The smallest representative unit of an element that reatins all the characteristics of that element.

The center of an atom containing the neutrons and protons.

No charge

Mass of about 1 dalton

Relative charge of +1

Mass of about 1 dalton

Relative charge of -1

Mass of about 0.0005 daltons

No two electrons in an atom may have exactly the same set of four quantum numbers

The energy given off when a neutral atom in the gas phase picks up an electron to form a negatively charged ion

PV = nRT

P = Pressure in atmospher or torr

V = Volume (Liters L)

T = Absolute temperature (Kelvins K)

n = moles of the gas

R = universal gas constant

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1. Intermolecular forces that exist between polar molecules . Active only when the molecules are close together. The strengths of intermolecular attractions increase when polarity increases.

A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom, especially a nitrogen, oxygen, or flourine atom, usually of another molecule

London dispersion forces

Van der Waals dispersion forces

A weak attractive force between atoms or nonpolar molecules caused by an instantaneous dipole moment of one atom or molecule that induces a similar temporary dipole moment in adjacent atoms or molecules

Gas --> Liquid

A substance that donates a proton to an aqueous solution

A substance that donates an electron pair.

Moles per liter

(Grams / molecular weight) / liters of solution

-log [H⁺] 

A measure of the acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing with increasing alkalinity and decreasing with increasing acidity. The pH scale commonly in use ranges from 0 to 14.

A solution that contains a weak acid or a weak base and a salt of that weak acid or weak base.

Number of equivalents in neutralization

The spontaneous flow of heat is always unidirectional from the higher to lower temperature.

A negative ΔH

Heat is evolved into the surroundings

Endothermic Reaction

or

Endergonic Reaction

A positive ΔH 

A reaction that requires additional heata from the surroundings

Entropy

The degree of disorder of a system.

Unrecoverable energy.

ΔS

A thermodynamic function of a system equivalent to the sum of intrernally energy of a system plus its volume multiplied by the pressure exerted on it by the environment.

ΔH

Gibbs free Energy

ΔG

The slowest step of a reaction that controls or determines the rate of the overall (usually multistep) reaction expressed as:

Rate= k[A]^a[B]^b

Where A & B are reactants and a & b are concentrations.

Activation energy

E_act

The minimum amount of energy necessary to transform reactants --> products

Energy difference between the starting energy and the top of the potential energy trajectory

A biological catalyst that substantially increases the rate of a reaction by allowing the reaction to follow a lower energy pathway that does not involve attaining the full energy of activation.

not used up in the reaction itself.

Equilibrium constant

K_eq

In a reversible reaction this is expressed as:

[C]^c[D]^d

[A]^a[B]^b

Where C & D are products and A & B are reactants

Principle that states that when a system is at equiliburium it will shift to relieve any stress placed on it.

ex: if too many reactants are added the system will shift to increase the amount of products to balance out the system

Specific gravity

Mass (m)

Volume (v)