slide 1
NITROGEN STUDIES Saratova Shishkina I.Yu.slide 2
Nitrogen is made with water sprats of mіtsnih spoluk, among them the most important is ammonia. The electronic formula of the ammonia molecule is as follows: Otrimannya ammonia. Laboratory: 2NH4Cl + Ca(OH)2 = CaCl2 + 2NH3 + 2H2O Industrial: N2 + 3H2 2NH3 + 92 kJ
slide 3
Chemical characteristics 1. Ammiac is a strong agent. 3Cu+2O + 2N-3H3 = 3Cu0 + N20 + 3H2O 2N-3 – 6e = N 2 Cu2+ + 2e = Cu 3 4NH3 + 3O2 = 2N2 + 6H2O : Cr2O3 4NH3 + 5O2 = 4NO + 6H2O
slide 4
Ammonia with potassium permanganate: NH3 + KMnO4 = N2 + H2O + MnO2 +KOH Interaction with halogens: 2NH3 + 3Br2 = 6HBr + N2 2NH3 + 3Cl2 = 6HCl + N2
slide 5
2. ammonium salts. Reactions from zasnuvannyam donor-acceptor bond. NH3 + H2O NH3. H2O NH4+ + OH- NH4OH NH4+ + OH- H NH3 + H+Cl- [ H N H ]+ Cl- H
slide 6
ammonium salts Ammonium salts come out with the interaction of ammonia or other aqueous solutions with acids. NH3 + HNO3 \u003d NH4NO3 NH3H2O + HNO3 \u003d NH4NO3 + H2O Ammonium salts interchange with various meadows, acids and other salts: (NH4) Cl + NaOH \u003d NaCl + H2O + NH3 END. 2NH4Cl + H2SO4 = (NH4)2SO4 + 2HCl (NH4)2SO4 + BaCl2 = 2NH4Cl + BaSO4
Slide 7
The mustache of ammonium salts expands when heated. (NH4)2CO3 = 2NH3 + H2O CO2 NH4NO2 = 2H2O + N2 NH4Cl NH3 + HCl (NH4)2Cr2O7 = Cr2O3 + 4H2O + N2
Slide 8
A similar reaction to ammonium ion. NH4+ + OH-H2O + NH3
Slide 9
Oxide nitrogen. Nitrogen satisfies six sour periods. oxidation step +1 N2O +2 NO +3 N2O3 +4 NO2, N2O4 +5 N2O5
slide 10
N2O Removal: NH4NO = N2O +2H2O
slide 11
NO +2 Importance: 1. In nature: N2 + O2 = 2NO 2. In industry: 4NH3 + 5O2 = 4NO + 6H2O + 2SO2 = 2SO3 + N20 non-saline
slide 12
N2O3 +3 Chemical power: NO2 + NO N2O3 Other: All power of acid oxides. acid oxide
slide 13
NO2 +4 Other: 1. 2NO + O2 = 2NO2 2. Cu + 4HNO3(c) = Cu(NO3)2 + 2NO2 + 2H2O Chemical power: 1. with water 2NO2 + H2O = HNO3 + HNO2 2. with meadows 2NO2 + 2NaOH = NaNO3 + NaNO2 + H2O 3. dimerization 2NO2 N2O4 toxic
slide 14
N2O5 +5 Minor: 1. 2NO2 + O3 = N2O5 + O2 2. 2HNO3 + P2O5 = 2HPO3 + N2O5
slide 15
Nitric acid. Nitric acid retention: KNO3 + H2SO4 = HNO3 + KHSO4 In the laboratory, with weak heating: In the industrial process, the nitric acid retention process can be divided into three stages: 1. Oxidation of ammonia on a platinum catalyst to NO: 4NH3 + 5O2 = 4NO + 6H2O2. sour NO2 to NO2: 2NO + O2 = 2NO2
slide 16
HNO3 diluted concentrated puddles and puddles Fe, Su important metals NH4NO NH3 NO puddles and puddles and puddles N2O NO2 Fe Cr Au Al Pt passive not interacting
slide 17
Dissolved nitric acid. Concentrated nitric acid. Ag + 2HNO3 = AgNO3 + NO2 H2O 3Ag + 4HNO3 = 3AgNO3 + NO + 2H2O 4Zn + 10HNO3 (split) = 4Zn(NO3)2 + NH4NO3 + 3H2O
slide 18
Nitric acid interacting with non-metals, oxidizing them to hydrous acids: 3P + 5HNO3 + H2O = 3H3PO4 + 5NO C + 4HNO3 = CO2 + H2O + 4NO2
slide 19
Nitrates - salts of nitric acid, otrimuyut at diacid on metal, xoxide and hydroxide. Saltpeter - salts of nitric acid and tin metals. NaNO3 - sodium nitrate KNO3 - potassium nitrate NH4NO3 - ammonium nitrate Ca(NO3)2 - calcium nitrate
slide 20
When heated, nitrates are decomposed into sour (O2) t MeNO3 MeNO2 + O2 t MeNO3 MeO + NO2 + O2 t MeNO3 Me + NO2 + O2 to Mg in the form of Mg to Pb after Cu
slide 21
Saltpeter vikoristovuyutsya as kind. KNO3 is vicorated for the preparation of black powder.
