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ADV CHEM
Unit 2- Atoms test - 10/10
| Term | Definition |
|---|---|
| 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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