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Chem. Study Guide
Chem. Study Guide from notes 1/2
| Term | Definition |
|---|---|
| Matter | ANYTHING that has mass and volume |
| Democritus | FIRST to claim that ATOMS EXIST |
| John Dalton | created the ATOMIC THEORY |
| J.J. Thomson | PLUM PUDDING model of an atom, discovered electrons ( cathode ray tube), |
| Electrons | NEGATIVE particles outside the atom in orbitals |
| Protons | POSITIVE particles in the nucleus |
| Neutrons | NEUTRAL particles in the nucleus |
| Robert Millikan | OIL DROP experiment (electron =-1) |
| Ernest Rutherford | GOLD FOIL experiment (atom= mostly empty space) |
| Atomic Number | Number of PROTONS |
| Mass Number | Atomic Mass ROUNDED (protons+neutrons) |
| Isotopes | SAME number of protons, but DIFFERENT numbers of neutrons |
| Atomic Mass | WEIGHTED AVERAGE MASS of stable isotopes |
| Niels Bohr | proposed that electrons are found in ORBITALS |
| Orbitals | different energy levels |
| Schrodinger | CLOUD MODEL |
| s- sublevel | 1 spherical, lowest(n=1), max of 2 electrons orbitals |
| p-sublevel | 3 dumbbell, (n=2), max of 6 electrons orbitals |
| d-sublevel | 5 double dumbbell, (n=3), max of 10 electrons orbitals |
| f-sublevel | 7, max of 14 orbitals |
| Aufbau Principle | each electron is put in the LOWEST available energy sublevel |
| Pauli Exclusion Principle | PAIRED electrons with OPPOSITE spins in any orbital (up-down) |
| Dot structure | outermost VALENCE electrons available (up-down in dots) |
| Dimitri Mendeleev | FIRST person to make the PERIODIC TABLE |
| Henry Moselsy | IDENTIFIED the atomic number using X-rays |
| Periodic Law | propertied of the elements are PERIODIC FUNCTIONS of their ATOMIC NUMBERS |
| Periods | number of VALENCE electron increase in rows |
| Groups | elements with SIMILAR properties in column |
| Metal | DENSE SOLIDS that are MALLEABLE, DUCTILE, GOOD CONDUCTORS of heat and electricity, have LUSTER, and LOSE electrons (CATION) |
| Transition Metals | HARD SOLIDS with HIGH melting points, MULTIPLE oxidation levels.. form IONS WITH VISIBLE COLOR (d-subshell) |
| Metalloids | characteristics of BOTH metal and nonmetals |
| Nonmetals | GASES that are NOT malleable or ductile, LACK luster, and are POOR conductors of heat and electricity.. form NEGATIVE ions (ANIONS) |
| Atomic raduis | DECREASES across periods, INCREASES down groups ( more protons=smaller radius) |
| Electronegativity | measures an atom's attraction for electrons WHEN BONDED to another atom( difference indicates IONIC OR COVALENT |
| Ionization Energy | The energy needed to REMOVE the most loosely bound VALENCE electrons |
| Groups 1,2, 17 | DO NOT naturally occur alone |
| Ionic Bonding | TRANSFER of electrons between atoms (strongest) |
| Covalent Bonding | SHARE of electrons between atoms (strong), polar &non-polar |
| Group 18 | Noble Gases |
| Intermolecular Bonding | Forms between MOLECULES (weak) |
| Cation | LOSES electrons (cat on a fence), Metals |
| Anions | GAINS electrons, Non-metals |
| Chemical bonds | Form between ELEMENTS (stable), loses energy |
| Non-Polar covalent bonds | 0-0.4 electronegativity difference |
| Polar covalent bonds | 0.5-1.6 electronegativity difference |
| sea of electrons | explains metallic properties |
| Asymmetrical molecules | polar covalent bonds, but a polar molecule |
| Symmetrical molecules | polar covalent bonds, but non-polar molecule |
| Polyatomic Ions | more than 1 atom, contain both ionic and covalent bonds (TABLE E) |
| Intermolecular Forces | determines if a compound is solid, liquid, or gas: forms between NEIGHBORING molecules |
