Accuracy

How close the value is to the true value

Precision

Consistently repeated measurements with each other

Percent error

((Observed - theoretical) / theoretical) * 100

Democritus

Atoms Cheese separation

John Dalton

Modernized the atom Sphere atoms

JJ Thomson

Discovered the electron through the Cathode ray tube experiment. Discovered that the atom is a mass of protons with negative pockets.

Ernest Rutherford

Discovered the nucleus Gold foil experiment Created the nuclear model, electrons orbiting the nucleus

Robert Millikan

Discovered mass and charge of the electron Opposites attract Oil drop experiment Electrons have negligible mass

Neils Bohr

Discovered the shells and wavelengths Each shell has a higher energy level Energy levels

Heisenberg and Schrodinger

Quantum model Determined the mathematical probability of an electron's position in any energy level. "The more you know where an object is, the less you know about its movement"

James Chadwick

Discover that protons and neutrons reside in the nucleus.

Protons

Determine the identity of an element

Electrons

Responsible for atom behavior

Neutrons

Stabilizes nucleus

Atomic Number

Number of protons in nucleus top left

Mass Number

Total number of protons and neutrons

Average Atomic Mass

Average of naturally occuring isotopes Bottom line

Number of neutrons =

Mass # - atomic #

Nuclear force

Stongest force Keeps nucleus together

Weak nuclear force

Prevents protons and neutrons from changing/switching identities

Electromagnetic force

Keeps electrons from being expelled from the atom weakest

Planks constant term

6.626x10^-34

Speed of light term

3.0x10^8 m/s

Multivariable energy equation

E = (Planks constant x Speed of light)/wavelength

Wave energy equation

E = (planks constant x Light frequency)

Particle equation

E = (particle mass x Speed of light^2)

Speed of light equation

C = (Wavelength x Light frequency)

Ultraviolet light

High energy Short wavelength High damage

Infrared (red) light

Low energy High wavelength Low damage

Isotopes

dif masses, dif neutrons

Isotope Name

Element-mass #

Isotope Symbol

Mass # top left, Element Symbol, atomic # bottom left

Fusion

2+ elements into 1 Creates more energy than what's used to start it

Fission

Big atom split into more Splits rapidly Fast reactions Power a lot but requires energy to start Hit with neutron (n)

Alpha Decay

Unstable atomic nucleus Decreases atomic number by 2 and mass number by 4 only be product

Beta Decay

High energy neutrons Neutron in nucleus turns into a proton Atomic number +1 Mass in unchanged

Fusion etc.

Positive protons Positive neutrons E ++++

Fission etc.

Negative proton Negative neutron E +++ important particle: n

D-Decay etc.

-2 protons -2 neutrons 4, He, 2

B-Decay etc.

+1 protons -1 neutrons o, e, -1

Aufbau's Rule

Lazy electron Fill in the lowest orbital first

Pauli's Exclusion Principle

No twins rule Can't occupy the same space at the same spot

Hund's Rule

Electrons must fill in individually, in the same direction Before making pairs Single before taken

Nobel gas notation

Stable Nearest nobel gas [element] Period (block) ^position in block

Abbreviated notation

Period (block) position

Orbital notation

The lot of arrows one

Electron Configuration

Describes the position and direction of electrons Orbital then # in

Quantum Theory

n = energy levels. The higher the n value, the greater the energy and distance from its nucleus. Numbers and letters are used to describe the pattern and position of electrons

Cation

Metals that shed valence electrons to become stable Positive

Anion

Non-metals that gain valence electrons to become stable

ductile

Can be pulled into wires Electricity

Substitutional Alloy

Some metallic atoms have been replaced with another metallic atom and form together

Interstitial Alloy

Smaller metallic atoms in-between larger metallic atoms

Exothermic

Heat is released from the reaction to the surroundings. Yields heat

Endothermic

Heat is absorbed from the surroundings. Heat in reaction

Covalent bond

When 2 atoms share a pair of electrons Share shells Ends in -ide

VSEPR

Valence Shell Electron Pair Repulsion

Lewis structure

Lines and dots between and surrounding a molecule. Dots - available valence Lines - connection (one line counts as 2

Octet Rule

Happens in covalent bonds. Provides each atom with its desired electrons, which is usually 8.

