The main classes of inorganic
compounds
 Classification of
inorganic
substances
Bases
Oxides
Acids
Salts
Genetically relationship
of classes
 Классификация
неорганических
веществ
Основания
Оксиды
Кислоты
Соли
Генетически
взаимосвязи классов
Acid, Base, Oxide, Salt
1. H2SO4
2. H2O
3. H3PO4
4. NaOH
5. CaCO3
6. K2O
7. LiOH
8. KH2PO4
Classify the following oxides:
K2O, CaO, NO2,
P2O5, H2O,SO2,
ZnO, SiO2, SO3,
N2O, TiO2.
Classify the following salts as acidic,
basic or neutral:
NaBr,
K2SO4,
KHCO3,
Mg(NO3)2,
FeS,
FeCO3,
ZnSO3,
MgOHBr,
Ca(HCO3)2,
KI,
Al2(SO4)3
Write the equations for the reactions of the
following oxides with water:
SO2,
N2O5,
K2O,
CaO.
Genetic relationship between different classes
of compounds
1.
2.
3.
4.
5.
6.
metal – basic oxide
non-metal – acid oxide
basic oxide – bases
acid oxide – acid
basic oxide; acid oxide – salt
basе; acid – salt
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-).
Classification
Классификация
Soluble in water (alkalis) and insoluble.
Amphoteric bases show also properties of
weak acids.
Растворимые в воде (щелочи) и
нерастворимые. Амфотерные
основания также могут проявлять
свойства слабых кислот.
Preparation
Получение
1. Reactions of active metals (alkaline and alkaline
earth metals) with water
2Na + 2H2O →→ 2NaOH + H2
Ca + 2H2O =Ca(OH)2 + H2
2.Interaction oxides of active metals with water
BaO + H2O = Ba(OH)2
3.Electrolysis water solutions of salts
2NaCl + 2H2O = 2NaOH + H2 + Cl2
Chemical properties
Alkalis
Insolublebases
1.
Actiontoindicators
litmus - blue
methylorange - yellow
phenolphthalein - crimson
––
2.
Interaction with acidoxides
2KOH + CO2 = K2CO3 + H2O
KOH + CO2 = KHCO3
3.
––
Interaction with acids (reaction of neutralization)
NaOH + HNO3= NaNO3 + H2O
4.
Cu(OH)2 + 2HCl = CuCl2 + 2H2O
Reaction of exchange with salts
Ba(OH)2 + K2SO4 = 2KOH + BaSO4↓
3KOH + Fe(NO3)3 = Fe(OH)3↓+ 3KNO3
5.
––
––
Thermal decomposition
t°
Cu(OH) =CuO + H O
Oxides - complex substances, consisting
from two elements, one of which oxygen.
Non-salts forming
(CO, N2O, NO)
Salts forming
Basicit 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
Acidit is oxide of nonmetals and metals with oxidation
number from +5 to +7.
SO2; SO3; P2O5; Mn2O7; CrO3
Preparation
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
cat. 4NH3 + 5O2=4NO + 6H2O2.
2. Decomposition some substances containing oxygen
(bases, acids, salts) under the heating:
Cu(OH)2 = CuO + H2O
(CuOH)2CO3 = 2CuO + CO2 + H2O
2Pb(NO3)2 = 2PbO + 4NO2 + O2
2HMnO4 = Mn2O7 + H2O
Basic oxides
Acid oxides
1.
Interaction with water
Base formed:
Na2O + H2O = 2NaOH
CaO + H2O = Ca(OH)2
Acid formed:
SO3 + H2O = H2SO4
P2O5 + 3H2O = 2H3PO4
2.
Interaction with acid or base
On reactions with acid salt and water are
formed
t°
MgO + H2SO4= MgSO4 + H2O
t°
CuO + 2HCl = CuCl2 + H2O
On reactions with base salt and water are
formed
CO2 + Ba(OH)2 = BaCO3 + H2O
SO2 + 2NaOH = Na2SO3 + H2O
3. Amphoteric oxides interact
with acids as basic:
ZnO + H2SO4 = ZnSO4 + H2O
4.
with bases as acid:
ZnO + 2NaOH = Na2ZnO2 + H2O
(ZnO + 2NaOH + H2O = Na2[Zn(OH)4])
Interaction of basic and acid oxide with each other leads to salt formation
Na2O + CO2= Na2CO3
5.
