Chapter 6
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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. Brain-Based Learning Name __________________ Proton Neutron Electron 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 Neutrons: no charge, contain mass of 1 - Electrons: Outside nucleus, negatively charged, insignificant mass Do Now!! Complete the chart: Part of Atom Proton Neutron Electron Charge Mass Objectives 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. To draw different atoms 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. So… if this is an atom… What makes atoms different? How is carbon different from oxygen? Different numbers of protons 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 (and electrons) Symbol- unique for each element. Atomic Mass- # of protons and neutrons 6 C 12.02 Lets practice!! 4 9.01 C 12.02 7 N Ne 20.18 Complete the missing information and include the number of protons, neutrons, and electrons. Objectives To practice drawing different atoms. To review parts of the atom by completing a worksheet activity. Neutron Partners… List the number of protons, neutrons, and electrons for the following… Mg Ca Fe Cl 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 Etc. Lets Draw Oxygen! What is the atomic number of oxygen? Let’s Practice… Please work on the worksheet in front of you! Finish for homework and bring to the next class. Let’s draw: 1. He 2. O 3. S 4. C 5. Cl 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 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 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 What is an isotope again? 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 to be neutral: Lose: form positive ions Gain: form negative ions Na Cl Do Now!! How many electrons does each of the following want to be “happy”? Oxygen Carbon Hydrogen Nitrogen 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. Lets Practice! List the number of protons, neutrons and electrons in each ion: ONa+ N3ClF+ Are any of these atoms happy? More practice… 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. Compounds A pure substance formed when 2 or more elements combine. Always formed using a specific ratio Ex: 2 molecules of Hydrogen + 1 molecule of Oxygen will give us water (H2O) 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 Let’s try some examples (electron partners) 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. Review! How many protons, neutrons, and electrons are in O2-? Is Cl a compound or an element? How do you find the # of neutrons? Using the formula 3C6H12O6, how many atoms of oxygen are present? 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 Molecule: compound held together by covalent bonds. 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) H2O Do Now!! What are the 2 main types of bonds? What happens with electrons in each type of bond? What is a compound? Objectives Define “Van Der Waals” Interactions. Explain what a chemical reaction is. Identify reactants and products in a reaction. Balance an equation. 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 When molecules come close together, the attractive forces between slightly positive and negative regions pull on the molecules and hold them together. The strength of the attraction depends on the size of the molecule, its shape, and its ability to attract electrons. 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 Do Now!! Glucose and oxygen react to form carbon dioxide and water. Identify: Products Reactants Is this a balanced equation? + ATP (energy) Do Now!! Identify: Products Reactants Is this a balanced equation? H2 + O2 H2O 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. 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 Electron Partners!! Balance the following equations: 1. ___ H2 + ___ O2 ---> ___ H2O 2. ___ Zn + ___ HCl ---> ___ ZnCl2 + ___ H2 3. ___ SiO2 + ___ HF ---> ___ SiF4 + ___ H2O 4. ___ K + ___ Br2 ---> ___ KBr 5. ___ Al + ___ FeO ---> ___ Al2O3 + ___ Fe 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. Energy in Reactions The activation energy minimum amount of energy needed for reactants to turn into products Types of Reactions Exothermic- released heat energy. o The energy of the product is lower than the energy of the reactants. Types of Reactions Endothermic - absorbed heat energy. The energy of the products is higher than the energy of the reactants. Demo time!! Endothermic or Exothermic?? Let’s do some practice! Get with your neutron partners!! 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. Mixing water with Epsom salt 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 enzymes! -Specialized proteins that act as “catalyst” (speeds up a reaction) - Usually end in “ase” -Not consumed in the reaction What do they do? How do they work? A substrate fits in the active site of an enzyme. This forms an enzyme substrate complex. They then break or form bonds. 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 Do Now!! Determine whether the following substances are heterogeneous or homogenous: Chicken noodle soup Lemonade Pudding Fruit Salad Cole Slaw Milk Chipotle Burritos Objectives Review acids and bases. 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. 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 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 Homogeneous Heterogeneous What is the difference? Mixtures Homogeneous- has a uniform composition throughout (a.k.a solutions). Heterogeneous- components remain distinct. Acids and Bases Acids- Releases hydrogen ions. Bases- Releases hydroxide ions. pH- measure of concentration of hydrogen ions in a solution. 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. (We want to keep our body fluids at a pH of 6.5-7.5) Hemoglobin 6.4 Macromolecules of Life Organic Chemistry - The element carbon is a component of almost all biological molecules. (Inorganic= no carbon) 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: 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 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. Run our labs! Molecules Macromolecules - large molecules formed by joining smaller organic molecules together. Are also called Polymers - molecules made from repeating units of identical (or nearly identical) compounds linked together by covalent bonds. 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. Carbohydrates Sources of energy (ex: glucose) Ratio of carbon : hydrogen : oxygen of 1:2:1 (CH2O)n n = # of CH2O in a chain *Where there’s a corner there’s a carbon!* Glucose Do Now!! - What are carbohydrates composed of? - Identify the carbohydrates: 1) C6H12O6 2) CH3 3) C4H2O2 4) C24H36O24 Objectives To explain how the body uses fats and proteins. To compare and contrast saturated vs. unsaturated fats. To discuss proteins and nucleic acids. Carbohydrates 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) Disaccharide Monosaccharide (glucose) Polysaccharide 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. Lipids Fats, oils and waxes Made mostly of C and H Used for energy storage and insulation Fat – solid at room temperature Oil – Liquid at room temperature 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 Central Carbon Atoms that make up Amino Acids: carbon, nitrogen, oxygen, hydrogen, and sometimes sulfur. Amino acids are connected together through a PEPTIDE BOND. 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. 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