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Atom

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The smallest particle of life. Something cannot be broken down anymore from this point.

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Element

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One specific type of atom. Listed on periodic table.

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Mixture

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When two or more different atoms are combined but can still be separated.

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Compound

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When two or more different atoms are combined but can only be broken down with chemical reactions.

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Ionic Compound

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When atoms are held together by lost or gained electrons.

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Covalent Compound

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When atoms are held together by shared electrons.

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Homogeneous Mixture

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When the percent composition of each object in the mixture is the same.

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Heterogeneous Mixture

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When the percent composition of each object in the mixture is different.

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Proton

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Plus one charge. Subatomic particle. Located in the nucleus. Relative mass of one.

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Neutron

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No charge. Subatomic particle. Located in the nucleus. Relative mass of one. Can be lost or gained to form isotopes.

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Electron

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Minus one charge. Subatomic particle. Located in the electron cloud. Relative mass of zero. Can be gained or lost to form ions. Discovered in Milikan's Oil Drop experiment.

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Chemical Change

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When the chemical composition of an object is changes through a chemical reaction. (Ex: burning a log)

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Chemical Property

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Having to do with the chemical composition of objects.

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Physical Change

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When the chemical composition of an object remains the same but the object may look different. (Ex: shredding paper)

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Physical Property

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Having to do with the appearance of objects.

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Volume

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How much space something has inside.

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Mass

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How much matter an object has.

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Isotopes

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When the number of neutrons has changed. results in a different mass number.

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Ions

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When electrons are gained or lost. Either anion or cation. Have charge.

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Mole

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Unit for amount of substance. Count of the total number of particles in an atom.

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Cation

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When electrons are lost. Positive.

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Anion

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When electrons are gained. Negative.

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Robert Milikan

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Conducted Oil Drop experiment. Found the size of the electron's mass and charge.

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J.J. Thomson

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Conducted Cathode Ray Tube experiment. Plum Pudding model. Found that subatomic particles exist and mass to charge ratio of electrons.

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Dmitri Mendeleev

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Created earliest periodic table. Ordered elements by atomic mass.

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John Dalton

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Inspired by Democritus. Came up with atomic theory similar to today's.

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Aristotle

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Well known Greek philosopher of the time. Believed the earth was composed of four elements: Earth, Fire, Water, Wind. He disagreed with Democritus. Everyone agreed with him.

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Democritus

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Greek philosopher who first came up with the concept of an atom. No one believed him.

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Solid

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Organized particles, definite shape and volume.

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Liquid

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Unorganized particles, indefinite shape but definite volume.

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Gas

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Unorganized particles, indefinite shape and volume.

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Plasma

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Very fast and random particles, so much energy that electrons are liberated.

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Avagadro's Number

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6.022x10²²

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AMU

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Atomic Mass Unit

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When balancing, add...

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Coeffecients

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When balancing, DON'T TOUCH...

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Subsripts

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Conservation of Mass

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Mass can't be created or destoyed.

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Why are equations balanced?

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To find an accurate and pricise measurement, along with correct atom counts.

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Reactants

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Left side

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Products

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Right Side

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Arrow

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Act as an equal sign in chemical reactions.

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Density

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D=^M/_V

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Endothermic Reaction

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When heat is released internally in a reaction.

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Exothermic Reaction

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When heat is released externally in a reaction.

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Luminous Intensity

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Candelas

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Electric Current

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Amperes

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Mass

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Kilograms

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Liquid

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Liters

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Time

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Seconds

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Temperature

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Kelvins

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Amount of Substance

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Moles

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Heisenberg Uncertainty Principle

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One cannot know the speed and location of an electron at the same time.

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Valence Level

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Highest energy level of atoms. This is where electrons are gained or lost.

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Monoatomic Ion

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An ion with only one element.

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Polyatomic Ion

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An ion with two or more elements.

