Important suffixes
Basic Chemistry III
Vladimíra Kvasnicová
ACID
anion
oxygen-free
hydro-.....-ic acid
-ide
oxo-acid
lower ox.state
-ous acid
-ite
oxo-acid
higher ox.state
-ic acid
-ate
Inorganic Compounds
Inorganic Compounds
Salts
are formed by neutralization:
acid + hydroxide → salt + water
acidic salts of ACIDS
cation: metal or NH4+
KH2PO4
potassium dihydrogen phosphate
K2HPO4
(di)potassium hydrogen phosphate
K3PO4
(tri)potassium phosphate (not acidic)
derived from the hydroxide (= cation of the hydroxide)
anion: oxygen-free or polyatomic anion
derived from the acid (= anion of the acid)
„cation hydrogen anion“
NH4HCO3 ammonium hydrogen carbonate
KCl, ZnS, CuCl2, Fe2S3, CaCO3, Na2CO3, (NH4)2SO4
Ca(HS)2
calcium hydrogen sulfide
Other types of compounds
Other types of compounds
basic salts of ACIDS
double salts of ACIDS
„cation hydroxy anion“
a) „cation1 cation2 anion“
Mg(OH)Cl
magnesium hydroxychloride
KMgF3
potassium magnesium fluoride
KLiSO4
potassium lithium sulfate
Sb(OH)2(NO3) antimony(III) dihydroxynitrate
Total charge of molecule is ZERO
Total charge of molecule is ZERO
Other types of compounds
Other types of compounds
double salts of ACIDS
HYDRATES OF SALTS
b) „cation anion1 anion2“
„cation anion multiple prefix hydrate“
CaCl(ClO)
calcium chloride hypochlorite
Cu3(CO3)2F2
copper(II) carbonate fluoride
MgCl2 . 6H2O
magnesium chloride hexahydrate
CaHPO4 . 2H2O calcium hydrogen phosphate
Total charge of molecule is ZERO
dihydrate
Other types of compounds
Other types of compounds
THIOACIDS AND THIOSALTS
POLYACIDS AND SALTS
„thio.... acid“
„multiple prefix.... acid“
H2S2O3
thiosulfuric acid
(H2SO4 = sulfuric acid)
H2B4O7
tetraboric acid
HSCN
thiocyanic acid
(HOCN = cyanic acid)
H2Cr2O7
dichromic acid
„cation thio....anion“
„cation multiple prefix....anion“
K2S2O3
potassium thiosulfate
Na2B4O7
sodium tetraborate
KSCN
potassium thiocyanate
K2Cr2O7
potassium dichromate
Problems – add formulas
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sodium sulfite
potassium phosphate
ammonium hydrogen phosphate
lithium dihydrogen phosphate
calcium hydrogen carbonate
silver sulfide
zinc sulfate
potassium permanganate
sodium hypobromite
barium nitrate
hydrargyric chloride
Problems – add formulas
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sodium tetraborate decahydrate
potassium aluminium sulfate
sodium aluminium sulfate dodecahydrate
ammonium carbonate
calcium sulfate hemihydrate (hemi = ½)
zinc sulfate heptahydrate
potassium dichromate
potassium magnesium fluoride
ammonium magnesium phosphate
led(II) chloride fluoride
cupric biscarbonate difluoride (bis = twice)
Chemical reactions
Chemical reactions
= chemical changes
stoichiometry = the reactants combine in simple wholenumber ratios (see stoichiometric coefficients: a, b, c, d)
aA+bB→cC+dD
equilibrium constant (K) describes the ratio of
concentrations of products and reactants in the
equilibrium
aA+bB↔cC+dD
• the single arrow (→) is used for an irreversible reaction
• double arrows (↔) are used for reversible reactions
chemical equilibrium = a state of a reversible chemical
reaction in which the concentrations of reactatnts and
products are not changing with time
ie
K = [C]c [D]d / [A]a [B]b
• K is constant for given reaction and fixed temperature
• the definition of K is called Guldberg-Waage´s law
(= law of chemical equilibrium)
the rates of both the forward and back reactions are equal
Chemical reactions
• a chemical reaction is described by a chemical equation
• the equation is balanced if substance amount of each
element is the same on both sides of a chemical equation
⇒ each element must be balanced in the order:
metal – nonmetal – hydrogen - oxygen
Conservation law (Law of conservation of mass / energy)
= the total magnitude of mass (or energy or charge)
remain unchanged even though there may be exchanges of
that property between components of the system
(the sum of masses of reactants equals
to the sum of masses of products)
Chemical reactions
• NEUTRALIZATION = acid-base reactions
H2SO4 + 2 NaOH → Na2SO4 + 2 H2O
acid +
base →
salt +
water
• PRECIPITATION
NaCl + AgNO3 → AgCl (s) + NaNO3
→ insoluble product = precipitate is formed
• REDOX reactions = oxidative-reduction reactions
→ oxidation states of elements are changed !!!