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Chem. Study Guide
Chem. Study Guide from notes
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 |