Basic Chemistry II
Vladimíra Kvasnicová
Exercise
Add names of the elements:
N
Na
K
Ca
Mg
Mn
Ag
Cd
Hg
Sb
nitrogen
sodium
potassium
calcium
magnesium
manganese
silver
cadmium
mercury
antimony
The figure is found at http://www.corrosionsource.com/handbook/periodic/periodic_table.gif (September 2007)
Inorganic Compounds
Make groups of compounds:
Na2O, HCl, CO2, Na2O2, Ca(OH)2, KClO, HCN, HNO2,
H2S, H2O2, BaO2, PbO2, H2SO3, KOH, MgSO4, NaF,
NH4HCO3, HI, Al(OH)3, HIO4, CdS, MgO2, NaH2PO4
? oxides
hydroxides
peroxides
acids
salts
Inorganic Compounds
Make groups of compounds:
Na2O, HCl, CO2, Na2O2, Ca(OH)2, KClO, HCN, HNO2,
H2S, H2O2, BaO2, PbO2, H2SO3, KOH, MgSO4, NaF,
NH4HCO3, HI, Al(OH)3, HIO4, CdS, MgO2, NaH2PO4
? oxides
hydroxides
peroxides
acids
salts
Inorganic Compounds
Oxides
anion: O-II
• acid-forming: nonmetal / oxygen
 use multiple prefixes (mono, di, tri,...)
• base-forming: metal / oxygen
 use sufixes –ous / -ic
or
(oxidation state)
• amphoteric
MnO2, N2O, BaO, CO, K2O, SO2, FeO, Cu2O, CaO
Inorganic Compounds
Peroxides
anion: O2-2

O-I
• s1 elements (hydrogen and alkali metals): M2O2
• s2 elements (alkali earth metals): MO2
sodium peroxide
magnesium peroxide
barium peroxide
potassium peroxide
hydrogen peroxide
lithium peroxide
Inorganic Compounds
Hydroxides
anion: (OH)-1
• basic properties (pH > 7)
• strong or weak hydroxides
• metal / hydroxide anion
 use sufixes –ous / -ic
or
(oxidation state)
• ammonium / hydroxide anion
NaOH, LiOH, NH4OH, Fe(OH)3, Cu(OH)2, Ca(OH)2
Inorganic Compounds
Acids
cation: H+
(pH < 7)
1) oxygen free acids
hydro-...................-ic acid
HF, HCl, HBr, HI, H2S, HCN (in aqueous solutions)
anion: -ide
• monoprotic / diprotic acids
Inorganic Compounds
Acids
cation: H+
2) oxoacids
 the highest oxidative state
per-.....-ic acid
 higher (or only) oxidative state
-ic acid
 lower oxidative state
-ous acid
 the lowest oxidative state
hypo-...-ous acid
anion:
-ic acid
→
-ate
-ous acid
→
-ite
Inorganic Compounds
The most important oxoacids:
H2CO3
H2SiO3
H2CrO4
H3BO3
H3PO4
H2SO3
H2SO4
HNO2
HNO3
carbonic acid
silicic acid
chromic acid
boric acid
phosphoric acid
sulfurous acid
sulfuric acid
nitrous acid
nitric acid
→ carbonate
→ silicate
→ chromate
→ borate
→ phosphate
→ sulfite
→ sulfate
→ nitrite
→ nitrate
Inorganic Compounds
The most important oxoacids:
HClO
hypochlorous acid
HClO2
chlorous acid
HClO3
chloric acid
HClO4
perchloric acid
(or Br, I)
HMnO4
permanganic acid
→ hypochlorite
→ chlorite
→ chlorate
→ perchlorate
H2S2O2
H2S2O3
→ thiosulfite
→ thiosulfate
thiosulfurous acid
thiosulfuric acid
→ permanganate
Keep in mind the rules:
1. names of compounds are derived from the
names of cations, anions and polyatomic
ions: cation anion (NaCl = sodium chloride)
2. all binary compounds end in –ide
CaO, H2O2, NaCl, HF(g), ZnS
3. binary compounds composed of two
nonmetals: Greek prefixes
SO2, N2O5, CO
Keep in mind the rules:
4. binary compounds composed of a metal ion
with fixed or variable oxidation numbers
and nonmetal ion: no Greek prefixes
a) -ous / -ic suffix system
b) Stock system (prefered)
CuCl2, CuCl, Fe2O3, FeO
Keep in mind the rules:
5. ternary compounds:
 hydrogen cation H+ (= acid)
 or metal cation (= salt or hydroxide)
(fixed or variable oxidation number)
 and a polyatomic anion (e.g. SO42- or OH1-)
H2SO4
Na2SO4
NaOH
Total charge of a molecule = 0
Inorganic Nomenclature
Call the compounds:
Na2O, HCl, CO2, Na2O2, Ca(OH)2, KClO, HCN, HNO2,
H2S, H2O2, BaO2, PbO2, H2SO3, KOH, MgSO4, NaF,
NH4HCO3, HI, Al(OH)3, HIO4, CdS, MgO2, NaH2PO4
Chemical reactions
= chemical changes
stoichiometry = the reactants combine in simple wholenumber ratios (see stoichiometric coefficients: a, b, c, d)
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 the
rates of both the forward and back reactions are equal
Chemical reactions
equilibrium constant (K) describes the ratio of
concentrations of products and reactants in the
equilibrium
aA+bBcC+dD
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)
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 !!!
Chemical reactions
oxidative-reduction reactions = REDOX reactions
→ oxidation states of elements are changed !!!
• two changes:
 one element is oxidized (its ox. state raises)
 other element is reduced (its ox. state lowers)
2 HCl + Zn → ZnCl2 + H2
Zn0 → Zn+II
zinc is oxidized (0 → +II)
H+I → H0
hydrogen is reduced (+I → 0)
Important terms:
• reactants / products
• stoichiometric coefficients
• substance amount
• relative atomic / molecular mass
• molar mass
• density
• concentration (molar, percent)
Exercise – 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
Exercise – 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)