Studied by 16 peopleFormula
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.
Note
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