energy and metabolism chapter 8. energy metabolism all the chemical reactions carried out by the...
TRANSCRIPT
Energy and Energy and MetabolismMetabolismChapter 8Chapter 8
Energy and Energy and MetabolismMetabolismChapter 8Chapter 8
Metabolism• Catabolic reactions: • Break down large molecules into
smaller substances• Exergonic:• Releases energy
Metabolism• Anabolic reactions: • Synthesis of large molecules from
smaller substances• Endergonic:• Requires energy
Metabolism• Biochemical pathways: • Reactions in a cell• Occur in sequence• Product of one reaction • Becomes substrate in the next• Pathways are highly regulated and coordinated• Feedback inhibition:• End product of a reaction blocks the pathway
from producing more.
Energy• Bioenergetics: • Analysis of how energy powers
activities of living systems • Growth, order, reproduction,
responsiveness & regulation
Energy• Energy: • The capacity to do work • Kinetic energy:• Energy of motion• Potential energy:• Energy of position or stored energy
Energy• Thermodynamics: • Study of energy “heat changes”• Most work done by living
organisms• Transformation of PE to KE
Energy• Sun main source of energy• Energy from sun• Combine smaller molecules to
make larger molecules• Energy is stored in the chemical
bond
Energy• Redox(oxidation-reduction)
reactions: • Transfer of an electron or electrons• Play a key role in the flow of energy in
biological systems• An electron is passed from one atom to
another energy is passed
Law of thermodynamics
• Laws of thermodynamics govern all energy changes in the universe.
• First law of thermodynamics: • Energy cannot be created or destroyed • Change from one form to another.
(potential to kinetic) • Total amount of energy stays the same
First law• In living organisms:• Eating transfers energy from the
bonds in food to organism• PE is transferred to KE
First Law• Heat: • Random motion of molecules • Heat can be lost in the system
during conversions• Sun replaces energy lost as heat
Second law• Second law of
thermodynamics:• Transformation of PE to heat
(random motion of molecules). • Entropy (disorder) in the universe
is increasing
Second law• Energy transformations tend to
proceed spontaneously • Convert matter from a more
ordered state to a less ordered or more stable state.
Second law• Entropy(s): • Disorder in a system• Enthalpy (H): • Heat content• Free energy(G): • Amount of energy available to do work in any
system.• Amount of energy available to break and then
make other chemical bonds
Second law• G=Gibbs free energy G = H - TS (T=Kelvin temp) G is positive • Products have more energy than
reactants• Due to more energy in the bonds or less
randomness • Endergonic reaction
Second lawG is negative• Products have less energy than
reactants• H is lower (bond energy) or
S is greater- more randomness• Exergonic:• Reaction that releases energy
Activation Energy• Energy needed to initiate a
reaction • All reactions require activation
energy.• Reactions with higher AE tend to
move forward more slowly
Enzymes• Catalyst in living organisms• Large three-dimensional globular
protein• Ribozymes:• RNA catalysts are specific & speed
up reactions
Enzymes• Substrate: • Molecule that is going to undergo the reaction• Active sites: • Specific spots on the enzyme that substrates binds• Enzyme-substrate complex:• Enzymes are bound to substrates with a precise fit.• Induced fit: • When the substrate causes the enzyme to adjust to
make a better fit• E+S ES E + P
Fig. 8-17Fig. 8-17Fig. 8-17Fig. 8-17
Substrates
Enzyme
Products arereleased.
Products
Substrates areconverted toproducts.
Active site can lower EA
and speed up a reaction.
Substrates held in active site by weakinteractions, such as hydrogen bonds andionic bonds.
Substrates enter active site; enzyme changes shape such that its active siteenfolds the substrates (induced fit).
Activesite is
availablefor two new
substratemolecules.
Enzyme-substratecomplex
5
3
21
6
4
Enzymes• Only small amounts are necessary• Can be recycled• Specific• Speeds up the reactions• Different types of cells have different
enzymes• Determine the course of chemical
reactions in the cell
Enzyme examples• Lipase, protease• Carbonic anhydrase
– CO2 + H2O H2CO3
• Lactate dehydrogenase– Lactate to pyruvate
• Pyruvate dehydrogenase– Enzyme that starts the Kreb cycle
Enzymes• Factors that affect the rate of enzyme• 1. Concentration of enzyme & substrate• 2. Factors that affect 3-D shape of the
enzyme • Temperature, pH, salt concentration
and regulatory molecules
Enzymes• Inhibitor: • Binds the enzyme• Prevents it from working• Occurs at the end of a pathway to stop
the reactions• Two types of inhibitors• Competitive• Noncompetitive
Fig. 8-19Fig. 8-19Fig. 8-19Fig. 8-19
(a) Normal binding (c) Noncompetitive inhibition(b) Competitive inhibition
Noncompetitive inhibitor
Active siteCompetitive inhibitor
Substrate
Enzyme
Enzymes• Allosteric site: • On/off switch for the enzyme• Usually at different location than the active
site• Allosteric inhibitor:• Binds at the allosteric site • Stops the enzyme activity• Activators: • Binds & increases the activity
Enzymes• Cofactor:• Assists enzyme function such as Zn, Mg, Cu• Coenzymes:• Cofactors that are not proteins but are organic
molecules • Help transfer electrons & energy associated
with the electrons• Vitamins are coenzymes • NAD+ important coenzyme
ATP• ATP powers the energy requiring
processes in the cell• 1. Chemical work (making
polymers)• 2. Transporting substances• 3. Mechanical work • Muscle movement, cilia