BIO187 Microbiology Prerequisite Options

BIO187 Microbiology with Lab Prerequisite Options

• To ensure BIO187 students have the opportunity to learn the course material successfully, there is a prerequisite.
• There are two separate options to meet the prerequisite.
• All students who wish to take BIO187 must meet prereqs regardless of program.

Option 1

• Students lacking college-level biology are encouraged to take BIO101, a 2-credit introductory course.
• Students will learn basics of biology: cells, structures, cell processes, enzymes, and biological molecule chemistry.

Option 2

• Students with a strong biology background can take the Microbiology Placement test.
• The test is administered by the Testing Center in Trustee Hall under the same guidelines at TEAS and Accuplacer exams.
• Students can take the test up to 3 times with a 2-week wait between attempts.
• Students must pass the placement test with a score of 75% or higher.
• Students who do not meet the requirement after three attempts must sign up for BIO101.

A&S Microbiology Placement Test Topics

• The main chapter references relate to Norman-McKay's Microbiology: Basic and Clinical Principles.
• Chapter 2: Atoms, molecules.
• Chemical bonds - ionic, covalent, polar vs. nonpolar.
• Hydrogen bonds.
• Water as a solvent.
• Hydrophilic, hydrophobic, amphipathic molecules.
• Chemical reactions, making and breaking bonds.
• Macromolecules of biology: Carbs, lipids, proteins, nucleic acids - the elemental components of each, monomers, production of each, protein folding, DNA, RNA, ATP.
• Chapter 3: Prokaryote cell anatomy: internal and external structures.
• Prokaryotic cell division.
• Plasma membrane.
• Gram, acid-fast stains.
• Cell transport.
• Structures for adhesion, movement, protection.
• Internal structures: nucleoid, ribosomes, cytoskeleton, inclusions.
• Endospores and endospore production.
• Chapter 4: Endosymbiotic theory.
• Differences between prokaryotes and eukaryotes: cell anatomy, cell division, cell transport.
• Eukaryotic cell anatomy.
• Cell division.
• Cell transport: active and passive.
• Classification of eukaryotes.
• Extracellular structures.
• Plasma membrane.
• Cell wall.
• Structures for adhesion, protection, movement.
• Intracellular structures.
• Membrane-bound organelles.
• Nucleus.
• ER: rough and smooth.
• Golgi apparatus.
• Lysosomes.
• Mitochondria.
• Peroxisomes.
• Chloroplasts.
• Vacuoles.
• Ribosomes.
• Cytoskeleton.
• Chapter 5: Heredity basics.
• Genotype/phenotype.
• Prokaryote/eukaryote genomes.
• DNA and RNA structure and function.
• DNA replication: enzymes, leading vs. lagging strand synthesis, differences between prokaryotes and eukaryotes.
• Protein synthesis: transcription and translation.
• Regulating protein synthesis: pre-transcriptional vs. post-transcriptional, epigenome controls, post-transcriptional controls.
• Mutations - types of mutations and results of each.
• Chapter 8: Metabolism - anabolism, catabolism.
• ATP.
• Enzymes.
• Redox reactions.
• Ways to produce ATP.
• Cellular respiration - basics of glycolysis, Kreb's cycle, electron transport chain.
• Pentose phosphate pathway.
• Entner-Doudoroff pathway.
• Fermentation.

Chapter 2 Topics

• Study the term atom and describe its parts.
• Determine the atomic mass, atomic number, and chemical symbol of an element using the periodic table.
• Describe the difference between an anion and a cation and state how they are formed.
• Discuss isotopes and explain how they are important in medicine.
• Define the terms molecule, compound, and isomer.
• Interpret and write a molecular formula.
• Differentiate between organic and inorganic compounds and recognize selected functional groups.
• Compare acids and bases and discuss their effects on pH.
• Summarize what pH is and list features of the pH scale.
• Define the term buffer and state why buffers are important in biological systems.
• Define the term valence electron and state how these electrons relate to bonding.
• Compare and contrast ionic and covalent bonds.
• Describe what electrolytes are and explain why they are important in biological systems.
• Discuss what polar covalent bonding is and how it sets the stage for hydrogen bonding.
• Explain what hydrogen bonds are.
• Describe van der Waals interactions.
• Define the terms hydrophobic, hydrophilic, and amphipathic and describe how they relate to micelle formation.
• Identify the reactants and products in a chemical equation.
• Define the term catalyst.
• Explain synthesis, decomposition, and exchange reactions.
• Define dehydration synthesis and hydrolysis reactions.
• Discuss what activation energy is and how it can be lowered in biochemical reactions.
• Compare and contrast endergonic and exergonic reactions.
• Detail what is meant by a reversible reaction and briefly describe the concept of equilibrium.
• Identify the four main groups of biomolecules and their building blocks.
• Describe glycosidic bonds, peptide bonds, and phosphodiester bonds.
• Explain the structural and functional characteristics of carbohydrates, lipids, nucleic acids, and proteins.
• Compare and contrast deoxyribonucleotides and ribonucleotides.
• Summarize how saturation impacts lipid characteristics.
• Describe the four levels of protein structure.
• State what chaperone proteins do and why they are important.