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Plum Pudding Model

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J.J. Thompson's model of the atom. The electrons represent the plum pieces. Looks like a chocolate chip cookie if you don't know what plum pudding is.

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Quantum Model

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The most recent and current model of the atom.

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Solar System Model

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Bohr's model of the atom. Only valid with Hydrogen.

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Electron Spin

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When an electron spins in the opposite direction than that of the electron which it shares the orbital with.

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Octet

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Meaning eight electrons. When an atom has all orbitals filled completely.

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MINOH

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The recommended order of balancing equations. Metals, Polyatomic ions, Non-metals, Oxygen, Hydrogen

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Noble Gas Exception

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Noble gases are extremely stable and do not react.

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Noble Gas Notation

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When you only list the electron configuration of an element after its preceding Noble Gas.

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Bunsen Burner

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Used for a flame in labs.

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Parts of a Bunsen Burner

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Barrel, Air ports, Gas inlet, Base, Needle Valve

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Matter

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Anything which takes up space.

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Recommended flame to use in labs

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Noisy, blue, stable, cone-shaped flame.

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Ernest Rutherford

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Conducted Gold Foil experiment. Found the nucleus and that atoms are mostly empty space.

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Lewis Dot Symbols

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When you write the element symbol and draw dots around it symbolizing how many valence electrons it shares.

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Atomic Radius

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How close the electrons are pulled to the nucleus.

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Oil Drop Experiment

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Oil was dropped and then charged in the middle of its fall. Found the size of the mass and charge of the electron. Done by Millikan.

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Cathode Ray Tube Experiment

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Electrons were passed through a tube and then placed against a negative charge. Found out about subatomic particles and mass to charge ratio of electrons. Done by Thompson.

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Gold Foil Experiment

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Radioactive alfa-particles were shot into a piece of gold. Found that atoms were mostly empty space and that nuclei exist. Done by Rutherford.

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Chemistry

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The study of matter and the changes it undergoes.

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Freezing

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Liquid to solid.

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Melting

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Solid to liquid.

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Evaporation

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Liquid to gas.

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Sublimation

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Solid to gas.

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Deposition

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Gas to solid.

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Condensation

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Gas to liquid

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Ionization

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Gas to plasma.

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Deionization

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Plasma to gas.

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Orbit

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The path electrons travel.

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Orbital

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A mathematical representation of the space electrons take up.

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Electronegativity

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An electron's ability to attract other electrons.

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Molar Mass

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Mass per mole.

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Percent Composition

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Finding out the percentages that each compound has of each element.

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Ionization Energy

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The energy required to form ions.

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Isoelectronic

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2 species with the same electron configuration.

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Molecular Formula

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The number of atoms of each element.

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Empirical Formula

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Ratio of the atoms of each element.

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Electron Configuration

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A method of showing how many electrons an element has by means of orbitals.

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S

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2

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P

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6

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D

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10

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F

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14

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Lewis Structure

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A drawing which shows the sharing of electrons between elements in a covalent compound.

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Mole

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The number of atoms of each element present in a molecule.

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Boyle's Law

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k=PV

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Charles' Law

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k=v/t

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Gay-Lussac Law

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k=p/t

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Ideal Gas Law

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PV=nRT

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Combined Gas Law

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PV=kT

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R

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.082 L*atm/mol*k

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Percent Yield

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The percent of the calculated yield versus the actually obtained amount.

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Limiting Reactant

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The reactant that determines how much of a product can be formed.

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Acid

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A substance that has to do with hydrogen ions.

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Base

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A substance that has to do with hydroxide ions.

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pH

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Power of Hydrogen or the strength of an acid or base.

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Salt

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A neutral precipitate formed.

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Neutralization Reaction

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A reaction in which an acid and a base cancel each other out.

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Redox Reaction

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A reaction in which electrons are transferred among elements.

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Precipitate Reaction

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A reaction in which a solid precipitate is formed.

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Precipitate

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An insoluble solid at the bottom of water.

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