleic Acids Nucleic acid function DNA is genetic material of all organisms and of many viruses Carries instructions for synthesis of RNA and proteins Controls synthesis of all molecules in an organism
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