Resonance

When a covalent bond has multiple positions as to where a double bond can be placed.

Formal Charge

# Valence Electrons - # Bonds - # Nonbonded Electrons Used to estimate the distribution of electric charge Priority over Octet Rule The lower the formal charge, the better

Synthesis

Two or more substances react to form a single new substance

Decomposition

A single compound breaks down into two or more substances

Combustion

Chemical compound reacting with Oxygen to yield heat/light. Water and carbon dioxide are the products

Oxidation

Process in which an atom or ion loses electrons

Reduction

Process in which an atom or ion gains electrons

Redox

An exchange of electrons among elements in a reaction Single replacements LEO GER

Avogadro's Number

6.02x10^23 particles/mole

ICE table

Initial amounts of moles Change based on mole ratio Ending amount Find x by setting it equal to 0 (mols - x = 0)

Solute

Substance BEING dissolved Salt

Solvent

Substance DOING the dissolving Water

Unsaturated

Not enough solute to reach pure saturation

Saturated

Solvents available space is taken up by the solute

Supersaturated

More solute than the solvent can hold

Colloid

Solutions with medium-sized particles Scatters light

Suspension

Solute will settle if not agitated because of the big particle size

Serial Dilution

Equal increments of concentration change in each dilution

Bronsted-Lowry Acid

Donates protons

Bronsted-Lowry Base

Accepts protons

Indicator

A substance that allows a color change when a titration is completed

Titration

Used to find an unknown concentration by adding a known acid to an unknown base. Equivalence and end point must be as close as possible.

Equivalence point

Two chemicals in a titration are in equal amounts to one another. All acids concerted to conjugate base

End point

The point when the indicator changes color

Titration curve

Y=pH X=Titration volume

Molar Mass (g/mol)

Sum of the average atomic masses for all atoms in a molecule

Group / family

Columns of a periodic table Verticle Those elements share the same number of valence electrons

Period

The rows of a periodic table 1 2 .... 7

Metalloid

Between metals and non-metals. In the form a staircase

Energy Level

Represented as n Top to bottom of periodic table Shells from inner to outer Electrons allowed = 2n^2

Block

The orbit pattern of an atom S - H, He, first 2 groups. Spherical pattern D - Transition metals, set as 1 less row like usual, clovers P - Right of table, dumb bell shaped. F - Separated bottom section, set as 2 rows less than usual, complex shapes.

Atomic Radius

Size of atom High radius in bottom left Low radius in top right (more protons in the nucleus means a stronger connection to nucleus)

Electronegativity

The ability to attract electrons Increases top right Decreases bottom left Same as ionization energy

Charge

How close something is to reach a stable level/closest nobel gas

ionization Energy

How difficult it is to take away an electron More difficult top right less difficult bottom left Same as electronegativity

Metallic character

Tendency of an atom to lose electrons Easier to lose bottom left harder to lose top right Opposite of ionization and electronegativity

Rule of Net Zero

Ionic Bonds - Form compounds with neutral charge

Electrostatic Attraction

A force that pulls in particles with opposite electric charges. Usually between a cation and an anion

Conductive

How well an atom conducts electricity when dissolved.

Flame Test

A way to determine unknown metallic ions Excites the electrons to jump energy levels

Lucky 7

7 diatomic particles H, N, O, F, etc.

Covalent Bond steps

Symbol, Prefix from subscript, repeat

Lewis Structure steps

Find valence electrons, center element has the lowest electronegativity, connect one line to each element, find initial amount needed then go from there, and make sure each atom follows octet and have the lowest formal charges.

