Chemistry: Periodic Table Terms and Definitions, Quizzes of Chemistry

Download Chemistry: Periodic Table Terms and Definitions and more Quizzes Chemistry in PDF only on Docsity! TERM 1 noble gases DEFINITION 1 with the exception of helium, they have 8 electrons in their highest occupied energy level; completely filled out shell; very stable TERM 2 representative elements DEFINITION 2 A group elements electrons are being added to either s or p orbitals highest energy electron in outer shell have very regular variations in their properties TERM 3 d-Transition elements DEFINITION 3 B group elements all are metals, sometime called transition metals electrons are being added to d orbitals exhibit smaller variations from row-to-row than the representative elements TERM 4 f-transition metals DEFINITION 4 sometimes called inner transition metals electrons are being added to f orbitals electrons are being added two shells below the valence shell very slight variations of properties from one element to another outermost electrons have the greatest influence on the chemical properties of elements TERM 5 atomic radii DEFINITION 5 describes the relative sizes of atoms increase within a column going from top to the bottom of the periodic table decrease within a row going from left to right on a periodic table decrease across a period because of the shielding or screening effect TERM 6 ionization energy DEFINITION 6 first: the minimum amount of energy required to move the most loosely bound electron from an isolated gaseous atom to form a 1+ ion= atom(g) + energy ---> ion+(g) + e- second: the amount of energy required to remove the second electron from a gaseous 1+ ion= ion+ + energy ---> ion2+ + e- measure how tenaciously atoms hold on to their electrons increase as you move towards the right and decrease as you move down a group He is always the biggest TERM 7 electron affinity DEFINITION 7 the amount of energy absorbed when an electron is added to an isolated gaseous atom to form an ion with a 1- charge have negative values when energy is released and positive values when energy is absorbed a measure of an atom's ability to form negative ions atom(g) + e- + EA ---> ion-(g) become more negative from left to right and from bottom to top Fluorine is the most negative TERM 8 ionic radii DEFINITION 8 cations are formed when atoms lose electrons and become positively charged ions; they are always smaller than their parent neutral atoms anions are formed when neutral atoms gain electrons to form negatively charged ion; always larger than their parent neutral atoms increase from right to left and top to bottom TERM 9 electronegativity DEFINITION 9 measure of the relative tendency of an atom to attract electrons to itself when chemically combined with another element increase from left to right and bottom to top fluorine is the most cesium and francium are the least TERM 10 element in a simple (monatomic) ion (oxidation #) DEFINITION 10 charge of the ion TERM 21 VIIA elemetns in binary compounds with metals (oxidation #) DEFINITION 21 -1 TERM 22 combustion DEFINITION 22 the highly exothermic combination of a substance with oxygen, usually with a flame TERM 23 ionic hydrides DEFINITION 23 hydrogen reacts with very active metals to produce ionic compounds called ionic hydrides; basic IA metals: 2K + H2 ---> 2KH or 2M + H2 ----> 2MH (general) IIA metals: Ba + H2 ----> BaH2 or M + H2 ---> MH2 (general) H- ions reduce water to produce H2 and OH- ions ex: H- + H2O ---> H2 + OH- or LiH + H2O---> H2 + OH + Li TERM 24 hydrogen reacting with 6A elements DEFINITION 24 form the binary covalent compounds of H2O, H2S, H2Se, and H2Te ex: 2H2 + O2 ---> 2H2O or 8H2 + S8 ---> 8H2S TERM 25 hydrogen reacting with 7A halogens DEFINITION 25 hydrogen reacts with nonmetals to produce molecular hydrides; acidic H2 reacts with halogens (Group 7A) to form covalent hydrogen halides; all are gases at normal temperatures and pressures general quation. H2 + X2 ---> 2HX TERM 26 metal hydrides DEFINITION 26 ionic compounds and form basic aqueous solutions TERM 27 nonmetal hydrides DEFINITION 27 covalent compounds and form acidic aqueous solutions TERM 28 Joseph Priestley DEFINITION 28 discovered oxygen in 1774 by the equation: 2HgO(s)---> 2 Hg(l) + O2(g) TERM 29 oxygen DEFINITION 29 common laboratory preparation method: 2KClO3(s) ----> 2 KCl(s) + 3O2(g) comercially, obtained from the fractional distillation of liquid air TERM 30 ozone DEFINITION 30 O3 allotropic form; two resonance structures very strong oxidizing agent angular and diamagnetic excellent UV light absorber formed from O2 in the upper atmosphere when O2 molecules absorb certain wavelengths of ultraviolet radiation TERM 31 oxides DEFINITION 31 formed from oxygen combining with all other elements except for the noble gases and unreactive metals (Au, Pd, Pt) binary compound that contains oxygen TERM 32 O2 with metals DEFINITION 32 produce solid ionic metal oxides with lithium and all other metals besides Group IA, a normal oxide is produced 4Li + O2 ---> 2Li2O or 2Sr + O2 ---> 2SrO or 3Fe + 2O2 ---> Fe3O4 with sodium a peroxide is produced; oxidation # of oxygen becomes -1 2Na + O2 ----> Na2O2 with K, Rb, and Cs superoxides are produced; oxidation of oxygen becomes -1/2 K + O2 ---> KO2 reacts with IIA metals to form normal oxides general equation: 2M + O2 ---> 2MO at high oxygen pressures IIA metals can form peroxides general equation: M + O2 ---> MO2 TERM 33 metal oxides with water DEFINITION 33 basic anhydrides react with water to form ionic metal hydroxides, bases with no change in oxidation state of metal Li2O + H2O ---> 2LiOH CaO + H2O ---> CO2 TERM 34 O2 with nonmetals DEFINITION 34 form covalentmolecular oxides 2C + O2 ---> 2CO (limited oxygen) C + O2 ---> CO2 (excess oxygen) TERM 35 nonmetal oxides with water DEFINITION 35 nonmetal oxides are acidic acidic anhydrides react with water to produce ternary acids many acid anhydrides dissolve in water to form acid with no change in oxidation state of the nonmetal CO2 + H2O ---> H2CO3 (carbonic acid) Cl2O7 + H2O --- >2HClO4 (perchloric acid)