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Ammonia NH 3 Kirillova Margarita Alekseevna teacher of chemistry at Lyceum No. 369 of the Krasnoselsky district

The structure of the nitrogen atom N Nitrogen 14.0067 2 5 7 2 s 2 2p 3 N 7 N II period V group 2 s 2p , each with one unpaired electron.

Formation of the ammonia molecule When bonds are formed in the ammonia molecule, the nitrogen atom is in the state of sp 3 - hybridization. 109 0 28 ’: N + H: N: H H H H: : H       H H H The shape of the molecule is pyramidal. H: : H

The structure of ammonia molecules Hydrogen bonds form between ammonia molecules: N-H bonds polar, the molecule has a pyramidal shape, common electron pairs are shifted towards the nitrogen atom. One of the vertices is occupied by a lone pair of electrons. The molecule is highly polar.

Physical properties of ammonia A colorless gas with a pungent odor. Almost two times lighter than air: When cooled to -33 0 C - c liquefies. It dissolves very well in water, tk. hydrogen bonds are formed between ammonia molecules and water molecules (700 V of ammonia dissolves in 1 V of water. 10% solution is “ammonia alcohol”. A concentrated solution contains 25% ammonia.

Methods for producing ammonia In industry: N 2 + 3H 2 2NH 3 The reaction is carried out by heating, under pressure, in the presence of a catalyst. In the laboratory: The action of alkalis on ammonium salts: 2NH 4 Cl + Ca (OH) 2 \u003d CaCl 2 + 2NH 3  + 2H 2 O Hydrolysis of nitrides: Mg 3 N 2 + 6H 2 O \u003d 3Mg (OH) 2 + 2NH 3 

Chemical properties ammonia NH 3 - the lowest oxidation state of nitrogen. -3 1. Ammonia - reducing agent Ammonia combustion reaction: 4NH 3 + 3O 2 = 2N 2 + 6H 2 O Catalytic oxidation of ammonia: 4NH 3 + 5O 2 = 4NO + 6H 2 O Ammonia can reduce some inactive metals: 3CuO + 2 NH 3 \u003d 3Cu + N 2 + 3H 2 O

II. The main properties of ammonia: When ammonia is dissolved in water, ammonia hydrate is formed, which dissociates: NH 3 + H 2 O NH 3  H 2 O NH 4 + + OH - ammonium ion Changes the color of indicators: Phenolphthalein - b / color  raspberry Methylorange - orange  yellow Litmus - violet  blue Forms ammonium salts with acids: NH 3 + HCl \u003d NH 4 Cl ammonium chloride 2NH 3 + \u003d (NH 4) 2 SO 4 ammonium sulfate NH 3 + H 2 SO 4 \u003d NH 4 HSO 4 ammonium hydrosulfate

The formation of the ammonium ion NH 3 + H + \u003d NH 4 + H:: H H:: H N N: H: + H + H:: H H:: N N: H: + The nitrogen atom is in the state of sp 3 - hybridization. Three bonds are formed by the exchange mechanism, the fourth - by the donor-acceptor mechanism. The donor, the nitrogen atom, provides a pair of electrons. The acceptor - ion H + - provides an orbital.

Ammonium salts The ammonium ion is similar in size and charge to ions alkali metals, so ammonium salts are similar to alkali metal salts. Crystalline substances. white color. Well soluble in water. Their dissolution in water is accompanied by the absorption of heat. Qualitative reaction on the ammonium ion - the interaction of salts with alkali solutions: NH 4 NO 3 + NaOH \u003d NaNO 3 + NH 3  + H 2 O characteristic pungent smell of ammonia

Decomposition of ammonium salts when heated Salts of volatile acids: NH 4 Cl \u003d NH 3 + HCl (NH 4) 2 CO 3 \u003d 2NH 3 + CO 2 + H 2 O C oli of non-volatile acids: (NH 4) 2 SO 4 \u003d NH 4 HSO 4 + NH 3  (NH 4) 3 PO 4 \u003d (NH 4) 2 HPO 4 + NH 3  without heating (NH 4) 2 HPO 4 \u003d NH 4 H 2 PO 4 + NH 3  with heating Salts with an oxidizing anion : (NH 4) 2 Cr 2 O 7 \u003d N 2  + Cr 2 O 3 + 4H 2 O NH 4 NO 3 \u003d N 2 O + 2H 2 O NH 4 NO 2 \u003d N 2 + 2H 2 O

Nitric acid Ammonium nitrate Ca(NO 3) 2 Ammonium sulfate (NH 4) 2 SO 4 Ammonium chloride NH 4 Cl Carbamide (urea) CO(NH 2) 2 Ammonia water NH 3  H 2 O Liquid ammonia NH 3 Ammonia Nitrogen fertilizers Drug production Rocket Fuel Oxidizer Ammonium Salts for Soldering Manufacturing explosives Obtaining soda refrigerant in industrial refrigeration units Production of photographic film and dyes Processing of precious metals Use of ammonia and ammonium salts

