Chem Lab Scioly, Chemistry - Science Olympiad, Science Olympiad Chemistry Lab

Boyle's Law

-The volume of a sample of a gas is inversely proportional to its pressure

-P1V1=P2V2

Zeroth Law of Thermodynamics

A law that if two systems are separately found to be in thermal equilibrium with a third system, the first two systems are in thermal equilibrium with each other; that is, all three systems are at the same temperature. Also known as thermodynamic equilibrium.

a=c=b b=a

First Law of Thermodynamics

Energy can be transferred and transformed, but it cannot be created or destroyed.

Second Law of Thermodynamics

-Every energy transfer or transformation increases the entropy of the universe.

-When energy is transformed, the quantity of energy remains the same, but its ability to do work diminishes.

Third Law of Thermodynamics

"The entropy of a perfect crystal is zero when the temperature of the crystal is equal to absolute zero (0 K)." "The crystal must be perfect, or else there will be some inherent disorder. It also must be at 0 K; otherwise there will be thermal motion within the crystal, which leads to disorder."

Gay-Lussac's Law

The pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.

Charles' Law

The volume of a given amount of gas held at constant pressure is directly proportional to the Kelvin temperature.

Avogadro's Law

1 mol = 22.4 L - The relationship between volume and amount of gas when pressure and temperature are held constant.

Hess' Law

The heat evolved or absorbed in a chemical process is the same whether the process takes place in one or in several steps. This is also known as the law of constant heat summation.

Le Châtelier's Principle

If a change is made to a system, then the system will react in such a way so as to absorb the force causing the change.

Ideal Gas Law

A combination of all the gas laws, applicable to any gas. Relates temperature, volume, and pressure to each other. Further explanation in van der Waals' equation.

van der Waals' Equation

As there are attractive forces between molecules, the pressure is lower than the ideal value. To account for this the pressure term is augmented by an attractive force term a/V2. Likewise real molecules have a volume. The volume of the molecules is represented by the term b. The term b is a function of a spherical diameter d known as the van der Waals diameter. The van der Waals' equation accounts for these inaccuracies.

Kinetic Theory of Heat (1)

The gas consists of very small particles, so the average distance between the gas particles is comparatively large.

Kinetic Theory of Heat (2)

Gas particles have the same mass.

Kinetic Theory of Heat (3)

The number of molecules is so large that statistical treatment can be applied.

Kinetic Theory of Heat (4)

Gas molecules are in constant, random, and rapid motion.

Kinetic Theory of Heat (5)

The rapidly moving particles constantly collide among themselves and with the walls of the container. All these collisions are perfectly elastic. This means, the molecules are considered to be perfectly spherical in shape, and elastic in nature.

Kinetic Theory of Heat (6)

Except during collisions, the interactions among molecules are negligible. (That is, they exert no forces on one another.) This implies the dynamics of the molecules can be treated classically. The equations of motion of the molecules are time-reversible.

"The average kinetic energy of the gas particles is proportional to the temperature of the system and depends only on it."

Kinetic Theory of Heat (7)

The time during collision of molecule with the container's wall is negligible as compared to the time between successive collisions.

Open System

Matter, heat, and work can cross the boundary to enter or exit the system.

Closed System

Heat and work can cross the boundary, but matter can't cross the boundary.

Isolated System

Neither matter, heat, or work can cross the boundary.

Diatheric System

Heat can cross the boundary, but nothing else.

Adiabatic System

Heat may not cross the boundary, but everything else can.

Isentropic process

No transfer of heat or matter, and the process is reversible.

ionic compound

In solid state, it has a high melting point

Volume of a cube formula

L•W•H

Density

D=m/v ; Intensive

specific heat formula

Q= mcP(change in Temperatures)

Sublimation

Process that convert a solid straight to a gas

List of thing that can be study w/o change identity of the substance

Texture, odor, melting point

Condensation occur where?

The line between gas and liquid

Forward reaction is best described as...

