1. Inorganic compounds

2. 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.

3. Inorganic compounds
Oxides
Acids
Bases
Salts
……..

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

5. 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.

6. 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

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

8. 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

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

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

11. 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

12. 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

13. 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

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

15. 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

16. 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↑

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

18. 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

19. 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

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

21. 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-

22. 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.

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

24. 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)

25. 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

26. 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+

27. Sources