semester 2 FINAL - honors chem - Mr.Hughes

Stoichiometry

a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitive data.

HNRUE table

Have, Need, Recipes, Used, Extra

Stoichiometry Definition 2

essential in chemistry because it allows us to determine how much of a substance is either NEEDED or PRODUCED in a reaction

Mole Ratio

A ratio that is determined by comparing the coefficients of any substance involved in a chemical reaction

Limiting reactant

The reactant that gets completely used up first in the chemical reaction and determines (limits) how much product is produced

Excess Reactant

the reactant(s) which are present as an abundance in a chemical reaction and will show up as excess after the reaction takes place.

Completion

all reactant is completed during the chemical reaction entirely

Theoretical Yield

the maximum amount of product that can be produced from a given amount of reactant

Actual Yield

the measured amount of product obtained from a chemical reaction

percentage Yield

(actual yield /theoretical yield) x 100

Kinetic Molecular Theory of Gasses

a theory that explains the behavior of masses depending on multiple variables including temperature, pressure, solve and moles of gas

Ideal Gas

a 'hypothetical gas' that is composed of many randomly moving particles that aren't subject to intermolecular forces

POSTULATES OF GAS (1)

particles of a has are traveling in straight lines, are in constant motion, and will eventually collide with one another as well as the container itself

POSTULATES OF GAS (2)

gasses are usually just empty space under MOST conditions they are so small that the space they occupy causes the volume to be RELATIVELY zero

POSTULATES OF GAS (3)

pressure is exerted on the sides of the container when the particles make contact. although the mass of the particles are small, the sum is significant

POSTULATES OF GAS (4)

Particles of gas DO NOT interact with each other, simply because they are so small, and the presence of intermolecular forces are nonexistent. the collisions of particles are elastic

POSTULATES OF GAS (5)

The average kinetic energy of the particles of the gas is PROPORTIONAL to the temperature of the gas in kelvin

Pressure

amount of force per unit area

Elastic

the ability for something to return to its natural state after being compressed, stretched if contacted

Kelvin

the temperature scale that directly relates to particle motion

Absolute Zero

No particle movement, No kinetic energy

Boyle's law

states that when temperature of a given mass of a confined gas is constant, the product of the pressure and volume are also constant

PV=PV (P1V1=P2V2)

Boyles law, meaning pressure and volume are inversely proportional

Charles Law

states that when temperature of a given mass of a confined gas is increased and all other variables remain constant, the gas will have a tendency to expand, resulting in a larger volume

V/T=V/T (V1/T1=V2/T2)

Charles Law, means that volume and temperature are directly proportional

Gay Lussac's Law

states that when temperature of a given mass of a confined gas is increased and all other variables remain constant the gasses will have more kinetic energy, resulting in more collisions on the container

P/T=P/T (P1/T1=P2/T2)

Gay Lussac's Law, higher pressure, this means that pressure and temperature are directly proportional

Avogadro's Law

states that when the number of moles of has are changed within a container, the volume will also have to change since there is a difference in number of thing occupying a fixed space

V/N=V/N (V1/N1=V2/N2)

Avogadro's law, this means that the volume and the moles of gas are directly proportional

STP

standard temperature and pressure

273K (0 degrees C) and 1 (atm)

IUPAC definition of STP

Combined gas law

(PV)/T = (PV)/T (P1V1)/T1 = (P2V2)/T2

PV=nRT

Ideal Gas law

Units of pressure

Atm, Kpa, torr, mmHg, Psi

Units of volume

milliliter, liter, cubic centimeter, cubic meter

Gas constants (R)

0.082 using atm, 8.314 using KPa, 62.36 using torr, 62.36 using mmHg

Units of temperature

Fahrenheit, Celsius, Kelvin

Density

defined as the amount of tangible material (mass) per space that the material occupies (volume)

Density of Gasses

D = (PMm)/(RT)

22.4L at STP

1 mol of ANY gas at stp will occupy 22.4L

solution

defined as any substance that is classified as a homogeneous mixture of 2 or more substance in a single phase

Homogeneous

uniform or the same

Heterogeneous

diverse or different

solute

a substance that is being dissolved

solvent

a substance that is doing the dissolving

aqueous

a solution that is made from water as a solvent

unviersal solvent

water

Alloy

a homogeneous mixture of two or more metallic elements

Gaseous solution

a homogeneous mixture of two or more substances in gas phase

suspension

a type of mixture that results in a separation of particles, unless the mixture is stirred or agitated

Colloid

a type of mixture that is not classified as true homogeneous or true heterogeneous, but somewhere in between due to the size of the particles being involved

