The Chemical Level of Organization Part 1 PDF

Chemical Level of Organizati on Part 1 Objectives: 1. Describe the structural and physical properties of water in an aqueous solution. 2. Describe the concepts of concentration and osmolarity. 3. Review enzymes and activation energy. 4. Identify the differences between inorganic and organic...

Chemical Level of Organizati on Part 1 Objectives: 1. Describe the structural and physical properties of water in an aqueous solution. 2. Describe the concepts of concentration and osmolarity. 3. Review enzymes and activation energy. 4. Identify the differences between inorganic and organic compounds. 5. Explain pH and its importance in physiology. 6. Describe the structure and function macromolecules and classify various types. 7. Outline the steps of cellular respiration. 4 most common elements in the body Oxygen – 65% Carbon – 18.6% Hydrogen – 9.7% Nitrogen - 3.2% 96.5%  What is an Atom? Smallest unit of matter Atoms are made of subatomic particles – Protons – Neutrons – Electrons Atoms combine together to form molecules Chemical Bonding (connection) Atoms join together through bonds to form chemicals with different characteristics. 4 Types Polar Covalent Bond Pure (Non-Polar) Covalent Bond Ionic Bond Hydrogen Bonds  Pure (Non- Polar) Covalent Bond Electrons are shared equally – Commonly with two atoms of the same element Atoms’ charge is equal on both “sides” – All the diatomic molecules are non-polar – Diatomic means they can bond with themselves – No, you don’t need to memorize which atoms are diatomic and which aren’t, but you do need to know what a diatomic molecule is.  Polar Covalen t Unequal sharing of electrons One atom has a stronger pull on the electron Electron(s) spend more time with one atom Because the electrons are negative, one side becomes negatively charged and the other becomes positively charged.  Unequal sharing of electrons One atom takes an electron from the other atom When an atom loses an electron it become more positive This creates a cation (positively charged atom) When an atom gains an electron it becomes more negative This creates an anion (negatively charged Ionic atom) Bond  Covalent Bond: Water Covalent bonding occurs between 1 Oxygen and 2 Hydrogen atoms This is a polar covalent bond because there is unequal sharing Oxygen holds onto Hydrogen’s electron more, making the oxygen more negative and the hydrogen more positive  Hydrogen Bonds Hydrogen bonds between H2O molecules cause surface tension (tendency for water molecules to attract one another) Hydroge n is Special Surface Tension & The Lungs If surface tension is too high in lungs, they collapse Role of surfactant – to decrease surface tension It disrupts the hydrogen bonding between water molecules Alveoli WITHOUT Surfactant (High surface tension) Alveoli WITH Surfactant (low surface tension) What would happen with someone born WITHOUT surfactant? Why?  H2O Surface Tension & The Lungs If surface tension is too high in lungs, they collapse – i.e. premature infants – Lack of surfactant makes inhalation difficult- more work to overcome surface tension – Premature infants that lack surfactant suffer from respiratory distress syndrome Role of surfactant – to decrease surface tension  Water How long can a body survive without food? An average adult male can survive for 30 to 40 days without food. How long can a body survive without water? The approximate amount of days that you could go without water in your organism is anywhere from 8-14 days. *So, you can see that water is important to the body’s function  Four Properties of Water 1. Solubility: water’s ability to dissolve a solute in a solvent to make a solution (i.e.. Sugar in water) 2. Reactivity: most body chemistry uses or occurs in water (aqueous solution) i.e. DNA only maintains its structure in water 3.High heat capacity: water’s ability to absorb and retain heat (Helps maintain homeostasis) 4.Lubrication: to moisten and reduce friction (joints)  Molecules and Water Hydrophilic: – hydro = water, philos = loving – reacts with water Hydrophobic: – phobos = fear – does not react with water  Electrolytes Substances that can dissolve in water and dissociate into ions. Electrolyte imbalance seriously disturbs vital body functions i.e. Decrease in Potassium, muscle cramps Sodium imbalance can disrupt nerve conduction Na+ Sodium ion K+ Potassium ion Cl- Chloride ion Ca2+ Calcium ion HCO3- Bicarbonate ion  Importance of Electrolytes Potassium K+ (Bananas, Avocados) Decrease below normal: General muscular paralysis Increase above normal: Weak and irregular heartbeats Homeostasis (balance of the ions) Electrolytes excreted or retained (Kidneys) What is pH and why do we need buffers?  