9th Grade Science Notes - Biochemistry PDF

Unit 2: Biochemistry Ch 1. Basic Chemistry Matter: ▪ Anything that has mass and volume (takes up space) ▪ States of matter are solids, liquids, and gases ▪ Building blocks of matter: atoms Atoms ▪ Smallest particle of matter that contains specific characteristics ▪ 3 components ▪ Pr...

Unit 2: Biochemistry Ch 1. Basic Chemistry Matter: ▪ Anything that has mass and volume (takes up space) ▪ States of matter are solids, liquids, and gases ▪ Building blocks of matter: atoms Atoms ▪ Smallest particle of matter that contains specific characteristics ▪ 3 components ▪ Proton,Neutron,Electron (draw this) Categorized into ELEMENTS Elements Elements are different types of atoms. - Examples: oxygen, nitrogen, carbon These can be seen in the Periodic Table of Elements! Structure: - Protons (+ positive electrical charge) and Neutrons ( 0 neutral electrical charge)) make up the nucleus (core). - Electrons (e-negative electrical charge ) make up outside orbitals around the nucleus. - Positive nucleus keeps negative electrons in place. - Neutral atom: proton # = electron # - Ions: atoms with a charge (+ or - ) Electrons are small that their mass is negligible They’re Located in regions called energy levels First level: 2 e- Second level: 8 e- Third level: 8 e- Electrons will always stay in an inner electron shell that Isn’t full before they will sit in an outer Electron shell. Electrons like to stay inside. :) Periodic Table How to read an element Atomic Number: The number of protons in the nucleus Mass Number: The amount of matter in that element Elements: pure substance that consists of only one type of atom. Isotopes: atoms of the same element with different numbers of neutrons. - Radioactive isotopes: atoms’ nuclei are unstable and break down at a constant rate over time, giving off matter and/or energy in the form of radiation. Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 Chemical Compounds Chemical combination of two or more elements in definite proportions Examples – H20 (water) – NaCl (salt) Properties of compound differ from the properties of the individual elements Chemical bonds What holds atoms and compounds together! Forces that hold elements together in a compound - Ionic Bonds One or more e- are transferred from one atom to another Ex: Salt, NaCl  - Covalent Bonds One or more e- are shared between atoms in a compound - Smallest particle of a covalent compound is a MOLECULE (neutral) Ex: water, H2O - Atoms that form chemical bonds are called Chemical Compounds - They are written by using a chemical formula: Ex: Water is made of two hydrogen (H) and one oxygen (O): H2O Carbon Carbon is unique because: - Carbon can form 4 covalent bonds, even with 4 different atoms! - Carbon can share TWO pairs of electrons and form double bonds! - Carbon can form long chains and rings to make different compounds with versatile functions! - Covalent Bond carbon Examples: Other types of bonds: 1. Van der waals forces - Intermolecular forces of attraction between molecules 2. Hydrogen Bonds: - Attraction between two atoms that already participate in other chemical bonds. Unbalanced: Fe + O2 -> Fe2O3 Balanced: 4Fe + 3O2 -> 2Fe2O3 **Atoms cannot be created or destroyed. So when a compound is made during a chemical reaction, the atoms are rearranged in a different way, keeping the same numbers of atoms.** Ch. 2 Properties of Water - H20 is the molecular format of water - Water is POLAR which means different ends of the molecule are oppositely charged. - Because it is polar it forms weak attractions with itself. These attractions are known as hydrogen bonds! - Individually hydrogen bonds are weak but collectively they are strong Because of water’s polarity, it has the following properties that make it a very good substance for living things to be made of or live in. These Properties are: Cohesion: Attraction between like molecules (water sticks to itself)  Adhesion: Attraction between unlike molecules (water stickers to other substances) - Capillary action in plants helps pull water up from the soil. Water sticks to itself and the sides of the vessels of the tree. Surface tension – This force on the top of water is like a “skin” at the water and the air interface. Water can hold a lot of heat: It holds a lot of heat before increasing in temperature (HIGH HEAT CAPACITY) - It’s good at cooling us off because it takes a lot of heat when it evaporates. Water is less dense as a solid: ICE FLOATS - Living things can live under the ice and be insulated from the cold air temperature outside the body of water. Water is good at dissolving other substances: dissolved substances are pulled apart in liquid by other substances. - Mixture is a substance that is formed when two or more substances combine. Suspension: When one substance is NOT dissolved in another - Ex blood cells in plasma. Solution: When substances are evenly dissolved in another. - Solvent dissolves the other substance - Solute