1. Chapter 2: Basic Chemistry and Applications I Concepts of matter and energy A. Matter: Anything that occupies space 1. There are three states of matter, all of which are present in your body: a. Solid: tissues, cells, organs a. Solid: tissues, cells, organs b. Liquid: blood plasma and interstitial fluid (surrounds all cells) b. Liquid: blood plasma and interstitial fluid (surrounds all cells) c. Gas: Air you breath, gases produced in large intestine c. Gas: Air you breath, gases produced in large intestine B. Energy: Ability to do work or put matter into motion 1. Two forms: a. Kinetic: energy is actually doing work (moving matter, using muscles to lift and object) a. Kinetic: energy is actually doing work (moving matter, using muscles to lift and object) b. Potential: Stored or inactive energy (like in an ATP bond) b. Potential: Stored or inactive energy (like in an ATP bond)

2. Chapter 2: Basic Chemistry and Applications I 2. Types of energy: a. Chemical energy: Stored in bonds, such as in high energy foods (complex carbohydrates); energy is released when bond is broken. b. Electrical energy: Movement of charged particles, such as the sodium/potassium pump used for nerve impulses. c.Mechanical energy: Directly moves matter, such as muscles moving a load. d.Radiant energy: Traveling in waves, such as the light energy that stimulates the retina in the back of your eye.

3. Chapter 2: Basic Chemistry and Applications 3. First law of thermodynamics: Energy can be neither created nor destroyed, it only changes form. a.Example from your body: ATP bond is broken to release energy → which powers the muscle to contract → some of the energy is lost has heat (unusable) → you sweat (giving off excess heat) as you exercise.

4. Chapter 2: Basic Chemistry and Applications IIComposition of matter and therefore YOU! A. All matter is made up of elements that cannot be broken down into smaller particles by ordinary means. B. The building block of an element is the atom Composition of the atom:

5. Chapter 2: Basic Chemistry and Applications C. Two or more atoms combined chemically are called a molecule. If the atoms are of different elements, the term is a compound. 1. Types of bonds that create molecules and compounds (filling that outer shell) a. Ionic: Electrons are transferred from one atom to another atom; this creates ions (charged atom) which are then attracted to each other. Compounds usually form salts. b. Covalent: Electrons are shared between the atoms. 1. Equally shared electrons orbiting compound = Nonpolar molecule (ex. methane, Carbon dioxide)

6. Chapter 2: Basic Chemistry and Applications 2. Unequally shared electrons orbiting compound = Polar molecule (ex. water) 3. Hydrogen bond: Weak bond between hydrogen (covalently bonded to large atom) and another large electron hungry atom of another molecule. Common between water molecules. Also can help stabilize large molecules (such as proteins).

7. Chapter 2: Basic Chemistry and Applications D. Patterns of chemical reactions (making and breaking bonds) 1. Synthesis Reactions: Combining smaller molecules to make larger more complex molecules. Ex. building proteins 2. Decomposition Reactions: Breaking down larger molecules into smaller components. Ex. digestion of food or breaking down toxins/drugs In the cartoon, the skinny bird (reactant) and the worm (reactant) combine to make one product, a fat bird. A + B ----> AB Synthesis Reaction AB ----> A + B Decomposition Rection

8. Chapter 2: Basic Chemistry and Applications III. Inorganic Compound A. Special Properties of water: Why your 8 glasses a day are Necessary Necessary 1. High heat capacity: Water can absorb and release large amounts of heat without having a drastic effect on the amounts of heat without having a drastic effect on the temperature of the water. temperature of the water. Ex. You can play sports on a hot day and your body temperature remains relatively constant by heat temperature remains relatively constant by heat loss through your sweat. loss through your sweat. 2. Polar Molecule → Solvent Properties (dissolves salts, ions, nutrients, gases, acids and bases) nutrients, gases, acids and bases) a. Important for chemical reactions to occur in the body, rxn. will not occur unless chemicals are dissolved (in water); also important for transport (blood plasma) b. Important for movement/lubrication/decrease friction

9. Chapter 2: Basic Chemistry and Applications 3. Chemical Reactivity: Important reactant in metabolic processes such as digestion. 4. Cushioning: Important with CSF (cerebral-spinal fluid) for cushioning brain and with amniotic fluid to protect fetus. B. Salts & Acids and Bases: Electrolytes (dissociate and ionize in water) a. Salts: Compounds formed from ionic bonding. Important for metabolic processes such as sodium/potassium pump for conducting nerve impulses; transport of oxygen by hemoglobin in red blood cells. Sodium/ Potassium Pump Sodium/ Potassium Pump b. Acid (proton donor) and Base (proton acceptor) Acid- substance that releases H+ ions (1-6.9 pH scale) Base- substance that release OH- ions (7.1-14)

10. Chapter 2: Basic Chemistry and Applications i. Balance in the body is important for proper functioning. pH differs in different places in the body. Ex. blood 7.4 (neutral) to pH 2 (gastric juices) ii. Buffers are present in the body to help maintain the proper pH level. Buffers are weak acids and bases.

