Bio 1100 Mid Term Chemistry

Front 1

Solid

Back 1

has definite shape and volume

Front 2

Liquid

Back 2

Has a definite volume but takes the shape of its container.

Front 3

Gas Pressure

Back 3

Force created when particles hit container walls.
1.measure of: 1 atm=29.9 inches of Hg=760mmHg.
2.More molecules in container at same temperature increases pressure.
3.P=force/Area

Front 4

Gas Volume

Back 4

Equal to the volume of container.

Front 5

Partial Pressure (Pp)

Back 5

Amount of a gas mixture id the sum of the partial pressures of the gases in the mixture

OR

The total pressure of a mixture multiplied by the % of gas in the mixture is the partial pressure of that gas in the mixture.

Front 6

Solution

Back 6

Mixture of one substance dispersed uniformly in another substance.
A. Solute - substance to be dispersed.
B. Solvent - substance that contains the solute; ususally present in a greater amount than solute.
C. Solute and Solvent do NOT react with each other so they can be mixed in various proportions.
D. May be gases, liquids or solids;solution has same state as solute
E. Characterstics
1.Small single particles that go through a filter and semipermeable membrane.
2.Uniformly Dispersed to give homogeneous solution that is transparent.
3. Particles do not settle out of solution.

Front 7

Ionic Solution

Back 7

A. To form liquid or solid solutions, there must be an attraction between the solute and the solvent so that both will seperate into individual ions or molecules.
B. Polar H of water attracts the Cl of ionic NaCl; polar O attracts the NA-; thus NaCl dissolves in water forming an ionic solution.

Front 8

Solubility

Back 8

The amount of solute that can dissolve in a solvent.

A. Like dissolves Like
1. Polar solvents attract polar solutes to form ionic solutions
2. Polar solvents(water) do not attract nonpolar solutes(iodine)

Front 9

Unsaturated Solution

Back 9

has less than the maximum amount of solute.

Front 10

Saturated Solution

Back 10

contains the maximum amount of solute.

Front 11

Colloid

Back 11

Particles are larger molecules or groups of molecules or ions.
1. Homogeneous mixture inwhich particles do NOT seperate out.
2. Particles pass through some filters but not semipermeable membranes.
3. Light into a colloid produces a Tyndall effect (like headlight into a fog)

types:
Aerosols, Foams, Emulsions, Sols (blood plasma, paint, cement, pearls).

Front 12

Suspension

Back 12

heterogeneous, nonuniform, opaque mixture.

Particles are often visible.
Muddy water, pennicilin.

Front 13

Diffusion

Back 13

particles spreading out following a concentration gradient until all particles are equally distributed.

Front 14

Osmosis

Back 14

solvent water moves through a semipermeable membrane from a dilute solution(more water molecules) to a concentrated solution(less water molecules)

Front 15

Dialysis

Back 15

small particles and water through a semipermeable membrane.

A. Seperates solutions from colloids
B. Used to remove urea and other wastes from blood when kidneys fail.

Front 16

Isotonic

Back 16

equal in osmotic pressure to the osmotic pressure within the cell.

No change in cell.

Front 17

Hypotonic

Back 17

less solutes and more water in the solution outside the cell.

Water moves into the more concentrated solution inside the cell

Causes cell to swell and possibly burst.

Hemolysis - causes red blood cells to rupture.

Front 18

Hypertonic

Back 18

more solutes and less water in the solution outside the cell.

Water moves out of the cell to the more concentrated solution

causes cells to shrivel up

Front 19

Crenation

Back 19

- causes red blood cells to shrivel.

Front 20

Acid

Back 20

Substances that produce H+ when dissolved in water.

Front 21

Ionic bond

Back 21

USUALLY metal and a non-metal

metal donates one or more electrons (cation) to a non-metal (anion) which takes it.

Ionic substances in solution conduct electricity because the ions are free to move and carry the electrical charge from the anode to the cathode.

Front 22

Covalent Bond

Back 22

sharing electrons

Occurs between 2 nonmetals
usually Identical nonmetals

equal sharing - nonpolar covalent bond

Front 23

Polar Covalent Bond

Back 23

Nonidentical Nonmetals

shared unequally
i.e. H2O O is a big electron compared to H

Front 24

Polyatomic Molecule

Back 24

Polyatomic ion – charged particle composed of 2 or more atoms covalently bonded together
Nonmetal P, S, C, & N will covalently bond to O to form a polyatomic ion
Have negative charge of -1, -2, or -3
SO4–2, NO3–1, PO4–3, HPO4–2, H2PO4–
Exceptions: OH–, CN–, NH+

Front 25

Molar Mass

Back 25

Total AMU of all atoms.

expressed as
Grams

Front 26

Exothermic reaction

Back 26

reactions release heat

reactant + reactant ->product + kalories

when energy of PRODUCTS is LOWER than the energy of the REACTANTS, heat is released.

Front 27

Endothermic reaction

Back 27

reactions absorb heat

kalories +reactant ->product

when the energy of the REACTANTS is lower than the energy of the PRODUCTS, heat is absorbed.

Front 28

Base

Back 28

substance that produces OH when disolved in water.

Front 29

pH Scale

Back 29

convenient way to describe the acidity of a solution.

pH scale 1 - 14

pH1 being most acidic
pH14 being most basic
pH7 being nuetral

Front 30

neutralization

Back 30

any acid + any base forms salt+water

complete nuetralization when the molarity of the acid present equals molarity of the base present; the pH is 7

Front 31

buffer

Back 31

a solution that resists a change in pH.

buffers contain a weak acid and a salt of that acid or a weak base and a salt of that base; strong acids and bases cannot make buffer solutions.

Front 32

Naming

Covalent and Ionic Bonds

Back 32

end with -ide

Front 33

Naming

polyatomic ions

Back 33

end with -ite or -ate

1less O is -ite
1more O is -ate

Front 34

prefixes

Back 34

1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
6 hepta
8 octa
9 nona
10 deca