Acids and Bases Acid: Electrolytes that dissociate to release hydrogen ions (H+) Base: Substances that release ions that combine with hydrogen ions.  pH (the POWER of hydrogen)! pH: – the RELATIVE concentrations of hydrogen ions (H+) and hydroxide (OH-) anions in a solution Neutral pH: – a balance of H+ and OH— – The number of H+ and OH— is exactly equal – pure water = 7.0 Acid (acidic): pH lower than 7.0 – high H+ concentration, low OH— concentration Base (basic): pH higher than 7.0 – low H+ concentration, high OH— concentration Which side is acidic and basic?  pH Scale Has an inverse relationship with H+ concentration: – more H+ ions mean lower pH, less H+ ions mean higher pH – More OH- ions means a higher pH, less OH- ions means a lower pH  Acids & Bases in the Body pH of blood = 7.35-7.45 – pH measures free H+ ions in solution Excess H+ ions (low pH): – damages cells and tissues – alters proteins – interferes with normal physiological functions Excess OH- ions (high pH) –In the blood, high pH can cause uncontrollable and sustained skeletal muscle contractions  Acid and Alkaline Acidosis: – excess H+ in body fluid (low pH) Alkalosis: – excess OH— in body fluid (high pH)  pH Homeostasis Buffers: chemicals that resist pH change weak acid/salt compounds neutralizes either strong acid or strong base  Organic and Inorganic Molecules Organic compounds: – MUST have C bonded to H – Often hydrocarbon chains Inorganic compounds: – Usually do NOT contain C and H atoms as primary structure – Most important in body: Carbon dioxide (CO2) Oxygen (O2) Water (H2O) Inorganic acids, bases and salts Label these molecules organic or inorganic H2O C4H2O2 CaCl2 HC6H7O6 CH3CO2H NH2 H2SO4  Functional Groups Molecular groups which allow molecules to interact with other molecules Note: no you don’t need to memorize these, but knowing them will help you in the long run. Macromolecules Carbohydrat es Proteins Fats (Lipids) Nucleic acids  Carbohydrates: Starches & Sugars Hydrophilic organic molecule Can be broken down into energy for use by the body  Monosaccharides and Disaccharides Monosaccharides: – simple sugars with 3 to 7 carbon atoms (i.e. glucose, galactose, fructose) – ’Mono’ means 1 Disaccharides: – 2 simple sugars condensed by dehydration synthesis Dehydration synthesis is the process of removing a water molecule – This creates a bond between two molecules – ‘Di-’ means 2 i.e sucrose = glucose + fructose Monosaccharides and Disaccharides – Dehydration Synthesis V ideo  Polysaccharides Chains of many simple sugars (glycogen) ‘Poly’ means many  Protein Structure Proteins- most abundant and important organic molecules Basic elements: – carbon (C), hydrogen (H), oxygen (O), and nitrogen (N) Basic building blocks: – 20 amino acids  Protein Functions 7 major protein functions: 1. support: 4. buffering: regulation of structural proteins metabolic regulation: enzymes 2. movement: 5. coordination and contro contractile proteins (muscles)hormones 3. transport: 6. defense: transport proteins antibodies  Amino Acids 1. central carbon 2. hydrogen 3. amino group (—NH2) 4. carboxylic acid group (— COOH) 5. variable side chain or R group  Peptides A dehydration synthesis between: – amino group of 1 amino acid – carboxylic acid group of t – Forms a peptide bond  Shape and Function Protein function is based on shape Shape is based on sequence of amino acids Only 20 different amino acids Denaturation: – loss of shape and function due to heat or pH  Primary Structure Polypeptide: – a long chain of amino acids Secondary Structure Hydrogen bonds form spirals or pleats  Tertiary Structure Secondary structure folds into a unique shape Quaternar y Structure Final protein shape: – several tertiary structures together