HAPS Anatomy & Physiology Learning Outcomes MODULE C: Chemistry & Cell Biology

Flashcards for HAPS Anatomy & Physiology Module C: Chemistry & Cell Biology

Compare and contrast atoms, elements, molecules, and compounds.

Atoms: Basic units of matter; Elements: Pure substances composed of only one type of atom; Molecules: Two or more atoms held together by chemical bonds; Compounds: Molecules containing two or more different elements.

Describe the charge, mass, and relative location of electrons, protons, and neutrons in an atom.

Electrons: Negative charge, negligible mass, orbit the nucleus; Protons: Positive charge, significant mass, located in the nucleus; Neutrons: No charge, significant mass, located in the nucleus.

Relate the number of electrons in an electron shell to the atom’s chemical stability and its ability to form chemical bonds.

Atoms are most stable when their outermost electron shell is full. This stability influences their ability to form chemical bonds.

Compare and contrast the terms ion, electrolyte, free radical, isotope, and radioisotope.

Ion: An atom or molecule with an electrical charge due to the loss or gain of electrons; Electrolyte: A substance that dissociates into ions when dissolved in water; Free Radical: An atom or molecule with an unpaired electron; Isotope: Atoms of the same element with different numbers of neutrons; Radioisotope: An isotope with an unstable nucleus that decays, emitting radiation.

Explain how ions and isotopes are produced by changing the relative number of specific subatomic particles, using one element as an example.

Ions are produced by the gain or loss of electrons, altering the charge. Isotopes are produced by changing the number of neutrons, affecting the mass.

Distinguish among the terms atomic number, mass number, and atomic weight.

Atomic Number: Number of protons in an atom; Mass Number: Total number of protons and neutrons in an atom; Atomic Weight: Average mass of all isotopes of an element.

Explain the mechanism of each type of chemical bond and provide biologically significant examples of each: covalent, ionic, and hydrogen bonds. Understand electronegativity and how this affects bonding and polarity.

Covalent Bond: Sharing of electrons between atoms (e.g., water); Ionic Bond: Transfer of electrons between atoms, creating ions that are attracted to each other (e.g., sodium chloride); Hydrogen Bond: Weak attraction between a hydrogen atom and an electronegative atom (e.g., hydrogen bonds between water molecules). Electronegativity influences how electrons are shared and the polarity of the bond.

Compare and contrast nonpolar covalent and polar covalent bonds.

Nonpolar Covalent Bond: Electrons are shared equally; Polar Covalent Bond: Electrons are shared unequally, creating partial charges.

List the following types of bonds in order by relative strength: nonpolar covalent, polar covalent, ionic, and hydrogen bonds.

Nonpolar covalent > Polar covalent > Ionic > Hydrogen

Describe the physiologically important properties of water.

Excellent solvent, high heat capacity, high heat of vaporization, cohesive and adhesive properties.

Compare and contrast the terms solution, solute, solvent, colloid suspension, and emulsion.

Solution: Homogeneous mixture of solute and solvent; Solute: Substance dissolved in a solvent; Solvent: Substance in which the solute dissolves; Colloid: Mixture with medium-sized particles; Suspension: Mixture with large particles that settle out; Emulsion: Mixture of two liquids that do not dissolve in each other.

Define the terms salt, pH, acid, base, and buffer.

Salt: Ionic compound formed from the reaction of an acid and a base; pH: Measure of hydrogen ion concentration; Acid: Substance that releases hydrogen ions in solution; Base: Substance that accepts hydrogen ions in solution; Buffer: Substance that resists changes in pH.

State the pH values for acidic, neutral, and alkaline (basic) solutions.

Acidic: pH < 7; Neutral: pH = 7; Alkaline (Basic): pH > 7

Relate the hydrogen ion concentration in a solution to the pH of a solution. Understand that a change in a unit of pH is a 10 fold change in the hydrogen ion concentration.

The higher the hydrogen ion concentration, the lower the pH (acidic); the lower the hydrogen ion concentration, the higher the pH (basic).

Relate changes in pH of a solution to changes in protein structure

Changes in pH can disrupt the hydrogen bonds and ionic bonds that maintain the protein's shape, leading to denaturation and loss of function.

Define the term organic molecule.

Molecules that contain carbon and are typically associated with living organisms.

Explain the relationship between monomers and polymers.

Monomers are small building blocks that combine to form larger polymers through polymerization.

Define and provide examples of dehydration synthesis and hydrolysis reactions.

Dehydration Synthesis: A chemical reaction that removes a water molecule to join monomers, forming a polymer. Hydrolysis: A chemical reaction that adds a water molecule to break the bond between monomers, breaking down a polymer.

Compare and contrast the general molecular structure of carbohydrates, proteins, lipids, and nucleic acids.

Carbohydrates: Sugars and starches, composed of C, H, and O; Proteins: Composed of amino acids; Lipids: Fats, oils, and waxes, composed of C, H, and O; Nucleic Acids: DNA and RNA, composed of nucleotides.

Describe the building blocks of carbohydrates, proteins, lipids, and nucleic acids, and explain how these building blocks combine with themselves or other molecules to create complex molecules in each class, providing specific examples.

Carbohydrates: Monosaccharides (e.g., glucose) combine to form polysaccharides (e.g., starch); Proteins: Amino acids combine to form polypeptides and proteins; Lipids: Fatty acids and glycerol combine to form triglycerides; Nucleic Acids: Nucleotides combine to form DNA and RNA.

Describe the four levels of protein structure and the importance of protein shape for function.

Primary: Amino acid sequence; Secondary: Local folding patterns like alpha-helices and beta-sheets; Tertiary: Overall 3D structure of a single polypeptide chain; Quaternary: Arrangement of multiple polypeptide chains in a protein complex. The shape is crucial for its specific function.

Define enzyme and describe factors that affect enzyme activity.

An enzyme is a biological catalyst that speeds up chemical reactions. Factors such as temperature, pH, substrate concentration, and inhibitors affect enzyme activity.

Describe the three main parts of a cell (plasma [cell] membrane, cytoplasm, and nucleus), and explain the general functions of each part.

Plasma (cell) membrane: Outer boundary of the cell, controls what enters and exits; Cytoplasm: Everything inside the cell membrane except the nucleus, site of many cellular processes; Nucleus: Contains the cell's genetic material (DNA), controls cellular activities.

Compare and contrast cytoplasm and cytosol.

Cytoplasm: Includes all cellular contents between the plasma membrane and the nucleus. Cytosol: The fluid portion of the cytoplasm, excluding organelles.

Describe the structure and roles of the cytoskeleton.

Provides structural support, helps with cell movement, and facilitates intracellular transport.

Define the term organelle.

A specialized subunit within a cell that has a specific function.

Describe the structure and function of the various cellular organelles.

Examples: Mitochondria (energy production), Ribosomes (protein synthesis), Endoplasmic Reticulum (ER, synthesis and transport), Golgi apparatus (modification and packaging of proteins), Lysosomes (waste disposal).