What are atoms? (1 of 4)

• Atoms are the smallest units of elements and are pure substances that make up ordinary matter.

What are atoms? (2 of 4)

• The center of an atom is the atomic nucleus and contains protons and neutrons.
• A cloud of electrons surrounds the nucleus.

What are atoms? (3 of 4)

• Protons are positively charged particles.
• Neutrons are noncharged (neutral) particles.
• Electrons are negatively charged particles.

What are atoms? (4 of 4)

• Atoms can vary their number of neutrons and/or electrons, but the number of protons remains constant.
• The number of protons is a defining feature and equal to the element's atomic number.
• Elements are organized by their atomic number in the periodic table.
• The periodic table of elements includes the chemical symbol, atomic number, and atomic mass.

The Periodic Table

• Atomic mass is the mass of the protons and neutrons in the atom (electrons have negligible mass).
• Atomic mass is the average mass of 6.022 x 10^23 atoms, or one mole, of the element.

Ions and Isotopes: Variations of Atoms (1 of 2)

• Two forms of atoms: ions and isotopes.
• All elements exist as a variety of isotopes, while only certain elements form ions.

Ions and Isotopes: Variations of Atoms (2 of 2)

• Ions are charged atoms that have an unequal number of protons and electrons.
• Cations are atoms that have lost electrons and have an overall positive charge.
• Anions are atoms that have gained electrons and have an overall negative charge.

Isotopes

• Isotopes are elements with the same number of protons but different numbers of neutrons.
• All elements exist as a mixture of isotopes.
• Isotopes are denoted by their atomic mass.
• Examples of carbon atoms: 99% are C-12 with 6 protons and 6 neutrons; <1% are C-13 with 6 protons and 7 neutrons; <1% are C-14 with 6 protons and 8 neutrons.

What are molecules?

• Molecules are formed when two or more atoms bond together. and Compounds are molecules made of more than one type of element.

Molecular Formulas (1 of 3)

• Molecules are noted by their molecular formula (chemical formula).
• Molecular formulas reveal the ratio of elements in a molecule.

Molecular Formulas (2 of 3)

• Rules for writing carbon-containing molecular formulas: Carbon (C) is listed first, followed by hydrogen (H) and then other elements in alphabetical order.
• Rule for writing molecular formulas if carbon is not present: Alphabetical order is usually followed.
• Rule for molecular formulas of ionic compounds: Positive ion listed first followed by the negative ion.

Molecular Formulas (3 of 3)

• Isomers are molecules with the same molecular formula but different molecular structures.
• The majority of biological molecules have at least one isomer.
• Example: C6H12O6 is the molecular formula for glucose, fructose, and galactose.

Organic versus Inorganic Molecules

• Organic molecules contain carbon and hydrogen (e.g., C6H1206).
• Inorganic molecules may contain carbon but lack the hydrogen (e.g., CO2).

Functional Groups

• Functional groups are molecules with shared chemical properties that often participate in chemical reactions.
• Organic molecules are classified and named based in part on the functional groups they contain.

Acids, Bases, and Salts (1 of 5)

• Solvents are dissolving agents.
• Solutes are dissolved substances.
• Most cellular chemistry occurs in an aqueous solution where water is the solvent.

Acids, Bases, and Salts (2 of 5)

• Acids add hydrogen ions (H+).
• Bases add hydroxide ions (OH-).

