Physical Changes

Changes without changing its chemical composition
(condense, freeze, melt, dissolve, grin, change in state)

Chemical Changes

When 1 or more substances change into new substances
Chemical compostion changes
Chemical Reaction
(change in odor, gas, precipitate, energy light, heat, color change)

Physical Property

observed without changing chemical compostion
(boiling point, melting point, solubility, color, odor, hardness, density)

Chmical property

ability to undergo a chem reaction
(flammable, rusting, not reacting)

Law of conservation of mass

matter is neither created no destroyed

Elements

a pure substance that can not be broken down into simpler substances

Compounds

pure substance made from atoms of 2 or more different elements that are chemically bonded (H20)

Dalton's Atomic Theory

1. All matter is made of atoms that are indivisible and indestructible
2. All atoms of a given element are identical in mass and properties
3. Compounds are formed by a combo of 2 or more different kinds of atoms
4. Chemical reactions rearrange atoms

Structure of an Atom

Nucleus: Made of protons and neutrons (In the center)
Electrons: Orbit around the nucleus in specific energy levels

Godl foil Experiment

ERnest Rutherford shot positively charged particles (alpha particles) at a thin piece of foil and some went right through while some reflected back
Conclusions:1. most of an atom is empty space 2. atoms have a nucleus (small dense core with a positvie charge)

# of protons=

atomic # and # of electrons

atomic # =

# protons and # electrons

Mass #=

# protons + # neutrons

Isotopes

forms of the same atom that vary in mass and have a different number of neutrons (common to al elements-not all natural)

Hyphen Notation

Cu-63 (63=mass)

Nuclear Symbol

63 CU
29 (63= mass 29 = atomic #)

Quantum Mechanical Model

(Schrodinger) Quantum- the amount of energy required to move an electron from its present energy level to the nest higher one
-Mathematical formula to describe the probability of finding electrons within a certain space

Energy level

(Floors) region aroudn teh nucleus where the electron is likely to be moving n= 1, 2, 3, 4, etc

Sublevels

(Rooms) each energy level is broken up into sublevels
# of sublevels= # of quantum for that energy level

Orbitals

(Beds) 2 electrons per bed
S-Spherical shaped
P-Dumbell Shaped
D-Clover shaped
F-too complex

Democritus

believed that matter was composed of atoms based on mental reasoning

John Dalton

believed atoms were solid and indivisible mass based on research

J.J Thomson

(plum pudding)discovered the electron, electrons stuck into a lump of positively charged material- didnt know specifics

Ernest Rutherford

Most of an atoms mass is concentrated in a small positively charged region called the nucleus

Neils Bohr

electrons orbit around the nucleus

Quantum Mechanical

Erwin Shrodinger- based on math- where the electrons are located

DeChancourtois

fully functioning periodic table on a cylinder

Canizaro

atomic mass

Mendeleyev

periodic table

Mosley

arranged table based on mass

Seaborg

Final version of the table

Light

Little packets of photons

Wavelength (h)

Visible light ahs a h of 700-750 nm
1nm = 1 x 10-9 m

Frequency

v

Velocity (C)

C=hv
Light travels throgh space at 3.00 * 108 m/s

Calculating energy of a photon

E=Hv
E= energy
H- Plancks constant= 6.662 * 10-34 Js
v= frequency

Brightness of a light depends on...

Amplitude

Ionization energy

energy required to remvoe an electron from an ion or atom

Electronegativity

low to high
amount of pull that an atom's nucleus exerts on another atom's electrons when they are bonded

Atomic Radius

an atom's size depending on the volume occupied by electrons around the nucleus

Octet Rule

atoms will have 8 valence elctrons

Chemical Bond

bodnign together of atoms due to an electrical attraction between the nuclei and valence elctrons (ionic and covalent)

Ionic bonds

attraction of ions in which atoms completely give up electrons to other atoms (cations+anions)

Ionic compound

combination of a metal cation and a non-metal anion in order to establish a stable, neutral compound

Cation

Positive charge (metals)

Anions

Negative charge (nonmetals)

Monoatomic Ion

Made up of one type of atom

Polyatomic Ion

Tightly bound group of atoms that act as a whole and have a charge- NH4

Calculating cation charge

1.Find the charge of the anion
2. Multiply the charge of anion by the subscript of the anion
3. Divide by the subscript on the cation

Covalent compounds

bonds form so atoms can be stable

Covalent bonds

forms from the sharing of one or more pairs of electrons

Non-polar covalent

Bonding electrons are being shared equally between the bonded atoms

polar covalent

shared pair of electrons is held more closely by one fo the atoms
-electrons closer to atom with higher electronegativity

Dipole

a molecule that has a positvie end and a negative end

Lewis Dot structure

Add together total number of valence electrons

Avogadros #

1 mole = 6.022 * 10 23

Molar Mass

mass in grams of 1 mole of a substance

Percent composition

Molar Mass of element *10
Molar mass of compound

Empirical formula

shows the simplest ration for elements
1. Conver % to grams
2. Convert grams to mol
3. Subscripts to whole number (divide by lowest)
(If its still not whole number mulitply by whole numbers)

Molecular formula

a whole number multipe of an empirical formula

Synthesis

A+B= AB

Decompostion

AB = A + B

Single Displacement

AB + M = MB + A

Double Displacement

AB + CD = AD + BC

Combustion

CxHyO2 = CO2 + H20

Diatomic

Br I N Cl H O F

Stoichiometry

use of reactatnts and products to perform calculations

Actual yield

measured amount of a product obtaienc from a reaction

Theoretical

max amount of product that can be produced in a given reaction

Limiting Reactant

1.convert both reactants to grams of the same product
2. Identify the L.R (one that produces least amount of product)

Kinetic Molecular Theory

1. used to predict gas behavior
2. states gas particles are in constant motion

Solvent

dissolving medium

Soute

what is being dissolved

Hydrogen Bond

bond between hydrogen and dipole

London dispersion

al the electrons are on one side and it is a temporary dipole

Dipole-dipole

like a battery

Heterogeneous Mixture

not uniform throughout, composed of dissimilar things, can be seperated

Homogeneous Mixture

uniform composition or structure throughout, same proportions throught can not be filtered

Suspension

particles are initially dispersed but will eventually settle out (Hetero)

Solution

Particles are dispersed throughout (homo)

Colloid

gas dispersed in liquid (particles are intermediate in size betweeen those of solutions and suspensions (S, L, G)

Electrolyte

a substance that dissolves in a liquid solvent and provides ions that conduct electricity

non-electrolyte

does not allow an electric curret to move through (no ions)

Saturated

Can not dissolve any more solute under conditions

Unsaturated

solution with less solute then the saturated solution-can dissolve more

Super Saturated

A soluton with more dissolved solute than a saturated and cannot dissolve more

Boiling Point Elevation

dissolved salt raises the boiling point causing water to boil at a higher temp

Freezing Point Depression

dissolved salt lowers the freezing point

Colligative Property

a property of a substance that is determined by the number of particles present in the system but independent of the properties of the particles themselves- the degree of the effect depends on the concentration

Reversible Reactions

products reform into the original reactants

Neutralization

Occurs when H30 and OH react to rofm H20 and salt

Equivalence Point

point at which neutralization reaction is complete

Titration

gradual additon of one solution to another reach teh equivalence point

self ionization

when a pair of H20 molecules are in equilibrium