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Do Now!! What is an atom? Why do we have a periodic table? What information can we find in a periodic table? Chapter 6 Biochemistry Objectives To define an atom. To determine the make-up of an atom. To list different elements that can be found on Earth. To explain what type of information can be gathered from the periodic table. Atoms Smallest particle of matter that still has chemical properties Matter: anything that takes up space and has mass Contain 3 parts: + Protons: positively charged, contain mass of 1 Location: Neutrons: no charge, contain mass of 1 Location: Electrons: Outside nucleus, negatively charged, insignificant mass Location: Atoms make up Elements A pure substance that can’t be broken down into other substances by physical or chemical means. Made up of only 1 type of atom Contain a unique name and symbol. Periodic Table of Elements Periods: horizontal rows Groups: vertical columns: elements in the same group have similar chemical and physical properties. **Organized based on the # of protons in the nucleus of an atom.** Periodic Table Information Atomic number- tells us the # of protons (as well as electrons) Symbol- unique for each element. Atomic Mass- # of protons + neutrons 6 C 12.02 * How would you determine the number of neutrons in an atom?? So… What makes atoms different? How is carbon different from oxygen? Different numbers of protons!! Think-Pair-Share List the number of protons, neutrons, and electrons for the following… Mg Ca Fe Cl Do Now!! Complete the chart: Part of Atom Proton Neutron Electron Charge Mass Do Now!! 4 9.01 C 12.02 7 N Ne 20.18 Complete the missing information and include the number of protons, neutrons, and electrons. Do Now!! List the number of protons, neutrons and electrons for the following… H P K Ni Ar Objectives To practice drawing different atoms. To review parts of the atom by completing a worksheet activity. Drawing an atom… Things to remember! Proton # = Electron # Protons and neutrons are in the nucleus and add up to the atomic mass. Electrons are arranged in energy levels: 1st energy level holds 2 electrons 2nd energy level holds 8 3rd energy level holds 8 *Valence electrons: electrons on outermost shell Lets Draw Oxygen! How many protons, neutrons and electrons does an atom of oxygen have? How many valence electrons are there? Practice Let’s draw: 1. He 2. Na 3. S 4. C 5. Cl Do Now!! Please complete the table below! Acid Base #’s on pH scale Release_____ in water Litmus paper is _____ in its presence Examples What is a neutralization reaction? What are the reactants? Products? Do Now!! Let’s draw: 1. Ar 2. Al 3. Na 4. Ne 5. Mg Objectives To discuss isotopes and relate their research to the medical field To determine the number of protons, neutrons and electrons of ions To identify types of bonds What is wrong with this picture? Carbon -atomic symbol “C” -atomic # 6 -atomic mass 12.02 Isotopes Isotopes contain the same # of protons and electrons as the element, but a different number of neutrons. Ex: Carbon-14 Contains 6 protons (still carbon) Also contains 8 neutrons, instead of 6 Radioactive Isotopes Changing the # of neutrons changes the stability of the atom: causes decay in the nucleus or causes it to break apart. Ex: Carbon-14 is used in carbon-dating. We can tell how old something is by how much carbon is left. Radioactive Isotopes Ex: Radioactive isotopes are used to help doctors diagnose disease and locate certain types of cancer. What happens if there are different number of ______ than a normal atom? Neutrons? More protons than electrons? More electrons than protons? “Happy” Atoms Atoms need to have the right number of electrons around them (happy) Ions- charged atom or groups of atoms Ions can lose or gain electrons: Lose: form positive ions Gain: form negative ions Na Cl How many electrons does each of the following want to be “happy”? Oxygen Carbon Hydrogen Nitrogen Lets Practice! List the number of protons, neutrons and electrons in each ion: ONa+ N3ClF+ Are any of these atoms happy? Do Now!! Think-Pair-Share: - If an ion is positively charged, does it gain or lose electrons? - Negatively charged? - How many electrons does O3- have? Objectives Identify protons, neutrons and electrons in ions. Identify compounds. Determine what information can be received from a chemical formula. Do Now!! Identify the element and then state if it is a normal atom, an isotope, or an ion. Objectives Practice identifying components of ions by completing a worksheet Identify compounds. Determine what information can be received from a chemical formula. Compare and contrast ionic bonding vs. covalent