CHEM VOCAB

WOOHOOOO DLAPS VOCAB

Formula

Represents an element or compound.

Compound

Two or more different elements bonded together.

Ion

Charged particle +/-

Cation

Positive ion

Anion

Negative ion

Precipitate

An insoluble solid.

Atom

The smallest part of an element that retains its properties.

Law of Conservation of Mass

The Mass of the reactants is equal to the mass of the product.

Law of Definite Composition (or Properties)

All samples of a given chemical compound have the same elemental composition by mass.

Atomic Number

The number of protons in an atom of an element.

Isotope

Atoms of the same element that differ in mass due to a different number of neutrons.

Atomic mass

The weighted average of all of the naturally occurring isotopes of an element.

Inert

Non reactive

Spectrum

A series of color which forms when light is refracted.

Spectroscope

A device using a prism to show colors in a beam of light.

Light Spectra

Each element has its own unique line spectrum.

Orbital

A region of space (or volume) where there is a high probability of finding an e-.

Valence e-

Electrons in the outermost PEL.

Hund’s Rule

1 electron in each orbital first.

Sublimation

Solid → Gas

Atom

The smallest particle of an element that retains the properties of that element.

Mass Number

The total number of protons and neutrons in the nucleus of an atom.

Atomic Mass Unit

1/12th of the mass of a carbon-12 atom.

Electron

Negatively charged subatomic particle.

Nucleus

The central part of an atom, containing protons and neutrons.

Neutron

Subatomic particle with no charge.

Proton

Positively charged subatomic particle.

Atomic Mass

Mass of one atom of an element in amu (Atomic Mass Unit). OR The weighted average of all the naturally occurring isotopes in an element.

Gram Atomic Mass (GAM)

Mass of one mole of atoms in grams.

Avogadro's #: Mole

6.02 x 10^23 molecules

Grams Formula Mass (GFM/ Molecular Mass)

Mass of one mole of a substance in grams.

Percent Composition

Mass % of an element in a compound.

Hydrate

A compound which contains H2O as part of its surface.

Empirical formula

Lowest whole number ratio of the elements involved.

Molecular formula

A formula giving the number of atoms of each element present in the molecular compound.

STP

Standard Temperature and Pressure

Room Temp

25degreesC

Captive Zeros

Between 2 non-zero digits.

Molar Mass

The mass of a substance in grams divided by the amount of moles in the substance

Limiting Reagent

The reactant that gets used up or consumed first.

Gas

A gas at room temperature.

Vapor

A liquid or solid at room temperature, but can turn into a gas.

Matter

Anything that has mass and takes up space (volume).

Pure Substances

Matter having identical properties and composition.

Endothermic Reaction

Energy being absorbed.

Exothermic reaction

Energy being released.

Elements

Substances that cannot be decomposed or broken down into simpler substances by chemical means.

Compounds

Two or more elements chemically bonded together.

Mixtures

Combinations of 2 or more substances which retain their original properties.

Physical properties

Those properties discerned from our senses.

Chemical Properties

Describes how a substance reacts.

Energy

The capacity to do work.

Temperature

Is a measure of a substance’s average kinetic energy.

Calorimetry

measure of energy changes in a reaction.

Calorimeter

Device used to determine energy changes.

Luster

Shine (Mirror)

Malleable

Can be hammered into sheets (sheet metal)

Ductile

Can be drawn into wire

Molecule

A particle made up of two or more atoms that are chemically bonded together.

Specific Heat

4\.18 J OF HEAT MUST BE ADDED TO 1g OF H2O TO RAISE ITS TEMPERATURE BY 1 DEGREE CELSIUS.

Binary

2 different elements

Ternary

3 different elements

Activated complex

The intermediate stage of a reaction

Solution

Homogeneous Mixture

Solute

The substance that dissolves.

Covalently Bonded Substances

Contains carbons and hydrogen only.

Kinetic Energy

Energy in motion.

Potential Energy

Stored Energy

Activation Energy

Minimum amount of energy required to start a reaction

Reaction Coordiante

The path that the reaction takes.

Heat of vaporization

The amount of energy added or released to vaporize one gram of a substance.

**Heat of Fusion**

The amount of energy added or realeased to melt or freeze one gram of a substance.

Gas

No definite shape or volume

Boyle’s Law

The temperature and amount of gas are kept constant as the pressure and volume vary.

Torricelli

Measure pressure (Torr)

Pressure

PPressure equals force per unit area.

Vacuum

Lower pressure (take air out)

Charles’ Law

Shows how the temperature (K) and volume if a gas vary, as pressure and amount of gas remain constant.

Diffusion

The movement of gas from a region of high concentration to a region of low concentration.

Graham’s Law

The relative rate of diffusion of gas 1 to gas 2 is equal to the square root of the reciprocal masses.

Dalton’s Law

The total pressure in a container of gasses, is equal to the partial pressure of each gas in the mixture.

Kinetic Molecular Theory

Model used to explain the behavior of gasses (Ideal Gas).

Vapor Pressure

The pressure exerted on the walls of a container by particles that escaped the liquid or solid phase.

Boiling Point

Temperature at which the vapor pressure of a the substance equals the external air pressure.”

“Normal” Boiling Point

It is a temperature at which the vapor pressure of the substance is equal to standard pressure, 101.3 KPa and 1 atm.

Allotrope

Same element with different stuctures.

Crystals

A regular, repeating, geometric pattern.