33 Biology Chapter 2: The Chemistry of Life title 4 pictures, with color (black and white don t count!)
34 Chapter 2: The Chemistry of Life Goals Highlight all unknown words
35-36 Chapter 2: The Chemistry of Life Vocabulary Mark each vocabulary word using the following key + I know this word I ve heard this word, but not sure what it means I ve never heard this word, have no idea what it means
37 2-1 The Nature of Matter (pt 1) What are the basic units of matter? Set up pg 1 for section 2-1 Notes Title Essential Question (top right) Name Date (top left) Page number (bottom corner)
37 2-1 The Nature of Matter (pt 1) At the top of your notes for today, write the following words: Atom Element Molecule
37 2-1 The Nature of Matter (pt 1) Atoms the basic unit of matter; made up of particles Nucleus Protons (positive) Neutrons (neutral) Orbiting Nucleus Electrons (negative)
37 2-1 The Nature of Matter (pt 1) Atoms are neutral Number of protons is equal to the number of electrons
37 2-1 The Nature of Matter (pt 1) Electrons are found in different orbitals (levels) 1 st holds 2 electrons 2 nd holds 8 electrons 3 rd holds 8 electrons
37 2-1 The Nature of Matter (pt 1) Element a pure substance; it contains only one type of atom Elements found in living things: Carbon, Hydrogen, Nitrogen, Sodium, Oxygen, Potassium, Calcium, Iron
Divide page one into 3 parts Top 1/3 Middle 1/3 Bottom 1/3
Draw on top 1/3 of page 1 Element name Carbon Atomic Number 6 Symbol C Atomic Mass 12.001
Write on middle 1/3 Atomic number = number of protons (+) Neutral atom positive = negative Protons = electrons Atomic mass = # protons + # neutrons Rewrite formula because solve for neutrons # neutrons = Atomic mass - # protons
Draw on bottom 1/3 of page 1 Neutrons and Protons are in the middle Electrons are on the outside shell
# protons = atomic # # protons = # electrons = # protons #electrons = # neutrons = Atomic mass # protons 12-6 =
Draw Carbon # protons = 6 # electrons = 6 # neutrons = 6
Divide page 2 into 4 squares
36 2-1 The Nature of Matter (pt 1) On the bottom half of pg 36, sketch a diagram the following atoms: Hydrogen Sodium Oxygen Nitrogen Carbon Neon Be sure to label the nucleus, protons, neutrons, and electrons (do each part in a different color). Also, label each atom with it s name. Use the Periodic Table at the back of your book to help you figure out how many of each particle to draw Atomic # = # of Protons Atomic Weight Atomic # = # of Neutrons # of Protons = # of Electrons
39 2-1 The Nature of Matter (pt 2) How / Why do atoms join to form molecules?
39 2-1 The Nature of Matter (pt 2) Chemical Compounds a different substance made from the chemical combination of 2 or more elements Held together by Chemical Bonds
2-1 The Nature of Matter (pt 2) Examples Water H 2 O Carbon Dioxide CO 2 Salt NaCl Sugar C 6 H 12 O 6 Hydrogen Gas Oxygen Gas Carbon Solid Sodium Solid, Metal Chlorine Gas Methane CH 4 Hydrogen Peroxide H 2 O 2
39 2-1 The Nature of Matter (pt 2) Types of Chemical Bonds The goal of every atom is to have a full outer electron orbital Only elements in the far right column of the periodic table have this naturally (this group is called Noble Gases)
39 2-1 The Nature of Matter (pt 2) Ionic Bonds electrons are transferred Sodium Atom To gain full outer levels, atoms can lose or gain electrons An atom that has lost or gained electrons is called an ion + Sodium Ion
39 2-1 The Nature of Matter (pt 2) Ionic Bonds Lose an electron positive ion Gain an electron negative ion Positive and Negative ions are attracted to each other +
2-1 The Nature of Matter (pt 2) Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na + ) Chloride ion (Cl - ) Protons +11 Electrons -11 Charge 0 Transfer of electron Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1
39 2-1 The Nature of Matter (pt 2) Covalent Bonds electrons are shared Pairs of electrons are shared between 2 atoms. They orbit the nucleus of both! Example: Water each H atom shares a single electron with the O atom Water Molecule
2-1 The Nature of Matter (pt 2) Some other covalent bonds 2 Hydrogen atoms, each has 1 electron Methane (CH 4 ) Carbon has 4 electrons to share and it bonds with 4 hydrogen atoms that each have 1 electron to share
38 2-1 The Nature of Matter (pt 2) Chemical Bonds Compare & Contrast Front of Flap: Type of Bond (already done for you) Picture to remind you of the type can t involve pictures of atoms and electrons no picture is necessary for Both Under Flap Technical info regarding each type of bond Ways the two types are similar and different
43 2-2 Properties of Water What is special about a water molecule?