slide 22
1 Ammiac for normal minds - tse ... 1) odorless gas without barrels 2) stormy, pungently smelling gas 3) barrelless, pungently smelling gas 4) barrelless country Testi: 2 Z concentrated nitric acid does not interact ... 1) Hg 2) Al 3) Cu 4) Zn 3 In industry, nitric acid is followed by the reaction: 1) NaNO3 (K) + H2SO4 (K) \u003d NaHSO4 + HNO3 2) Ba (NO3) 2 + H2SO4 \u003d BaSO4 + 2HNO3 3) 4NO2 + O2 + 2H2O \u003d 4HNO3 4) N2O5 + H2O \u003d 2HNO3 4 Ammonium salts react with meadows, that’s why when you ... up to a deaco deaky mineral dobriva vipav white siege. Calcium nitrate ... 1) calcium nitrate 2) potassium nitrate 3) ammonium nitrate 4) sylvinite 4) N2O5 9 with the greatest electrical negativity in the cases of May: 1) Be 2) B 3) S 4) N 10
slide 23
II option 1 nitric acid is a strong acid, that’s why… 1) it’s dissociated in water 2) it’s different 3) it’s strong oxidizer 4) it’s good in water 6 It’s rotten and it’s mineral good… 1) ammonium chloride 2) chloride nitrate 3) silvinit 4) superphosphate 4 ammonium salts according to water ... 1) good retail 2) bad retail 3) unrefined 4) ¾ retail and unrefined 3) N2O5 + H2O = 2HNO3 4) NaNO3(K) + H2SO4(K) = NaHSO4 + HNO3 HNO3 N2O +… + H2O is good 1) 1 2) 2 3) 3 4) 4 2 H2SO4 3) H2CO3 4) H3SiO3 9
slide 24
1. Decompose the mass of ammonia, which is required for the extraction of 200 kg of nitric acid with a mass fraction of HNO3 60%. When rozrahunka vrahuyte, scho often output end product during synthesis to become 80%. Task: 2. When heated with sodium nitrate, the sour mixture is 280 ml (normal wash). Yaka masa salt was recognized by the distribution. 3. Degrease the mass of calcium(II) hydroxide, which can be neutralized with the help of 630 g of nitric acid, in which the mass fraction of HNO3 is 20%. mass 300 g. Designate the mass fraction of the output of ammonium nitrate. 5. On the sum of midi and midi (II) oxide, 75 g of weight was added with excess HNO3 (concentrated). With this, the gas was settled with a total of 26.88 liters (normally wash). Assign the mass fraction to the mid(II) oxide in the outer sum. 6. Ammia with a volume of 7.84 l (normal urine) was recognized as catalytic oxidation and further conversion to nitric acid. As a result, they won a prize of 200g. Considering the HNO3 output is equal to 40%, take the mass fraction in the original range.
Nitrogen(I) oxide N2O
N2O - nitric oxide (I), nitrous oxideabo "cheerful gas",
zbudzhuyuche dіє on
human nervous system
vikoristovuyut in medicine like
anesthetic zasib.
