Bio chapter 2 part B

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126 Terms

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kinetic energy

the energy of motion ex.) heat/thermal energy is a form of kinetic energy

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potential energy

stored energy ex.) elevator up

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4 forms of energy

chemical

electrical

mechanical

radient

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chemical energy

energy stored in chemical bonds

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mechanical energy

moving matter ex.) amino acids, muscles

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electrical energy

movement of charged particles (neurons)

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radient energy

energy travelling in waves (x-rays)

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Thermodynamics

the study of energy transformation that occur in a collection of matter

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first law of thermodynamics

energy cannot be destroyed or created only transferred from one for to another

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second law of thermodynamics

energy transfers reduce the order of the universe and increase entropy which is disorder

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Entropy meaning

the amount of disorder or randomness in a system

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physical properties

those detected with our senses or are measurable

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chemical properties

the way atoms interact with one another

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4 major elements

oxygen

carbon

hydrogen

nitrogen

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neutrons

have no charge

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protons

have a positive charge

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electrons

have a negative charge

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atomic number

protons in each atom of an element

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mass number

number of protons and neutrons in atoms nucleus

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isotopes

elements that have different numbers of neutrons

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molecule

two or more atoms joined together chemically

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compound

molecule that has at least two or more different elements

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compounds and molecules

all compounds are molecules but not all molecules are compounds

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mixtures

two or more components physically mixed no chemically bonded

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solvent

substance present in greatest amount

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solute

substance present in smaller amount

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colloids

heterogeneous mixtures whose solute don’t settle out

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suspensions

heterogeneous mixtures with visible solutes that tend to settle out

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the further an electron is from the nucleus…

the more energy it has

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chemically inert

their outermost energy level is fully occupied by electrons

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chemically reactive shells

don’t have their outermost energy level fully occupied

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octet rule

when valence shell wants 8 electrons by sharing with other atoms

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ions

charged atoms resulting from the gain or loss of electrons

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anions

have gained one or more electrons resulting in a negative charge

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cations

have lost one or more electrons resulting in a positive charge

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ionic bonds

form between atoms by the transfer of one or more electrons

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attraction of opposite charges result in a

ionic bond

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covalent bonds

strong bonds formed when two atoms share valence shell electrons

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non polar covalent

equal sharing of electrons

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polar covalent

unequal sharing of electrons

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is water polar

yes

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electronegative

atoms with 6 or 7 valence shell electrons

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electropositive

atoms with one or two valence shell electrons

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complete transfer of electrons

ionic bond

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when do chemical reactions occur

when chemical bonds are formed

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all chemical equations have

reactants and products

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patterns of chemical reactions

synthesis reaction (anabolic)

decomposition reaction (catabolic)

exchange/displacement reactions (bonds are both made and broken)

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anabolic pathway

energy in (building)

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catabolic pathway

energy out (breakdown)

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OIL RIG

oxidation is losing

reduction is gaining

always occur together

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dehydrogenase

an enzyme that catalyzes redox reactions so a chemical is losing H ions

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hydrogen atoms consist of

electron and proton

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two general types of chemical reactions in cells

endergonic reactions

exergonic reactions

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endergonic reactions

requires a net input of energy to yield products rich in potential energy

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where is energy stored

covalent bonds of product molecules

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exergonic reactions

releases energy to yield products lower in potential energy than the reactants

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covalent bonds of reactants contain

more energy than those of the products

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why many biological reactions are irreversible

energy requirements

removal of products

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are all chemical reactions reversible

theoretically yes

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factors influencing rate of chemical reactions

temperature

particle size (smaller=faster)

concentration (higher concen= faster)

catalysts

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catalysts

increase the rate of a reaction without being chemically changed

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biological catalysts

enzymes

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inorganic compounds

don’t contain carbon

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organic compounds

carbohydrates

fats

proteins

and nucleic acids

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60%-80% of volume in living cells

water

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polar solvent properties

dissolves and dissociates ionic substances

forms hydration layers around large charged molecules like proteins

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reactivity

a necessary part of hydrolysis and dehydration synthesis reactions

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cushioning

protects certain organs from physical trauma

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dehydration synthesis

pulling water out

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hydrolysis

releases energy when bonds break due to water rupture

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acids

proton donors (pH below 7)

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bases

protons acceptors (pH above 7)

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acidic

higher hydrogen concentration so lower pH

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alkaline

lower hydrogen concentration so higher pH

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buffers

convert stong acids or bases into weak acids or bases

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carbonic acid and bicarbonate

resist pH changes in blood (equilibrium)

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macromolecule

giant biological molecule in a living system

carbohydrates

lipids

proteins

nucleic acids

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monomers

building blocks of polymers

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polymers

large molecules consisting of similar units strung together in long chains

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oligo

5-100

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poly

over 100

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carbohydrates

simple and complex sugar molecules

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single monomer

monosaccharide

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two monomers

disaccharide

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multi-unit monomer

polysaccharide

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CH2O

general monosaccharide formula

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two important monosaccharides

glucose and fructose

they come together through dehydration synthesis

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disaccharides

two monosaccharides joined by dehydration synthesis

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most common disaccharide

sucrose linkage of a glucose monomer to a fructose monomer

also maltose and lactose

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oligosaccharides are linked by

dehydration synthesis

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polysaccharides

carbohydrate polymer linked by covalent bonds and dehydration synthesis

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examples of polysaccharides

starch -plant (potato tuber cell)

glycogen-animal (granule in muscle tissue)

cellulose-plant (plant cell wall)

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lipids

carbon and hydrogen atoms linked by covalent bonds

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fats

large lipid molecule made from glycerol and fatty acids

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glycerol

three carbon alcohol molecule with three hydroxyl groups

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fatty acid

carboxyl group and a hydrocarbon chain with 15 carbons

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what are fatty acid and glycerol molecules joined by

dehydration synthesis

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why are fats hydrophobic

nonpolar covalent bonds of the fatty acids

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fats are a form of

energy storage

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triglyceride

glycerol molecule joined to three fatty acids