1.Matter and Organic Compounds Matter =

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1 The Chemistry of Life Notes Unit 2 1.Matter and Organic Compounds Matter = All things are made of matter Name Matter is made up of substances Chemical substance = definite composition throughout Either or Elements = Found in the of Elements Roughly elements are found in nature, with more created by man (mostly radioactive) Metals copper, magnesium, iron Nonmetals oxygen, hydrogen, nitrogen, phosphorus Metalloids silicon Compound = The smallest particle of a compound = Example = (H2O) Created by chemical reactions (ionic, covalent, hydrogen) Forces that keep together 1

2 2. Water, Acids, and Bases Water (H2O) Almost % of Earth s surface is covered in water 3 states of matter (most abundant first) Composed of 2 atoms bonded to 1 atom Properties of Water:, tasteless and Polar molecule due to of e - Oxygen slight charge Hydrogens slight charge Hydrogen bonding, due to between H2O molecules, is responsible for: (between H2O and other molecules) (between H2O molecules) Relatively boiling point Solid form (ice) is dense than liquid form Water and Life is composed of approximately 70% water. Water many substances that organisms depend on Water is needed for many biochemical Photosynthesis 6 CO H 2O + energy C 6H 12O 6 6 O 2 Cellular respiration C 6 H 12 O O 2 6 CO H 2 O + energy Solutions Solution = that has the same composition throughout Made up of a solute that is mixed into a solvent H2O is a universal solvent Some solutions are or Acids = excess ions(h3o + ) Bases = excess ions (OH - )ions 2

3 Acids and Bases = measure of hydronium ions (H3O + ) in a solution Use ph scale to measure ph 7 = (pure water) ph below 7 = acidic strongest is closer to ph above 7 = basic strongest is closer to taste sour, can damage proteins (organisms) and materials at really low ph levels taste bitter, can damage proteins (organisms) and materials at really high ph levels 3

4 3. Macromolecules Organic compounds compounds made of mainly Make up many compounds found in Other structures of organisms Compounds that perform life processes Carbon can form stable bonds with other carbons and other elements Roughly, 10,000,000 - compounds in living things Living things can use organic compounds as an source. Carbon s capability to form 4 bonds is the reason for carbon s success = energy Breaking bonds -> energy Forming bonds -> energy Macromolecules - Also called Made up of smaller called. Examples: (DNA and RNA) Type of Organic Molecule Carbohydrates Examples Elements Functions Carbon, Hydrogen, Oxygen Lipids Carbon, Hydrogen, Oxygen Chart cont.--> 4

5 Type of Organic Molecule Proteins Examples Elements Functions Carbon, Hydrogen, Oxygen, Nitrogen, Sulfur Nucleic Acids Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorus How are macromolecules formed? Also called Forms by combining by removing. How are macromolecules separated or digested? separates molecules by adding CARBOHYDRATES the most type of compound. Functions Store (sugars, starch, glycogen) (cellulose, chitin) built of small, units that form bonds with each other to make a larger molecule the small repeating units are called Monosaccharides - sugars of carbohydrates Job : sugars contain stored Examples: - generally results from the digestion of other carbohydrates. Glucose is used for energy by the cells - is found in fruit - is found in milk (makes up lactose) 5

6 Disaccharides: sugars Examples: table sugar malt sugar (grain) milk sugar Polysaccharides: A carbohydrate that forms when simple sugars bind together in a chain. 2 main functions: energy structures of living things. Examples: Black Green Red 6

7 LIPIDS Lipids are, & Three major roles: 1. Store (more energy per gram than carbohydrates) 2. Form 3. Used as chemical Monomer: Formed by a combination of acids &. Saturated Fatty Acids In saturated fatty acids, carbon atoms are bonded to as many atoms as possible. This causes the molecules to form chains The straight chains can be allowing them to store energy in a compact form saturated fatty acids are at room temperature. use saturated fatty acids to store energy. Example: butter and lard Unsaturated Fatty Acids In unsaturated fatty acids, some carbon atoms are not bonded to as many atoms as possible some and bonding between carbons It causes chains to The bent chains cannot be packed together very tightly unsaturated fatty acids are at room temperature. use unsaturated fatty acids to store energy. Example: Oils 7

8 Types of Lipids Lipids may consist of fatty acids alone, or they may contain other molecules as well. some lipids contain or groups. They include 1. : the main form of stored energy in animals 2. : the major components of cell membranes 3. : serve as chemical messengers and have other roles such as cholesterol in the cell membrane PROTEINS Made up of C, H, O and N Monomers are called Amino Acids are carbon chains with an group attached to one end and a group on the other end. Protein Structure: When amino acids bind together, they form a long chain called a. A protein consists of one or more polypeptide chains. levels of structure: The lowest level, a protein s structure, is its sequence of amino acids. The complex structures of different proteins give them unique properties, which they need to carry out their various jobs in living organisms. 8

9 Protein Jobs: 1. Help carry out chemical (ex. enzymes) 2. Pump in & out of cells. (channels) 3. Responsible for cell (cilia and flagella) NUCLEIC ACIDS Made of: C, O, H, N & P Monomer: Include 1. 5 carbon sugar (pentose) 2. Phosphate Group 3. Nitrogenous Base Types of Nucleic Acids: Ribonucleic Acid (RNA) Contains the sugar Deoxyribonucleic Acid (DNA) Contains the sugar ( deoxy means less oxygen) Job of Nucleic Acids Transmit 4. Chemical Reactions and Enzymes Biochemical Reactions A biochemical reaction is a process that changes some chemical substances into others. a substance that a chemical reaction is called a a substance that as a result of a chemical reaction is called a. During a chemical reaction, the are used up to create the products. reactant + reactant product(s) Combustion Example: Methane gas + oxygen gas burns to create carbon dioxide and water OR CH4 + 2O2 CO2 + 2H20 Arrow represents a reaction has occurred! 9

10 Conservation of Matter The QUANTITY of each element does change Reactants elements = Products elements # of atoms of each element appears on each side of the reaction arrow Exothermic Reactions heat (as energy) Reactants Products + Example: Endothermic Reactions energy from the environment (feels cold) Reactants + Products Example: Activation Energy ALL CHEMICAL REACTIONS NEED ENERGY TO GET STARTED! Starting energy = Activation energy gives the needed for chemicals to interacting reacting with each other Some reactions require more energy than others 10

11 Biochemical Reactions. take place inside = sum of all biochemical reactions in an organism Catabolism reaction molecules into smaller ones Example digesting food, using glucose Anabolism reaction large molecules from smaller ones Example storing fat, building muscle Enzymes that up biochemical reactions allow biochemical reactions to proceed with Are used up during reaction (recycled) Depend on several factors: ph Brainstorm: How would the functionality of our bodies by different if enzymes did not exist? 11