Inorganic compounds

Inorganic compound Any substance in which two or more chemical elements (usually other than carbon) are combined, nearly always in definite proportions. Compounds of carbon are usually classified as organic when carbon is bound to hydrogen.

Inorganic compounds Oxides Acids Bases Salts ……..

Oxides Chemical compounds with one or more oxygen atoms combined with another element

Nomenclature and formulas Oxides are maned by name of non-oxygen atom + oxide eg. Hydrogen oxide, H2O. Oxidatnion state of non-oxygen element should be given eg. Sulfur (IV) oxide, SO2. Sometimes, non-oxygen/oxygen ratios are used to name oxides eg. monooxide, dioxide, trioxide etc. In the industry, oxides are named by contracting the element name with „a”, eg. magnesia oxide, MgO.

Theory of Acids and Bases There are three major classifications of substances known as acids or bases. The Arrhenius definition The Brønsted-Lowry definition The Lewis definition

Arrhenius definition An acid produces H+ in solution and a base produces OH-. This theory was developed in 1883.

Brønsted-Lowry definition Acids are defined as proton donors; whereas bases are defined as proton acceptors. A compound that acts as both a Brønsted-Lowry acid and base together is called amphoteric

Lewis definition Acids act as electron pair acceptors and bases act as electron pair doners.

Acids /Arrhenius/ Substance that gives H+ ions when dissolved in water. General Structure HR, where: H is proton (cation) and R in an anion

Nomenclature of oxygenless acids The most important is anion. After that word „acid”. If there is no oxygen in acid, the acid is named with the hydro- prefix. Then is the root. The root in the name of the element. At the end is suffix –ic. The name of anion with suffix –ide instead of –ic. H2S: hydro sulfur ic acid, sulf –ide HCl: hydro chlor ic acid, chlor -ide

Nonmenclature of oxoacids When there is an oxigen in anion, the name of acid if from the anion, after that word „acid”. The root is formed from the name of central element, that build anion with the suffix –ic. Oxidation state of central atom should be indicated. The name of anion is build in the same way, but with suffix –ate instead of –ic. H2SO4: sulfur ic (IV) acid, sulf ate (IV) anion

Reactions oxygenless acids hydrogen + nonmetal → acid H2 + Cl2→ 2 HCl HCl + H2O → HCl(aq) oxoacids acid anhydride + water → acid SO3 + H2O → H2SO4 P4O10 + 6 H2O → 4 H3PO4 Cl2O7 + H2O → HClO4

Analysis acid → acid anhydride + water H2CO3 → CO2 + H2O 2 HNO3 → N2O5 +H2O

Neutralization acid + metal oxide → salt + water MgO + H2SO4 → MgSO4 + H2O Na2O + HCl → NaCl + H2O 2 FeO + 6 H2SO4 → Fe2(SO4)3 + 3 SO2 + 6 H2O acid + base → salt + water KOH + HNO2 → KNO2 + H2O Ca(OH)2 + HNO3 → Ca(NO3)2 + 2 H2O

Neutralization acid + metal → salt + hydrogen H2CO3 + 2 Na → Na2CO3 +H2↑ 2 H3PO4 + 3 Mg → Mg3(PO4)2 + 6 H2↑ HNO3 + Fe → Fe(NO3)2 + H2↑

Reactions Metal oxide + nonmetal oxide (acid anhydride)→ salt Na2O + CO2 → Na2CO3 electrolytic dissociation HBr→ H+ + Br- H2CO3→ H+ + HCO3- HCO3- → H+ +CO32-

Bases /Arrhenius/ Substance that gives OH- ions when dissolved in water. General Structure M(OH)x, where: M is usually metal (cation) and OH is a hydroxylic group Nomenclature: cation (metal) (oxidation state) + hydroxide Co(OH)3 cobalt (III) hydroxide

Creation metal + water → base + H2↑ 2 Na + 2H2O --> 2NaOH + H2 Ca + 2H2O --> Ca(OH)2 + H2 metal oxide + water → hydroxide + salt FeCl3 + 3 NaOH ---> Fe(OH)3 + 3Na Cl CuSO4 + 2 NaOH ---> Cu(OH)2 + Na2SO4

Creation metal hydride + water → base + H2↑ metal peroxide + water → base + H2O2 metal carbide + water → base + unsaturated hydrocarbon↑

Reactions non metal oxide + base → salt + water SO2 + 2 KOH → K2SO3 + H2O base + non metal oxide → salt + water 2 NaOH + CO2→ Na2CO3 + H2O electrolytic dissociation NaOH → Na+ + OH-

Salts An ionic compound that results from the neutralization reaction of an acid and a base. Salts are composed of related numbers of cations and anions so that the product is electrically neutral.

Nomenclature Name of the cation, then name of the anion, same rules like for acids and bases. Fe2(SO4)3: Iron (III) sulfate (VI)

Acid salts Salts formed by the partial neutralization of diprotic or polyprotic acids. Acid is only partially neutralized, one or more hydrogen atoms still remain in the structure. To indicate hydrogen presence word hydro- is given between cation and anion. Amount of hydrogen atoms should be indicated: NaH2PO4: sodium di hydro phosphate (V)

Basic salts Salts formed by the partial neutralization of dihydroxylic or polyhydroxylic basess. Base is only partially neutralized, one or more hydroxylic group still remain in the structure. To indicate OH- group presence word hydro- is given between cation and anion. Amount of hydrogen atoms should be indicated: Cu2(OH)3Cl: dicopper (II) trihydroxyl chloride

Reactions with salts salt1 + acid1(stronger) → salt2 + acid2 (weaker) MgCO3 + 2 HCl→ MgCl2 + CO2 + H2O salt1 + salt2→ salt3 + salt4↓ CaCl2 + Na2CO3 → CaCO3↓ + 2 NaCl Ca2++2Cl- + 2Na+ + CO32- → CaCO3↓ +2Na+ + 2Cl- AgClO4 + NH4Cl → AgCl↓ + NH4ClO4 Ag+ + ClO4- + NH4+ + Cl-→ AgCl↓ + ClO4- + NH4+

Sources http://chemwiki.ucdavis.edu/Core/Inorganic_Chemistry/Descriptive_Chemistry/Main_Group_Reactions/Compounds/Oxides http://chemwiki.ucdavis.edu/Core/Physical_Chemistry/Acids_and_Bases/Acid