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ADV CHEM

Unit 2- Atoms test - 10/10

TermDefinition
Democritus thought there was a limit to how many time you could cut something in half. everything was made of small particles
atomos (greek) indivisible
Law of Conservation of Mass matter is neither created nor destroyed (same # before and after physical or chemical change)
Antoine Lavoisier founded Law of Conservation of Mass
Law of Definite Proportions elements that compose compounds are always in a certain proportion by mass (if you had 2 hydrogen and 1 oxygen you would only ever get H2O, and if you didn't have those then you would never get H2O)
Joseph Proust founded Law of Definite Proportions
John Dalton First to use experiments. Billiard ball model, Atomic theory
Billard Ball Model model of an atom, viewed as a small solid sphere
Atomic Theory All matter is atoms All atoms of 1 element are exactly alike atoms are indestructible and cannot be divided atoms of diff elements simple whole-number rations to form chemical compounds chemical reactions, atoms are combined, separated or rearranged
electron a subatomic particle that has a negative charge
J. J Thomson founded the electron using the cathode ray experiment, formed the plum pudding model
Plum Pudding Model electrons sitting on a positive charged plate
Rutherford's Gold Foil Experiment shot alpha particles to gold foil and the bounced off the nucleus of the gold
conclusions of Gold Foil Experiment atoms were mostly empty space most of the mass was concentrated in the center region, the atomic nucleus is where the proton is found
protons positively charges particles, found in nucleus
neutrons the particles of the nucleus hat have no charge, found in the nucleus
atomic number represents the number of PROTONS there are in an atoms, also represents the number of ELECTRONS in a neutral element
ions atoms or groups of atoms that carry a positive or negative charge as a result of gaining or losing one or more electrons
Isotopes atoms of the same elements that have different numbers of neutrons
atomic mass weighted average of the isotopes
mass volume and mole relationship mass- molar mass/ 1.00 mole volume- 1.00 mole/ 22.4 L Atoms/ Molecules- 1.00 mole/6.022 x 10 ^23
cathode ray experiment stream of electrons with positive plates on top and bottom
Fredrick Soddy Discovered Isotopes
mass number (mass number is MASSIVE) the count of total protons and neutrons in a atom's nucleus (P+N)
nuclear symbol subscript ^ indicated the mass number and the subscript (under) indicated the atomic number
Dalton's Atomic Theory Revised Elements are made of extremely small particles called atoms atoms can have different mass (ions) can be divided into subatomic particles law of Conservation of Mass Law of Definite Proportions
Amedeo Avogardo discovered how many particles are in a given amount of gas (the mole)
Avogardo's Number 6.022 x 10^23
molar mass mass of grams in one mole of atoms or molecules (g/mol)
mole to atoms (molecules) 6.022 x 10^23 = 1 mole
hydrate a compound that absorbs water molecules from its environment that included them in their structures
1 mole of any gas at STP 22.4 L
Atom the smallest particle of an elements, but still has properties of that element
small deflection ___↗.
wide deflection ___↖.
changes made to the Atomic Theory Atoms of a given elements are identical in size mass and other properties. atoms cannot be subdivided
What part of Dalton's Atomic Theory was supported by the Law of Definite Proportion atoms are different elements can combine to form simple whole- number ratios to form chemical compounds
What part of Dalton's Atomic Theory was supported by the Law of Conservation of Mass In chemical reactions, atoms are combines, separated, or rearranged
Created by: stella_koe
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