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AMMONIA

Completed students of 9 "B" class Nesterova M.; Shutkina Alena

• The composition of the substance
• The structure of matter
• How to get
• Chemical properties
• Formation of the ammonium ion

The composition of the substance

N +7)) II period H +1) I period

Nitrogen 2 5 V group Hydrogen 1 I group

NH 3

The structure of matter

The molecule is formed by a covalent polar bond

How to get

In industry:

In the laboratory:

The action of alkalis on ammonium salts:

2NH4Cl + Ca(OH)2 = CaCl2 + 2NH3 + 2H2O

Hydrolysis of nitrides:

Mg3N2 + 6H2O = 3Mg(OH)2 + 2NH3

The reaction is carried out under heating, under pressure,

in the presence of a catalyst.

• Colorless gas with a pungent odor
• Almost twice as light as air
• When cooled to -33 degrees - liquefies
• 10% solution - “ammonia”.
• Concentrated solution contains 25% ammonia
• It dissolves very well in water, since hydrogen bonds are formed between ammonia molecules and water molecules (700 V of ammonia dissolves in 1 V of water.

Chemical properties

• The combustion reaction of ammonia:

4NH 3 + 3O 2 = 2N 2 + 6H 2 O

• Catalytic oxidation of ammonia:

4NH 3 + 5O 2 = 4NO + 6H 2 O

• Ammonia can restore some

inactive metals:

3CuO + 2NH 3 = 3Cu + N 2 + 3H 2 O

II. The main properties of ammonia:

• When ammonia is dissolved in water, it forms

ammonia hydrate, which dissociates:

NH 3 + H 2 O NH 3 H 2 O NH 4 + +OH -

• Changes indicator coloring :

Phenolphthalein - b / color  crimson

Methyl orange - orange  yellow

Litmus - purple  blue

• Forms ammonium salts with acids:

NH 3 + HCl =NH 4 Cl ammonium chloride

2NH 3 + = (NH 4 ) 2 SO 4 ammonium sulfate

NH 3 + H 2 SO 4 =NH 4 HSO 4 ammonium hydrosulfate

Formation of the ammonium ion

The nitrogen atom is in the -hybridized state. Three bonds are formed by the exchange mechanism, the fourth -

according to the donor-acceptor.

The donor, the nitrogen atom, provides a pair of electrons.

Acceptor - ion H + - provides

orbital.

The use of ammonia and ammonium salts

refrigerant in

industrial

refrigeration

installations

Receipt

soda

Production

medicines

Production

photographic film and

dyes

Ammonia

Oxidizer

missile

fuel

Nitric acid

Treatment

precious

metals

salt

ammonium

soldering

Nitrogen

fertilizer

Ammonium nitrate Ca(NO 3 ) 2

Ammonium sulfate (NH 4 ) 2 SO 4

Ammonium chloride NH 4 Cl

Carbamide (urea) CO(NH 2 ) 2

Ammonia water NH 3  H 2 O

Liquid ammonia NH 3

Production

explosive

substances

Ammonia

Tasks to repeat

• Carry out a chain of transformations:
• N 2 →Li 3 N→NH 3 →NO→NO 2 →HNO 3

• Determine the coefficients in the reaction equation using the electron balance method:
• Determine the coefficients in the reaction equation using the electron balance method:

• NH 3 + O 2 → NO + H 2 O
• NH 3 + O 2 → N 2 + H 2 O

This story took place during World War I.

The structure of ammonia

(NH 3 )

+7 N ))

+1 h)

Physical Properties

• Ammonia - this is colorless gas with sharp smell, 2 times lighter than air .

• Ammonia should not be inhaled for a long time, because. he poisonous.
• It liquefies easily.
• On contact with the skin, frostbite of varying degrees occurs.
• T pl = -78 0 FROM
• Highly soluble in water:

a) 25% solution - aqueous ammonia (ammonia water)

B) 10% solution - ammonia.

T kip = -33,5 0 FROM

Chemical properties

• According to the donor-acceptor mechanism:

A) Interaction with acids:

NH 3 + HCl \u003d NH 4 Cl

:NH 3 +□H + = NH 4 +

B) Interaction with water:

NH 3 + H 2 O ↔ NH 4 OH

ACCEPTOR

DONOR

Chemical properties

2) Interaction with metals:

2NH 3 + Na \u003d NaNH 2 + H 2

2NH 3 + O 2 \u003d 2H 2 O + N 2

2NH 3 + 3Br 2 \u003d 6HBr + N 2

Ammonia production

1) Industrial: synthesis from nitrogen and hydrogen:

N 2 + 3H 2 ↔2NH 3

2) Laboratory:

Ca (OH) 2 + NH 4 Cl \u003d CaCl 2 + NH 3 + 2H 2 O

Receipt

In the laboratory

NH 3

NH 4 Cl

Ca(OH) 2

Application

Production of nitrogen

In refrigeration

installations.

