STRONG ACIDS HCl HBr HI HNO3 HClO4 HClO3 H2SO4 WEAK ACIDS HF CH3COOH HCN H2CO3 H2SO3 H3PO4 COOH 2 STRONG BASES I A 1 H 3 Li 11 Na 19 K 37 Rb 55 Cs 87 Fr LiOH NaOH KOH RbOH CsOH Ca OH 2 Sr OH 2 Ba OH 2 II A 4 Be 12 Mg 20 Ca 38 Sr 56 Ba 88 Ra hydrochloric acid hydrobromic acid hydroiodic acid nitric acid perchloric acid chloric acid sulfuric acid hydrofluoric acid acetic acid hydrocyanic acid carbonic acid sulfurous acid phosphoric acid oxalic acid lithium hydroxide sodium hydroxide potassium hydroxide rubidium hydroxide cesium hydroxide calcium hydroxide strontium hydroxide barium hydroxide WEAK BASES NH3 2 CO3 HCO3 as far as insoluble bases are concerned most transition metal hydroxides are insoluble ammonia carbonate ion bicarbonate ion SOLUBILITY RULES SOLUBLE IN WATER INSOLUBLE IN WATER all common inorganic acids and low molecular weight organic acids all common compounds of the group IA metal ions Li Na K Rb Cs all common compounds of the ammonium ion NH4 common nitrates NO3 common acetates CH3COO common chlorates ClO3 common perchlorates ClO4 common chlorides Cl common bromides Br common iodides I common fluorides F common sulfates SO4 2 exceptions AgCl Hg2Cl2 PbCl2 INSOLUBLE exceptions AgBr Hg2Br2 PbBr2 INSOLUBLE exceptions HgBr2 MODERATELY SOLUBLE exceptions many heavy metal iodides INSOLUBLE exceptions MgF2 CaF2 SrF2 BaF2 PbF2 INSOLUBLE group IIA fluorides Pb exceptions PbSO4 BaSO4 HgSO4 INSOLUBLE exceptions CaSO4 SrSO4 Ag2SO4 MODERATELY SOLUBLE SOLUBLE exceptions group IA and group IIA metals the strong bases SOLUBLE exceptions group IA metals and NH4 exceptions BaCO3 MgCO3 MODERATELY SOLUBLE SOLUBLE exceptions group IA metals and NH4 SOLUBLE exceptions group IA metals and NH4 SOLUBLE exceptions group IA metals group IIA metals and NH4 common metal hydroxides OH common carbonates CO3 2 common phosphates PO4 3 common arsenates AsO4 3 common sulfides S2 POLYATOMIC IONS THAT YOU STILL NEED TO STUDY NH4 ClO ClO2 ClO3 ClO4 CH3COO MnO4 NO2 NO3 SCN O2 S2 HSO3 2 SO3 HSO4 2 SO4 HCO3 2 CO3 CrO4 Cr2O7 3 PO4 AsO4 2 2 3 PROTONS NEUTRONS AND ELECTRONS p and e is the same as the atomic mass p n PERIODIC NAMES group IA metals alkali metals group IIA metals alkaline earth metals ammonium ion hypochlorite ion chlorite ion chlorate ion perchlorate ion acetate ion permanganate ion nitrite ion nitrate ion thiocyanate ion oxide ion sulfide ion hydrogen sulfite ion sulfite ion hydrogen sulfate ion sulfate ion hydrogen carbonate ion carbonate ion chromate ion dichromate ion phosphate ion arsenate ion ATOMIC SPECTRA absorption spectrums mostly used with transition metals ground state are mostly used with group IA and group IIA metals emission spectrums observing the energy light emitted when electrons return to their observing energy absorbed by electrons when they get excited are ELECTRON CONFIGURATIONS Aufbau Principle enters the lowest energy atomic orbital available the electron that distinguishes an element from the previous element no two electrons in an atom may have identical sets of four Pauli Exclusion Principle quantum numbers pairing begins these unpaired electrons have parallel spins exceptions are the elements in the Cr and Cu columns Hund s Rule electrons must occupy all of the orbitals in a given sublevel singly before PERIODIC TRENDS atomic radii ionization energy orbital Be B electron affinity increases and more protons means smaller atomic radius across a period increases and IE2 IE1 it takes more energy to remove an electron from a filled orbital than a partially filled 2s2 takes more energy to remove this electron 2s22p1 than it does to remove this electron increases becomes more positive and and increases becomes more negative and exceptions for filled and half filled subshells Be N 2s2 filled 2p3 half filled EA 0 EA 0 other half filled elements small neg values a EA value signifies an endothermic reaction energy is absorbed while a EA value signifies an exothermic reaction energy is released the highest EA value is the one closest to zero while the lowest EA value is the most negative value ionic radii increases and looks more like this Na Mg2 Al3 N3 O2 F more electrons fighting for fewer protons causes repulsion 7N3 8O2 9F 10 e 10 e 2 10 e 3 7 p 8 p 9 p electronegativity increases and the higher the number the more attracted the element is to the electrons values range from 0 7 4 0 when the EN of the two elements 2 electrons are given away NAMING COMPOUNDS metal non metal binary ionic compound regular stem ide examples LiBr lithium bromide MgCl2 magnesium chloride transition metal non metal binary ionic compound regular Roman numerals stem ide examples FeBr2 iron II bromide SnO2 tin IV oxide TiCl2 titanium II chloride Fe NO3 3 iron III nitrate pseudobinary ionic compounds examples KOH potassium hydroxide Ba OH 2 barium hydroxide Fe OH 3 iron III hydroxide Ba CN 2 barium cyanide NH4 2S ammonium sulfide NH4CN ammonium cyanide Cr2S3 chromium III sulfide AlN aluminum nitride binary molecular covalent compounds examples SO2 sulfur dioxide CS2 carbon disulfide SF4 sulfur tetrafluoride binary acids in gas g form they re named hydrogen stem ide in aqueous aq form they re named hydro stem ic acid examples HF g hydrogen fluoride while HF aq hydrofluoric acid HCl g hydrogen chloride while HCl aq hydrochloric acid H2S g hydrogen sulfide while H2S aq hydrosulfuric acid H2Se g hydrogen selenide while H2Se aq hydroselenic acid ternary acids and their salts group oxidation states ous ite 1 2 3 4 group 3A group 4A group 5A group 6A group 7A acid salt ic ate 3 4 5 6 1 hypo stem ous hypo stem ite 3 stem ous stem ite 5 stem ic stem ate 7 per stem ic per stem ate examples HClO hypochlorous acid and its salt NaClO socium hypochlorite HClO2 chlorous acid and its salt NaClO2 sodium chlorite HClO3 chloric acid and its salt NaClO3 sodium chlorate HClO4 perchloric acid and its salt NaClO4 sodium perchlorate TYPES OF REACTIONS combination usually redox element element compound metal non metal binary ionic compound 2Mg s 8Fe0 0 O2 0 s S8 0 g 2Mg2 O2 s s 8Fe2 S2 s non metal nonmetal covalent binary compound 5 O10 g P4 P4 2 0 0 s 5O2 s compound element compound 0 As3 Cl3 2C2 O2 s Cl2 0 g O2 g As5 Cl5 2 g 2C4 O2 s g compound compound compound g N3 H4 SO3 2 Li2 decomposition usually redox g H Cl O2 S4 O2 N3 H3 Li2 s Cl 2 0 O2 2N2 Ca2 Cl2 compound element element g 2N2 l Ca2 compound compound element aq 2H g O2 l Cl2 l O2 2O2 2H2 O2 g g g 0 0 compound compound compound displacement always redox also