Medical Terminology, Part 2

Front 1

Mass number

Back 1

= protons + nuetrons

Front 2

Radioactive isotopes; half-life

Back 2

Unstable isotopes that decay overtime to a more stable configuration; the time required for half of the radioactive isotope atoms in a sample to decay

Front 3

Molecule

Back 3

A compound where atoms share electrons

Front 4

Compound

Back 4

A substance that contains atoms of two or more different elements

Hint 4

H20 is a compound, but O2 is not

Front 5

Free radicals

Back 5

Atom with an unpaired electron in its outermost shell; unstable and highly reactive; becomes stable when giving up the electron

Front 6

The types of chemical bonds

Back 6

Ionic, covalent, hydrogen

Hint 6

3 types

Front 7

Chemical bond

Back 7

The forces that hold together the atoms of a molecule or a compound

Front 8

Chemically stable

Back 8

The atom has a full valance shell; all atoms want to be chemically stable and have a full outer shell.

Front 9

Ionic bond

Back 9

Strong electrical attraction between two opposite charged ions; electrons are transferred and not shared, creating positive and negative charges on the atoms due to the uneven amount of protons and electrons.

Front 10

Covalent bond

Back 10

Atoms share their electrons, not gain or lose them.

Front 11

Nonpolar covalent bond

Back 11

Two atoms share the electrons equally; no tug of war; if they are two identical atoms of the same element, they will always have a nonpolar covalent bond.

Front 12

Polar covalent bond

Back 12

The sharing of electrons between two atoms is unequal because one atom is more electronegative - the power to attract electrons to itself; there is a tug of war over the electrons and the strongest one has a better lead.

Front 13

Electronegativity

Back 13

The power to attract electrons to itself.

Front 14

Hydrogen Bonds

Back 14

Forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms; form weak single bonds; establish important links between molecules (ex. H2O) or between different parts of a large molecule (such as proteins or nucleic acids) binding it into a specific 3-D shape.

Front 15

Chemical reaction

Back 15

Occurs when new bonds form or old bonds break between atoms; the interactions of valence electrons are the basis of all chemical reactions

Front 16

Metabolism

Back 16

Sum of all the chemical reactions in the body or a cell.

Front 17

Activation Energy

Back 17

The collision energy needed to break chemical bonds in the reactant molecules so a reaction can start; the initial energy investment needed to start a reaction; Then as enough energy is absorbed, the reactants' bonds become unstable and form new combinations. As new bonds form, energy is released to the surroundings.

Front 18

Catalysts

Back 18

Chemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur; lowers the amount of energy needed to start the reaction; properly orient the colliding parts in the right spot; catalyst molecules are unchanged and can be used repeatedly to speed up more reactions.

Front 19

Enzymes

Back 19

The most important catalysts in the body; replace using harmful higher temperatures and concentrations for chemical reactions to occur in the body, as temp. and concentrations are originally too low in the human body for chemical reactions to occur.

Front 20

Anabolism; Synthesis Reactions

Back 20

When atoms or molecules combine to form new and larger molecules; usually endergonic reaction (absorbs energy)

Front 21

Catabolism; Decomposition reactions

Back 21

Split up larger molecules into smaller atoms, ions, or molecules; usually exergonic (releases energy)

Front 22

Collision influences

Back 22

Temperature and concentration of particles. The higher, the more likely a collision will occur and cause a chemical reaction

Front 23

Inorganic compound

Back 23

Usually lack carbon and are structurally simple; include water and electrolytes (salts, acids and bases)

Front 24

Organic compound

Back 24

Always contain carbon & usually hydrogen; always have covalent bond; most are large molecules, made up of long carbon atom chains; proteins, carbohydrates, lipids, nucleic acids, ATP

Front 25

Water

Back 25

Most important and abundant inorganic compound in living systems; medium of nearly all chemical reactions; the polarity makes an excellent solvent for other ionic or polar substances (ex: salt or sugar), gives it more cohesion (sticks together), and makes it absorb and release heat slowly.

Front 26

Importance of water

Back 26

Cells: Good solvent and aids in the transport of solute through the plasma membrane and inside the cell itself; Helps maintain body temperature as it absorbs and releases heat slowly; Helps to cool skin by the evaporation of sweat from the surface of the skin; it is an important reactant in digestion of food.

Front 27

Hydrolysis reactions

Back 27

Water participates as a reactant; Chemical reaction where water is added to a large molecule to separate it into two smaller molecules; Aids in digestion of nutrients

Front 28

Dehydration synthesis reaction

Back 28

Water participates as a product; two small molecules are joined to form a larger molecule releasing a water molecule; a hydrogen atom is removed from one monomer, and a hydroxyl group is removed from the other, to form a polymer and a molecule of water

Front 29

Water as a lubricant

Back 29

Mucus in respiratory and digestive systems; synovial fluid in joints; serous fluid in chest and abdominal cavities where internal organs touch and slide over one another.

