Bio chapter 2 part B

kinetic energy

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

potential energy

stored energy ex.) elevator up

4 forms of energy

chemical

electrical

mechanical

radient

chemical energy

energy stored in chemical bonds

mechanical energy

moving matter ex.) amino acids, muscles

electrical energy

movement of charged particles (neurons)

radient energy

energy travelling in waves (x-rays)

Thermodynamics

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

first law of thermodynamics

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

second law of thermodynamics

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

Entropy meaning

the amount of disorder or randomness in a system

physical properties

those detected with our senses or are measurable

chemical properties

the way atoms interact with one another

4 major elements

oxygen

carbon

hydrogen

nitrogen

neutrons

have no charge

protons

have a positive charge

electrons

have a negative charge

atomic number

protons in each atom of an element

mass number

number of protons and neutrons in atoms nucleus

isotopes

elements that have different numbers of neutrons

molecule

two or more atoms joined together chemically

compound

molecule that has at least two or more different elements

compounds and molecules

all compounds are molecules but not all molecules are compounds

mixtures

two or more components physically mixed no chemically bonded

solvent

substance present in greatest amount

solute

substance present in smaller amount

colloids

heterogeneous mixtures whose solute don’t settle out

suspensions

heterogeneous mixtures with visible solutes that tend to settle out

the further an electron is from the nucleus…

the more energy it has

chemically inert

their outermost energy level is fully occupied by electrons

chemically reactive shells

don’t have their outermost energy level fully occupied

octet rule

when valence shell wants 8 electrons by sharing with other atoms

ions

charged atoms resulting from the gain or loss of electrons

anions

have gained one or more electrons resulting in a negative charge

cations

have lost one or more electrons resulting in a positive charge

ionic bonds

form between atoms by the transfer of one or more electrons

attraction of opposite charges result in a

ionic bond

covalent bonds

strong bonds formed when two atoms share valence shell electrons

non polar covalent

equal sharing of electrons

polar covalent

unequal sharing of electrons

is water polar

yes

electronegative

atoms with 6 or 7 valence shell electrons

electropositive

atoms with one or two valence shell electrons

complete transfer of electrons

ionic bond

when do chemical reactions occur

when chemical bonds are formed

all chemical equations have

reactants and products

patterns of chemical reactions

synthesis reaction (anabolic)

decomposition reaction (catabolic)

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

anabolic pathway

energy in (building)

catabolic pathway

energy out (breakdown)

OIL RIG

oxidation is losing

reduction is gaining

always occur together

dehydrogenase

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

hydrogen atoms consist of

electron and proton

two general types of chemical reactions in cells

endergonic reactions

exergonic reactions

endergonic reactions

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

where is energy stored

covalent bonds of product molecules

exergonic reactions

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

covalent bonds of reactants contain

more energy than those of the products

why many biological reactions are irreversible

energy requirements

removal of products

are all chemical reactions reversible

theoretically yes

factors influencing rate of chemical reactions

temperature

particle size (smaller=faster)

concentration (higher concen= faster)

catalysts

catalysts

increase the rate of a reaction without being chemically changed

biological catalysts

enzymes

inorganic compounds

don’t contain carbon

organic compounds

carbohydrates

fats

proteins

and nucleic acids

60%-80% of volume in living cells

water

polar solvent properties

dissolves and dissociates ionic substances

forms hydration layers around large charged molecules like proteins

reactivity

a necessary part of hydrolysis and dehydration synthesis reactions

cushioning

protects certain organs from physical trauma

dehydration synthesis

pulling water out

hydrolysis

releases energy when bonds break due to water rupture

acids

proton donors (pH below 7)

bases

protons acceptors (pH above 7)

acidic

higher hydrogen concentration so lower pH

alkaline

lower hydrogen concentration so higher pH

buffers

convert stong acids or bases into weak acids or bases

carbonic acid and bicarbonate

resist pH changes in blood (equilibrium)

macromolecule

giant biological molecule in a living system

carbohydrates

lipids

proteins

nucleic acids

monomers

building blocks of polymers

polymers

large molecules consisting of similar units strung together in long chains

oligo

5-100

poly

over 100

carbohydrates

simple and complex sugar molecules

single monomer

monosaccharide

two monomers

disaccharide

multi-unit monomer

polysaccharide

CH2O

general monosaccharide formula

two important monosaccharides

glucose and fructose

they come together through dehydration synthesis

disaccharides

two monosaccharides joined by dehydration synthesis

most common disaccharide

sucrose linkage of a glucose monomer to a fructose monomer

also maltose and lactose

oligosaccharides are linked by

dehydration synthesis

polysaccharides

carbohydrate polymer linked by covalent bonds and dehydration synthesis

examples of polysaccharides

starch -plant (potato tuber cell)

glycogen-animal (granule in muscle tissue)

cellulose-plant (plant cell wall)

lipids

carbon and hydrogen atoms linked by covalent bonds

fats

large lipid molecule made from glycerol and fatty acids

glycerol

three carbon alcohol molecule with three hydroxyl groups

fatty acid

carboxyl group and a hydrocarbon chain with 15 carbons

what are fatty acid and glycerol molecules joined by

dehydration synthesis

why are fats hydrophobic

nonpolar covalent bonds of the fatty acids

fats are a form of

energy storage

triglyceride

glycerol molecule joined to three fatty acids