| Dipole Interactions | occur between POLAR molecules (weakest) |
| Hydrogen bonds | occur between a hydrogen atom and NITROGEN, OXYGEN, or FLUORINE atom |
| London Dispersion Forces | Substances that lack polarity; no attraction between molecules (weak) |
| Graphite | Network solid of carbon sheets; Vander Waals forces hold carbon sheets together |
| Diamond | ball-and-stick format (Stigma-bonds); |
| Buckminster Fullerence | CO60 molecule; hollow sphere; similar to soccer ball; (Bucky balls) |
| Transmutation | when the atomic nucleus of one element is charged into the nucleus of a different element |
| Nuclear Reaction | a change that occurs within or among atomic nuclei and is represented by a nuclear equation |
| Unstable Elements | all atomic numbers greater than 83 (Radioactive) |
| Nuclear Force | The positively charged protons repel each other,( nucleus is held together by strong nuclear force) |
| Radioactive Decay | emits alpha particles, beta particles, positrons, and gamma rays |
| Natural Transmutations | emit particles as a result of unstable neutrons to proton ratios (not 1:1) |
| Artificial Transmutation | are created in labs |
| Fission | splitting heavy nucleus to produce lighter nuclei and energy (1>2) |
| Fusion | Combining light nuclei to produce a heavier nucleus and energy (2>1) |
| Einstein's equation | (E=mc^2) E= energy, m= mass, c= speed of life |
| half-life | the time it takes for half the number of atoms in an element to decay (T) |
| Fraction remaining | (1/2)^n=(1/2)^(t/T) |
| number of half- lives | n=(t/T)=time of decay/ half-life |
| Positive uses for radioisotopes | Radioactive dating, chemical tracers, Industrial Applications, Medical Applications |
| Radiation risks | mutations, illness, death |
| Physical Change | physical appearances changes (freeze, melt, boil, condense) |
| Chemical Change | material changes completely (burn, color, bubles) |
| Exothermic | loses heat energy, raises the surrounding temperature |
| Endothermic | gains heat energy, lowers the surrounding temperature |
| Law of Conservation | matter can neither be created nor destroyed |
| Diatomic elements | Br, I, N, Cl, H, O, F |
| Qualitative | tells which elements are in the compound (symbols) |
| Quantitative | Tells the number of atoms of each element in a compound (subscripts) |
| Molecular Formulas | represent the ACTUAL RATIO of atoms in a single covalently bound molecule |
| Empirical Formulas | represent the SIMPLEST INTEGER RATIO of atoms in a compound |
| Hydrates | ionic compounds that trap water in a crystal lattice structure |
| Naming Ionic Compounds | metal + non-metal, polyatomic ions, balancing charges (-ide) |
| Naming Covalent Compounds | non-metal +non-metal, (prefixes) (-ide) |
| prefix for 1 | mono- |
| Prefix for 2 | di- |
| Prefix for 3 | tri- |
| Prefix for 4 | tetra- |
| Prefix for 5 | penta- |
| Prefix for 6 | hexa- |
| Prefix for 7 | hepta- |
| Prefix for 8 | octa- |
| The Stock System | (Roman numerals), metals |
| Synthesis Reactions | two or more reactants combine to form a single product |
| Decomposition Reactions | A single compound is broken down into two or more simpler substances |
| Single Replacement Reactions (Table J) | a single element replaces another element that is part of a compound (an element and a compound) |
| Double Replacement Reactions | Ionic compounds that reacts in solution to produce a solid precipitate, a gas, or a molecular compound |
| Aqueous | a substance dissolved in water |
Created by:
ifolckemer
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