Mr. Carpenter s Biology Biochemistry. Name Pd

Transcription

1 Mr. Carpenter s Biology Biochemistry Name Pd

2 Chapter 2 Vocabulary Atom Element Compound Molecule Ion Cohesion Adhesion Solution Acid Base Carbohydrate Monosaccharide

3 Lipid Protein Amino acid Nucleic acid Nucleotide ATP Energy Activation energy Enzyme Substrate Active site

4 Chapter 2 Section 1 Notes What is an atom? o An atom is very! Consists of: center of the atom Protons (p + ): subatomic particles with a (+) charge. Neutrons (n o ): subatomic particles with charge. Both have about the same = 1 atomic mass unit (1 amu) outside the nucleus. Electrons (e - ): subatomic particles with a (-) charge. Electrons move in pathways called or. Mass of an electron is. Key difference between atoms of different elements is the number of and they contain. Atoms have numbers of protons and electrons, so atoms are electrically. o Opposites Attract The (+) charge of the attracts and holds the negatively charged in their orbitals. What is an element? o A chemical is a substance that cannot be broken down into any other substance. o The unit of a chemical element is a particle called the. naturally occurring elements. 20 elements have been produced in labs. elements total to date The of most elements link up with each other in different arrangements and combinations these links are called bonds. When chemicals bond they form substances called chemical. Atoms form bonds in an attempt to become more which means they seek to have a out shell.

5 Ionic Bonds o One must remember that with bonds that elements are constantly trying to make their outer shells!!! Atoms on the left side of the periodic table tend to or electrons. Atoms on the right side of the periodic table tend to or electrons o When an atom gains or loses an electron, the result is an. A ion has gained 1 or more electrons. A ion has lost 1 or more electrons. o The strong attraction between ions is called an ionic bond. Covalent Bonds o When electrons are between atoms a bond is formed. o The electrons in the covalent bond, the more strongly the 2 atoms are joined. Types: Single bond share electrons Double bond share electrons Triple bond share electrons Not easy to. A group of atoms united by covalent bonds typically acts as a single unit called a. A can contain from 2 to millions of atoms! Chemical formula Shorthand to describe a chemical compound. Indicates the that form the compound and the in which they combine.

6 Carbon The Backbone of Biological Molecules Although cells are water, the rest consists mostly of -based compounds. Carbon is unparalleled in its ability to form,, and diverse molecules.,,,, and other molecules that distinguish living matter are all composed of carbon compounds. compounds range from simple molecules to colossal ones. o Most organic compounds contain atoms in addition to atoms Carbon atoms can form diverse molecules by bonding to other atoms. o Electron is the key to an atom s characteristics. o Electron configuration determines the kinds and number of an atom will form with other atoms. The Formation of Bonds with Carbon o With four electrons, carbon can form four bonds with a variety of atoms. o This makes large, complex molecules possible. o In molecules with multiple carbons, each carbon bonded to four other atoms has a shape. o However, when two carbon atoms are joined by a bond, the molecule has a shape. o The electron configuration of carbon gives it covalent compatibility with many different. o The valences of carbon and its most frequent partners (,, and ) are the building code that governs the architecture of living molecules Molecular Diversity Arising from Carbon Skeleton Variation o Carbon chains form the of most organic molecules. o Carbon chains vary in and. o Carbon atoms can partner with atoms other than hydrogen; for example: Carbon dioxide: Urea: Hydrocarbons o Hydrocarbons are organic molecules consisting of only and. Many organic molecules, such as, have hydrocarbon components. Hydrocarbons can undergo reactions that release a large amount of. Functional groups are the parts of molecules involved in chemical reactions.

