Chapter 2.2: Inorganic Compounds Flashcards
(12 cards)
Inorganic compounds
Generally do not contain Carbon bonded to Hydrogen.
Ex. Water, acids, bases & salts
Properties of h2o
Makes up 50-65% of body mass
1.) Absorbs heat w/o changing significantly in its own temp
2.) Carries heat with it when it changes from liquid to gas (sweat evaporation)
3.) Cushions and protects body’s structures b/c it is denser than organs
4.) Acts as lubricant b/t adjacent surfaces
Water as a solvent
Water is the body’s primary solvent
Known as the universal solvent b/c so many solutes fully or partially dissolve in it.
*Since water is a polar molecule, its partial charges on hydrogen (-) and oxygen (+) and its shape allows it to grab certain solutes and pull them apart.
Hydrophilic and Hydrophobic
Hydrophilic solutes have fully or partially charged ends that attract the oppositely charged ends of water molecules due to attraction between positives & negatives.
*Thus, IONIC & POLAR COVALENT compounds are hydrophilic.
Hydrophobic solutes lack charged ends, this they are not pulled apart by opposite charges and will not dissolve in water.
*UNCHARGED NON-POLAR COVALENT MOLECULES OR COMPOUNDS are hydrophobic
Ex. methane, oils & fats
Solubility in water: “like dissolves like”
Partially or fully charged compounds (ionic & polar covalent bonds) will interact w/ the charges in h2o & dissolve.
Uncharged Non-Polar Covalent molecules will not interact w/ the charges in h2o, but will dissolve in Non-Polar Covalent solutions.
Hydrogen Ion (H+)
Hydrogen behaves as a non-metal most of the time, in that it form covalent rather than ionic bonds; however, when certain Hydrogen containing compounds are placed in h2o, Hydrogen behaves like a metal and will donate its e- to produce a H+ ion.
h2o —-> H+ + OH-
<——
Behavior of acids & bases in h2o
Acids: An acid (HCl) releases H+ (hydrogen cation) and an anion, which increases the H+ concentration of the solution. Also known as proton donors b/c H only has one subatomic particle, the proton in its nucleus.
HCl (in h2o) <—-> H+ + Cl-
Bases: A base/ alkali (NaHCO3) binds free H+ and decreases the H+ concentration of the solution.
NaHCO3 (in h2o) <—-> Na+ + HCO3-
Acids and Bases are defined according to their behavior with respect to H+ ions.
Acids donate H+
Bases accept H+
pH Scale
A logarithmic scale. Each number represents a 10-fold increase/decrease.
0 thru 14:
0 to 6: Acidic (higher conc. of H+)
7: Neutral
8 to 14: Basic (lower conc. of H+)
Buffers
Chemical systems that resist changes in pH.
Consists of a weak acid & its corresponding anion
A major buffer in the body is:
the carbonic acid-bicarbonate ion buffering system
H2CO3 <—-> H+ + HCO3-
Carbonic acid <—> H ion plus Bicarbonate ion
Acidosis vs Alkalosis
Acidosis: blood pH below 7.35
Alkalosis: blood pH above 7.45
Respiratory and Urinary systems are the main organ systems concerned w/ buffering.
Salt
Any metal cation and non-metal anion held together by an ionic bond.
Electrolytes
Salts dissolve when placed in h2o and the resulting cation & anions are electrolytes.
They conduct an electrical current in h2o.