43 2-2 Properties of Water Water is ESSENTIAL to life on earth ¾ of the surface of the planet is water A Blue Planet The single most abundant compound in living things
43 2-2 Properties of Water The net charge of a water molecule is neutral (10 positive protons = 10 negative electrons) But, the O atom has a stronger attraction for the electrons. Electrons are more often on the O end than the H ends O end has a slight negative charge and the H ends have a slight positive charge
43 2-2 Properties of Water A water molecule is a POLAR MOLECULE because there is an uneven distribution of electrons between the oxygen and hydrogen atoms
43 2-2 Properties of Water A water molecule is a POLAR MOLECULE because there is an uneven distribution of electrons between the oxygen and hydrogen atoms
43 2-2 Properties of Water Because water is polar, the opposing ends are attracted to each other in Hydrogen Bonds Water molecules stick to other water molecules This results in: Cohesion, Adhesion, Capillary Action
2-2 Properties of Water Cohesion Adhesion
43 2-2 Properties of Water Cohesion attraction between water molecules (spheres of water) Adhesion attraction between water molecules and different substances (Sheets of water) Capillary Action water will move upwards, against gravity, through small tubes
45 2-3 Carbon Compounds What is the chemical difference between living and non-living?
2-3 Carbon Compounds Go back to pg 36 and review the sketch of the carbon atom you drew. 6 C 12.011
2-3 Carbon Compounds What type of bond do you think carbon will form (covalent or ionic)? Protons: 6 Neutrons: 6 Electrons: 6
35-36 2-3 Carbon Compounds 2-3 Vocabulary Polymer (made out of Monomers) Carbohydrate (made out of simple sugars) Lipid (made out of fatty acids and glycerol) Nucleic Acid (made out of Nucleotides) Protein (made out of Amino Acids)
45 2-3 Carbon Compounds The Chemistry of Carbon Carbon is present in all living things Carbon can make some large, complex molecules (like long chains or rings) Organic Chemistry study of compounds containing carbon Methane Acetylene Butadiene Benzene Isooctane
45 2-3 Carbon Compounds Macromolecules Large Organic Molecules found in living things Also called Organic or Carbon Compounds, or Polymers Atoms make small molecules (MONOMERS) Small molecules make Macromolecules (POLYMERS)
45 2-3 Carbon Compounds Macromolecules MONOMERS POLYMER
45 2-3 Carbon Compounds Macromolecules 4 Types of Macromolecules Carbohydrates Lipids Proteins Nucleic Acids
44 2-3 Carbon Compounds Organic Macro-Molecules Flip Chart, pg 44 Front of Flap: Name of Macromolecule and a picture to remind you what it is Back of Flap: Monomer Under Flap: What the macromolecule does
Red goes on the left side. Blue goes on the right side Black goes on the front slip.
