Chemistry Midterms Flashcards

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Matter

Everything that makes up the physical universe.

Atoms

Tiny discrete particles that make up matter.

Solid

Incompressible state of matter with its own shape and high density.

Liquid

State of matter that flows freely, takes the shape of its container, and has no definite shape.

Gas

State of matter with particles that are far apart and bounce against each other, takes the shape of its container, and has low density.

Plasma

State of matter made of positively and negatively charged ions, formed by heating and ionizing gas.

Bose-Einstein Condensate

Cloud of bosons cooled to temperatures close to absolute zero, where some of it condenses.

Physical Properties

Observable characteristics of matter without changing its composition, such as phase, color, solubility, density, melting and boiling points, volatility, viscosity, and conductivity.

Chemical Properties

Observable characteristics of matter that involve a change in chemical composition, such as flammability and combustibility.

Intensive Properties

Properties of matter that depend on the type of matter, such as density, color, phase, melting and boiling points, and thermal conductivity.

Extensive Properties

Properties of matter that depend on the amount of matter, such as mass, length, size, and volume.

Pure Substance

Matter with a specific composition

Element

only one kind of atom

Compounds

two or more elements chemically combined

Mixture

Different pure substances that are physically combined.

homogenous mixture

thismixture has auniform appearance

heterogeneous mixture

this mixture’s substances can be distinguished from one another

Crystallization

Physical method of separating mixtures by extracting pure crystals from impure mixtures.

Evaporation

Physical method of separating mixtures by heating to separate dissolved solid from liquid.

Distillation

Physical method of separating mixtures by vaporization to separate two liquids with different boiling points.

Filtration

Physical method of separating mixtures by using filters to separate solids from liquids.

Decantation

Physical method of separating mixtures by slowly pouring the liquid, leaving the sediments.

Magnets

Physical method of separating mixtures by separating magnetic from non-magnetic substances.

Sublimation

Physical method of separating mixtures by separating volatile from non-volatile substances.

Chromatography

Physical method of separating mixtures by using a moving and stationary fluid to separate substances with different solubilities.

Molecules

Atoms that are chemically bonded to form a stable and electrically neutral entity.

Isotopes

Atoms of the same element with the same number of protons but different number of neutrons.

Ions

Electrically charged particles formed when atoms gain or lose electrons.

Law of Conservation of Mass

The mass of the substances in a chemical reaction is equal to the mass of the reactants.

Law of Definite Proportions/Composition

A compound will always be made of the same elements in the same amount.

Law of Multiple Proportions

Elements that can form different compounds are in small whole number ratios.

4 statements of Dalton's Atomic Theory

matter is made up of atoms

Matter is made up of atoms of the same element are identical but different from those of other elements

compounds are formed when atoms of different elements combine in certain whole number ratios

atoms rearrange only during a chemical reaction to form new compounds

Electron

A subatomic particle with a negative charge

Joseph John Thomson

he discovered the electron in 1987

Proton

A subatomic particle with a positive charge

Ernest Rutherford

discovered proton in 1920

Neutron

A subatomic particle with no charge, discovered by James Chadwick in 1932.

James Chadwick

Discovered neutron in 1932

Cathode Rays

Rays of electrons emitted from the cathode in a vacuum tube.

Wilhelm Conrad Roentgen.

discovered X-ray

X-ray

A type of electromagnetic radiation discovered by

Radioactivity

The property of certain elements to spontaneously emit radiation

Henri Becquerel

studied radioactivity

Gold Foil Experiment

An experiment conducted by Ernest Rutherford in 1911 that led to the discovery of alpha and beta rays.

Atomic Number

The number of protons in an atom, discovered by Henry Moseley in 1913.

Isotopic Symbol

A symbol used to represent an isotope of an element, consisting of the element's symbol, atomic number, and mass number.

Ionic Compound

A compound formed by the transfer of electrons between a metal and a non-metal.

Cation

A positively charged ion, typically formed by a metal atom.

Anion

A negatively charged ion, typically formed by a non-metal atom.

Metal Ions

Ions formed by metals, named after the metal's name (e.g., Na+ is called sodium).

Transition Metals

Metals that can form multiple ions, named using either the classical method (lower:-ous; higher:-ic) or the stock method ([element] [charge in roman numerals]).

Non-metal Ions

Monoatomic ions formed by non-metals, named with the suffix -ide (e.g., Br- is called bromide).

Non-metal Polyatomic Ions

Polyatomic ions formed by non-metals, named with the suffixes -ite (lower O) or -ate (higher O) (e.g., NO2- is called nitrite, NO3- is called nitrate).

Halogens

Elements in Group 17 of the periodic table that can form polyatomic ions with oxygen.

Ternary Polyatomic Ions

Polyatomic ions composed of three elements, named with the prefix bi- or Greek prefixes for the number of hydrogen atoms (e.g., CO32- is called carbonate, HCO3- is called bicarbonate).

Hydrated Salts

Ionic compounds that contain water molecules, named with the prefix -[greekprefix]hydrate for the number of water molecules (e.g., CuSO4 is called anhydrous copper(II) sulfate, CuSO4 · 5H2O is called copper(II) sulfate pentahydrate).

Acids

Substances that give off hydrogen ions when dissolved in water, named using the prefix hydro- and the suffix -ic acid for the anions (e.g., HCl is called hydrochloric acid).

Greek Prefixes

Prefixes used to indicate the number of atoms in a polyatomic ion (e.g., mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-).

Classical Polyatomic Ions

Polyatomic ions named based on the no. of O atoms, with lower and higher endings (-ous and -ic) (e.g., Cl2- is called chlorite, Cl3- is called chlorate).

Stock Polyatomic Ions

Polyatomic ions named using the element's name and the charge in roman numerals (e.g., Fe2+ is called ferrous iron(II), Fe3+ is called ferric iron(III)).

cupr-

root word of copper

aur-

root word of gold

ferr-

root word of iron

plumb-

root word of lead

stann-

root word of tin

carb-

root word of carbon