7 o Distinctive properties of organic molecules depend not only on the skeleton but also on the components attached to it. o Certain groups of are often attached to skeletons of organic molecules. groups are the components of organic molecules that are most commonly involved in chemical. The and of functional groups give each molecule its unique properties The four functional groups that are most important in the chemistry of life: Hydroxyl group - Carbonyl group - Amino group - Phosphate group - Glucose Hydroxyl Saturated Fats Carbonyl Carbonyl Unsaturated Fats ATP ATP Amino

8 Chapter 2 Section 2: Water A water molecule ( ), is made up of three atoms --- one and two. Draw water molecule: Water is Polar o In each water molecule, the atom attracts more than its "fair share" of. The oxygen end acts The hydrogen end acts Causes the water to be Hydrogen Bonds Exist Between Water Molecules o Formed between a highly oxygen atom of a polar molecule and a hydrogen atom. o One hydrogen bond is, but many hydrogen bonds are. What are the Properties of Water? o o o o o o Cohesion between particles of the substance ( why water is attracted to itself) Results in (a measure of the strength of water s surface) Produces a surface on water that allows insects to walk on the surface of water o Adhesion Attraction between two substances. Water will make bonds with other surfaces such as glass, soil, plant tissues, and cotton. -water molecules will each other along when in a thin glass tube. Example: transpiration process which and trees remove water from the soil, and paper towels up water.

9 o High Specific Heat At sea level, pure water boils at C and freezes at C. The temperature of water at higher elevations (lower atmospheric pressure). For this reason, an egg will take to boil at higher altitudes Water temperature change, both for heating and cooling. To determine, it is the amount of heat needed to raise or lower g of a substance C. Water can absorb or release large amounts of heat energy with change in actual temperature. o High Heat of Vaporization Heat of vaporization is determined by the amount of to convert 1g or a substance from a liquid to a gas. In order for water to evaporate, hydrogen bonds must be Water's heat of vaporization is cal/g. In order for water to evaporate, each gram must 540 calories (temperature doesn t change o C). As water evaporates, it removes a lot of with it (cooling effect). Water vapor forms a kind of global which helps to keep the Earth. Heat from the sun warmed surface of the earth is absorbed and held by the. o Water Density Ice is less dense as a than as a liquid ( ) Liquid water has hydrogen bonds that are constantly being and. Frozen water forms a crystal-like lattice whereby molecules are set at distances. o Homeostasis Ability to maintain a state despite changing conditions Water is important to this process because: Makes a good temperature change Universal

10 Ice protects against temperature (insulates frozen lakes) o Solutions & Suspensions Water is usually part of a. There are two types of mixtures: o Solution - compounds disperse as in water Evenly - Substance that is being dissolved - Substance into which the solute dissolves o - Substances that dissolve but separate into tiny pieces. Water keeps the pieces so they don t settle out. o Acids, Bases and ph One water molecule in 550 million naturally dissociates into a Hydrogen Ion ( ) and a Hydroxide Ion ( ) Water Equation: The ph Scale - Indicates the of ions Ranges from ph of 7 is ph 0 up to 7 is increased ph above 7 14 is increased Each ph unit represents a factor of change in concentration For Example: ph 3 is 10 x 10 x 10 ( ) stronger than a ph of 6 Acids o Strong Acids have a ph of o Produce lots of Bases o Strong Bases have a ph of o Contain lots of OH - ions and fewer Buffers o Weak or that react with strong acids or bases to prevent sharp, sudden changes in ph ( ). o Produced naturally by the body to maintain

11 Chapter 2.3: The Compounds of Life Macromolecules Monomers, meaning units, are molecules. Polymers, meaning units, are assembled by combining monomers to form molecules. Macromolecules, meaning molecules, are polymers. Carbohydrates Include and Composed of C, H, and O. Generally contain atoms for every O atom. term storage of and structural components of some cells. Monosaccharides simple sugars (one unit). - found in milk. found in fruit. found in the cells of every organism. They are - All have the formula C 6 H 12 O 6, but each has a slightly different of its atoms. Disaccharides simple sugars bonded together. table sugar milk sugar malt sugar The above are isomers of each other. Polysaccharides - many bonded together. storage form of energy for plants. storage form of energy for animals. structural component of plant cells. structural component of exoskeletons and fungi. Lipids Made from C, O and H., or compounds. Long-term of energy. Oils and fats: Composed of fatty acid chains and a glycerol backbone. Act as and. Waxes: Different backbone than oils and fats. Act as materials for plants and animals. Phospholipids Composed of fatty acid chains, a glycerol backbone and a phosphate group. Forms the structural basis of. Sterols Series of carbon rings.

