BIOCHEMISTRY MR. HULSE BVHS BIOLOGY MATTER Matter - anything that occupies space and has mass Lacked clarity and flow BIOCHEMISTRY INTRODUCTION Biochemistry study of chemical and physiological process occurring within living organisms Why is this important to understand and study? Unit 2 LT 1 List the most common elements in living things and describe the relationship between elements and compounds. ORGANIZATION? Dmitri Mendeleev organized our periodic table of elements into the order and appearance we now use Based his organization on atomic mass, valence shell electrons, and key physical characteristics
ATOMS THE BASIS OF EVERYTHING Atoms smallest particle of an element the basis of all matter Subatomic Particles Nucleus Dense center of an atom Protons positively charged particle Neutrons neutrally charged particle Electrons negatively charged particle surrounding nucleus How can we describe the size of an atom? ONE AND ONLY Each atom is uniquely different from every other atom Distinguished by their number of protons Element - pure substance that cannot be broken down into other substances by chemical or physical means Atomic number number of protons in an atom's nucleus; is unique for each element ATOMIC STRUCTURE Neutrons (Ø) Protons (+) Electrons (-) THE SQUARE Atomic Number (# of protons) Atomic Symbol Atomic Name Atomic Mass (# of protons + # of neutrons)
IDENTIFY THE PARTS Atomic Number? 6 Atomic Mass? 12.011 Atomic Symbol? C Atomic Name? Carbon # of Protons? 6 Look at the atomic number # of Neutrons? 6 Atomic Mass Atomic Number =? 12.011-6 = 6.011 Can we have 6.011 neutrons? Unit 2 LT 2 Describe the structure of an atom Can and how we atoms have are 6.011 neutrons? ISOTOPES Isotope - one of several forms of an element, each containing the same number of protons in their atoms but a different number of neutrons Essentially neutrons will vary from atom to atom Carbon (C) has 15 known isotopes! The isotopes range from 8 C to 22 C Only 12 C and 13 C are stable Half-life radiocarbon dating uses 14 C Isotopes decay every 5,700 years IDENTIFY THE PARTS Atomic Number? 7 Atomic Mass? 14.007 Atomic Symbol? N Atomic Name? Nitrogen # of Protons? 7 protons Look at the atomic number # of Neutrons? 7.007 Atomic Mass Atomic Number =? 14.007-7 = 7.007 7 neutrons Unit 2 LT 2 Describe the structure of an atom Can and how we atoms have are 6.011 neutrons? RADIOCARBON DATING 14 C 12 C
RADIOCARBON DATING 14 C 12 C CHARGED ATOMS Neutrons (Ø) Protons (+) Electrons (-) BONDING HOW IS BONDING POSSIBLE? Compound - substance containing two or more elements chemically combined in a fixed ratio Covalent Bond Ionic Bond Hydrogen Bond Valence shell electrons: Each atom has shells of electrons In their most stable state these shells want to be full! Most commonly these atoms will either exchange or share electrons in order to fill their outer shells Unit 2 LT 1 List the most common elements in living things and describe the relationship between elements and compounds.
IONIC BOND Ionic Bond chemical bond that occurs when an atom transfers an electron to another atom Example: Unit 2 LT 3 Explain the difference between ionic, covalent, and hydrogen bonds. POLAR MOLECULE Polar Water Molecule Unit 2 LT 3 Explain Unit 2 LT the 3 Describe difference the between structure ionic, of a covalent, water molecule and hydrogen and bonds. h it l t t th i ti f t COVALENT BOND Covalent Bond chemical bond that forms when two atoms share electrons Example: Unit 2 LT 3 Explain the difference between ionic, covalent, and hydrogen bonds. HYDROGEN BOND Hydrogen Bond bond created by the weak attraction of a slightly positive hydrogen atom to a slightly negative portion of another molecule Example: Unit 2 LT 3 Describe the structure of a water molecule and how it relates to the unique properties of water. Unit 2 LT 3 Explain the difference between ionic, covalent, and hydrogen bonds.
