Bio 141 Notes

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Molecule

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2 or more atoms that are held together by a chemical bond

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Compounds

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2 or more different atoms held together by a chemical bond * All compounds can be molecules but not all molecules can be compounds*

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Mixtures of how matter is combined

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mixtures consist of 2 or more intermixed substances, natural or synethic

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1. Characteristics of Mixtures
a. Homogenous mixtures/compounds

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a. same content no matter where in the mixture the sample is taken from

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b. Heterogenous mixtures/compounds

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b. consists of two different content or makeup depending on where the sample is taken from

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2. Solutions

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are homogenous mixtures, can be solid, liquid or gas

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a. solvent

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dissolving agent for the solution, constitutes greatest volume ex. water

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b. solute

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substance that is dissolved in the solvent

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- molarity (M)/Moles per liter

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based on molecular weight, weigh out sample in grams and add water to get liter

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- avogadros number

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equals 6.02 x 10'23 solute particles, one molar solution

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3. colloids aka emulsion

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heterogenous mixtures can be transulcent to a milky color and reflect light

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a. solutes are

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very large, tend to stay suspended

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b. have ability of sol-gel transformation

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ability to change from solid to liquid and back again ex. jello, cell cytoplasm, blood plasma

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4. Suspensions (heterogenous)
a. has large solute particles

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that do settle out or parcipitate to bottom ex. blood cells in solution

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C. Distinguishing Mixtures from Compounds
*mixtures are not connected by chemical bonds but compounds are*

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a. mixtures can be easily separated, evaported, or filtrated; compounds you have to break chemical bonds to separate
b. compounds are homogenous only, mixtures can be both

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IV. Chemical Bonds

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equals the electron energy found b/w 2 atoms

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1. electron shells

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regions of space that conseculatively the nucleus of the atom; they give us energy levels

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2. energy levels

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varies on which shell the electron occupies and its distance from the nucleus; the further away the greater the potential energy the more interactive the electron will be the higher the energy level

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3. filling of electron shells

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shell one holds max of 2 electrons, shell 2=8 shell 3=18 increases exponentials

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a. they are considered full with

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8 electrons with exception shell one which is full with 2

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b. valence

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outer most shell that has an electron, highest energy level

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c. rules of eight aka octet rule

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shell that will have the reactive electron; atoms will interact in order to achieve a shell that is full

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4. chemically inert elements

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have outer shell hat already has 8 electrons, full valence shell, non reactive atoms ex. noble gases

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5. chemically active elements

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valence shell that is not full, they can gain, lose, or share electrons

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B. Three Types of Chemical Bonds

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ionic, covalent, hydrogen

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1. Ionic bonds

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are formed by electron transfer b/w atoms, positive and neg attract

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a. Ions

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atoms that have a charge that can be pos or neg

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b. anions

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ions that carry one or more charge, therefore they are attracted a positive pole, considered electron acceptors

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c. cations

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ions with one or more pos charge, therefore they are attracted a neg pole, electron donor

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d. crystals

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large groups of anions and cations held together by ionic bonds; formed when an element or compound silitafies in a dry state

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2. Covalent bonds

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chemical bonds formed by sharing of electrons b/w atoms

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a. sharing of electrons

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will occupy one single orbit that is common to both atoms

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b. multiple covalent bonds

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double, triple or quad bond formations

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c. polar and non polar molecules
1. nonpolar molecules

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electriclly balanced, electrons are shared equally b/w atoms

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2. polar molecules

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unsymmetrical in shape and are electrically unbalanced, electrons not shared equally

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a. polar molecules are

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determined by shape and the following: electronegativity, electropositivity, dipoles

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b. electronegativity

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equals having a strong attraction for electrons due to having a valence shells of 6 or 7 electrons

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c. electropositivity

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low attraction for electrons, usually lose their one or two valence shell electrons to other atom

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d. dipoles

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aka polar molecule

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2. Covalent Bonds
D. charge distribution

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D. based on electropositivity and electroneg

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3. Hydrogen Bonds (polar)

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weak bonds where hydrogen forms a bridge b/w electroneg. atoms, common b/c dipoles

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a. surface tension

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measure of how difficult it is to stretch or break the surface of a liquid due to cohesion

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b. cohesion

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tendency of water molecules to stick together and cohesion is due to hydrogen bonds

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c. intramolecular bonds

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(within molecular bonds) hydrogen bond different parts of large molecules together to form 3d shapes- maintains and stabilizes the structures ex. final structre of protein, dna, water.

