A&P - 2.4 Inorganic Compounds Essential to Human Functioning

inorganic compound

substance that does not contain both carbon and hydrogen

monomer

• small, individual molecule (simplest molecules) that serves as a building block

• form polymers (two or more chemically-bonded monomers)

dehydration synthesis

• chemical reaction that joins two molecules together, forming a larger molecule while simultaneously releasing a water molecule as a byproduct

• takes water out, glues them together

• monomer 1 becomes linked to monomer 2 by covalent bond (monomers link to form polymers)

• process for building essential macromolecules (proteins, carbohydrates, DNA, and RNA)

hydrolysis

• a chemical reaction where water breaks a bond in a compound

• put water into it, splits them apart

• covalent bond is broken splitting them back into monomer 1 and monomer 2 (polymers are split to form monomers)

dissociation of sodium chloride in water

• when salt (sodium chloride, NaCl) dissolves in water, the water molecules act like tiny magnets, negative ends of the water molecules (oxygen) are attracted to the positively charged sodium ions (Na⁺) and positive ends of the water molecules (hydrogen) are attracted to the negatively charged chloride ions (Cl^-) which causes the sodium and chloride ions to be pulled apart from each other, breaking the crystal structure of the salt

• this results in the sodium and chloride ions becoming surrounded by water molecules dispersing throughout the water, forming a salty solution

acid

• releases hydrogen (H⁺) ions when placed in solution

• proton donors - donates a positive charge to something else

• a very strong ion donates a lot of H⁺ ions (acidic)

• a pH of less than 7 is acidic solution (H⁺ > OH^-)

• the more H⁺ ions released by the substance the more acid the substance is (closer to 1)

• example: lemon juice

base

• proton acceptor (accepts H⁺ ions) - this removes H⁺ ions from a solution, raising the pH making the solution basic

• many bases release hydroxide (OH^-) ions when placed in solution (alkalinity)

• a pH of greater than 7 is basic solution (OH^- > H⁺)

• the more OH^- ions release the more alkaline the substance is (closer to 14)

• example: ammonia or bleach

pH

• hydrogen ion (H⁺) concentration in the body of fluids is measured on the pH scale

• acidity or alkalinity of a solution

• opposite poles - as one gets stronger the other gets weaker

neutrals

• release equal numbers of H⁺ and OH^- when placed in solution

• pH of 7.0 (H⁺ = OH^-)

• example: distilled water

buffers

• chemical solutions that resist changes in pH

• helps bring you back to homeostatic pH

• solution containing a weak acid or a weak base that opposes wide fluctuations in the pH of body fluids

pH of blood

• normal pH of blood is 7.35 to 7.45

• maintaining normal (slightly basic) pH of blood is crucial for physiological functions - abnormal fluctuations in pH (too acidic or too alkaline) can result in illness, disease, and death