gets dissolved Dissociation of Water Some water molecules that are not forming hydrogen bonds are getting pulled apart. This is called disassociating. H20 -> H+ + OH- Hydrogen ion Hydroxide ion Adding more substances changes this equal balance of H+ and OH- A substance that increases H+ to a solution is called an acid A substance that increases OH- is a base. PH SCALE Acid Base Stronger Neutral Stronger Ch. 3 Organic compounds We’re mostly made of water (water is inorganic) An inorganic compound does not contain carbon. Ex, Salt,H20 Only living things can have carbon compounds (naturally) Our bodies are also made of organic compounds. Organic compounds contain both carbon and hydrogen ex glucose, protein. Carbon is a versatile atom for compounds to be made from 4 bonds rings,chains,single,double bonds. Carbon is missing 4e There are 4 groups of organic compounds: 1) Proteins 2) Lipids (fats) 3) Carbohydrates 4) Nucleic Acids (DNA) Each group has a monomer which is a small building block or subunit monomers are put together to build the polymer of the group. Cells link monomers to form polymers from dehydration synthesis. Polymers broken down to monomers by the reverse process hydrosis Your body is constantly building and breaking down these compounds for digestion and growth. 1. Carbohydrates - Foods with carbs: fruits,vegetables,pasta,cereal,potatoes,rice - Function: energy storage and structure - The monomers for carbs are monosaccharides. - Characteristics: Contain, Carbon,Hydrogen, and oxygen Always have a 2:1 ratio of hydrogen to oxygen. - Monomer: simple sugar called monosaccharide - Ex: glucose C6H12O6 - Isomers are other monosaccharides that have the same formula as glucose but their structures are different. Formula: C6H12O6  - Their different structures give them different functions - Glucose + Glucose = Maltose (malt sugar) - Glucose + Galactose = Lactose - Glucose + Fructose = Sucralose Polymer: complex carbohydrates called polysaccharides. Ex: starches in plants and glycogen in animals are used for energy storage. Cellulose in plants for structure. A disaccharide is made from two monosaccharides bonded together. Lipids Foods with lipids: Salmon,Butter,cheese,red meats,chocolate, ice cream, nuts,olive oil. Function: Energy storage(2x carbs),Cell membrane structure, chemical messengers (hormones). Made of Carbon,Hydrogen, and oxygen. Oils: Liquid at room temp. Fats: Solid at room temp. Monomer: Glycerol and three fatty acids Saturated fats aren’t as healthy. Trans Fats are artificial fats made from unsaturated fats that are very bad for the heart. Unsaturated Fats are Oils Saturated fats are dairy, meat Lipids with single bonds are saturated Lipids with double bonds are unsaturated; they also lack two hydrogen for every double bond. Polymer: Sterols: cholesterol that make up your hormones Phospholipids: Part of the cell membrane Proteins Contain: Carbon,Hydrogen,Oxygen and Nitrogen. Functions:Movement (muscles), help chemical reactions (enzymes - catalysts), immunity (antibodies), messengers (hormones), transporters (in blood) THEY CANT STORE ENERGY Foods with proteins: Meat, eggs,cheese, fish,yogurt. There are 20 amino acids. 11 are non essential which you already have and 9 that are essential you need from food. Meat and Soy are complete proteins with all 9. Monomers: Amino acids The R changes between the 20 Polymer: peptide chain is an arraignment of the 20 amino acids in different orders Building a peptide polymer: ^^^ The sequence of amino acids in the chain will determine the protein's shape and function. Nucleic acids Made of Carbon, Hydrogen,Oxygen,Nitrogen,Phosphorus Monomer: nucleotides Polymer: DNA,RNA Function:Storage of genetic information. Ch. 4 Enzymes Chemical reactions occur all the time in living things. They may be spontaneous (give off energy) but many reactions in your body don’t occur very quickly.  Enzymes are a type of catalyst which is a substance that speeds up the rate of a chemical reaction. - Enzymes lower the energy needed to start a chemical reaction. And therefore speed up the reaction rate. - Enzymes are made of proteins Many chemical reactions require energy to occur Enzymes don’t give energy but lowers the energy requirements. The enzyme can be reused if it keeps it shape (doesn’t become part of the product) Enzymes have a specific shape that matches the shape of the chemical substrate to help move the reaction along. The substrate is the reactant that an enzyme acts upon. Certain factors can affect enzyme activity 1. Temperature change Low temp = slower reaction High temp = faster reaction Until and optimal temp is reached, and then a temp increase will slow and eventually stop the reaction before the shape of the enzyme is denatured (permanently deformed) 2. Ph change (acids or bases) :many enzymes have an optimal PH pepsin - stomach trypsin- small intestine Raising the temperature too high can deteriorate the enzyme so the substrate doesn’t fit anymore.