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V. Chemical Reactions

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occur when bonds are formed, broken, or altered- atoms are always in motion, even in solid form

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A. chemical reactions

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a symbolic written form of a chemical reaction

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1. reactants

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the substances that are taken part in the reaction- the prefix designates the # of atoms present

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2. products

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the result of chemical bonding, reacts bonding together- the subscript designates the # of atoms that have been joined together

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3. molecular formula

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representation of the product with the use of subscripts- should be described in moles, such as a mole of nitrogen, oxygen, water

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B. Patterns of Chemical Reactions
1. Synthesis (combination) reaction

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reactants with form a product that is large and more complex- anabolic-always has bond formation

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2. Decomposition Reaction

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reactant is broken down into its parts-catabolic-bonds are always broken

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3. Exchange (displacement) reaction

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both synthesis and decomposition are occuring- reactants will exchange atomic partners

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4. Oxidation Reduction Reactant

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generally decomposition type reaction- breakdown of food or fuel to generate energy or ATP, one reactant gives up an electron or electrons it is considered the electron donor and oxidized- while the other reactant recieves the electrons so its the accptor and it is said to be reduced ex. cellular respiration

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C. Energy flow in chemical reactions
1. Exergonic

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give off or release energy, products are going to be less energy in thier bonds than reactants did-catabolic reaction

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2. Entergonic

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use energy, products will have more energy in bonds than reactants-anabolic reaction

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D. Reversibilty of Chemical reactions

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technically reactions are reversible but most do not b/c energy or product gets used up so they are not availible- arrows indicate the prominant direction of the reaction- can be in chemical equilibrium

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E. Factors influencing Chemical Reactions

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atoms have to collide with enough force for chemical reaction to occur

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1. Temp

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the higher the temp the higher the kenetic energy then the higher the collision rate

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2. Particle Size

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the smaller the particle the faster it will be therefore the higher collision rate

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3. Concentration

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the greater the reactant concentration the greater chance you have for collision

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4. Catalysts

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come into play when one through three (above) are not possible- substances that increase the rate of a chemical reaction without itself being used up or changed- enzymes are biological catalysts

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PART 2 INORGANIC COMPOUNDS
I. inorganic compounds

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any compound that do not contain carbon

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A. Water

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60- 80% of every living cell

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1. High heat capacity

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absorbs and releases large amount of heat before it itself changes in temp, due to making and breaking of hydrogen bonds- helps maintain body temp against wind, sun, and muscle activity- within the blood helps to redistibute heat throughout the tissues

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2. High heat of vaporization

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is transformation from liquid to gas under extreme amount of heat ex. sweat: provides cooling system

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3. Polarity/ Solvent Properties

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almost every body reaction is going to use water as a solvent

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a. ionic compounds

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break up in water due to polarity in water

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b. water can also form hydrogen layers by

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surrounding charged molecules, water tends to surround proteins keeps things from settling

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c. acts as

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biological colloid, blood plasma

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4. Reactivity

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will only occur in one of two ways: Hydrolysis- the splitting apart with water, adding water to reactant to make smaller product, Dehydration Synthesis- removing water to make a larger product

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5. Cushioning

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can occur in a few diff ways: serous fluid, synobial fluid, CSF

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B. Salts

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any ionic compound other than hydroxil or hydrogen

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1. in ionic form, acts as electrolytes

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that conduct electrical current ex. NA+ and K+ conduct nerve impulses and aid muscle contraction

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adenoma

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tumor of gland

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adrenal glands

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endocrine glands above kidney

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anabolism

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building up from complex to simple

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anastomosis

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surgical connection b/w two parts

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anemia

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no blood- reduction in erythrocytes or hemoglobin in circulating blood

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anomaly

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a deviation from normal especially of a bodily part

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ante cibum

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before meals

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anterior

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toward the front

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arthralgia

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pain in a joint

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atrophy

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a wasting away, a diminution in the size of a cell, tissue, organ, or part

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bursitis

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the bursa becomes inflamed and movement is limited and painful

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catabolism

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chemical complex, food broken down from complex to simple

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caudal

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toward the cauda or tail

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cell membrane

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structure surrounding and protecting the cell

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cells

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smallest living unit

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cephalgia

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headache, head pain

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cholecystectomy

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surgical removal of gallbladder

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chronic

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persisting over long period of time

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combining vowel

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usually o , links the root to the suffix or root to another root.

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common bile duct

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carries bile from the liver and gallbladder to the duodenum, also called the choledochus

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coronal

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vertical plane from head to foot and parallel to the shoulders

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cytologist

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studies cytology

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cytoplasm

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includes all the material outside the nucleus and enclosed by the cell membrane

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defecation

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expulsion or passage of feces from the body through the anus

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deglutination

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swallowing

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diaphoresis

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sweating

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diaphragm

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muscle separating the abdominal and thoracic cavities