2 A&P Basic Biochemistry (2)

Page 1: Introduction to Biochemistry

• Basic Biochemistry: An overview for Anatomy and Physiology

• Creator: Dr. Jarod Lynn for OpenStax A&P

• Word Cloud of related contents and quantities.

Page 2: States of Matter

• Definition: Anything that occupies space and has mass.

• States:

  • Solid: Has a definite volume and shape.

  • Liquid: Has a definite volume, shape determined by the container.

  • Gas: No definite shape or volume.

Page 3: Elements and Compounds

• Elements: Fundamental substances making up all matter.

  • Examples: Hydrogen (H), Helium (He), Oxygen (O), Carbon (C).

• Compounds: Substances composed of two or more elements joined by chemical bonds.

  • Examples: Glucose (C6H12O6), Methane (CH4), Carbon dioxide (CO2).

Page 4: Major Elements of the Human Body

• Composition:

  • Oxygen (O) - 65.0%

  • Carbon (C) - 18.5%

  • Hydrogen (H) - 9.5%

  • Nitrogen (N) - 3.2%

  • Calcium (Ca) - 1.5%

  • Phosphorus (P) - 1.0%

  • Others: Potassium (K), Sodium (Na), Chlorine (Cl), Magnesium (Mg), and trace elements like iron (Fe), zinc (Zn).

Page 5: Subatomic Particles

• Structure of Atoms: Contains

  • Protons: Positive charge, mass of 1 amu, located in the nucleus.

  • Neutrons: Neutral charge, mass of 1 amu, located in the nucleus.

  • Electrons: Negative charge, mass of 1/2000 amu, orbiting the nucleus.

• Balance of Charges: Atoms maintain equal numbers of protons and electrons.

Page 6: Isotopes

• Definition: Atoms that have the same number of protons but differ in the number of neutrons.

• Heavy Isotopes: Isotopes with more neutrons, often unstable and radioactive; used in medical imaging.

Page 7: Kinetic vs. Potential Energy

• Kinetic Energy: Energy associated with movement (high kinetic).

• Potential Energy: Stored energy that can be used later (low kinetic).

Page 8: Forms of Energy

• Types of energy:

  • Kinetic Energy: Movement energy.

  • Potential Energy: Stored energy.

  • Thermal Energy: Energy of moving particles (heat).

  • Chemical Energy: Energy stored in food and fuels.

  • Mechanical Energy, Sound Energy, Electrical Energy: Various forms of usable energy in different contexts.

Page 9: Law of Conservation of Energy

• Total energy remains constant; it can change form but not be created or destroyed.

• Equation: KEi + PEi + Wnc + OEi = KEf + PEf + Oef

  • KE: Kinetic energy, PE: Potential energy, W: Work, OE: Other energy.

Page 10: The Periodic Table Overview

• Atomic Number: Number of protons.

• Atomic Symbol: Unique one to three letter designation.

• Atomic Mass: Average mass of all isotopes of an element.

Page 11: Electron Orbitals

• Structure of Electron Orbitals:

  • Shells around the nucleus hold electrons.

  • First shell: 2 electrons; subsequent shells can hold 8 electrons.

  • Outermost shell (valence shell) determines reactivity.

Page 12: Valence Shells and Reactivity

• Valence Shells: Atoms with full outer shells are stable and unreactive (He, Ne, Ar).

• Unfilled valence shells lead to reactivity and bond formation.

Page 13: Molecules and Compounds

• Distinction between molecules and ions:

  • Molecules: Two or more atoms bonded together.

  • Ions: Charged particles can be cation (+) or anion (-).

Page 14: Ionic Bonds

• Cations: Atoms that lose electrons (positive charge).

• Anions: Atoms that gain electrons (negative charge).

• Example: Sodium (Na) donates an electron to Chlorine (Cl).

Page 15: Ionic Bonds and Electrolytes

• Formation: Cations and anions attract each other to form ionic bonds.

• Salts: Form from ionic bonds, can dissociate in water.

Page 16: Covalent Bonds

• Types of Covalent Bonds:

  • Single Bond: H-H

  • Double Bond: O=O

  • Triple Bond: N≡N

• Polarity: Non-polar share equally, polar share unequally.

Page 17: Hydrogen Bonds

• Definition: Attraction between slightly positive hydrogen atoms and negatively charged atoms.

• Example: Water molecules exhibiting surface tension due to hydrogen bonds.

Page 18: Types of Chemical Reactions

• Synthesis Reaction: Two substrates form a product.

• Decomposition Reaction: One substrate breaks down into two or more products.

• Exchange Reaction: Two substrates exchange portions, forming different products.

Page 19: Factors Influencing Reaction Rates

• Influencing factors:

  • Size of molecules, state (gas/solid), temperature, concentration, pressure, and presence of enzymes.

Page 20: Organic vs. Inorganic Compounds

• Organic Compounds: Contain both Carbon (C) and Hydrogen (H).

• Inorganic Compounds: Do not contain both.

Page 21: Roles of Water in the Body

• Functions of water:

  • Lubrication, temperature regulation, cushioning, solvent properties.

Page 22: Types of Mixtures

• Solution: Homogeneous mixture (e.g., seawater).

• Colloid: Particles scatter light (e.g., milk).

• Suspension: Heterogeneous mixture with suspended particles (e.g., blood).

Page 23: Salts and Ions in Water

• Salts dissociate into charged particles when dissolved in water;

  • A substance that releases ions other than H+ or OH-.

Page 24: Acids and Bases

• Acids: Release H+ ions in solution.

• Bases: Release OH- ions or accept H+ ions.

Page 25: pH Scale

• Definition: Measure of acidity or alkalinity; ranges from 0 to 14.

• pH of 7: Neutral (pure water); lower pH = higher acidity.

Page 26: Human Blood pH

• Normal range: 7.35-7.45; fluctuations can be hazardous.

• Buffer: Weak acid and its conjugate base that maintains pH.

Page 27: Functional Groups in Organic Chemistry

• Hydroxyl, Carboxyl, Amino, Methyl, Phosphate: key functional groups that define organic compounds.

Page 28: Carbohydrates

• Monosaccharides: Simple sugars, such as glucose;

• Disaccharides: Formed by two monosaccharides (e.g., sucrose);

• Polysaccharides: Long chains of monosaccharides, storage and energy.

Page 29: Lipids

• Types: Triglycerides (fat storage), phospholipids (cell membranes), steroids (cholesterol and hormones).

Page 30: Proteins

• Made of 20 different amino acids; functional structure defined by sequence and bonds (peptide bonds).

Page 31: Enzymes

• Catalysts that lower activation energy; are not altered by the reactions they catalyze.

Page 32: Nucleic Acids

• Components: Pentose sugar (ribose or deoxyribose), phosphate group, and nitrogenous bases (adenine, guanine, cytosine, thymine, uracil).

Page 33: Adenosine Triphosphate (ATP)

• Structure: Composed of adenine, ribose, and three phosphate groups; acts as a primary energy carrier in cells.