Reduction up to simple substances:
3CuO + 2NH3 = 3Cu + N2 + 3H2O
P2O5 + 5C = 2P + 5CO
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).
Oxygenless:
Salts name:
HCl - hydrogen chloride (hydrochloric)
monobasic
chloride
HBr - hydrogen bromide
monobasic
bromide
HI - hydrogeniodide
monobasic
Iodide
HF - hydrogen fluorine (hydrofluoric)
monobasic
fluoride
bibasic
sulphide
monobasic
nitrate
H2SO3 – sulphurous
bibasic
sulphite
H2SO4 – sulphuric
bibasic
sulphate
H2CO3 – carbonic
bibasic
carbonate
H2SiO3 – silicon
bibasic
silicate
H3PO4 – ortophosphoric
tribasic
ortophosphate
H2S - hydrogensulphide
Containing oxygen:
HNO3– nitric
Preparation
1.
Interaction of acid oxides with water (for oxoacids):
SO3 + H2O = H2SO4
P2O5 + 3H2O = 2H3PO4
2.
Interaction of hydrogen with non-metals and following
dissolution product in water (for oxygenless acids).
H2 + Cl2 = 2HCl
H2 + S = H2S
3.
Reactions of exchange between salt and acid
Ba(NO3)2 + H2SO4 = BaSO4↓ + 2HNO3
including displacement weak, flying or slightly soluble acid from
its salts by means of more strong acids.
Na2SiO3 + 2HCl = H2SiO3↓+ 2NaCl
Chemical properties
1.
Action to indicators.
litmus - red
methylorange – pink
2.
Interaction with bases (reaction of neutralisation)
H2SO4 + 2KOH = K2SO4 + 2H2O
2HNO3 + Ca(OH)2 = Ca(NO3)2 + 2H2O
3.
Interaction with basic oxides.
CuO + 2HNO3=Cu(NO3)2 + H2O
4.
Interaction with metals.
Zn + 2HCl = ZnCl2 + H2
2Al + 6HCl = 2AlCl3 + 3H2
(metals standing in the electrochemical series before hydrogen, acid-oxidizers).
5.
Interaction with salts (reactions of exchange) at which stands out gas or formed residual.
H2SO4 + BaCl2 = BaSO4↓ +2HCl
2HCl + K2CO3 = 2KCl + H2O + CO2
Salts - complex substances, which consist
from atoms of metal and acid residuals. This
the most multiple class of inorganic
compounds.
Salts
Medium
Acid
Basic
Double
Mixed
Complex
Medium salts. 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:
Na2SO4= 2Na+ +SO42CaCl2=Ca2+ + 2ClAcid salts. In the time of dissociation give only metal cations (or
NH4+), hydrogen anions and anions of acid radical. Products of
incomplete substitution hydrogen atoms of multibasic acid to
atoms of metal:
NaHCO3= Na+ + HCO3-= Na+ + H+ + CO32Basic salts. 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:
Zn(OH)Cl= [Zn(OH)]+ + Cl-=Zn2+ + OH- + Cl-
Double salts.
In the time of dissociation gives two cations and one
anion:
KAl(SO4)2 = K+ + Al3+ + 2SO42Mixed salts.
Formed by means of one cation and two anions:
CaOCl2 = Ca2+ + Cl- + OClComplex salts. Contain complex cations and anions:
[Ag(NH3)2]Br = [Ag(NH3)2]+ + Br Na[Ag(CN)2] = Na+ + [Ag(CN)2]-
Medium salts
Preparation
1)
Metal with non-metal:
2Na + Cl2= 2NaCl
2)
Metal with acid:
Zn + 2HCl = ZnCl2 + H2
3)
Metal with solution of salt of less active metal:
Fe + CuSO4= FeSO4 + Cu
4)
Basic oxide with the acid oxide:
MgO + CO2= MgCO3
5)
Basic oxide with acid:
CuO + H2SO4=CuSO4 + H2O
6)
Bases with acid oxide:
Ba(OH)2 + CO2= BaCO3↓ + H2O
7)
Bases with acid:
Ca(OH)2 + 2HCl = CaCl2 + 2H2O
8)
Salts with the acid:
MgCO3 + 2HCl = MgCl2 + H2O + CO2
BaCl2 + H2SO4 = BaSO4 ↓ + 2HCl
9)
Bases solution with salt solution:
Ba(OH)2 + Na2SO4= 2NaOH + BaSO4↓
10) Solutions of two salts:
3CaCl2 + 2Na3PO4 = Ca3(PO4)2↓ + 6NaCl
Chemical properties
1.
