Pure substance of one type of atom.

Example: diamond, O2

anything made of multiple elements bonded together.

Ex: H2O, CO2

Change according to the amount of matter. 

Examples: weight, mass, volume, surface area.

Do not rely or change as the amount of matter changes.

Examples: luster, boiling point, melting point, color, taste, density.

Something observed without changing identity.

Examples: 5 states of matter(gas, liquid, solid, plasma), freezing/melting point, temperature, dissolving, shredding, cutting down a tree, solubility, density.

Substances ability to undergo change into a new substance.

Examples: oxidizing(rusting), burning, cooking is always a chem reaction, rotting/decomposing.

blend of 2 or more kinds of matter which retains their original properties/identity.

"uniform in composition," evenly mixed a.k.a. solution.

Examples: sugar water, salt water, mayo, coke, birdseed, italien dressing (only if it is physically seperated into being homogeneous!!!!)

"not uniform in composition." Can physically seperate to become homogeneous!

Examples: salde, water and oil, italien dressing (note from homogeneous!) 

fixed composition, different from mixtures:

1. all samples have identical properties (behaves same)

2. all samples have identical compositions (same chemical makeup)

note: cannot vary at all

length-meters

mass-kilograms

time-seconds

amount of substance-moles(n)

temperature- Kelvin (K)

kilo-kg-10^3   1000g=1kg

deci-dg-10^-1  10dg=1g

centi-cg-10^-2   100cg=1g

milli-mg-10^-3   1000mg=1g

micro-ug-10^-6   100000ug=1g

nano-ng10^-9   1000000000ng=1g

Qualitative: descriptive

Quantitative: numerical

PE= absolute value of TY(theoretical yield) - AY(actual)

over TY multiplied by 100

PY= AY over TY times 100

1st Atomic Theory combined of 5 postulates and 3 laws:

-Law one: law of conservation of mass. Mass cannot be created or destryed.

-Law two: law of definite proportions. If you break a chemical apart it will be the exact same pieces combined in the exact same way.

Law three: law of multiple proportions. Having no half atoms, must have whole number ratio's.

5 postulates:

1. all matter is made of tiny particles called atoms.

2. atoms of a single element are identical in size, mass, and properties; atoms of different elements difeer in size, mass, and properties.

3. atoms cannot be subdivided or destroyed.

4. atoms of different elements combine in whole number ratios

5. chemical reactions= atoms are combined, seperated, or rearranged.

NOTE:one of the postulates that is not considered true today is that atoms are indivisible

He said that all atoms of a given element are alike.

This is not true due to the existence of isotopes.

Isotopes are atoms of the same element that have

different masses because they have different

numbers of neutrons.

During a chemical reaction, atoms can change their identities

uses cathode ray to discover negative parts of the atom.

Plum Pudding Model

a form of energy that exhibits wave-like behavior as it travels through space. 

ex:gamma rays extremely high, but radio waves are low.

Frequancy is the amount of ways in a certain time.

C=λν; C=speed of light (3.00x10^8 m), λ=wavelength measured in nm, ν=frequency

E=hν; E=energy, h= Plancks Constant (6.626x10^-34 J/s), ν=frequency

GS= normal, flat energy level 

ES= high energy

3D region around nucleus where an electron probably is found.

specific properties of orbitals and properties of electrons is orbitals.

1. Principle Quantum #: n, 1 to infinity, main energy level

2. Angular Momentum Quantum #: l , n-1 to zero, sublevel (s=0, p=1, d=2, f=3) s is 1 orbital, p is 3 orbitals, d is 5 orbitals, f is 7 orbitals (one orbital holds 2 electrons)

3. Magnetic Quantum #: m_{l is -l to l}

4. Spin Quantum: s +1/2 and -1/2 spin of an electron

n=row number

l= block type (s=0,p=1,d=2,f=3)

m_{l= column in block (ex -1, 0, 1 for if l=p) (-l or l)}

s=spin (-1/2 if arrow is down, +1/2 if arrow is up)

the amount of particles required to have 12g of Carbon-12

6.02x10^23 parts over 1 mol

 parts can equal atoms, molecules,or some other tiny particle.

the mass of one mole of a pure substance 

MM=g/mol

periodic table measured in g/mol