Acids, Bases, and Salts (3 of 5)

• Salts form when acids and bases react with each other: the acid contributes the anion and the base contributes a cation.

Acids, Bases, and Salts (4 of 5)

• The concentration of a solution is determined by the amount of solute dissolved in a specific volume of solvent.

Acids, Bases, and Salts (5 of 5)

• Molarity measures the concentration of a given solute in a liter of solvent (mol/L).
• Weight-volume proportion measures solute in mass in a volume of solvent (e.g., mg/mL).
• Intravenous solutions are typically labeled as having a particular percentage of a given solute: a 0.9% saline contains 9 grams of NaCl per L.

pH: A Measure of Acidity (1 of 6)

• Acidity and basicity is determined by H+ and OH- ions.
• The pH scale describes the acidity and basicity of a solution. and pH values typically between 0-14..

pH: A Measure of Acidity (2 of 6)

• The pH logarithmic scale creates a 10-fold difference in H+ ions for every whole-number increment on the scale.

pH: A Measure of Acidity (3 of 6)

• Pure water contains equal concentration of H+ and OH- and is chemically neutral (pH 7).
• Basic (alkaline) has more OH- than H+ and pH greater than 7.
• Acidic features have more H+ than OH- (pH less than 7).

pH: A Measure of Acidity (4 of 6)

• Acids added to basic solutions decrease the overall pH.
• Bases added to acidic solutions increases the overall pH.

pH: A Measure of Acidity (5 of 6)

• pH indicators can be added to growth media to observe acidic, neutral, or basic by-products.

pH: A Measure of Acidity (6 of 6)

• Microbes grow best at a pH of 6.5-8.5.
• Arterial blood has a pH of 7.35-7.45.
• Acidosis is lower than normal blood pH
• Alkalosis is higher than normal blood pH.
• Buffers stabilize pH by absorbing or releasing H+ ions.

CHEMICAL BONDS (1 of 2)

• Define valence electron and state how these electrons relate to bonding.
• Compare and contrast ionic and covalent bonds. • Describe what electrolytes are and explain why they are important in biological systems. • Discuss what polar covalent bonding is and how it sets the stage for hydrogen bonding. • Explain what hydrogen bonds are.

CHEMICAL BONDS (2 of 2)

• Describe van der Waals interactions.
• Define the terms hydrophobic, hydrophilic, and amphipathic and describe how they relate to micelle formation.

Electrons determine what bonds can form (1 of 3)

Chemical bonds are the "forces" binding atoms in molecules.

• Atoms contain elections arranged in electro shells.
• Each shell has a maximum capacity for number of elections. " The outermost shell is the valence shell.

Electrons determine what bonds can form (2 of 3)

• Valence Electrons (electrons in the valence shell) participate in chemical reactions.

Electrons determine what bonds can form (3 of 3)

• Atoms with FULL valence shells have stable electron configurations that leave them nonreactive (inert): noble gases.
• Atoms with NOT FULL valence shells - such elections - are reactive.

Ionic Bonds (1 of 2)

• Ionic bond - forms when electrons are transferred to make ions - creates Electrostatic force of attraction that exists between.

Ionic Bonds (2 of 2)

• Form electrolytes when dissolving.

Covalent Bonds (1 of 2)

Electrostatic attraction of atoms by sharing one or more pairs of atoms.

• A single covalent bonds is one shared pair with atoms.
• A double covalent bond is multiple shared pairs with atoms

Covalent Bonds (2 of 2)

• Carbon is the Core atom of organic molecules as it can form 4 covalent bonds with Catenation • Capable of catenation due to the its of atoms to create chains due to 4 links.

Polar Covalent Bonds (1 of 2)

Result from a partial equalization of electrons.

Polar Covalent Bonds (2 of 2)

• Highly electronegative atoms (O, N, F) hog electrons in covalent bond forms partial negitative charge/
• Forms A dipole results causespartial positive and negative ends.

Hydrogen Bonds: Noncovalent Interactions (1 of 2)

• Electrostatic attraction between 2 molecules or within one molecule.

Hydrogen Bonds: Noncovalent Interactions (2 of 2)

• Can have intermolecular (formed between molecules) and Intramolecular type (within 1 single mole).

Van der Waals Interactions

• These are temporary dipoles. That have attraction due to Van Der Waals interaction.
• Has significant molecules can stabilizing effects!