Polyatomic Atoms

Composed of multiple atoms held together by covalent bonds. Singular unit with brackets and charge # total electrons = Total valence - charge

Non-polar bond

Electrons are even shared between atoms Atomic e-neg difference LESS than 0.5

Polar bond

Electrons are not evenly shared between atoms Atomic e-neg difference is GREATER than 0.5

Polar ionic bond

Electrons are not shared between atoms Atomic e-neg difference is GREATER than 1.7

VSEPR chart steps

Find bonding regions, find nonbonded electrons, locate on chart

Molecular Polarity

How a molecule behaves chemically as it is being dissolved

Molecular Polarity checks

At least 1 polar bond Molecule is asymmetrical

Polarity

Atoms with a higher electronegativity attract more bonds and is more negative than its lesser atom.

Ionic polarity

A big difference in electronegativity causes the higher atom to have the "winner takes all" situation, stealing the electrons from tis lesser counterpart.

Ionic Bonds

Metal and a non-metal

Ionic Bond properties

Brittle solids Conductive when dissolved Soluble in water High melting and boiling point BECAUSE of multidirectional attraction

Ionic naming

Cation (base name anion) -ide

Transition Ionic Naming

Cation (Cation charge in roman numerals) base name anion -ide

Ionic Substance forms

Solid or Aqueous

Covalent Substance forms

Solid, Liquid, Gas, Aqueous, etc.

Metallic Substance forms

Usually solid except for mercury

Activity Series

One metal will replace another if it is more reactive: Halogens decrease activity as you go down Single replacement and Double replacement Top elements increase in oxidation

LEO

Lose Electrons -> Oxidation

GER

Gain Electrons -> Reduction

Acid and Base reactions

Always yield water and salt Both have neutral pH levels

Endothermic energy

High activation energy Energy absorbed More product made

Exothermic energy

Low activation energy Energy released Little product made

Endo or Exo? Melting Ice

Endothermic because it requires heat and energy is absorbed

Endo or Exo? Combustion

Exothermic because heat is released

Endo or Exo? Photosynthesis

Endothermic because heat is absorbed to create energy

Endo or Exo? Cellular respiration

Exothermic because heat and energy are released by reactions

Finding limiting reactant

1. Balance if needed 2. Convert reactants to moles 2. find mole ratios 3. ICE table

Binary Acids

H(anion) Hydro (anion) -ic acid

Oxyacids (polyatomic)

Hydrogen, Oxygen, Anion Ends -ate, turns to -ic Ends in -ite, turns to -ous

Lewis Acid

Accepts electron pair

Lewis Base

Donates electron pair

General Acid info

Corrosive to metal Sour Conductive

General Base info

Caustic (Corrosive to organic matter) Bitter Slippery

Weak base/acid

Doesn't separate (dissociate)

Strong base/acid

Does separate (dissociate)

[H+] to pH

-log[H+]

pH to [H+]

antilog - pH

[H+] to [OH-]

Kw/[H+]

[OH-] to [H+]

Kw/[OH-]

Kw

[H+] [OH-] (=1.00x10^-14)

[OH-] to pOH

-log [OH-]

pOH to [OH-]

antilog [OH-]

Molarity

mol/L

Dilution equation

M1V1 = M2V2

Neutralization calculations

MaVa = BaVa

Boyle's Law

Pressure (X), and Volume (Y). As pressure increases, volume decreases. Inversely proportionate.

Charle's Law

Temperature (X) and Volume (Y). As temperature increases, volume increases. Linear

Gay-Lussac's Law

Temperature (X) and Pressure (Y). As temperature increases, pressure increases. Linear

Boyle's Equation

P1V1 = P2V2

Charle's Equation

(V1/T1) = (V2/T2)

Gay-Lussac's Equation

(P1/T1) = (P2/T2)

Combined Gas Law Equation

(P1V1)/T1 = k

Ideal Gas Law

P(atm)V(L) = n(moles)R(0.082114L*atm/K*mol)T(K)

Which blocks are different?

D block has 1 less row F block has 2 less row

Special Formal Charge elements

H: 1 bond O: 2 bonds N: 3 bonds C: 4 bonds