EDIBLE ATOMS LAB Make sure you follow ALL directions! Please be careful with your edible pieces, you will not be given additional supplies Most importantly Have Fun! ELEMENT ELEMENTS, ISOTOPES, AND IONS ELEMENT: What is an element? pure substance that cannot be broken down into other substances by chemical or physical means COMMON ELEMENTS Carbon Hydrogen Nitrogen Oxygen Phosphorus Sulfur
TRACE ELEMENTS Definition: An element critical to health that makes up less than 0.01 percent of body mass ISOTOPE Creating a Bohr s Model Atomic # will always equal the number of protons (p+) The number of electrons (e-) in the atom, in its natural state, will always equal the number of protons (p+) The number of neutrons (N) will equal that atomic mass atomic number. N = atomic mass atomic # ELEMENTS, ISOTOPES, AND IONS ELEMENT: pure substance that cannot be broken down into other substances by chemical or physical means ISOTOPE: What is an isotope? one of several forms of an element, each containing the same number of protons in their atoms but a different number of neutrons ISOTOPE Creating a Bohr s Model # of protons = 6 # of electrons = 6 Atomic mass = 12.011 # of neutrons = 12.011 6 = 6
ISOTOPE Creating a Bohr s Model 6 p+ 6 N ISOTOPES # of protons = 19 # of electrons = 19 Atomic mass = 39.098 # of neutrons = 39.098 19 = 20 Is this an isotope? NO! ISOTOPE Natural State Element Isotopes ISOTOPES # of protons = 19 # of electrons = 19 Atomic mass = 39.098 # of neutrons = 39.098 19 = 20 Is this an isotope? NO! This is potassium s natural state as it Is found on the Periodic Table of Elements
ISOTOPES # of protons = 19 # of electrons = 19 Atomic mass = 39.098 # of neutrons = 39.098 19 = 20 But the atomic mass can sometimes be 40 40 ISOTOPES Definition: one of several forms of an element, each containing the same number of protons in their atoms but a different number of neutrons ISOTOPES 40 # of protons = 19 # of electrons = 19 Atomic mass = 39.098 # of neutrons = 39.098 19 = 20 Atomic mass can sometimes be 40 # of protons = 19 # of electrons = 19 Atomic mass = 40 # of neutrons = 40 19 =21 ELEMENTS, ISOTOPES, AND IONS ELEMENT: pure substance that cannot be broken down into other substances by chemical or physical means ISOTOPE: one of several forms of an element, each containing the same number of protons in their atoms but a different number of neutrons IONS: What is an ion? atom that has become electrically charged as a result of gaining or losing an electron
IONS Element: The number of protons is equal to the number of electrons P+ = e- Unit 2 LT 5 Explain the differences between acids and bases and how they are represented on the ph scale 2H 2 O --> H 3 O + + OH - ph scale A measure of dissolved hydroxide (OH - ) and hydrogen (H + ) ions High concentration of H + = ACID High concentration of OH - = BASE ION An ion is formed once the number of protons and electrons are not equal - Cation positively charged ion Anion negatively charged ion Unit 2 LT 5 Explain the differences between acids and bases and how they are represented on the ph scale HOW IS WATER NEUTRAL? 2H 2 O --> H 3 O + + OH - H + H 2 O OH - H 2 O OH - OH - H + H 2 O OH - = 7 H + = 7 H 2 O H + H OH - + H 2 O OH - H 2 O H + H 2 O OH - H + H + OH - H 2 O
Unit 2 LT 5 Explain the differences between acids and bases and how they are represented on the ph scale 2H 2 O --> H 3 O + + OH - Imbalance of H + and OH - ACIDS BASES Unit 2 LT 5 Explain the differences between acids and bases and how they are represented on the ph scale HOW DO WE MEASURE? Unit 2 LT 5 Explain the differences between acids and bases and how they are represented on the ph scale HOW DO WE MEASURE? Increasing H + Increasing OH - Balance of concentrations Unit 2 LT 6 Explain the role of buffers HOW CAN WE ALTER THE PH? We can always dilute the solution By adding water to the solution, we are reducing the concentration of either H + or OH - Or we can use a buffer Buffer: substance that maintains a fairly constant ph in a solution by accepting H+ ions when their levels rise and donating H+ ions when their levels fall
Unit 2 LT 6 Explain the role of buffers PH BUFFERS IN HUMANS Unit 2 LT 6 Explain the role of buffers HOLD YOUR BREATH Instructions: Hold your breath as long as possible please do not hold until you pass out!!! Just before you need to take another breath let out your held breath very slowly Unit 2 LT 6 Explain the role of buffers PH BUFFERS IN HUMANS Stomach aches and heart burn are typically caused by an elevated acidity We can fight this by adding bicarbonate Our bodies have natural bicarbonate, but not always enough Unit 2 LT 6 Explain the role of buffers WHY CAN T WE HOLD OUR BREATH LONGER?
Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water PROPERTIES OF WATER What type of bonding creates a water molecule? Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water PROPERTIES OF WATER Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water PROPERTIES OF WATER Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water PROPERTIES OF WATER (-) (+)
Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water PROPERTIES OF WATER COHESION Definition: Tendency of molecules of the same kind to stick to one another ADHESION Definition: attraction between unlike molecules Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water TEMPERATURE Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water TEMPERATURE Definition: measure of the average energy of random motion of particles in a substance What is energy? Thermal energy: total amount of energy associated with the random movement of atoms and molecules in a sample of matter SOLUTION Is this a solution? Mixture
Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water SOLUTION Solutions must be a uniform mixture of two or more substances + = Solution Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water AQUEOUS SOLUTION When water serves as the solvent we are creating an aqueous solution Definition: a solution in which water is the solvent Unit 2 LT 4 Explain the structure of a water molecule and how it relates to the unique properties of water SOLUTE VS. SOLVENT SOLVENT substance in a solution that dissolves the other substance and is present in the greater amount SOLUTE substance in a solution that is dissolved and is present in a lesser amount DENSITY Definition: Mass per unit of volume Which has more mass...
DENSITY Definition: Mass per unit of volume Which has more mass... MOLECULES OF LIFE Proteins Lipids (fats) Carbohydrates (sugars) Nucleic Acids (DNA/RNA) PROPERTIES OF WATER LAB When you are finished with the lab Edmodo Quiz due Friday! Response questions: Explain how 1. Density was demonstrated in lab. 2. Temperature was demonstrated in lab. 3. ph was demonstrated in lab. 4. Cohesion/Adhesion was demonstrated in lab 5. The phases of water were demonstrated in lab Be sure to include Unit 2 vocabulary in your responses! MOLECULES OF LIFE Proteins Lipids (fats) Carbohydrates (sugars) How?
MOLECULES OF LIFE In-organic compounds Non-carbon-based molecules Organic compounds Carbon-based molecules ORGANIC CHEMISTRY Organic chemistry- the study of all compounds that contain bonds between carbon atoms Carbon can bond w/ up to a maximum of 4 different atoms ORGANIC CHEMISTRY Organic chemistry- the study of all compounds that contain bonds between carbon atoms Carbon can bond w/ up to a maximum of 4 different atoms 1 4 2 3 ORGANIC CHEMISTRY Living organisms are made of molecules that consist of carbon and other elements. Chains of carbon can even close upon themselves to form rings. Carbon chains can have different properties by adding different atoms to them.
MONOMER VS. POLYMER Monomer Small molecular unit that is the building bloc of a larger molecule (polymer) Polymer Long chain of smaller molecular units (monomers) CARBOHYDRATES STARCH: Main energy source in plants GLYCOGEN: Main energy source in animals BIOLOGY MOLECULES Common Biological Molecules (4 of them) Monosaccharide Disaccharide Polysaccharide Glycogen: Starch: Cellulose: Saturated vs. Unsaturated Fats Cholesterol Proteins: Enzymes Amino acids Polypeptides CARBOHYDRATES Are Carbohydrates made of monomers and polymers? Single sugar molecules = monosaccharides monosaccharides = monomer These include glucose, galactose (a component of milk), and fructose (found in many fruits). Multiple sugar molecules = polysaccharides. Polysaccharides = polymers
CARBOHYDRATES Monomers? Polymers? LIPIDS What are lipids monomers and polymers? Lipid monomer = fatty acids Lipid polymer = Lipid chains LIPIDS Lipids: used for long-term energy storage Some lipids are important parts of cell membranes and waterproof coverings LIPIDS
LIPIDS PROTEINS Proteins = the machinery of cells Provide both structural and enzymatic roles PROTEINS PROTEINS Monomers and polymers of Proteins? Monomers = peptides called amino acids Polymer = polypeptide chains called Proteins Proteins also serve as enzymes Enzyme: specialized protein that catalyzes the chemical reactions of a cell
PROTEINS Proteins also serve as enzymes Enzyme: specialized protein that catalyzes the chemical reactions of a cell Catalyst? Something that speeds up a chemical reaction ENZYMES