Physical power: gas, without
color and smell. Viyavlyaє
oxide of power, easy
spread out. non-saline
oxide.
2N2O = 2N2 + O2
Nitrogen(II) oxide
NO - nitrogen oxide (I I)barrelless gas, thermal
stable, rotten
water, practical mittevo
interaction with sour
(At room temperature).
non-saline oxide.
2NO+ O2= 2NO2
Nitrogen(III) oxide
N2O3 – nitric oxide (III) rіdinadark blue color, thermal
nesting, t kip. = 3.5 0С, tobto.
іsnuє in a rare state
only when cold, in animals
minds go over gas
mill. Acid oxide, at
get settled with water
nitrous acid.
N2O3 + H2O = 2HNO2
Nitrogen(IV) oxide
NO2 - nitrogen oxide (IV) or dioxidenitrogen, brown gas, good retail
the water will more and more react with it.
Є strong oxide.
2NO2 + H2O = HNO2 + HNO3
Disproportionation reaction
Shows all powers
acid oxides
Oxide to nitrogen (V)
N2O5 - oxidenitrogen (V),
nitrogenous
anhydride, bile
harder
speech (tpl. =
410C). Viyavlyaє
acidic
dominance, є
even stronger
oxidizing.
The product of the reaction
acidic
oxide and water
acid
Nitric acid. HNO3
nitrogen4HNO3=4NO2+2H2O+O2
acid
–
bezbarvna
hygroscopic
Motherland, May sharp
smell,
"dim"
on the
povitri, uncircumcised
disperse by the water,
tbp = 82.6 0С. Rozchini
nitric acid and save
at the jar of dark
slope,
those.
tobto.
won
laid out on the light: stock. Budov. power.
HNO3
H-O-N
O
O
nitrogen oxidation stage
valency to nitrogen IV
+5
chemical link
covalent polar Nitric acid (HNO3)
Classification
Nitric acid for:
I'm sour:
kissen revenge
basicity:
diversity near the water:
monobasic
retail
volatility:
flying
stage of electrical dissociation:
strong Obsession with nitric acid in industry
NH3
NO
NO2
1. Contact oxidation of ammonia to
nitric oxide (II):
4NH3+ 5O2 = 4NO + 6H2O
2. Oxidation to nitric oxide (II) into oxide
nitrogen (IV):
2NO+O2 = 2NO2
3. Adsorption (claying) oxide
nitrogen (IV) water with excess sour
4NO2 + 2H2O + O2 = 4HNO3
HNO3 In the laboratory, nitric acid is obtained
concentrated sulfuric acid on nitrate at
weak heating.
Store the equal reaction of the presence of nitric acid.
NaNO3 + H2SO4 = NaHSO4 + HNO3
1. Types of dominance of acids
2. Interaction of nitric acid with metals
3. Interactions of nitric acid with non-metals Chemical power of nitric acid
Nitric acid shows all types of dominance of acids.
Override the dominance characteristic of acids.
Acids interact with basic and amphoteric
oxides, with bases, amphoteric hydroxides,
salts.
Store equal reactions of nitric acid:
1 with midi (II) oxide, aluminum oxide;
2 with sodium hydroxide, zinc hydroxide;
3
with ammonium carbonate, sodium silicate.
Look at the reactions from t. sp. TED.
Give the names of the otrimanim speeches. Designate type
reactions. 1
2HNO3 + CuO = Cu(NO3)2 + H2O
2H+ + 2NO3– + CuO = Cu2+ + 2NO3– + H2O
2H+ + CuO = Cu2+ + H2O
6HNO3 + Al2O3 = 2Al(NO3)3 + 3H2O
6H+ + 6NO3– + Al2O3 = 2Al3+ + 6NO3– + 3H2O
6H+ + Al2O3 = 2Al3+ + 3H2O
2
HNO3 + NaOH = NaNO3 + H2O
H+ + NO3– + Na+ + OH– = Na+ + NO3– + H2O
H+ + OH– = H2O
2HNO3 + Zn(OH)2 = Zn(NO3)2 + 2H2O
2H+ + 2NO3– + Zn(OH)2 = Zn2+ +2NO3– + 2H2O
2H+ + Zn(OH)2 = Zn2+ + 2H2O 3
2HNO3 + (NH4)2CO3 = 2NH4NO3 + CO2 + H2O
2H+ + 2NO3– + 2NH4+ + CO22– = 2NH4+ +2NO3– + CO2 + H2O
2H+ + CO22– = CO2 + H2O
2HNO3 + Na2SiO3 = ↓H2SiO3 + 2NaNO3
2H+ + 2NO3– + 2Na+ + SiO32– = ↓H2SiO3 + 2Na+ + 2NO3–
2H+ + SiO32– = ↓H2SiO3
Active acids and vitamins remove weak cells or
non-refining acids from refining salts. Interactions of nitric acid with metals
How do metals react with different acids?
