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| the scientific discipline that studies the composition, properties, and transformations of matter |
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| homogeneous mixture of more than one substance; can have gas, liquid, or solid solution |
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| simplest substance that has a distinct chemical identity, cannot be broken down further; pure substance |
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| consists of 2 or more elements held together by chemical bonds |
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| same throughout; example clean air, wine, brass |
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| contains regions that are different in structure and property; example rocks, particles in air |
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| property which can be measured without changing the identity of the substance; example color, odor, density changes of state |
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| property which describes how a substance changes its identity to form other substances; example burning coal |
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| does not depend on the amount of the substance present; example color, density |
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| depends on the amount of substance present; example mass, volume, length |
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| an equation defining units where the two units are set equal |
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| a ratio relating the same quantity in two systems of units that is used to convert the units of measurement |
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| has mass and occupies space |
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| definite shape, definite volume |
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| no definite shape, definite volume |
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| no definite shape, no definite volume |
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| homogeneous or heterogeneous |
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| separation using boiling points of two substances in the mixture |
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| separation using how well a substance adheres (sticks) to another substance, absorption |
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| the number of protons in the nucleus of an atom of an element |
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| the sum of the number of protons and neutrons in the nucleus of a particular atom |
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| atoms of the same element (same number of protons) with different numbers of neutrons in the nucleus |
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| indicates the active number and kind of atoms in a molecule |
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| gives the relative number and kind of atoms in a compound shown as lowest whole number ratio |
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| gives arrangement of atoms in a compund |
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| combination of more than one non-metallic elements |
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| a positively charged atomic species, missing an electron |
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| a negatively charged atomic species, an extra electron |
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| an electrically charged group of two or more atoms |
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| force of attraction between oppositely charged ions |
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| the attraction involving the sharing of electrons between two nuclei |
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| polyatomic anions which contain oxygen |
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| the apparent charge on an individual atom in a compound or a polyatomic unit |
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| invisible particles called "atamos" |
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| 1661, definition of element |
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| 1774, isolation of oxygen |
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| 1789, law of conservation of mass |
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| 1806, law of definite proportions |
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| 1808, postulates of atomic theory and law of multiple proportions |
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| 1809, determining chemical formulas |
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| 1811, equal volumes of gases contain an equal number of particles |
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| early 1800s, symbols for elements |
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| 1896, proposed concept of radioactivity |
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| 1903, measured charge-to-mass ratio of an electron |
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| 1909, oil drop experiment to measure the charge of an electron |
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| 1911, proved existence of nucleus of the atom |
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| 1913, devised the atomic number system |
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| each element is composed of atoms |
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| atoms of the same element are identcal |
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| atoms of different elements are different in some fundamental way and have different properties |
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| atoms are neither created or destroyed in chemical reactions |
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| compounds are formed when atoms of more than one element combine |
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| in a compound, the relative numbers and kinds of atoms are constant |
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| First Law of Atomic Theory |
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| law of definite proportions |
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| Second Law of the Atomic Theory |
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| law of conservation of matter |
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| Third Law of the Atomic Theory |
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| law of multiple porportions |
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| Fourth Law of Atomic Theory |
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| 12 atomic mass units (amu) |
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| -1 unit charge, weighs 5.486x10-4 amu |
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| +1 charge, weighs 1.0073 amu |
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| zero charge, weighs 1.0087 amu |
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| composed of protons, neutrons, and electrons, consists of a dense core (protons and neutrons) surrounded by an electron cloud |
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| What defines and element? |
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| the number of protons in the nucleus |
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| equal number of protons and neutrons |
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| total number of protons and neutrons |
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| positive ion, has fewer electrons than protons |
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| negative ion, has more electrons than protons |
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| atomic size, 1 A = 1x10-10 m |