45 2-3 Carbon Compounds Carbohydrates MAJOR SOURCE OF ENERGY Structural support for plants Monomer: simple starches or simple sugars Examples: Sugars: glucose, fructose, lactose, sucrose Starches: glycogen, cellulose
45 2-3 Carbon Compounds Starch Glucose
45 2-3 Carbon Compounds Lipids Used to store energy and important in the function/composition of cell membranes Chemical messengers Monomers - Glycerol & Fatty Acids Examples: Fats, Oils, Waxes, Steroids, Cholesterol
45 2-3 Carbon Compounds
45 2-3 Carbon Compounds Nucleic Acids Store and transmit genetic (hereditary) information Monomer: nucleotides Examples: DNA (deoxyribonucleic acid) RNA (ribonucleic acid)
45 2-3 Carbon Compounds Protein Controls rates of chemical reactions in cells Some form bones and muscles Some transport substances through cells Some help the immune system Monomer: Amino Acids Examples: Enzymes, Hemoglobin, Hair, Muscle, Exoskeletons
45 2-3 Carbon Compounds Amino group Carboxyl group General structure Alanine Serine
45 2-3 Carbon Compounds Amino acids
47 2-4 Chemical Reactions & Enzymes How / Why do chemical reactions take place in living things? 2-4 Vocabulary, pg 36
2-4 Chemical Reactions & Enzymes CH 3 COOH + NaHCO 3 CO 2 + H 2 O + CH 3 COONa
47 2-4 Chemical Reactions & Enzymes C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O
47 2-4 Chemical Reactions & Enzymes Chemical Reactions Changes in the chemical bonds that join atoms in compounds Results in different compounds Reactants Products H 2 O 2 H 2 O + O 2 C 6 H 12 O 6 + O 2 CO 2 + H 2 O
47 2-4 Chemical Reactions & Enzymes When chemical bonds are broken, energy is released Living things must have a source of energy to make these reactions occur
47 2-4 Chemical Reactions & Enzymes Activation Energy the amount of energy required to get a reaction started Energy-Releasing Reaction Activation energy Reactants Products
47 2-4 Chemical Reactions & Enzymes Living things have LOTS of chemical reactions, but they often occur too slowly Catalyst any substance that speeds up chemical reactions Reaction pathway without enzyme Reactants Reaction pathway with enzyme Activation energy without enzyme Activation energy with enzyme Products
47 2-4 Chemical Reactions & Enzymes Enzyme A special type of protein that acts as a biological catalyst Reaction pathway without enzyme Reactants Reaction pathway with enzyme Activation energy without enzyme Activation energy with enzyme Products
2-4 Chemical Reactions & Enzymes Enzyme Example #1: H 2 O 2 H 2 O + O 2 Cells produce hydrogen peroxide (H 2 O 2 ) as a waste product, it s poisonous to cells An enzyme quickly converts it into water and oxygen two harmless substances If allowed to react at normal speed, H 2 O 2 would build up in cells An enzyme makes the reaction happen faster
2-4 Chemical Reactions & Enzymes Enzyme Example #2: CO 2 + H 2 O H 2 CO 3 CO 2 in cells reacts with H 2 O in blood to form Carbonic Acid (H 2 CO 3 ) Blood carries acid to lungs Then the acid turns back into CO 2 and H 2 O CO 2 gas is exhaled If allowed to react at normal speed, CO 2 would build up in cells too fast An enzyme makes the reaction 10 million times faster
46 2-4 Chemical Reactions & Enzymes Read about Enzymes on pg 51-52 Affix Enzyme Action to pg 46 Identify the Reactants, Products, Enzyme, and Active Site Describe what is happening during each step of the flow chart
46 2-4 Chemical Reactions & Enzyme Demonstration Enzymes Enzymes provide a place for the reaction to happen, they are unaffected by the reaction 1. Reactants bind to the enzyme 2. Reaction takes place on the enzyme 3. Products are released from the enzyme The enzyme remains unchanged and able to catalyze another reaction!
46 After, the enzyme is left unchanged Enzyme Products Reactants / Substrate Products are released Active Site Reactants are converted into products Reactants bind to the enzymes Active Site
47 2-4 Chemical Reactions & Enzymes Enzymes Enzymes are Reaction Specific An enzyme only works on 1 type of reaction Enzymes are reusable Enzymes work best at certain temperatures (high temps are BAD!) Cells can turn enzymes on and off
47 2-4 Chemical Reactions & Substrates Enzymes Product Active Site Enzyme
46 Enzyme Demonstration 1. What happens when liver is combined with hydrogen peroxide? 2. What gas is released? What liquid remains in the test tube? 3. What happens when more peroxide is added to the liver? Why? 4. What happens when more liver is added to the liquid? Why? 5. How does temperature affect the activity level of enzymes? 6. Many mammals have body temps close to 37 C. What problems do you think mammals might have if there body temps were lower or higher than 37 C?
Read your notes, start to finish Get with a partner (groups of 2 or 3) and go over your notes together. Check for missing things Circle important stuff Put a? next to things you don t understand Schedule time to study between now and the test.