Front 30

Acids

Back 30

Dissociate into H+ ions and anions

Front 31

Bases

Back 31

Dissociate into OH- ions and cations

Front 32

Salt

Back 32

Product of acid and base (neutralization reaction); dissociate into anions and cations, that aren't either H+ or OH-; exist as crystals in absences of water; high melting and boiling points; most important salts in the body are calcium phosphates which contribute to hardness of bones and teeth

Front 33

Electrolytes

Back 33

Flow of ions; Important salts in the body that carry electrical currents (in nerve or muscle tissue).

Front 34

Concept of pH

Back 34

pH scale runs from 0 to 14 - concentration of H+ in moles/liter; A pH of 7 is neutral and H+ and OH+ are equal; pH below 7 = acidic; pH above 7 = alkaline (basic);

ex: pH of 4 would be 0.0001 (10^-4) mol/L. It also has 10 times more H+ than pH of 5, and 100 times more than pH 6, etc.

Front 35

pH

Back 35

pH = log1 / [H+] = -log [H+]

Reciprocal of hydrogen ion concentration.

Normal arterial blood = pH 7.4 (range 7.36 - 7.44)

Normal venous blood and intersitial fluid = pH about 7.35

Front 36

Acidosis

Back 36

Too much of acid in body and not enough base

Front 37

Alkalosis

Back 37

Too much base in body and not enough acid

Front 38

Buffer Systems

Back 38

Help maintain almost constant pH in body; Function to convert strong acids or bases into weak acids or bases to avoid acidosis and alkalosis; body fluids vary in pH:

Bile 7.6 to 8.6

Saliva 6.35 to 6.85

Gastric juice 1.2 to 3.0

Front 39

Buffer

Back 39

The chemical compounds that convert strong acids or bases into weak ones; the most important extracellular buffer is carbonic acid - bicarbonate buffer system; it catches H+ ions or provides H+ ions as needed

Front 40

Organic compunds

Back 40

Always contain carbon and hydrogen; usually contain covalent bonds; usually large, unique molecules with complex functions; make up 40% of body mass.

Front 41

Macromolecules

Back 41

When small organic molecules combine into very large molecules; they are usually polymers (a large molecule formed by the covalent bonding of many identical or similar small building-block molecules called monomers).

Hint 41

Macro = large

Front 42

Carbohydrates: Monosaccharides

Back 42

Called simple sugars; contain 3 to 7 carbon atoms; the monomers used to build carbohydrates; our bodies can only absorb 3 simple sugars without further digestion in our small intestine and into our blood stream - glucose (main blood sugat), fructose (fruit), galactose (milk)

Hint 42

-sacch = sugar, mono- = one

Front 43

Carbohydrates

Back 43

-Diverse group of substances from C, H, and O; ratio of hydrogen to oxygen atoms is usually 2:1, like water; ratio of one carbon atom for each water molecule

- main function: source of energy for ATP formation; building blocks of DNA and RNA (ribose sugars)

- forms 2-3% of body weight

-include sugars, glycogen, starches, and cellulose

Hint 43

"Watered carbon" for its 1:1 carbon:water ratio

Front 44

Carbohydrates: Disaccharides

Back 44

Simple sugars. Consists of two monosaccharides that have combined by dehydration synthesis;

Sucrose = glucose and fructose

Maltose = glucose and glucose

Lactose = glucose and galactose (lactose intolerance)

Can be split into smaller, simpler substances by hydrolosis.

Front 45

Carbohydrates: Polysaccharides

Back 45

Contains 10s or 100s of monosaccharides joined together through dehydration synthesis;

-In animals: glycogen is a polysaccharide chain of hundreds of glucose (sugar) molecules, which is stored in the liver and skeletal muscle. Liver hydrolyzes (breaks down) glycogen to release glucose in the blood when sugar levels are low.

-in plants: starch and cellulose are large carbohydrate molecules used for energy storage... cellulose however isn't digested by humans.

Front 46

Lipids

Back 46

Make up 18-25% of body mass; insoluble (hydrophobic); to become more soluble in blood plasma, lipid molecules join with hydrophilic protein molecules to, resulting in lipoproteins;

Lipids consist of:

-Fatty acids (smallest lipids)

-Triglycerides

-Phospholipids

-Steroids

-Eicosanoids

-Vitamins

Hint 46

Lip- = fat

Front 47

Importance of lipids

Back 47

-Used in the structure of cell parts (membranes)

-supply energy

-protection and insulation

-protective coating to prevent infection and excess loss or gain of water

-some hormone composition