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| Group 1A on the Periodic Table |
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| Group 2A on the Periodic Table |
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| Group 5A on the Periodic Table |
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| Group 6A on the Periodic Table |
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| Group 7A on the Periodic Table |
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| Group 7A on the Periodic Table |
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| Group 8A on the Periodic Table |
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group of 14 columns
first series-lanthanides
second series-actinides |
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| B, Si, Ge, As, Sb, Te, and At |
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| Ionic Compounds Consist of |
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1) metal + non-metal
2) metal + polyatomic anion
3) polyatomic cation + non-metal
4) polyatomic cation + polyatomic anion |
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| atoms held together by covalent bonds, consist of two or more non-metals bonded together, can also result in polyatomic ions |
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| Naming Binary Molecular Compounds |
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| often formed between non-metals, more positive element first then the more negative ending in -ide, use prefixes mono-, di-, tri-... |
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| Naming Ionic Compound Cations |
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can only form one cation-name of element
can form more than one cation-romen numerals in parentheses to indicate charge
-ous for cation with lower charge, ic for cation with higher charge |
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| Naming Ionic Compound Anions |
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| name of monotomic anion-element with suffix -ide |
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-ite, lower amount of oxygen
-ate, higher amount of oxygen
hypo--ite, fewer oxygen than -ite form
per--ate, more oxygens than -ate form |
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Derived from the name of the anion
replace -ide with -ic and prefix hydro-
replace -ate with -ic
replace -ite with -ous |
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| the weight and average of the masses of the naturally occurring isotopes of an element |
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| the sum of the atomic weights for all of the atoms that appear in the formula of a compound |
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| the sum of the atomic weights for all the atoms in a molecule |
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| the number of particles in an amount of matter equal to the number of atoms in exactly 12 grams of the Carbon-12 isotope, 1 mole = 6.022x1023 particles |
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| the mass of one mole of a substance in grams, equal to the formula wieght |
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| the number of 12C atoms in exactly 12 g of 12C, equals 6.022x1023 molecules |
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| a starting substance in a chemical reaction |
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| a substance produced in a chemical reaction |
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| the substance which is completely consumed in a chemical reaction and thereby limits the amount of product formed |
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| the amount of product actually obtained in the laboratory |
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| Quantity of product that is calculated to be produced when all of the limiting reagent has reacted |
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| actual yield/theoretical yield x 100 |
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| Percent Composition of an Element in a Formula |
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| (# of atoms in a formula)(atomic weight)/formula weight x 100 |
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| Percent Composition of a Unit in a Formula |
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| formula weight of the unit/total formula weight x 100 |
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| Formula Units per Molecule |
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| molecular weight/formula weight |
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| Single Displacement Reaction |
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| Double Displacement Reactions |
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| reactant + O2 --> products |
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| the dissolving medium of a solution |
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| a substance dissolved in a solvent to form a solution |
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| a mixture of substances that has a uniform composition |
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| the quantity of solute present in a given quantity of solvent or solution |
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| the concentration of a solution expressed as mole of solute per liter of solution, M |
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| substances which form ions in aqueous solution (water) |
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| completely forms ions, falls apart in solution |
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| substance that does not form ions in an aqueous solution |
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| partially dissociates in aqueous solution |
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| a substance capable of increasing the H+ ion concentration in an aqueous solution |
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| a substance capable of increasing the OH- ion concentration in an aqueous solution |
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| a chemical reaction in which excess OH- ions from a base combined with H+ ions from an acid to produce water |
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| the maximum amount of a substance that will dissolve at a given temperature |
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| a chemical equation showing complete neutral compound formulas of reactants and products |
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| a chemical reaction in which all soluble strong electrolytes are expressed as ions in aqueous solution |
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| ions which appear in exactly the same form with the same stochiometric coefficient |
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| ionic equation from which the spectator ions have been removed |
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| an ionic compound formed by replacing one or more hydrogens of an acid by other cations |
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| solid formed as a product from an aqueous solution |
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| a chemical change which promotes a chemical reaction |
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| Loss of one or more electrons |
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| gain of one or more electrons |
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| a ranking of metals in order of their ease of oxidation |
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| number of moles of solute/volume of the solution in L, moles/L, intensive property |
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| Identifying Strong Electrolytes |