bonding. Explain what “Vanderwalls interactions” are. Molecules and Compounds Molecule: Forms when two or more atoms form chemical bonds Compound: A pure substance formed when 2 or more different elements combine Always formed using a specific ratio Ex: fuel in cars (hydrocarbons) Chemically and physically different from the elements that make them up Must be broken down CHEMICALLY, not physically Chemical Formulas The number before the formula states how many molecules Ex. 4 H2O = 4 water molecules The subscript number states how many of that type of atom Ex. H2O = 2 hydrogen atoms, 1 oxygen atom O H H Let’s try some examples For the following examples list the total number of atoms for each element and how many of each molecule. 1. C6H12O6 2. 3CH4 3. 5CO2 4. 3O3 5. 4HCl Do Now!! For the following examples list the total number of atoms for each element and how many of each molecule. 1. 2H2SO4 2. 4HNO3 3. 5MgCl2 4. NaOH 5. 4C6H8O7 Objectives Compare and contrast ionic bonding vs. covalent bonding. Explain what “Vanderwalls interactions” are. Explain what a chemical reaction is. Identify reactants and products in a reaction. Balance an equation. How do compounds stay together? Bonds! 2 most common types 1. Covalent- atoms share electrons 2. Ionic- atoms gain or lose electrons to bond Covalent Bonding Carbon (C) – form 4 bonds (another 4 e) Hydrogen (H) – form one bond (1 e) Nitrogen (N) – form 3 bonds (3 e) Oxygen (O) – form 2 bonds (2 e) Ex: H2O Ionic Bond Some atoms tend to donate or accept electrons more easily than other atoms. Ex. Metals (D) and Non Metals (A) Van Der Waals Interactions o When molecules come close together, the attractive forces between slightly positive and negative regions pull on the molecules and hold them together. o The strength of the attraction depends on the size of the molecule, its shape, and its ability to attract electrons. Do Now!! Please take out your ion worksheet! Objectives To define chemical reaction To differentiate between endothermic and exothermic reactions To illustrate types of reactions in a lab activity 6.2 Chemical Reactions A chemical reaction -atoms or groups of atoms are reorganized into different substances. Chemical Reactions: Production of heat or light Formation of a gas, liquid, or solid Parts of a Reaction Reaction- Molecules breaking or coming together Reactants- What goes in the reaction Products- What comes out of the reaction Ex: Na+ + Cl- NaCl Energy in Reactions The activation energy minimum amount of energy needed for reactants to turn into products Types of Reactions Exothermic- releases heat energy: o The energy of the product is LOWER than the energy of the reactants. Types of Reactions (cont.) Endothermic - absorbs heat energy The energy of the products is HIGHER than the energy of the reactants. Demo time!! Endothermic or Exothermic?? Do Now!! Glucose and oxygen react to form carbon dioxide and water. Identify: Products Reactants Is this a balanced equation? + ATP (energy) Objectives To balance equations. To identify types of reactions. To explain how an enzyme works. To determine the difference between a solute and a solvent. Do Now!! Determine whether or not the following are Exothermic or Endothermic reactions: 1. Combustion reactions of fuels 2. melting ice cubes 3. Nuclear Bomb 4. a candle flame 5. cooking an egg 6. Photosynthesis Objectives To identify types of reactions. To explain how an enzyme works. To determine the difference between a solute and a solvent. To list the properties of water. What you should know about Type of Substrate enzymes!! Specialized proteins that act as “catalysts”: Aka they speed up reactions! Usually end in “ase” NOT consumed in the reaction: They are reused!! Enzyme Product Lipase Protein Amino Acid Protease Fats Fatty Acid Carbohydrase Carbohydrates Glucose Lactase Lactose Glucose Amylase Carbohydrates Glucose Pepsin Protein Amino Acid What do they do? o Lower the activation energy needed!! o Activation energy barrier is like a wall between two parts of a pond. o If an enzyme lowers the wall, more frogs have enough energy to reach the other side. How do they work? A substrate fits in the active site of an enzyme: Specific to one kind of substrate Lock and key This forms an enzyme substrate complex. Will then break or form bonds. Denaturing Enzymes Enzymes have specific optimal conditions: Temperature pH If those conditions change, enzyme is permanently damaged: Denatured! Cannot do its job Do Now!! What is the purpose of an enzyme? What was the enzyme used in your liver lab? What is a substrate? What was the substrate in your liver lab?? Objectives To identify types of reactions. To explain how an enzyme works. To