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Oxides.Classification. Preparation of oxides.






INORGANIC SUBSTANCES

 


  SIMPLE        
           
Metals   Non-metals   COMPLEX  
(Cu, Na, Al, Fe)   (S, Cl, C, As)      
Oxides Bases Acids Salts
Oxides - complex substances, consisting from two elements, one of which oxygen.   Bases - complex substances, in which atoms of metals bonded with one or several hydroxyls groups (according to electrolytic dissociation theory bases - complex substances, which under the dissociating in water solution are formed metal cations (or NH4+) and hydroxide anions OH-). Acids - complex substances, consisting from hydrogen atoms and acid radical (according to electrolytic dissociation theory: acids - electrolytes, which under the dissociating form only H+ in the capacity of cations). Salts - complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds.

OXIDES

Salts-forming Non-salts forming
  CO, NO, N2O
Basic Amphoteric Acid
It is a metal oxides in which metals display low oxidation number +1, +2 Na2O, MgO, CuO (for metals with oxidation number +3, +4). As a hydrates it corresponding amphoteric hydroxide ZnO, Al2O3, Cr2O3, SnO2 It is oxides of nonmetals and metals with oxidation number from +5 to +7. SO2, SO3, P2O5, Mn2O7, CrO3

Basic, amphoteric- corresponding bases; amphoteric, acid- corresponding acids. BASES Amphoteric Show also properties of weak acids. Alkalies(soluble in water) Hydroxides (insoluble in water)

 

     
     
 

ACIDS

On composition On hydrogen atoms number, which capable to substituted on metal

 

Oxygenless Oxoacids (containing oxygen)   Monobasic (monoprotic) Dibasic (diprotic) Tribasic (triprotic)
HCl, HBr, HI, H2S, HCN HNO3, H2SO4, HClO4, H3PO4   HCl, HNO3, HI, HClO3 (Those having one acidic proton) H2SO4, H2SO3 H2SiO3 H3PO4

On the basis of strengths or capacity to donate hydrogen ions, acids can be described as: Strong acids: Which are completely (100%) ionized in aqueous solutions. Hence at equilibrium, the concentration of acid molecules is very less and concentration of hydrogen ion reaches to maximum, e.g., HCl, HNO3, HClO4. Weak acids: They are only partially ionized in solution at equilibrium state. At equilibrium state, acid molecules are present and the concentration of hydrogen ion is less, e.g., HF, CH3COOH.

SALTS

Medium acidic basic Double mixed complex
In the time of dissociation give only metal cations (or NH4+) and anions of acid radical. Products of full substitution hydrogen atoms of acids to atoms of metals. Ex.: Na2SO4 In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid radical. Products of full substitution hydrogen atoms of multibasic acid to atoms of metal. Ex.: NaHCO3 In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical. Products of incomplete substitution OH groups, corresponding bases to acid radicals Ex.: Mg(OH)Cl In the time of dissociation gives two cations and one anion. Ex.: KAl(SO4)2 Formed by means of one cation and two anions. Ex.: CaOCl2 Contain complex cations or anions Ex.: [Ag(NH3)2]Br Na[Ag(CN)2]

BINARY COMPOUNDS. A binary compound is a chemical compound that contains exactly two different elements. Examples of binary ionic compounds include calcium chloride (CaCl2), sodium fluoride (NaF), and magnesium oxide (MgO), while examples of a binary covalent compounds include water (H2O), and sulfur hexafluoride (SF6).Corresponding to the two limiting types of element, metal and nonmetal, there are three limiting types of binary compound: Metallic These are formed principally by the combination of a metal with a metal, and have the characteristics of a metal.Nonmetallic These are formed principally by the combination of a nonmetal with a nonmetal, and have the characteristics of a nonmetal.Salt-like These are formed principally by the combination of a metal with a nonmetal, and constitute a new class of material. In the formula for a binary compound, the element that attracts electrons less is usually written fi rst. The elements are assigned an electronegativity that refl ects their affi nity for electrons in chemical bonds. The elements that attract electrons most are said to have the highest electronegativities or to be the most electronegative. Fluorine, the most electronegative element, is assigned an electronegativity of 4.0, and the other elements have values relative to that of fl uorine. The elements that attract electrons least are said to have the lowest electronegativities or to be the most electropositive. Binary compounds naming rules. 1. The Cation (positive ion) is named first, the Anion second.2. Monoatomic Cations take the element nameNa+ → SodiumCa2+ → Calcium3. Monoatomic Anions take the elements name and ends with " -ide" Cl- → ChlorideNaCl → Sodium Chlorid Names of binary compounds.

Anion Compounds name Example Anion Compounds name Example
H- hydride NaH – sodium hydride S2- sulfide Na2S – sodium sulfide
B3- boride Li3B – lithium boride Cl- chloride LiCl – lithium chloride
C4- carbide Al4C3 – aluminum carbide As3- arsenide AlAs – aluminum arsenide
N3- nitride Mg3N2 – magnesium nitride Se2- selenide MgSe – magnesium selenide
O2- oxyde CaO – calcium oxyde Br- bromide CaBr2 – calcium bromide
O22- peroxyde K2O2 – potassiun peroxide Sb3- antimonide K3Sb – potassiun antimonide
O2- superoxide (hyperoxide) CsO2 – ceasium superoxide Te2- telluride Cs2Te – ceasium telluride
O3- ozonide KO3 – potassium ozonide I- iodide KI – potassium iodide
F- fluoride NaF – sodium fluoride Bi3- bismuthide Na3Bi – sodium bismuthide
Si4- silicide Mg2Si – magnesium silicide N3- azide AgN3 – silver azide
P3- phosphide Ca3P2 – calcium phosphide C22- acetylenide Cu2C2 – copper acetylenide

Binary covalent compounds are formed between two nonmetals. Although these compounds do not contain ions, they are named very similarly to binary ionic compounds. In the naming of binary covalent compounds, the following rules apply: 1. The fi rst element in the formula is named fi rst, using the full element name.2. The second element is named as if it were an anion.3. Prefi xes are used to denote the numbers of atoms present.4. The prefi x mono- is never used for naming the fi rst element. For example, CO is called carbon monoxide, not monocarbon monoxide.

Oxides.Classification. Preparation of oxides.

Oxides - complex substances, consisting from two elements, one of which oxygen.Oxides: BASIC- It is a metal oxides in which metals display low oxidation number +1, +2. Na2O, MgO, CuO.AMPHOTERIC-(for metals with oxidation number +3, +4). As a hydrates it corresponding amphoteric hydroxide.ZnO, Al2O3, Cr2O3, SnO2.ACID- It is oxides of nonmetals and metals with oxidation number from +5 to +7.SO2, SO3, P2O5, Mn2O7, CrO3 1. Interaction of simple and complex substances with oxygen: 2Mg + O2 → 2MgO. 4P + 5O2 → 2P2O5.S + O2 → SO2.2CO + O2 → 2CO2.2CuS + 3O2 → 2CuO + 2SO2.CH4 + 2O2 → CO2 + 2H2O  
     
       

2. Decomposition some substances containing oxygen (bases, acids, salts) under the heating:

  tоС  
Cu(OH)2 CuO + H2O
  tоС  
(CuOH)2CO3 2CuO + CO2 + H2O
  tоС  
2Pb(NO3)2 2PbO + 4NO2 + O2
  H2SO4 (conc.)  
2HMnO4 Mn2O7 + H2O
       

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