chemistry of microbes
DESCRIPTION
LECTURES IN MICROBIOLOGY. Chemistry of Microbes. LESSON 2. Sofronio Agustin Professor. Topics. Fundamental Building Blocks Macromolecules The Cell. Fundamental Building Blocks. Atoms Elements Molecules and compounds. Atoms. Subatomic Particles Proton = positive charge - PowerPoint PPT PresentationTRANSCRIPT
Chemistry of Microbes
LECTURES IN MICROBIOLOGY
LESSON 2
Sofronio AgustinProfessor
2
Topics
Fundamental Building Blocks
Macromolecules
The Cell
3
Fundamental Building Blocks
Atoms
Elements Molecules and compounds
4
Atoms
Subatomic ParticlesProton = positive chargeNeutron = neutralElectron = negative charge
Atomic number = no. of protons Atomic mass = no. of protons and neutrons
5Models of Atomic Structure
Atomic Structure
6
Isotopes
Atoms with same number of protons but differ in number of neutrons are called isotopes.
Example: 12C, 13C, and 14C are isotopes of carbon.
Radioisotopes emit radiation in the form of alpha or beta or gamma rays or photons.
7
Major Elements of Life
8
Molecules and Compounds
Molecule = combination of two or more elements (e.g.H2)
Compound = combination of two or more different elements (e.g. H2O)
Molecules are held together by chemical bonds
9
Chemical Bonds
Covalent
Ionic Hydrogen
10
Chemical Bonds
Chemical bonds involve atoms sharing, donating or accepting electrons
11
Covalent Bonding
Examples of covalent bonding
12
Polar Covalent Bond
Polarity occurs when atoms electrons unequally due to differences in electronegativities. This is seen in water (H2O).
More electronegative atoms tend to pull electrons toward them creating a polar molecule.
13
Ionic Bonding
Sodium chloride (table salt) is an example of ionic bonding, that is, electron transfer among atoms or redox reaction.
14
Ionization
Molecules formed by ionic bonding breakup (ionization) when dissolved in water (solvent), producing separate positive (cation) and negative (anion) ions.
These ions conduct electricity and thus called electrolytes.
15
Hydrogen Bond
Hydrogen bonding is formed between the partially positive (hydrogen) end of a polar molecule and the negative end of another (e.g. O2 or N2).
Example : Water molecules
16
pH
pH – measurement of the H+ ion concentration in a solution.
General rule: Acidic = excess H+ ions in solution Basic = excess OH- ions in solution Neutral = equal amounts of H+ and OH- ions
17
The pH Scale
The pH of an environment (exterior or interior of a cell) is important for living systems.
18
Molecules
Molecules important to life consist of inorganic and organic substances.
Inorganic – either C or H maybe present (e,g, CO2, H2)
Organic- C and H (hydrocarbons) are present
(e.g. CH3)
19
Organic Molecules
Carbon, a tetravalent atom, is an ideal element for life because it serves as the skeleton for macromolecules.
Functional groups (R) attached to these carbons confer unique properties to these macromolecules.
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Macromolecules
Carbohydrates Lipids Proteins Nucleic acids
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Carbohydrates
Simple Sugars
Disaccharides
Polysaccharides
22
Classes of Carbohydrates
Major sugars (monosaccharides) in the cell are glucose, galactose and fructose.
Several sugars bonded together are called polysaccharides.
23
Glycosidic Bond
Sugars are bonded by special kind of covalent linkage called glycosidic bonds.
Water is released (dehydration) after the bond is formed.
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Polysaccharides
Peptidoglycan in bacteria is an example of a polysaccharide.
25
Lipids
Fats Phospholipids
Steroids
26
Fats
Synthesis and structure of a triglyceride (fat), a storage molecule.
27
Phospholipids
Phospholipids serve as a major structural component of cell membranes.
It is an amphiphatic molecule. Its phosphate “head” is hydrophilic and its fatty acid “tail” is hydrophobic.
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Cholesterol: An Alcoholic Steroid
Cholesterols are associated with cell membranes of some cells such as those of eukaryotes.
29
Proteins
Proteins are the predominant organic molecules in cells.
Proteins consist of a series of amino acids (e.g. peptides, polypeptides)
Peptide bonds link amino acids together. Examples: hormones, enzymes, antibodies, etc.
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Amino Acids
An amino acid has a central carbon, to which carboxylic, amino and R groups are attached.
Amino acid types vary according to the reactive (R) groups present.
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The 20 Naturally Occurring Amino Acids
32
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A peptide bond (covalent) forms between the amino group on one amino acid and the carboxyl group on another amino acid with the accompanying loss of water.
Peptide Bond
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Levels of Structures of Protein
Proteins take on a variety of shapes due to extensive folding of the molecule. This enable them to perform specific functions and interactions with other molecules.
34
Nucleic acids
Deoxyribonucleic acid (DNA) Ribonucleic acid (RNA) DNA contains genetic information and
transfers it to RNA RNA translates the DNA information into
proteins
35
Nucleic Acid Polymers
Nucleic acids are polymers of repeating units called nucleotides.
36
The Sugars and Nitrogenous Bases
The pentose sugars and nitrogen bases determine whether a molecule will be DNA or RNA.
37
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The DNA configuration is a double helix similar to “a spiral staircase”
Sugar and phosphate backbones are held together by hydrogen bonds formed between nitrogenous bases.
The DNA Molecule
38
DNA : The Molecule of Inheritance
DNA serves as a template for the synthesis of new DNA strands as well as mRNA, tRNA and rRNA.
DNA replication is an important step in cell reproduction.
39
The Cell
Fundamental characteristics shared by all living organisms: Reproduction Metabolism Motility (Response to molecules) Protection and Storage (Cell wall or
membrane) Nutrient transport