Lesson 2

Pregunta	Respuesta
Isotopes	atoms of an element having the same atomic number but different mass number (differ in number of neutrons) chemically similar
Ionic Bonds	Cations and Anions
Covalent Bonds	Strongest Bond; single, double, and triple bonds H2, O2, N2
Hydrogen Bonds	formed by electrical attraction between H atoms carrying a slight positive charge and another atom carrying a slight negative charge. Weak bonds. Maintain the shape of large molecules (proteins, DNA)
Endergonic Reactions	require energy, anabolic absorbs energy (if the energy is heat energy, the reaction is called endothermic) A + energy--> B + C
Exergonic Reactions	Release Energy, Catabolic looses energy as heat, light or sound (if energy is heat energy, the reaction is called exothermic) A + B --> C + energy
Rate of Reactions: Temperature	higher temperature means a greater velocity of particles means more collisions means greater rate of reaction (greater amount of product generated per unit of time)
Rate of Reactions: Concentration	greater particles means greater number of particles means more collisions means greater rate of reaction (greater amount of product generated per unit of time)
Rate of Reaction: Surface Energy	greater number of particles means more collisions means greater rate of reaction (greater amount of product generated per unit of time)
Rate of Reactions: Catalyst	substance that increases the rate of a reaction by decreasing the activation energy without itself being changed chemically in the reaction the catalysts in the body are called enzymes
Chemical Equilibrium: Changes in energy (heat)	increase in temp-->increased rate of energy requiring reaction (reverse, endothermic) decrease in temp-->increased rate of energy releasing reaction (forward, exothermic)
Mixtures: Solutions	mixture of a solute (soluble material) into a solvent (dissolving medium); small solute particles; pass through cell membranes; clear, transparent; do not settle
Mixtures: Colloids	larger than solution particles (size dispersed in water); mixtures with particles too large to be a true solution, but small enough not to settle; particles too large to pass through cell membranes; cloudy, milky, translucent
Mixtures: Suspensions	have larger solute particles that will settle when gravity becomes effective force (not stable transparent); particles are too large to pass through a cell membrane; opaque appearance; i.e. clay or sand in water, blood cells in plasma
Saturated	solution containing max amount of solute for a given solvent at a constant temp and pressure; incapable of dissolving more solute (completely filled with solute)
Unsaturated	solution to which more solute can be added; contain less solute than the saturated one at constant temp and pressure (can dissolve more solute)
pH in Body Compartments	Blood= 7.35 to 7.45 Stomach= 2 (1.5 to 3.5) pancreatic juice= 8 intestinal juice= 7.5 urine= 6 (4.5 to 8)
Physiological Buffeer	Resits changes in pH (convert strong acids or bases to weak ones) System that controls output of acids, bases or CO2 ex: urinary system buffers greatest quantity, takes several hours; respiratory system buffers within minutes, limited quantity
Chemical Buffer Systems	Resits changes in pH (convert strong acids or bases to weak ones) Restore normal pH in fractions of a second ex: bicarbonate, phosphate and protein systems bind H+ and transport H+ to an exit (kidney/lung)
Acidosis (Acidemia)	drop in blood plasma pH below 7.35; causes a depress in the CNS causes coma causes death Causes: respiratory (CO2 accumulates in blood-hypo-ventilation, pneumonia, asthma) or metabolic (strenuous work, low fat diets, starvation)
Alkalosis (Alkalemia)	rise in plasma pH above 7.45 (to 7.8) overexcites CNS; may lead to muscle tetany, extreme nervousness, convulsions, respiratory arrest causes: hyperventilation, temper tantrums, asthma, anxiety, high altitude, excessive vomiting, laxatives

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