CHEM 1441 EXAM 3

Soluble if it Contains:

Li+, Na+, K+, NH4+, NO3-

Three things that affect reaction rate:

1. temperature

2. reactant concentration

3. adding a catalyst

Diabetes insipidus

polydipsia and polyuria

lack of antidiuretic hormone function

kidneys cannot retain water

urine osmolality is low

artificial ADH

diabetes mellitus

polydipsia and polyuria

lack of insulin function

water leaves kidneys though osmosis along with glucose

urine osmolality is high

artificial insulin

Explain respiration using Boyle’s Law

Boyle’s Law states that pressure and volume of a gas are inversely related.

During inhalation, the volume of the lungs expand resulting in the inverse of decreased pressure in the lungs.

During exhalation, the volume of the lungs decreases resulting in the pressure to increase in the lungs.

Heating Curve

Bends

tissue damage caused by nitrogen coming out of solution (blood) during rapid ascent (depressurization); Decompression sickness

Hyperbaric

high pressure therapy

Bonding Pair

two electrons in a covalent bond between two non-metal atoms

Lone Pair

two electrons on a covalently-bonded atom that are not in a bond

Double Bond

four electrons shared between two atoms

Triple Bond

six electrons shared between two atoms

Resonance Structures

Two or more wats a valid dot structure can be drawn

VSEPR

valence shell electron pair repulsion theory; electron groups repel and seek the greatest distance between them

Electronegativity

Tendency of atoms to attract shared electrons

Polarity

unequal sharing of electrons resulting in partial charges on opposite sides of a bond or molecule

Polar Covalent Bond

electronegativity difference between 0.5 and 1.7

Non-Polar Covalent Bond

electronegativity difference less than 0.5

Dipole

polar covalent bond that has a separation of charges

Polar Molecule

dipoles don't cancel out

Non-polar Molecule

dipoles don't exist or cancel each other out

Dipole Moment

The overall dipole characteristics of a polar molecule

Dipole-dipole Interactions

when the positive end of one dipole is attracted to the negative end of a second dipole

Hydrogen Bond

especially strong dipole-dipole attractions, occur between polar molecules containing hydrogen atoms bonded to very electronegative atoms such as fluorine (F), nitrogen (N), and oxygen (O)

Dispersion Forces

very weak attractive forces that occur between nonpolar molecules that occur when electron movement induces a temporary distortion of the electrons in a molecule, creating a temporary dipole

Amino Acids

building blocks of proteins; contain amino and carboxylic acid groups as well as Hand R-groups

Melting

solid to liquid

Vaporization

liquid to gas

Condensation

gas to liquid

Freezing

liquid to solid

Sublimation

solid to gas

Deposition

gas to solid

Solid

particles in fixed array; vibrational movement only; definite volume; definite shape; not compressible

Liquid

particles touching; freely moving; definite volume; indefinite shape; not compressible

Gas

particles very far apart; moving very fast in straight lines; indefinite volume; indefinite shape; compressible

Heat of Fusion

Energy required to convert 1 gram of a substance from a solid to a liquid

Specific Heat Capacity

energy required to raise the temperature of 1 g of a substance 1°C

Boiling Point

Molecules have enough energy to overcome their attractive forces and become a gas within the liquid; vapor pressure equals external pressure

Heat of Vaporization

Energy required to convert 1 gram of a substance from liquid to gas

Atmospheric Pressure

the pressure exerted by a column of air from the top of the atmosphere to the surface of the

Earth; 760 mm Hg; 760 torr

Pressure

force/area

Boyle’s Law

Pressure is inversely related to volume

Charles’ Law

Volume is directly related to temperature

Gay-Lussac’s Law

Pressure is directly related to temperature

Vapor Pressure

the pressure above a liquid at equilibrium in a closed container

Combined Gas Law

P1•V1/T1 = P2•V2/T2 when number of moles are constant

Avogadro’s Law

Volume is directly related to number of moles of has - when temp and pressure are held constant

STP

standard temperature and pressure; 0°C, 1 atm

Ideal Gas Law

PV = nRT

Dalton’s Law of Partial Pressures

the total pressure of a gas mixture equals the sum of the partial pressures of all gases in the mixture

Diabetes Insipidus

loss of antidiuretic hormone (vasopressin) function directly resulting in excessive urination

Diabetes Mellitus

loss of insulin function resulting in excessive glucose levels in blood and urine, causing excessive urination due to osmotic action of excessive glucose in urine

Solution

homogeneous mixture

Solute

solution component of lesser amount

Solvent

solution component of greater amount

Strong Electrolyte

completely dissociates to produce ions and conduct an electric current

Weak Electrolyte

partially dissociates to produce few ions and slightly conduct an electric current

Non-electrolyte

completely dissolves, but produces no ions and does not conduct electricity

Solubility

the maximum amount of solute that dissolves in a specific amount of solvent; generally increases with temperature for solids, but decreases with temperature for gases

Saturated Solution

contains the maximum amount of solute that can dissolve

Total Ionic Equation

all ions in solution before and after mixing as well as the solid formed upon mixing

Net Ionic Equation

solid formed upon mixing of dissolved ions and the ions that react to form it

Mass Percent (m/m)

mass of solute (g) x 100% / mass of solute (g) + mass of solvent (g)

Volume Percent (v/v)

volume of solute x 100% / volume of solution

Mass/Volume Present (m/v)

mass of solute (g) x 100% / 100 mL of solution

Molarity

moles of solute / liters of solution

Dilution Formula

C1•V1 = C2•V2

Colligative

properties of solutions depend on the number of solute particles in the solution, not the solute identity

Molality

moles of solute particles per kg of solvent

Addition of Solute

causes freezing point depression and boiling point elevation

Osmosis

water (solvent) flows from the lower solute concentration into the higher solute concentration

Osmotic Pressure

produced by the solute particles dissolved in a solution as water moves to dilute the solute

Semipermeable Membrane

filters out solute particles, but not water

Isotonic

exerts the same osmotic pressure as body fluids such as blood

Hypertonic

has a higher solute concentration, water flows out of the cell by osmosis, causing the cell to shrink

Crenation

shrinking of a cell due to being in a hypertonic solution

Hypotonic

has a lower solute concentration, water flows into the cell by osmosis, causing the cell to swell

Lyse

bursting of a cell

Hemolysis

bursting of red blood cells

Collision Theory

a reaction takes place only when molecules collide with the proper orientation and sufficient energy

Activation Energy

the minimum amount of energy required to break the bonds between the atoms of reactants

Reaction Rate

change in [reactant] or [product] / change in time

Rate Influencers

temperature, concentration, presence of catalyst

Catalyst

increases reaction rate without being consumed by lowering energy of activation; does not affect Kc

Reversible Reaction

occurs in both the forward and reverse direction

Equilibrium

the rate of the forward reaction is equal to the rate of the reverse reaction; no further change in reactant or product concentrations

Kc

equilibrium constant = products / reactants

Kc for heterogenous Reaction

solids and liquids not included since their concentration does not change

Large Kc

mostly products at equilibrium

Small Kc

mostly reactants at equilibrium