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| 14679840936 | Law of Conservation of Mass | Mass is neither created nor destroyed in chemical reactions | 0 | |
| 14679843169 | Law of Definite Proportions | -A given compound always contains exactly the same proportion of elements by mass -Ex, Copper Carbonate is always 5.3 part copper, 4 parts oxygen, and 1 part carbon | 1 | |
| 14679844658 | Law of Multiple Proportions | -When two elements form a series of compounds, the ratio of the masses of the second element that combine with 1 gram of the first elements can always be reduced to whole numbers | 2 | |
| 14679848579 | Dalton's Atomic Theory | 1. Each element is made up of atoms 2. The atoms of a given element are identical 3. When atoms of different elements combine, chemical compounds are formed. A given compound always has the same relative numbers and types of atoms. 4. Chemical reactions involve the rearrangement of atoms. The atoms are not changed. | 3 | |
| 14679853463 | J.J. Thomson | -Discovered the electron by doing experiments where high voltage was applied to a tube which produced a cathode ray -Ray was repelled by the negative pole of the electric field in the tube, resulting in the discovery that it was filled with negative charges, called electrons | 4 | |
| 14679856236 | Plum Pudding Model | -Thomson Model -Electrons are embedded in a uniform, + charged sphere |  | 5 |
| 14679862697 | Radioactivity | -Spontaneous emission of particles and/or radiation -3 types of radioactive emission: Gammy (y) rays: high energy light Alpha (a) rays: +2 charge Beta (B) rays: electron | 6 | |
| 14679865768 | Earnest Rutherford | -Discovered that the Atom contains a nucleus which is an accumulation of + charged -Most of the atom is empty space --This is why the majority of the particles passes right through | 7 | |
| 14679890566 | Atom | -Nuclear Atom: An atom with a dense center of positive charged with electrons moving around the nucleus at a distance that is large relative to the nuclear radius -Subatomic particles: Protons (+): in Neuclue, very small mass Neutrons (/): in nucleus Electrons (-): in orbit | 8 | |
| 14679893003 | Atomic Number | # of Protons in the nucleus of an atom (also e- bc neutral) | 9 | |
| 14679894481 | Mass Number | # of Neutrons and Protons present in the nucleus of an atom | 10 | |
| 14679895684 | Isotopes | Atoms of the same element that have different numbers of neutrons -Show almost identical chemical properties | 11 | |
| 14679903860 | Diatomic molecule vs polyatomic | Diatomic molecule: Contains only 2 atoms Polyatomic molecules: Contains more than 2 atoms | 12 | |
| 14679907637 | Structural formula | Individual bonds of the module are shown | 13 | |
| 14679913050 | Ion | An atom or group of atoms that has a positive or negative charge. | 14 | |
| 14679914642 | Ionic bonding | Chemical bonding that results from the electrical attraction between cations and anions | 15 | |
| 14679915908 | Cation | positively charged ion (loses electrons) | 16 | |
| 14679917035 | Anion | negatively charged ion (gained electrons) | 17 | |
| 14679923047 | Molecular formula | Shows the exact number of atoms of each element in the smallest unit of the substance Ex, O2 | 18 | |
| 14679924232 | Allotrope | One of two or more distinct forms of an element Ex, O2 vs O3 | 19 | |
| 14679927367 | Empirical formulas | Tells the elements present and the simplest whole number ratio of their atoms Simplest chem formulas (not truest) | 20 | |
| 14679932542 | metals vs nonmetals | Metals: Good conductors of heat and electricity malleability, and ductility Tent to form positive ions Nonmetals: To the right of the stairs on the PT tend to gain electrons | 21 | |
| 14679934000 | Groups/Families | -Vertical columns -Have similar chemical properties -Different Families: Alkali metals (1A) Alkaline Earth Metals (2A) Halogens (7A) Noble Gases (8A) Monatomic: meaning the only exist in nature as a single atom | 22 | |
| 14679936212 | Periods | -Horizontal rows -By atomic number | 23 | |
| 14679939084 | 1. Naming Type I Binary Ionic Compounds | -Only consist of two elements -The cation is always named first then the anion second -Cation uses its normal name -Anion uses its root + ide Ex, NaCl = Sodium Chloride | 24 | |
| 14679940947 | 2. Naming Type II Binary Ionic Compounds | -For transition metals that have varying charge -Charge of the metal ion must be specified (use roman numeral) -Anion root + ide Ex. HgO = Mercury (II) oxide | 25 | |
| 14679943200 | Naming Compounds With Polyatomic Ions | -Special names of the polyatomic ions must be memorized -Oxyanions: anions containing an atom of a given elements and different numbers of oxygen atoms 1. Smallest number of oxygen ends in ite 2. Large number of oxygen ends in ate If there are more than 2 oxyanions making up the series: 1. Prefix hypo (less than) used for the least number of oxygen 2. Prefix Per (More than) used to name the members with the most oxygen atoms | 26 | |
| 14679945628 | 3. Naming Binary Covalent Compounds (Type III) | -Formed between two nonmetals 1. Prefix + Cation 2. Prefix + anion root + ide *Prefix indicate number of atoms*: Mono = 1 Di = 2 Tri = 3 tetra= 4 penta= 5 hexa= 6 hepta= 7 octa= 8 nona= 9 Deca = 10 Mono is never used for naming the first elements Drop the "o" or "a" before the prefix 3. ex, PCl5 = Phosphorus Pentacholride | 27 | |
| 14679951166 | Acids | Molecule in which one or more H+ ions are attached to an anion | 28 | |
| 14679952288 | Naming acids without oxygen | Hydro(anion root)ic acid | 29 | |
| 14679952289 | Naming acids without oxygen | 1. Anion ends in ite (root)ous acid 2. Anion ends in ate root(ic) acid | 30 | |
| 14679961004 | Formula to name Flowchart |  | 31 |