Endothermic reaction in which energy is absorbed

Mass

extensive

Boiling point

intensive

odor

Extensive

Melting point

Intensive

Length

Extensive

Density

Intensive ; 2.8 g/cm^3

Volume

Extensive ; 15dm^3

Luster

(n.) the quality of giving off light, brightness, glitter, brilliance. ; intensive

Temperature

Extensive

Ductility

The ability to be pulled into thin wires ; intensive

Area

Extensive

Conductivity

Intensive

Hardness

Intensive

Color

Intensive

Malleability

the ability of a solid to be hammered without shattering ; intensive

Shape

Extensive

Weight

Extensive

Mixture

Can be identify with (aq)

Which element presents in all organic compounds?

Carbon

Physical changes

The product stay almost the same to the reactants

Four properties of acids

Less than 7.0 on pH scale; contains H+ ions; turn blue litmus red; it is liquid

Three properties of a base

More than 7.0 on pH scale; slippery; turn litmus paper blue; taste bitter

covalent bond

Covalent chemical bonds involve the sharing of a pair of valence electrons by two atom

Polar Covalent/ dipole-dipole interactions

in which the sharing of the electron pair is unequal, with the electrons spending more time around the more nonmetallic atom

Hydrogen bonding

H-F, H-O, H-N

Non-polar/ London dispersion forces

Ionic bond

In chemical bonds, atoms can either transfer or share their valence electrons. In the extreme case where one or more atoms lose electrons and other atoms gain them in order to produce a noble gas electron configuration, the bond is called an ionic bond.

When ask about who have the higher boiling point

The one that have more carbon

Measuring Concentration (units)

~Molarity

~Molality

~Ppm

~Ppb

Molarity

moles of solute/liters of solution

Molality

moles of solute/kg of solution

ppm (parts per million)

(mass of solute/mass of solution)*10^6

ppb (parts per billion)

(mass of solute/mass of solution)*10^9

acid

~a substance that produces (donates) hydrogen ions in solution

~accepts electrons

base

~substance that takes (accepts) hydrogen ions in water

~donates electrons

pH

equal to the negative logarithm of the concentration of Hydrogen Ions in the solution

pOH

the negative of the common logarithm of the hydroxide ion concentration

pH+pOH=....

14 (always)

strong acids

~HCI (hydrochloric)

~HClO4 (perchloric)

~HClO3 (chloric)

~H2SO4 (sulfuric)

~HNO3 (nitric)

~HBr (hydrobromic)

~HI (hydroiodic)

strong bases

(usually salts)

~NaOH

~KOH

~Ca(OH)2

~Mg(OH)2

Weak acids and bases

acids

~Acetic acid (vinegar)

~Ascorbic acid (vitamin C)

bases

~ammonia

dynamic equilibrium

state of weak acids and bases

Equilibrium constant (K)

The value obtained when equilibrium concentrations are substituted into the reaction quotient

Ka

acid dissociation constant

Kb

-base dissociation constant

Kb=([B+][OH-])/([BOH])

-the smaller the Kb, the weaker the base

Ions

Alkali and Alkaline Metals (Groups 1 and 2)

Strong Acids

Carbonates - CO32-

Bicarbonates - HCO3-

Sulfites - SO32-

Bisulfites - HSO3-

Oxides - O2-

Acetate - CH3COO-

Ascorbate - C6H7O6-

Neutralization

~Acids react with bases in neutralization reactions

~Forms water and a salt (for all of the acids and bases we need to know for this)

~Net Ionic Equations

physical properties

Any property that can be observed without changing the composition of the object

examples of physical properties

Density

Color

Conductivity

Boiling and Melting Points

Resistance

Elasticity

Heat Capacity

Specific Heat

Solubility

Magnetism

Extensive and Intensive properties

extensive properties

depend on the amount of matter that is present

intensive properties

do not depend on the amount of matter present

examples of extensive properties

mass

length

volume

solubility

examples of intensive properties

Conductivity

Density

Color

Temperature

Resistance

Magnetism

Boyle's Law

-The volume of a sample of a gas is inversely proportional to its pressure

-P1V1=P2V2