IPC FINALS

Matter

Anything that takes up space and has mass

Substance

Matter with a composition that is always the same

Solution

Homogenous Mixture

Solvent

substance that exists in the greatest quantity in a solution

Solute

any substance in a solution other than the solvent

Physical Property

a characteristic of matter that you can observe or measure without changing the identity of the matter

Solubility

the maximum amount of solute that can dissolve in a given amount of solvent at a given time and pressure

Malleability

the ability of a substance to be hammered or rolled into sheets

Luster

they way a mineral reflects or absorbs light at its surface

Conductivity

the ability of matter to conduct, or carry along electricity or heat

Magnetism

attractive force for some metals, especially iron

Ductility

the ability to be pulled into thin wires

Mixture where the composition is uniform

homogenous mixture

Mixture where the composition is not uniform

heterogenous mixture

Matter that can be physically separated

mixture

Matter that cannot be physically separated

pure substance

pure substance that can be chemically decomposed

Compound

Pure substance that can’t be chemically decomposed

element

Chemical property

the ability or inability of a substance to combine with or change into one or more new substances

the ability of a substance to burn; ability of a substance to rust

examples of chemical properties

bubbles; change in color; change in odor; formation of a precipitate; change in temperature; release of light

observations that show a chemical reaction took place

Melting + Freezing

Physical property

Tearing; crushing

physical property

Hardness; texture; shape

physical property

rusting; flammability; burning; sourness

chemical property

a substance that consists of only one type of atom

Element

Atom

small particle that is the building block of matter; the smallest piece of an element that still represents that element

Protons, neutrons, electrons

Parts of an atom

Molecule

two or more atoms that are held together by covalent bonds; act as a unit

Compound

a substance containing atoms of tow or more different elements chemically bonded together

Chemical Formula

group of chem. symbols and numbers that represent the elements and the numbers of atoms of each element that make up a compound

Subscript

the small # after a chemical symbol; shows the number of atoms of each element in a compound

Coefficient

a # placed in front of an element symbol or chemical formula in an equation

Viscosity

a measurement of a liquid’s resistance to flow

Melting

solid to liquid

Freezing

liquid to solid

the 2 types of vaporization

evaporation an boiling

Vaporization

liquid to gas

condensation

gas to liquid

deposition

gas to solid

sublimation

solid to gas

the 3 important factors which describe gas behavior

temperature; volume; pressure

Gay Lussac law

increase in temp= increase in pressure

Charles Law

increase in temp.= increase in volume

Boyles Law

increase in pressure= decrease in volume

John Dalton

created the first atomic theory + saw the atom as a ball

J.J. Thomson

discovered electrons; developed the raisin bun model

Ernest Rutherford

discovered the nucleus+ protons through his gold foil experiment

Niels Bohr

created the planet model

James Chadwick

discovered neutrons

Erwin Schrodinger

created the Electron Cloud Theory

Mendeleeve

Creator of the periodic table

Marie Curie

studied radioactivity; discovered polonium and radium

Atomic number

is equal to the number of protons

Atomic mass

is equal to the number of protons + neutrons

The number of protons

is equal to the number of electrons

Valence Electrons

the outermost electrons of an atom that participates in chemical bonding

Isotope

atoms of the same element that have different numbers of neutrons

Metals

shiny; conduct thermal energy and electricity, luster, ductile, malleable, almost all re solids; dense; strong; boiling and melting points are much higher

non metals

gases; do not conduct thermal energy and nonmetals

metalloids

have properties of both metals and nonmetals

alkali metals

react quickly with other elements, nature= only occur in compounds, silvery appearance, low densities

alkali earth metals

react quickly, but not as quick as alkali metals, form compounds, soft and silvery, low density

Halogens

react readily with other elements, form compounds

Noble Gases

only react with other elements in a lab

Radioactive Decay

atomic nuclei of radioactive isotopes release fast moving particles and energy, causing the identity of an atom to change to produce a new element

Nuclear reactions

involve the particles of the nuclei of an atom

the 2 types of nuclear reactions

fission and fusion

Alpha decay

nucleus gives off an alpha particle which is 2p and 2n. Decreases the original nucleus by 2p and the atomic # by 2. It also decreases the mass number by 4

Beta Decay

a neutron in an unstable nucleus changes into a negatively charged beta particle and a proton. The beta particle is a fast moving electron given off by the nucleus. The new proton remains in the nucleus, which is left with one less N, and one more P

Gamma Radiation

produced along with alpha and beta decay. High energy rays similar to x-rays

Proton

a positively charged particle

Atom

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

Atomic Mass

Total number of protons and neutrons

Electron

a negatively charged subatomic particle that weighs almost nothing

Mendeleev

Creator of the Periodic Table of Elements

Isotopes

Atoms with the same number of protons but with a different number of neutrons

Atomic #

The number of protons in the atom

Alpha particle

2 protons and 2 neutrons emitted from a nucleus during radioactive decay

nucleus

the central part of an atom which contains protons and neutrons

neutrons

a subatomic particle with no charge

Dalton

He proposed the first Atomic theory and said the atom looked like a ball

Thompson

he proposed the raisin pudding model of an atoms and discovered the existence of an electron

Bohr

said that electrons move in orbits around the atom’s nucleus like moons around planets

Marie Curie

Won Nobel prize for discovering radioactivity

Rutherford

He discovered the dense nucleus of the atom and the existence of protons with his gold foil experiment

Luster

The way that a surface of a mineral reflects light

Fission

when a nucleus breaks apart, releasing energy

Chadwick

Discovered the neutron

Ionic

between non metals and a metal

Covalent

between 2 nonmetals

cation

positively charged ion

anion

negatively charged ion

ionic bonds

transfer valence electrons

covalent bonds

share valence electrons

Polar

unequal sharing of electrons; partially positive and partially negative

nonpolar

equally sharing of electrons

Diatomic Molecules

2 atoms of the same element bonded together

chemical reaction

a process in which atoms of one or more substances rearrange to form one or more new substances

reactant

a starting substance in a chemical reaction