Water prefers to interact with polar molecules

• Polar covalent water forms.
• Hydergoen bombs for polar substance solving.
• great solvent with that capacity but doesn't' for nonpolar substanc

Hydrophobic, Hydrophilic, and Amphipathic Molecules (1 of 2)

• Hydrophilic substances are "water loving" and readily dissolve in water.
• Hydrophobic substances are "water fearing" and do NOT readily dissolve in water.

Hydrophobic, Hydrophilic, and Amphipathic Molecules (2 of 2)

• Amphipathic molecules have hydrophobic and hydrophilic properties (e.g., micelles and phospholipids.) Chemical reactions = Reactents to Products

CHEMICAL REACTIONS

· Define catalysis. · Explain synthesis, decomposition,and exchange reactions. Define dehydration synthesis and.hydrolysis reactions. • Discuss.what activation energy

Chemical reactions make and break chemical bonds

• Reactions are the ingredients of a chemical reaction. • Product are the substances generated as a result of the reaction.

Chemical Equations: Recipes for Reactions

• Catalysts have is an to accelerate.

Synthesis Reactions (1 of 2)

• Synthesis combine.
• A+B=AB.

Synthesis Reactions (2 of 2)

• Dehydrationsynthesis reactants. water formed..
• Remove H2O to form bond. HO. longer molecule

Decomposition Reactions (1 of 2)

Reations down . AB= A+B

Decomposition Reactions (2 of 2)

Hydrolilis reactions ads. bonds.

• Addition bonds water. protein, unk.
• • Four amino acids Amo acid 1

*Exchange reactions

Reations involves swapping one or components in a .

• AB=AC +B.

Chemical reactions consume or release energy

=Reations invovle •Require energy.

Exchange reactions

Single and Double.

Checal consum relase and

minum energy start

Endergonic versus Exergonic Reactions

• Exergonic energy product to reactions. : release energy.
• *Endergonic reations released Reaetions use. produets higher enegy released

BIOLOGICALLY IMPORTANT MACROMOLECULES

Name and Describe 4 groups of their blocks. · Deseribe glycosidic bonds, bondi,and phoester bonds. Explain a functional characteristics ofs, ,nucleic and protein. . Compare and contrast and ribonucleotides.

• Surmmarize how impacts lipid characteristics .. State do . Compare and contrast and bonde protein.

There are four main classes of biomolecules (1 of 2)

• lipids, and the for. main classes of biomolecules.

There are four main classes of biomolecules (2 of 2)

• Biological macromolecules .by

Carbohydrate Structures (1 of 2)

• Monosaccharides.
• Disaccharides. Ch2oh. -O H2O. -OH Monoshacaride

Carbohydrate Structures (2 of 2)

• Glycosidic and and to adds

Carbohydrate Functions (1 of 3)

• Function
• Energysource
• structral bilemolecules

Carbohydrate Functions (2 of 3)

sructurels.

Carbohydrate Functions (3 of 3)

Capsule Based by bacteria Adhere surfaces.

Lipids include fats, oils, waxes, and steroids

• collection.
• All made of carbon, hydrogen, .
• Some contain makes

Lipid Structures (1 of 3)

• Saturateldouble and acids.
• Pack tightly usually room Examples: butter - Glycerol. acid

Lipid Structures (2 of 3)

• Unsatruaed contains double bonds on
• Chains prevent tightly butter

•Lipid, structures (3of 3)

Lipid functions (1 of 3.

Lipid Functions (2 of 3)

• Organize in lipid bilaers
• Glycosides
• -Lipiprpteins

Lipids (3 of 3 )

Nucleic acids include DNA and RNA

• Nucleic acids the genetic.
• • • stranded •Single -

Nucleic structures

nucleic acid structures

DNA , cytosine thyimine. Bases and 5 -11.

• RNA. Contains Bases: cytosine and 5- carabon .sugar and phosphate

Nucleic Structures

Protein Structures (1.2 )

PrimaryStructure

Peptides link

SecondaryStructure

TheEnd!

Learn about the two prerequisite options for BIO187 Microbiology with Lab: BIO101 and Microbiology Placement test. Students lacking college-level biology are encouraged to take BIO101, a 2-credit introductory course. Alternatively, students with a strong biology background can take the Microbiology Placement test.