metal,
stand
at low activity
to acidity
water,
take off
Features
vzaimodії
nitrogen
with metals:
yoga
isodine
acids.
metal,
stand
after water
acid yogo
1. Hi
metal
never
don't see
with nitric acid
not
take off,
tobto. do not interact
with acids
not
water.
Seen
different business
nitrogen:
vary
them. N2+1O, N20,
N+4O2, N+2inO,
N-3H3 (NH4NO3)
N-3H4+
N20
N2+1O
N+2O
N+4O2
acid concentration
metal activity
2. Metals react with nitric acid, which stand up to i
after a week of activity.
dosvid
dosvid
3. Nitric acid does not interact with Au, Pt
4. Concentrated nitric acid passive metal:
Al, Fe, Be, Cr, Ni, Pb and others
oxide melting). When heated and when diluted with nitrogen
acids and metals are different in them.
dosvid Store equal reactions in combination with concentrated
nitric acid and mercury. Look at the reaction from t. sp. OVR.
4HN+5O3 + Hg0 = Hg+2(NO3)2 + 2N+4O2 + 2H2O
N+5 + 1e → N+4 1 2
Hg0 – 2e → Hg+2 2 1
HNO3 (for N+5 scale) – oxide, renewal process;
Hg0 - oxidizer, oxidation process. Add reaction schemes:
1)
HNO3(conc.) + Cu → Cu(NO3)2 + … + H2O
2)
HNO3(rozb.) + Cu → Cu(NO3)2 + … + H2O
Take a look at the transformation at the OVR light
1) 4HN+5O3(conc.) + Cu0 = Cu+2(NO3)2 + 2 N+4O2 + 2 H2O
oxidizer
guide
N+5 + 1e → N+4 1 2
Cu0 – 2e → Cu+2 2 1
renewal
oxidation
2) 8 HN+5O3(conc.) + 3 Cu0 = 3Cu+2(NO3)2 + 2 N+2O + 4 H2O
oxidizer
guide
N+5 + 3e → N+2 3 2
Cu0 – 2e → Cu+2 2 3
renewal
oxidation Interactions of nitric acid with non-metals
Nitric acid is a strong oxide
Oxidize non-metal to vydpovidnyh acids.
Concentrated (more than 60%) nitric acid restores up to
NO2, and also the concentration of acid (15 - 20%), then to NO.
Find the coefficients in the schemes using the electronic balance method.
4 HNO3 + С → СO2 + 2 H2O + 4 NO2
N+5 + 1e → N+4 1 4
С0 – 4e → С+4 4 1
dosvid
HNO3 (for N+5 rahunok) – oxidizing agent, in.
C - oxidizer, oxidation process
5 HNO3 + P → H3PO4 + 5 NO2 + H2O
dosvid
N+5 + 1e → N+4 1 5 HNO3 (for N+5) – oxidising agent, in.
P - oxidizer, oxidation process
P0 – 5e → P+5 5 1
5 HNO3 + 3 P + 2 H2O → 3 H3PO4 + 5 NO
N+5 + 3e → N+2 3 5 HNO3 (for N+5) – oxidizer, in.
P0 – 5e → P+5 5 3 P – redundant, oxidation process Stasis of nitric acid
1
Variety of nitrogen and complex compounds
dobriv.
