Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Biological aspects of fluorine wikipedia , lookup
Expanded genetic code wikipedia , lookup
Protein adsorption wikipedia , lookup
List of types of proteins wikipedia , lookup
Gaseous signaling molecules wikipedia , lookup
Photosynthesis wikipedia , lookup
Nucleic acid analogue wikipedia , lookup
Microbial metabolism wikipedia , lookup
Evolution of metal ions in biological systems wikipedia , lookup
Biosynthesis wikipedia , lookup
Do Now 1. Why does a coach tell athletes to eat carbohydrates the night before a game? 2. Why do body builders drink protein shakes? Biochemistry Biochemical compounds Organic Inorganic Organic Compounds • Contain carbon and hydrogen • Ex: C6H12O6 CH4 • Some organic compounds: – Carbohydrates – Lipids – Nucleic acids – Proteins Carbon • The basis of all life • Organic chemistry studies • • all compounds that contain bonds between carbon atoms Carbon can covalently bond with many other elements because it has four valence electrons Carbon can form chains or rings by bonding with other carbon atoms Macromolecules • “Giant molecules” made up of smaller molecules • Polymerization = process joining smaller molecules, monomers, to form larger molecules, polymers Carbohydrates • Made up of carbon, hydrogen, and oxygen atoms usually • • • • in a 1:2:1 ratio Living things use carbohydrates as their main source of energy. Plants use carbohydrates for structural purposes. Monosaccharides or simple sugars (glucose/galactose/fructose) is broken down for immediate energy for all cell activities Extra sugar is stored as polysaccharides or complex carbohydrates (starches/glycogen/cellulose) Figure 2-13 A Starch Section 2-3 Starch Glucose Go to Section: Lipids • Mostly made up of carbon and hydrogen atoms and generally are not soluble in water – Fats – Oils – Waxes • Store energy or provide waterproofing • Many lipids are formed by a glycerol molecule combining with fatty acids to form chains – Saturated = the fatty acids contain the max number of hydrogen atoms with single bonds throughout – Unsaturated = there is at least one carbon-carbon double bond – Polyunsaturated = more than one double bond Nucleic Acids • Macromolecules containing • • hydrogen, oxygen, nitrogen, carbon and phosphorus Polymer made up of covalently bonded monomers called nucleotides Nucleotides are made up of – a 5-carbon sugar – a phosphate group – a nitrogenous base • Nucleotides store and transmit hereditary, or genetic, information – Ribonucleic acid (RNA) – Deoxyribonucleic acid (DNA) Proteins • Macromolecules that contain • • • • nitrogen, carbon, hydrogen, and oxygen Proteins are polymers made up of covalently bonded amino acids Amino acids are compounds with an amino group (-NH2), a carboxyl group (-COOH) on opposite ends and different “R” groups The instructions for arranging amino acids into different proteins are stored in DNA Each protein has a specific role such as controlling the rate of reactions, regulating cell processes, transporting molecules, or fighting disease. Figure 2-16 Amino Acids Section 2-3 Amino group Carboxyl group General structure Go to Section: Alanine Serine Concept Map Section 2-3 Carbon Compounds include Carbohydrates Lipids Nucleic acids Proteins that consist of that consist of that consist of that consist of Sugars and starches Fats and oils Nucleotides Amino Acids which contain Carbon, hydrogen, oxygen Go to Section: which contain Carbon, hydrogen, oxygen which contain which contain Carbon, hydrogen, oxygen, nitrogen, phosphorus Carbon, hydrogen, oxygen, nitrogen Inorganic compounds • Do not contain carbon and hydrogen!!! • Ex: CO2 NH3 CaCl2 Water • The single most abundant compound in most living things • The molecule is neutral with 10 protons and 10 electrons Polarity • Since the oxygen molecule has 8 protons (compared to hydrogen only having 1 proton), the oxygen has a stronger attraction for the electrons • Thus, there is a slightly negative charge at the oxygen end and a slightly positive charge at the hydrogen end • Water is a polar molecule because it has an uneven distribution of charge from the uneven distribution of electrons between the oxygen and hydrogen atoms. Hydrogen bonds • Polar molecules can attract each • • • • • other The charges are in parentheses to show they are weaker than ionic charges Hydrogen bonds form between the hydrogen and oxygen atoms, which are weaker than ionic or covalent bonds, but the strongest bond between molecules The hydrogen bonding explains many of water’s properties such as cohesion (water beads) and adhesion (meniscus and capillary action) Cohesion is an attraction between molecules of the same substance. Adhesion is an attraction between molecules of different substances. Mixtures • Two or more elements or compounds that are physically mixed together, but not chemically combined. – Solutions – Suspensions Solutions • Mixtures where all of the components are evenly distributed throughout – Solute – the substance that dissolves – Solvent – the substance in which the solute dissolves Suspensions • Mixtures where some materials do not dissolve pH • A water molecule can react to form the ions H+ • • and OHThe pH scale indicates the concentration of hydrogen ions [H+] compared to the concentration of hydroxide ions [OH-] in solution The pH scale ranges from 0 to 14 and increases by a factor of 10 – pH of 7 = neutral because there’s an equal number of H+ & OH- ions – pH < 7 = acids because there’s more H+ ions than OH- ions – pH > 7 = bases because there’s less H+ ions than OH- ions pH • The pH will affect chemical reactions that take place within cells • Thus, controlling pH within a neutral range is important for maintaining homeostasis • Buffers are weak acids (pH 4-6) or bases (pH 8-10) that can react with strong acids (pH 0-3) or bases (pH 11-14) to prevent sudden pH changes