11. Chapter 2: Basic Chemistry and Applications IVOrganic Compounds A. Carbohydrates 1. Contain carbon, hydrogen and oxygen in a 1:2:1 ratio 2. Classified based on size: a. Monosaccharides: 1 sugar (smallest unit); ex. Glucose (blood sugar), fructose, galactose, ribose, deoxyribose b. Disaccharides: double sugars; ex. sucrose (cane sugar), lactose (found in dairy), and maltose (malt sugar) c. Polysaccharides: many sugars (larges); insoluble (used for storage) and lack sweetness. Ex.Glycogen 3. Main function: cellular energy (glucose is oxidized and energy released is stored in ATP. If not used immediately, energy released is stored in ATP. If not used immediately, will be stored as glycogen or fat. will be stored as glycogen or fat. 4. Secondary function: Structural components of cells (1% to 2% of cells), surface proteins on membrane, component of 2% of cells), surface proteins on membrane, component of DNA and RNA. DNA and RNA.

12. Chapter 2: Basic Chemistry and Applications IVOrganic Compounds B. Lipids 1. Contain: carbon, hydrogen, and oxygen (no set ratio) 2. Are non-polar compounds so they do not dissolve in water 3. 3 categories of lipids: a. Neutral Fats: triglycerides i. solid- saturated fats - animal fat ii. liquid – unsaturated – plant oils iii. Bodies most abundant source of usable energy as well as shock absorber and insulation. b. Phospholipid: Similar to triglycerides with a phosphorous containing group. Molecule has a charged region for interacting with water and ions and a fatty acid end (hydrophobic). Very important for selective permeability of plasma membrane.

13. Chapter 2: Basic Chemistry and Applications IVOrganic Compounds c. Steroids: Have a ring structure and are fat soluble. Ex. c. Steroids: Have a ring structure and are fat soluble. Ex. cholesterol found in cell membranes, used to form cholesterol found in cell membranes, used to form vitamin D and some hormones. vitamin D and some hormones. C. Proteins A. Accounts for 50% of your organic matter, made from amino acids. Composed of carbon, hydrogen, oxygen, nitrogen and sulfur. B. Function and structure of a protein is linked to the sequence of amino acids (controlled by genes). If the order of amino acids changes the structure and function of that protein will be altered. Ex. like our language, floor → flour

14. Chapter 2: Basic Chemistry and Applications IVOrganic Compounds c. Two structural types: i. Fibrous (structural) proteins. Important for binding structures and providing strength in body tissues. Ex. collagen (tendons, cartilage and skin) and actin and myosin (make up muscles) ii. Globular (mobile/functional) proteins. Involved in most body processes. Ex. antibodies (fight disease), hormones (long term regulation), transport proteins (hemoglobin) and enzymes (catalyze chemical reactions). ii. Globular (mobile/functional) proteins. Involved in most body processes. Ex. antibodies (fight disease), hormones (long term regulation), transport proteins (hemoglobin) and enzymes (catalyze chemical reactions). D. Destruction of proteins/Denaturing Proteins D. Destruction of proteins/Denaturing Proteins i. Fibrous proteins are very stable (not many hydrogen bonds holding together an intricate structure). Globular proteins have many hydrogen bonds and are very fragile ii. Factors that denature (break hydrogen bonds) proteins alter the active site that reacts with the substrate. Factors include increased temperature, pH and/or salinity. Ex. why a high fever is not healthy.

15. Chapter 2: Basic Chemistry and Applications D. Nucleic Acids a. Composed of nucleotides (phosphate group, sugar and nitrogen base). b. Two types: i. DNA (deoxyribonucleic acid)-compose your genes which are responsible for the basic organism blueprint as well as growth and development. All done by dictating protein structure!! ii. RNA (ribonucleic acid)-carries out the orders of DNA genes helping with transcription and translation of gene information into proteins.

16. Chapter 2: Basic Chemistry and Applications E. One more important molecule – ATP (adenosine triphosphate) Molecule that stores chemical energy used by all your body cells. Energy is stored in the high energy third phosphate bond.