Dispersion Medium

the thing that contains the dispersed substance

Dispersed Substance

the thing that spreads through the dispersion medium

COLLOID: Liquid Aerosol

a LIQUID dispersed in a GAS medium

COLLOID: Solid Aerosol

a SOLID dispersed in a GAS medium

COLLOID: Foam

a GAS dispersed in a LIQUID medium

COLLOID: Sol

a SOLID dispersed in a LIQUID medium (liquid)

COLLOID: Gel

a SOLID dispersed in a LIQUID medium (semisolid)

COLLOID: Liquid Emulsion

a LIQUID dispersed in a LIQUID medium

COLLOID: Solid Emulsion

a LIQUID dispersed in a SOLID medium

Tyndall effect

a phenomenon in which l might is scattered by colloidal particles that are dispersed in a transparent medium

Light Ray -> (not visible in solution) (visible in colloid) (visible in suspension)

Dissolution

the chemical process in which a solid solute will dissolve in a solvent to create a solution

FACTORS AFFECT DISSOLUTION (1)

increasing the surface area

FACTORS AFFECT DISSOLUTION (2)

Agitating the solution

FACTORS AFFECT DISSOLUTION (3)

heating the solvent

Solubility

the maximum amount of solute that can dissolve in a solvent at a particular temperature

Saturated solution

a solution that contains the maximum amount of dissolved solute

Unsaturated solution

a solution that contains less solute than saturated solution under given conditions

Supersaturated solution

a solution that contains more dissolved solute than a saturated solution contains under given conditions

Miscibility

the property of 2 substances ABLE TO mix in all proportions (that is to fully dissolve in each other at any concentration) forming a homogeneous mixture

immiscibility

The property of 2 substances UNABLE TO mix in all proportions (that is to fully dissolve in each other at any concentration) not being able to form a homogeneous mixture

Like dissolves like

polarity will effect miscibility

Concentration

referring to the amount of substance within a defined area, typically associated with solutions

Molarity (equation)

(moles of solute)/(liters of solution)

Molality

(moles of solute)/(kilograms of solvent)

Molarity (definition)

the number of moles of solute per liter of solution (M)

Stock solution

a solution that is created in order to conserve materials, save preparation time, and reduce storage space, usually with a high concentration

Diluted solution

stock solution altered with a change in amount of solvent (ex. water) this is because we don't need the amount go solute present in the stock solution

CV = CV (C1V1=C2V2) (MV=MV)

Dilution, C=concentration, V=volume

Net Ionic equation

a chemical equation that focus on compounds and ions that undergo a chemical change in a reaction in an aqueous solution

Spectator ions

ions that appear on both sides of the equation

Acid

a chemical substance that has the ability to offer protons (Usually as hydrogen ions), and neutralize bases

B/L Base

a chemical substance that has the ability to accept p+ (usually as hydrogen ions) and neutralize acids

oxyacid

an acid that is made from hydrogen, oxygen and a nonmetal. (rare instances like chromium and manganese will form oxyacids in their highest oxidation states)

Logarithmic

a term to describe something logarithms the inverse of exponential logarithms are useful as they allow is to see how many times a base number needs to be multiplied by itself to bet a certain number

Arrhenius Acid

A chemical compound that increases the concentration of hydrogen ions (H+) in other words they are H+ donors when dissolved in water

Arrhenius base

a chemical compound that increases the concentration of hydroxide ions (OH-) in other words, they are OH- donors when dissolved in water

proticity

the capability of being able to donate a hydrogen ion (H+)

monoprotic

donate a single H+ per molecule

Aprotic

unable to donate a single H+ per molecule

Diprotic

donate 2 H+ per molecule

Bronsted-Lowry acid

A molecule or ion that considered a proton donor since hydrogen ions (H+) are just a single proton, all Arrhenius acids are classified as Bronsted-lowtry acids

Bronsted-Lowry Base

A molecule or ion that considered a proton acceptor. Arrhenius hydroxide bases aren't classified as bronsted-lowry base, however, anions are usually B/L bases

Conjugate acid

a chemical species that remains after a bronzed-lowry base has received a proton

Conjugate base

a chemical species that remains after a bronzed-lowry acid has donated a proton

Amphoteric

the ability for a species to act as either an acid or base (ex. water)

Lewis Acid

an atom, ion, or molecule that accepts an electron pair to form a covalent bond

Lewis Base

an atom, ion, or molecule that donates an electron pair to form a covalent bond

strong acids

HCl, HBr, HI, HNO3, H2SO4, HCLO4