12 Important role in building and carrying in the body. and steroid hormones. Proteins Polymers of amino acids ( common amino acids). Amino acids are composed of: Central carbon atom Hydrogen atom Amino group (-NH 2 ) Carboxyl group (-COOH) An R group The R group is what makes each amino acid. Amino acids join between the amino and carboxyl groups to form a. Chain of amino acids =. Principal components of, skin and. Help chemical reactions to proceed ( ). Pump small molecules of cells. Nucleic Acids carrying molecules. and Assembled from. Nucleotides consist of: group base 5-C sugar either (DNA) or (RNA). different nucleotides in both DNA and RNA. of the nucleotides determines the that the nucleic acid contains. ATP energy storage in cells Composed of

13 Chapter 2 Section 4: Energy and Enzymes Energy for Life Processes is the ability to move or change matter. Energy exists in many forms including,, energy, energy, and energy and it can be converted from one form to another. Energy can be or by chemical reactions. Energy in Chemical Reactions In chemical reactions, energy is absorbed or released when are broken and new ones are formed. is the term used to describe all of the chemical reactions that occur within an organism. Activation Energy Enzymes The energy needed to start a chemical reaction is called. Activation energy is simply a that starts a chemical reaction. Even in a chemical reaction that energy, activation energy must be supplied before the reaction can. are substances that the of chemical reactions Most enzymes are. Enzymes are, which are substances that the activation energy of a chemical reaction. An increases the speed of a chemical reaction by reducing the of the reaction. Enzyme Specificity A substance on which an enzyme acts during a chemical reaction is called. Enzymes act only on substrates.

14 An enzyme s determines its activity. Typically an enzyme is a large with one or more deep on its surface. These folds form pockets called. An enzyme acts only on a specific substrate because: Step 1: Step 2: Step 3: Factors in Enzyme Activity Any factor that changes the of an enzyme can affect the enzyme s. and can alter an enzyme s effectiveness. The that are active at any one time in a cell determine what happens in that cell.

15 Chapter 1 Section 1 1. What are the three parts of the atom? What is the charge of each part? a. Part: Charge: b. Part: Charge: c. Part: Charge: 2. How are elements represented? 3. If the element carbon (C) has 6 protons, how many electrons does it have? 4. Carbon 14 is an isotope. What does it mean to be an isotope? 5. What holds atoms together in compounds? 6. What are chemical formulas used for? 7. What is a covalent bond? 8. Circle true or false. The closer the electrons are to the nucleus the more energy they contain. 9. When does an atom become stable? 10. What happens to an atom that does not have a full outer electron shell? 11. What are poles? 12. What are polar molecules? 13. What type of bond holds water molecules together? 14. Why do ions have an electrical charge?

16 15. How does an ion become negatively charged? 16. How does an ion become positively charged? Chapter 2 Section 2 1. What percentage of the human body is water? 2. Identify how each of the following properties of water are important to organisms: a. Storage of energy: b. Cohesion: c. Adhesion: 3. Why is it important for substances within the body to dissolve in water? 4. What enables substances to dissolve in water? Chapter 2 Section 3 1. What are organic compounds? 2. What is the function of carbohydrates? 3. Where are carbohydrates found in food? 4. Explain the structure of each of the following carbohydrates and an example of each: a. Monosaccharide:

17 b. Disaccharide: c. Polysaccharide: 5. What are the functions of each of the following four types of lipids? a. Fats b. Phosopholipids c. Steroids 6. What are the seven different sources of proteins in the body? a.. b.. c.. d.. e.. f.. 7..How many different amino acids exist? 8. What are the building blocks of proteins? 9. What are the building blocks of nucleic acids? 10. What are the two types of nucleic acids? a.. b What is ATP used for? Chapter 2 Section 4 1. What are 5 different forms of energy? a.. b.. c.. d.. e.. 2. What happens when bonds are broken or formed?

18 3. Does cold water take or give energy? 4. What are catalysts? 5. What is the function of enzymes? 6. What 2 factors affect enzyme activity? a.. b..

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