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| most salts, most common bases, some acids (HCl, HBr, HI, HNO3, H2SO4, HClO3, and HClO4) |
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| Identifying Weak Electrolytes |
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| most acids and ammonia (base) |
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| all nitrates, acetates, chlorates, ammonium and compounds of the group 1A elements are soluble |
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| all chlorides, bromides, and iodides are soluble except for the silver, lead, and mercurous compounds |
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| all sulfates are soluble except the compounds of silver, mercurous, lead, and heavy alkaline earths (Ca, Ba, Sr) |
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| all carbonates, sulfites, and phosphates are insoluble except the compounds formed with the group 1A elements and ammonium |
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| all hydroxides are insoluble except compounds of group 1A elements, ammonium, and the heavy alkaline earths (Ca, Ba, Sr) |
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| all sulfides are insoluble except groups 1A, 2A, and ammonium |
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1) formation of a precipitate
2) formation of a lowly ionized species (water, weak acids and bases)
3) formation of a gas
4) redox process
5) formation or breakage of one or more covalent bonds |
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| metals on the left side of the periodic table are more easily oxidized than those to the right |
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| reductant, the substance which causes another species to be reduced and is thereby itself oxidized |
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| oxidant, the substance which causes another species to be oxidized and is thereby itself reduced |
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| a chemical equation that shows either the reduction or the oxidation process separately |
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| a chemical reaction which occurs by a TRANSFER of electrons from one species to another |
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| the arrangement of electrons in an atom |
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| the time required for one cycle of a wave to pass a specific point in space, in seconds |
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| Electromagnetic Radiation |
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| the periodic displacement of the electromagnetic field |
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| the number of cycles which pass a specific point in space in one second, 1/s |
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| the distance between corresponding point on a wave, in meters |
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| a spectrum containing radiation of only specific wavelengths |
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| a separation or categorization of light according to its frequency or wavelength |
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| a quantum (discrete bundle) of radiant energy (light) |
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| a spectrum containing radiation distributed over all wavelengths in the range of interest |
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| the lowest energy state the electron can be in |
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| an energy state of an electron other than the ground state |
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| the probability of finding an electron at a certain point in space |
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| the specific allowed values of the energy |
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| a region in space with a high (90%) electron density |
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| a situation in which two ore more orbitals have the same energy |
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| values which describe the probable location and energy of an electron in an atom |
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| point of no deflection on a wave |
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| 1687, laws of classical physics |
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| 1900, quantization of energy |
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| 1905, explained photoelectric effect |
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| 1914, model of hydrogen atom |
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| 1924, exclusion principle |
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| 1926, uncertainty principle |
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| on an atomic scale, matter gains or loses energy in discrete amounts called quanta |
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| Planck's Constant (h) = ? |
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| light of a sufficiently high frequency can stimulate emission of electrons from the surface of a metal |
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| Delta E for Emission of Energy |
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| Delta E for Absorption of Energy |
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h/mv
planck's constant/mass x volume |
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| both matter and electromagnetic radiation can exhibit wave-like and particle-like behavior |
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| Heisenberg Uncertainty Principle |
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| it is impossible to determine the exact location and momentum of a particle simultaneously |
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n = 1,2,3,... (integer values)
defines the shell in which the electron is located |
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| Azimuthal (Orbital Angular Momentum) Quantum Number |
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l = 0, 1, 2, 3,..., n-1 (integer values)
defines shape of the orbital, each n has its own set of l values |
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| ml = -l, (-l+1), ..., 0, ..., (l-1), l
defines the orientation of the orbital in space, each l has its own set of ml values |
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| Electron Spin Quantum Number |
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| ms = -1/2, +1/2
defines the direction of spin of the electron |
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| the outermost electrons of an atom, higher in energy than the core electrons, used in bonding |
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| the electrons that are not in the outermost shell of an atom |
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| listing of the populates subshells in an atom (in order of lowest to highest energy) |
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| the net positive charge experienced by an electron in a many-electron atom |
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| the energy required to remove an electron from a gaseous atom when the atom is in its ground state |
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| the energy change that occurs when and electron is added to a gaseous atom or ion |
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| the measure of the ability of an atom participating in a bond to pull electron density toward itself |
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| an extent to which an element exhibits the physical and chemical properties of a metal |
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| a series of atoms, ions, or molecules having the same number of electron |
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