2
The production of vibukhov speeches
3
Variety of barvniks
4
Virobnitstvo likіv
5
Weaving,
nitrolacquers, nitroemals
6
Virobnitstvo
piece fibers
7
As a component of nitrous
sumishi, for trawling
metals in metallurgy Salts of nitric acid
What are the salts of nitric acid called?
spend
Nitrates K, Na, NH4+ are called saltpeters
Store the formulas for resurfacing salts.
KNO3
NaNO3
NH4NO3
Nitrati - white crystal
speeches. Stronger electricity,
in some ways dissociate
on ion. Join the exchange reaction.
How can you identify nitrate-ion in retail?
To salt (what to avenge nitrate-ion) add to the sirchan
acid and mid. Sumіsh trohi play. Vision
brown gas (NO2) to indicate the presence of nitrate-ion. Potassium nitrate (potassium nitrate)
Bezbarvni crystals Significantly
less hygroscopic in porous soil
sodium, so it is widely zastosovuєtsya in pyrotechnics as an oxide.
When heated to 334.5 ºС
melt higher than the temperature
spread out from the sight of the sour.
sodium nitrate
Zastosovuetsya like kindness; in
glassware,
metalworking industry; for otrimanna
vibukhovi
speeches,
missile
paleva and pyrotechnical sumishes. ammonium nitrate
Crystalline
speech
white
colori. Melting point 169.6 °C,
when heated more per qiu temperature
start step by step
layout
speech, and at a temperature of 210 ° C
vіdbuvaєtsya outside the layout. When heated, they are laid out more, lower
to the right in the electrochemical series, the metal is stressed,
I make strength.
Li K Ba Ca Na
Mg Al Mn Zn Cr Fe Co Sn Pb Cu
nitrite + O2
metal oxide + NO2 + O2
Ag Hg Au
Me + NO2 + O2
Store equal reactions to nitrate
sodium, lead nitrate, silver nitrate.
2NaNO3 = 2NaNO2 + O2
2Pb(NO3)2= 2PbO + 4NO2 + O2
2AgNO3 = 2Ag + 2NO2 + O2
Stasis of nitric acid.
PlasticsBarvniki
Dobriva
Vibukhov speeches
Faces
"Oxid vugletsyu IV" - Nezabar water becomes kalamutnoy. Physical power of CO2. Dry Ice Non-toxic, do not conduct electrical strum. Zastosuvannya oxide of carbon (ІV). Dry ice is also CO2. A gas required by roslin for photosynthesis. In nature. The amount of carbon dioxide in the atmosphere is perceptibly small 0.04 - 0.03.
"Nitric oxide" - 2. Cylinder with nitrogen oxide (II) closed with a plate. Oxidizing agent: 2NO + 2SO2 = 2SO3 + N2 Nitrous method of containing sulfuric acid. 1. Three closed cylinders: with nitric oxide (IV), with nitrogen, with ammonia. No-oxide to nitrogen (II). Kindness spreads by the water. N2O5. All oxides to nitrogen, cream N2O, є brittle cavities.
"The layout of oxides" - the classification of oxides. Basic oxides. Oksidi. Amphoteric oxide. Acid oxides. Glossary. Indifferent oxides (non-saline). Classif. Zmist. Manager. Dopomoga for uchniv.
"Oxidi" - in nature. Metal ore. CHROME OXIDE cr2o3. The amount of carbon dioxide in the atmosphere is perceptibly small, totaling 0.04-0.03%. Bilila. For example: chervonium, magnetic and stormy floods, bauxite (aluminum oxide), a gas required for photosynthesis by roslins. Carbon oxide (II) CO. Titanium oxide (IV) - TiO2 - has the same power values.
"Oxide of coal" - For oxide of coal (II) it is characteristic for its power. but carbon dioxide is a gas without color and smell. Z. Vugletsyu oxide (II). Carbon oxide (IV). Obsession with carbon dioxide (IV). Vikoristani TsOR: Demonstration planning. Oxide the corner.
“Khimichni oksidi” - speeches, to the warehouse of which kisen enter. Quartz sand. H2O. Carbon oxide (IV). Oksidi - folded speech. Boxing. The pigment is olive-green farby. It's not extinguished. Metal oxide. Oksidi. Carbon oxide (II).
Themes have 14 presentations in total