Thermal decomposition
CaCO3 = CaO + CO2
2Cu(NO3)2 = 2CuO + 4NO2+ O2
NH4Cl = NH3 + HCl
2.
Hydrolysis
Al2S3 + 6H2O = 2Al(OH)3 ↓ + 3H2S
3.
Exchange reactions with acids, bases and other salts
AgNO3 + HCl = AgCl↓ + HNO3
4.
Oxidation-reduction reactions, stipulated by properties of cation or anion
2KMnO4 + 16HCl = 2MnCl2 + 2KCl + 5Cl2 + 8H2O
Acid salts
Preparation
1.
Interaction of acid with the deficit of basis.
KOH + H2SO4= KHSO4 + H2O
2.
Interaction of bases with plenty acid oxides.
Ca(OH)2 + 2CO2 = Ca(HCO3)2
3.
Interaction of medium salts with acid.
Ca3(PO4)2 + 4H3PO4 = 3Ca(H2PO4)2
Chemical properties
1.
Thermal decomposition with medium salts formation.
Ca(HCO3)2= CaCO3↓ + CO2 + H2O
2.
Interaction with the alkali. Reception of medium salts.
Ba(HCO3)2 + Ba(OH)2 = 2BaCO3↓ + 2H2O
Basic salts
Preparation
1.
Hydrolysis of salts, formed by weak base and strong acid.
ZnCl2 + H2O = [Zn(OH)]Cl + HCl
2.
Addition (by drops) a small quantities of alkalis to solutions of medium salts of metals.
AlCl3 + 2NaOH = [Al(OH)2]Cl + 2NaCl
3.
Interaction of weak acids salts with medium salts.
2MgCl2 + 2Na2CO3 + H2O = [Mg(OH)]2CO3 + CO2 + 4NaCl
Chemical properties
1.
Thermal decomposition.
[Cu(OH)]2CO3= 2CuO + CO2 + H2O
2.
Interaction with the acid: formation of medium salts.
Sn(OH)Cl + HCl = SnCl2 + H2O
1. Make a poster with definition, their
classification and properties.
 ACID
 BASE
 OXIDE
 SALT
2.Find the X compound
 Si→ X→ H2SiO3
→Na2SiO3
 Ca →CaO
→X→Ca3(PO4)2
Mg → MgO → X →
MgCl2
3. If this is the answer, then what
would the question be?
 Answer: "Produces a sour
taste and turns blue litmus
paper red.“
 Answer: "Forms when a metal
reacts with oxygen.“
 Answer: "Commonly used to
neutralize acids.“
 Answer: "Typically composed
of a metal cation and a nonmetal anion.“
 Answer: "Examples include
sulfuric acid, hydrochloric acid,
and nitric acid.“
 Answer: "May be soluble or
insoluble in water, depending
on their chemical structure.“
 Answer: "Often used as
preservatives, flavor
enhancers, and in food
preparation."
Answer: "Often have a bitter taste and feel slippery.“
Answer: "Formed by the reaction between an acid and a base.“
Answer: "Some examples include carbon dioxide, sulfur
dioxide, and nitrogen dioxide."
Solve the problem
 Calculate the mass of salt that is produced from the
reaction of 96 g of magnesium with an excess
hydrochloric acid.
 Determine the mass of iron(III) oxide formed when
72 g of iron reacts with excess oxygen gas to
produce iron(III) oxide.
 Calculate the mass of silver chloride produced
when 25 g of silver nitrate reacts with excess
sodium chloride to form silver chloride and sodium
nitrate .
1.Balancing the combustion of propane (C₃H₈) with oxygen gas (O₂) to
form carbon dioxide (CO₂) and water (H₂O):
C₃H₈ + O₂ → CO₂ + H₂O
2.Balancing the reaction between sodium hydroxide (NaOH) and
hydrochloric acid (HCl) to form sodium chloride (NaCl) and water (H₂O):
NaOH + HCl → NaCl + H₂O
3.Balancing the reaction between iron (III) oxide (Fe₂O₃) and carbon
monoxide (CO) to form iron (Fe) and carbon dioxide (CO₂):
Fe₂O₃ + CO → Fe + CO₂
Define your posters and evaluate
your classmates work