In medicine,

for soldering

Production

fertilizer

Production

explosive

Check of knowledge

1. What is the oxidation state of nitrogen in ammonium nitrate?

2. Compose chemical equations the following transformations:

nitrogen→ammonia→ammonium chloride

3. Additional task: Determine the coefficients in the following diagram chemical reaction using the electronic balance method:

Cu + NH 3 → N 2 + Cu + H 2 O

Homework

Ammonia NH3

Ammonia - NH3, hydrogen nitride, under normal conditions - a colorless gas with a pungent characteristic odor (the smell of ammonia)
Ammonia is almost twice as light as air, MPCr.z. 20 mg/m3 - IV hazard class (low hazardous substances) according to GOST 12.1.007. The solubility of NH3 in water is extremely high - about 1200 volumes (at 0 °C) or 700 volumes (at 20 °C) in a volume of water. In refrigeration, it is called R717, where R is Refrigerant (refrigerant), 7 is the type of refrigerant (inorganic compound), 17 is the molecular weight.

The ammonia molecule has the shape of a trigonal pyramid with a nitrogen atom at the top. Three unpaired p-electrons of the nitrogen atom participate in the formation of polar covalent bonds with 1s-electrons of three hydrogen atoms (N-H bonds), the fourth pair of external electrons is lone, it can form a donor-acceptor bond with a hydrogen ion, forming an ammonium ion NH4+. Due to the fact that the non-bonding two-electron cloud is strictly oriented in space, the ammonia molecule has a high polarity, which leads to its good solubility in water.

Condition (St. cond.)tgas

Molar mass t17.0306 g/mol
Density t0.0007723 (n.s.)
Physical Properties

Condition (St. cond.)tgas
Rel. molek. mass t17.0306 a. eat.
Molar mass t17.0306 g/mol
Density t0.0007723 (n.s.)
Physical Properties

Condition (St. cond.)tgas
Rel. molek. mass t17.0306 a. eat.
Molar mass t17.0306 g/mol
Density t0.0007723 (n.s.)
Physical Properties

Application

Ammonia is one of the most important products of the chemical industry, its annual world production reaches 150 million tons. It is mainly used for the production of nitrogen fertilizers (ammonium nitrate and sulfate, urea), explosives and polymers, nitric acid, soda (ammonia method) and other chemical products. Liquid ammonia is used as a solvent.
In refrigeration, it is used as a refrigerant (R717)
In medicine, a 10% ammonia solution, often called ammonia, is used for fainting (to stimulate breathing), to stimulate vomiting, as well as externally - neuralgia, myositis, insect bites, and to treat the hands of a surgeon. If used incorrectly, it can cause burns of the esophagus and stomach (in case of taking an undiluted solution), reflex respiratory arrest (when inhaled in high concentrations).
Apply topically, inhalation and inside. To excite breathing and bring the patient out of fainting, carefully bring a small piece of gauze or cotton wool moistened with ammonia to the patient's nose (for 0.5-1 s). Inside (only in breeding) to induce vomiting; also, as part of ammonia-anise drops - as a mucolytic (expectorant) agent. With insect bites - in the form of lotions; with neuralgia and myositis - rubbing with ammonia liniment. In surgical practice, they are bred in warm boiled water and wash their hands.
Since ammonia is a weak base, it neutralizes acids when interacting with them.
The physiological effect of ammonia is due to the pungent smell of ammonia, which irritates specific receptors of the nasal mucosa and excites the respiratory and vasomotor centers of the brain, causing increased breathing and increased blood pressure.
Antifreeze additive for dry mortars related to accelerators. The recommended dosage is 2…8% by weight of the components of the dry mixture, depending on the application temperature. Ammonia water is a product (NH3*H2O), which is gaseous ammonia NH3 dissolved in water.
Application

For insect bites, ammonia is applied externally in the form of lotions. A 10% aqueous ammonia solution is known as ammonia.
Side effects are possible: with prolonged exposure (inhalation use), ammonia can cause reflex respiratory arrest.
Topical application is contraindicated in dermatitis, eczema, other skin diseases, as well as open traumatic injuries of the skin.
In case of accidental damage to the mucous membrane of the eye, rinse with water (for 15 minutes every 10 minutes) or a 5% solution of boric acid. Oils and ointments are not used. With the defeat of the nose and pharynx - 0.5% solution of citric acid or natural juices. In case of ingestion, drink water, fruit juice, milk, preferably 0.5% citric acid solution or 1% acetic acid solution until the contents of the stomach are completely neutralized.
Interaction with other drugs is unknown.
Ammonia in medicine