Ch. 2, Lecture 2 Flashcards
(chemical reactions)
Synthesis Reactions
• Two or more small molecules combine to form a larger one.
A+B—>AB
(chemical reactions)
Decomposition Reactions
• Large molecule breaks down into two or smaller ones.
AB—>A+B
(chemical reactions)
Exchange Reactions
• Two molecules exchange atoms or group of atoms
AB+CD—>ABCD—>AC+BD
Stomach acid (HCl) and sodium bicarbonate (NaHCO3) from the pancreas combine to form NaCl and H2CO3.
(chemical reactions)
Reversible Reactions
- Can go in either direction under different circumstances.
* Symbolized with double headed arrow
(chemical reactions)
CO2+H2O->H2CO3->HCO3-+H+
<- <-
- Most common equation discussed in the book
* Respiratory, urinary, and digestive physiology
Metabolism
• All the chemical reactions of the body
(metabolism)
Catabolism
• Energy-storing (exergonic) synthesis reactions
- breaks covalent bonds - produces smaller molecules - releases useful energy
(metabolism)
Anabolism
• Energy-storing (endergonic) synthesis reactions
- requires energy input - production of protein or fat - driven by energy that catabolism releases
(Metabolism)
Catabolism and anabolism are-
• Inseparably linked
Reaction Rates
• Basis for chemical reactions is molecular motion and collisions
- Reactions occur when molecules collide with enough force and the correct orientation rates are affected by- - concentration - temperature
(reaction rates)
Catalysts
• Substances that temporarily bond to reactants, hold them in favorable position to react with each other, and may change the shapes of reactants in ways that make them more likely to react.
(reaction rates)
Enzymes
• Most important biological catalysts
Inorganic Molecules
• Smaller molecules like water and oxygen that lack carbon and hydrogen.
Water (1)
• Polar covalent bonds and V-shaped molecule gives water a set of properties that account for its ability to support life.
- solvency - cohesion - adhesion - chemical reactivity - thermal stability
Water (2)
• Water helps stabilize the internal temperature of the body.
Has high heat capacity—the amount of heat required to raise the temperature of 1g of a substance by 1 degrees Celsius
- Hydrogen bonds inhibit temperature increases by inhibiting molecular motion
- Water absorbs heat without changing temperature very much.
Acid
• Proton donor (releases H+ ions in water)
Base
• Proton acceptor (accepts H+ ions)
- Releases OH- ions in water
pH
• Measure derived from the molarity of H+
- a pH of 7.0 is neutral pH (H+=OH-)
- a pH of less than 7 is acidic solution (H+>OH-)
- a pH of greater than 7 is basic solution (H+<OH-)