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Chemistry Review for Allied Health Majors Essential concepts: atoms, molecules, chemical bonds and pH
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Chemistry and Biochemistry for Microbiology
Part 1
By BugLady
Structure and Function
Atoms and molecules
Chemical bonds strength
Water: the molecule of life
Carbohydrates: (energy source, storage, and cell structure)
Lipids (energy storage and membrane main component)
Proteins (enzymes, transporters, movement)
Nucleic acids (genetic material, small effector molecules)
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Check point
Electron
Nucleus
Neutron
Proton
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Biologically Important Elements
Present in large amounts
C= every organic molecule, CO2
H= water, H+ , all organic molecules
O=water, e- acceptor, all organic molecules
N= proteins, nucleic acids, some vitamins
P= phospholipids, inorganic P, nucleic acids
S= proteins, some vitamins
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Why isn’t calcium mentioned as a most abundant element in this class?
Biologically Important Elements
Elements required in smaller amounts
Electrolyte balance, protein stabilization, shells of some microorganisms o Cations: K+ (potassium), Na+ (sodium), Fe2+/3+
(iron), Ca2+ (calcium), Mg2+ (magnesium)
o Anions: Cl- (chlorine), PO4-3 (inorganic
phosphate)
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Biologically Important Elements
Essential elements required in trace amountsoMetals: Zinc, Vanadium, Chromium, Molybdenumo Lithium, Iodine, Selenium etc…
Found in vitamins and enzymesEssential functions in a cell will be compromised if trace elements are missing in a diet.
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Chemical Bonds
Chemical bond: Atoms form interactions involving their outer most electrons
There are 4 main types of chemical bonds.
Covalent bonds
Ionic Bonds
Hydrogen Bonds
Hydrophobic (non polar) Interactions
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Comparison of Chemical BondsStrength of Bonds:
Covalent>ionic>hydrogen bonds>non polar interactions
Non covalent interactions are individually weak but collectively strong.
Ionic bonds and hydrogen bonds are polar or hydrophilic
Non polar interactions are hydrophobic
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Covalent BondsCovalent bonds may have an equal or unequal attraction for the shared electrons
Nonpolar covalento Bonds formed between identical atoms or
between atoms that have similar attraction of electrons H-H or C-H
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National Institute of General Medical Sciences
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Covalent Bonds
Polar covalento One atom has a greater attraction to the
electrons than the othero Produces a slight charge within the molecule
Ionic Bonds
Loss and gain of electrons leads to charged atoms (ions)
Ionic bonds are attractions between ions of opposite charge.
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Ionic Bonds
Ionic bonds in solution are weaker than covalent bonds
o Bonds dissociate in water Easily broken at room temperature Approximately 100 time weaker than covalent
bonds
Important among weak forces holding biological molecules together
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Hydrogen BondsWeak bonds formed from the attraction of positively charged hydrogen atoms
o Hydrogen atoms in polar molecules are attracted to negatively charged atoms or molecules Most commonly oxygen or nitrogen
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Hydrogen Bonds
Hydrogen bonds occur between molecules and within molecules (water, proteins, DNA)
Covalent bonds occur within moleculeso Hydrogen bonds hold molecules togethero Covalent bonds hold atoms together
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Nonpolar (Hydrophobic) Interactions
Nonpolar residues (lipids or hydrophobic regions of proteins) are exposed at the surface of two different molecules.It is energetically more favorable for polar water molecules to approach each other closely displacing the "oily" non-polar molecules from between them.
o Example: plasma membranes.
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Properties of Water
Stabilized by hydrogen bonds in liquid state: H----O
High heat capacity
High surface tension
Excellent solvent
H+ and OH participate in chemical reactions
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National Institute of General Medical Sciences
The Universal Solvent
Ionic compounds dissociate, forming soluteso Salts, acids, bases
Polar compounds form hydrogen bonds with water moleculeso Small alcohols, aldehydes, quaternary
ammonium compounds, vitamins
Apr 11, 2023 18Figure 2.5
Interaction with Water
Hydrophilic- “water-loving”o Readily dissolve in watero Ions and molecules that contain polar covalent
bonds Sugars, salts, protein hormones, some vitamins, small
organic molecules
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Courtesy USDA
Interaction with Water
Hydrophobic- “water-fearing”o Do not readily dissolve in watero Hydrocarbons, lipids, non polar solvents, lipid
soluble vitamins, steroidsAmphipathic moleculeo Have both polar or ionized regions at
one or more sites and nonpolar regions at other sites Detergents are amphipatic
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Renee Comet NCi
Micelle by SuperManu CC BY-SA 3.0
Acid-Base Balance
pH is a measure of the concentration of H+ in a solution.
pH =7.0 is neutral (pH of freshly distilled water)
pH>7.0 is basic
pH<7.0 is acidic pH = log 1/[H+]=log[H+]
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Acid-Base Balance
Increasing [H+] increases acidity. pH decreases.
Increasing [OH] or pH increases alkalinity.
Most organisms grow best between pH 6.5 and 8.5
Optimal pH for most bacterial growth is slightly basic.
Optimal pH for fungal growth is slightly acidic.
Why Measure pH?Acidic pH of skin and stomach are part of our innate immune system
Proper function of proteins requires a specific pH.
DNA stability is dependent on pH.
Most biochemical assays used for bacteria identification measure changes in pH.
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Lactose positive and lactose negative colonies of Escherichia coli on Mac Conkey agar
Buffers
Buffered solutions resist change in the pH of a solution when hydrogen ions (protons) or hydroxide ions are added or removed.
Buffers are critical to the maintenance of life.
Buffered systems mean that organisms can maintain a suitable pH environment in their cells and tissues.
One of the most common buffers is the bicarbonate buffer.
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