Cycle 3 BMP Workshop Flashcards
List and Describe:
Types of energy
- Kinetic: From moving particles
- Potential: “Stored” by position or chemical structure
- Chemical: From chemical reactions
List and explain:
Types of systems
- Open: Exchange matter AND energy (e.g. cells)
- Closed: Exchange energy only
- Isolated: Neither
List and explain:
The first two laws of thermodynamics
Law 1: Energy CANNOT be made or destroyed, it can only be converted
Law 2: Entropy (“disorder”) of the universe ALWAYS INCREASES
How do cells fight the 2nd Law of Thermodynamics?
Cells use energy to build “ordered” molecules
They are “islands” of low entropy (energy taken in to replace other things broken down)
State:
The levels of protein structure
- Primary (denatured)
- Secondary
- Tertiary (functional proteins)
- Quaternary (functional proteins)
Describe the structure and bonding of:
Primary structure protein
- Unfolded, 1 linear chain of amino acids
- Peptide bonds joining amino acids
Describe the structure and bonding of:
Secondary structure protein
- 1 chain of amino acids (alpha-helix form or beta-barrel form)
- Peptide + Hydrogen bonds
What are hydrogen bonds disturbed by?
Urea
Describe the structure and bonding of:
Tertiary structure protein
- 1 fully folded 3D chain
- Peptide, Hydrogen + any other bond (dipole-dipole, disulfide bridges etc.)
Describe the structure and bonding of:
Quaternary structure protein
- Multiple fully folded 3D chains
- Peptide, Hydrogen + any other bond (dipole-dipole, disulfide bridges etc.)
Describe:
Most reduced molecules
- More C-H bonds
- HIGH free energy
- Electrons are easy to remove
Describe:
Most oxidized molecules
- More C-O bonds
- LOW free energy
- Electrons are more tightly bound to oxygen
Explain:
Heterotrophs
- “We like, we want”
- Consume: Matter and energy combine through our carbs + fats
Explain:
Autotrophs
- “We hate, we expel”
- Consume matter (CO2) and energy (light)
State the type of equation and explain:
The values in the equation:
ΔG = ΔH - TΔS
Thermodynamic Equation
* ΔG: Free energy, = Products - Reactants
* ΔH: Enthalpy
* ΔS: Entropy
State the meaning of:
ΔG > 0
ΔG < 0
Free Energy
* ΔG > 0: Endergonic, requires energy
* ΔG < 0: Exergonic, spontaneous
State the meaning of:
ΔH > 0
ΔH < 0
Enthalpy
* ΔH > 0: Endothermic
* ΔH < 0: Exothermic
State the meaning of:
ΔS > 0
ΔS < 0
Entropy
* ΔS > 0: More spread out (less order)
* ΔS < 0: Less spread out (more order)
What do enzymes do?
Enzymes LOWER ACTIVATION ENERGY to speed up the reaction
True or False:
Enzymes change ΔG
False
True or False:
Enzymes do not give energy
True
What is required for endergonic reactions to occur?
Energy providers (e.g. ATP)