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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