determine the difference between a solute and a solvent. To list the properties of water. How do they work? http://www.youtube.com/watch?v=XTUm-75-PL4 6.3 Solutions Solution = Mixture of a solute dissolved in a solvent (ex: iced tea!) How do things dissolve? Polar Covalent Bond: Slight positive and negative charges Ex. H2O (universal solvent!) and NaCl (salt) Non-polar: Do not dissolve in water Ex. Lipids and Fats Mixtures Solute- substance that is dissolved Solvent- substance that the solute dissolved in. Ex. Hot chocolate (Water and Coco Powder) Mixtures Heterogeneous Homogeneous What is the difference? Mixtures Homogeneous- has a uniform composition throughout (a.k.a solutions). Heterogeneous- components remain distinct. Buffers What happens to enzymes in a strong pH? Buffers are mixtures that can react with acids or bases to keep the pH within a particular range: Ex: Keep body fluids at a pH of 6.5-7.5 Ex: Hemoglobin 6.4 Macromolecules of Life Organic Chemistry – The study of organic compounds: The element carbon is a component of almost all biological molecules (organic) Inorganic = no carbon C arbon H ydrogen N itrogen O xygen P hosphorus S ulfur Six most abundant elements of life!! Molecules Macromolecules - large molecules formed by joining smaller organic molecules together. Are also called Polymers – made from repeating units of identical (or nearly identical) compounds (monomers) Polymer monomer monomer monomer Do Now!! Determine whether the following substances are heterogeneous or homogenous: Chicken noodle soup Black coffee Jello Jello fruit salad Cole Slaw Whole milk Chipotle Burritos Do Now!! Label the parts of the reaction below: Objectives List the 4 macromolecules of life. Identify the 3 different types of carbohydrates. Explain the importance of carbs in the body. Explain why low-carb diets can be harmful. Carbohydrates Sources of energy Ratio of carbon : hydrogen : oxygen of 1:2:1 (CH2O)n Glucose n = # of CH2O in a chain * Ex: glucose (C6H12O6) *Where there’s a corner there’s a carbon!* * * * * Identify the Carbohydrates! 1) C6H12O6 2) CH3 3) C4H2O2 4) C24H48O24 Carbohydrates (cont.) Monosaccharide- values of n ranging from three to seven (simple sugar) ex: glucose (n = 6) Disaccharide - Two monosaccharides joined together ex: lactose Polysaccharide- many monosaccharides joined together ex: glycogen (energy storage in muscle) Monosaccharide (glucose) Disaccharide (lactose) Polysaccharide (glycogen) Do Now!! (P. 5) What are the four macromolecules? What are some differences between simple and complex carbohydrates? Which of the following are carbohydrates? CH2O C6HO6 C12H24O12 C6H12O5 Lipids Fats, oils and waxes Made mostly of C and H: Triglycerides Used for energy storage and insulation Fat – solid at room temperature Oil – Liquid at room temperature Lipids (cont.) Saturated vs. Unsaturated Saturated Fats - Only Single bonds between the carbons Solid at room temperature (typically) More unhealthy Unsaturated Fats Double bonds between the carbons Liquid at room temperature (typically) More healthy Proteins Made of small carbon compounds called amino acids o Atoms contain carbon, nitrogen, oxygen, hydrogen, and sometimes sulfur. Central Carbon Proteins in the Body Involved in nearly every function of your body. structural - hair, collagen, muscle, skin etc. made of proteins enzymes – speed up chemical reactions Nucleic Acids Store and transmit genetic information. Made of smaller repeating subunits called nucleotides Composed of carbon, nitrogen, oxygen, phosphorus, and hydrogen atoms. Think – Pair – Share Let’s Try These Think – Pair - Share Try THESE! Balancing Equations The law of conservation of mass states matter cannot be created or destroyed The number and types of atoms must be the SAME on both sides of the equations Ex. ___ H2 + ___O2 ___H2O Do Now: Please complete the table! Chemical/ Symbol Carbon – C Atomic Number 6 Hydrogen – H Atomic Mass Bonds Formed 12 4 1 1 1 Nitrogen – N 7 14 3 Oxygen – O 8 16 2 Phosphorus - P 15 31 5 Sulfur - S 16 32 2 Let’s Review Carbon has _____ electrons in its outermost energy level. One carbon atom can form _____ covalent bonds with other atoms. Bonds enable carbon atoms to bond to each other = variety of important organic compounds. Do Now!! What are the four macromolecules of life? What are some examples of saturated and unsaturated fats? What is a trans fat? Objectives To explain how the body uses fats and proteins. To compare and contrast saturated vs. unsaturated fats. To discuss proteins and nucleic acids. Acids and Bases Acids- Releases hydrogen ions. Bases- Releases hydroxide ions. pH- measure of concentration of hydrogen ions in a solution.
