STRONG ACIDSHCl hydrochloric acidHBr hydrobromic acidHI hydroiodic acidHNO3nitric acidHClO4perchloric acidHClO3chloric acidH2SO4sulfuric acidWEAK ACIDSHF hydrofluoric acidCH3COOH acetic acidHCN hydrocyanic acidH2CO3carbonic acidH2SO3sulfurous acidH3PO4phosphoric acid(COOH)2oxalic acidSTRONG BASESI A1H II ALiOHNaOHKOHRbOHCsOHCa(OH)2Sr(OH)2Ba(OH)2lithium hydroxidesodium hydroxidepotassium hydroxiderubidium hydroxidecesium hydroxidecalcium hydroxidestrontium hydroxidebarium hydroxide3Li4Be11Na12Mg19K20Ca37Rb38Sr55Cs56Ba,87Fr88RaWEAK BASESNH3ammoniaCO32-carbonate ionHCO3-bicarbonate ion*as far as insoluble bases are concerned, most transition metal hydroxides are insolubleSOLUBILITY RULESSOLUBLE IN WATER INSOLUBLE IN WATERall common inorganic acids and low-molecular-weight organic acidsall common compounds of thegroup IA metal ions (Li+, Na+, K+, Rb+, Cs+)all common compounds of theammonium ion (NH4+)common nitrates (NO3-)common acetates (CH3COO-)common chlorates (ClO3-)common perchlorates (ClO4-)common chlorides (Cl-) exceptions: AgCl, Hg2Cl2, PbCl2 (INSOLUBLE!)common bromides (Br-) exceptions: AgBr, Hg2Br2, PbBr2 (INSOLUBLE!)exceptions: HgBr2(MODERATELY SOLUBLE!)common iodides (I-) exceptions: many heavy-metal iodides (INSOLUBLE!)common fluorides (F-) exceptions: MgF2, CaF2, SrF2, BaF2, PbF2 (INSOLUBLE!) [group IIA fluorides + Pb]common sulfates (SO42-) exceptions: PbSO4, BaSO4, HgSO4 (INSOLUBLE!)exceptions:CaSO4, SrSO4, Ag2SO4(MODERATELY SOLUBLE!)(SOLUBLE!) exceptions:group IA and group IIA metals (the strong bases!)common metal hydroxides (OH-)(SOLUBLE!) exceptions:group IA metals and NH4+common carbonates (CO32-)exceptions:BaCO3, MgCO3(MODERATELY SOLUBLE!)(SOLUBLE!) exceptions:group IA metals and NH4+common phosphates (PO43-)(SOLUBLE!) exceptions:group IA metals and NH4+common arsenates (AsO43-)(SOLUBLE!) exceptions:group IA metals, group IIA metals, and NH4+common sulfides (S2-)POLYATOMIC IONS THAT YOU STILL NEED TO STUDYNH4+ammonium ionClO-hypochlorite ionClO2-chlorite ionClO3-chlorate ionClO4-perchlorate ionCH3COO-acetate ionMnO4-permanganate ionNO2-nitrite ionNO3-nitrate ionSCN-thiocyanate ionO2-oxide ionS2-sulfide ionHSO3-hydrogen sulfite ionSO32-sulfite ionHSO4-hydrogen sulfate ionSO42-sulfate ionHCO3-hydrogen carbonate ionCO32-carbonate ionCrO42-chromate ionCr2O72-dichromate ionPO43-phosphate ionAsO43-arsenate ionPROTONS, NEUTRONS, AND ELECTRONS # p+ and # e- is the same as the atomic # mass # = # p+ + # nPERIODIC NAMES group IA metals = alkali metals group IIA metals = alkaline earth metalsATOMIC SPECTRA absorption spectrums (observing energy absorbed by electrons when they get excited) are mostly used with transition metals emission spectrums (observing the energy/light emitted when electrons return to their ground state) are mostly used with group IA and group IIA metalsELECTRON CONFIGURATIONS Aufbau Principle – the electron that distinguishes an element from the previous element enters the lowest-energy atomic orbital available Pauli Exclusion Principle – no two electrons in an atom may have identical sets of four quantum numbers Hund’s Rule – electrons must occupy all of the orbitals in a given sublevel singly before pairing begins; these unpaired electrons have parallel spins- exceptions are the elements in the Cr and Cu columnsPERIODIC TRENDS atomic radii- increases  and - more protons means smaller atomic radius across a period ionization energy- increases  and - IE2 > IE1- it takes more energy to remove an electron from a filled orbital than a partially-filled orbitalBe 2s2  takes more energy to remove this electronB 2s22p1  than it does to remove this electron electron affinity- increases (becomes more positive)  and and increases (becomes more negative)  and exceptions for filled and half-filled subshells:Be 2s2  filled EA ~ 0N 2p3  half-filled 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!7N3-7 p+10 e- ) ) -8O2-8 p+10 e- ) ) 2-9F-9 p+10 e- ) ) ) 3- 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 awayNAMING COMPOUNDS metal + non-metal = binary ionic compoundregular (stem)ideexamples: LiBr = lithium bromide MgCl2 = magnesium chloride transition metal + non-metal = binary ionic compoundregular(Roman numerals) (stem)ideexamples: FeBr2 = iron(II) bromide SnO2 = tin(IV) oxide TiCl2 = titanium(II) chloride Fe(NO3)3 = iron(III) nitrate pseudobinary ionic compoundsexamples: 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) compoundsexamples: SO2 = sulfur dioxide CS2 = carbon disulfide SF4 = sulfur tetrafluoride binary acidsin 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 saltsgroup # oxidation states-ous -ic  acid-ite -ate  saltgroup 3A +1 +3group 4A +2 +4group 5A +3 +5group 6A +4 +6group 7A +1 +3 +5 +7hypo(stem)oushypo(stem)ite(stem)ous(stem)ite(stem)ic(stem)ateper(stem)icper(stem)ateexamples: 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