This document discusses hydrides of nitrogen, including ammonia and hydrazine. It provides details on their structures, properties, preparation methods, and uses. Ammonia is a colorless gas that is lighter than air. It is prepared through reactions involving ammonium chloride or metal nitrides. Ammonia is used as a fertilizer and cleaning product. Hydrazine is a reducing agent that exists as a colorless liquid. It is prepared through reactions of sodium hypochlorite with ammonia or urea. Both compounds are discussed in terms of their molecular structures and chemical properties.

1. DEPARTMENT OF CHEMISTRY
KIRORI MAL COLLEGE
ASSIGNMENT
GE-CHEMISTRY
SUBMITTED BY :SWATI SINGH
SUBMITTED TO :DR.ARUN KANT SIR
ROLL NO :1934127
COURSE :B.Sc BOTANY (HONOURS)

2. ASSIGNMENT TOPIC
Hydrides of Nitrogen
•What is hydride
•Example of hydride
•Uses of hydride
•Ammonia (NH3)
•Introduction
•Properties
•Structure
•Preparation
•Chemical reaction
•Uses
•Hydrazine (N2H4)
•Introduction
•Properties
•Structure
•Preparation
•Chemical reaction
•Uses

3. •What is hydrides?
•Hydride, in simple terms, is said to be the anion of hydrogen.
•It is a chemical compound where the hydrogen atoms exhibit
nucleophilic, basic or reducing properties.
• Usually, in a hydride, the hydrogen has the oxidation
number equal to −1.
• Some of the most popular examples include water (H2O),
methane (CH4) and ammonia (NH3). What are Hydrides.
•However, the properties may vary depending on the type of
intermolecular force that exists between the elements, its
molecular masses, temperature, and other factors.

4. Types of Hydrides
Hydrides are mainly divided into three major types or groups. The categories are
decided based on what elements the hydrogen forms bonds with or simply on the
basis of chemical bonding. The three types of hydrides are ionic, covalent, and
metallic hydrides.
•Ionic Hydrides: Nah, KH, CaH2, etc. These contain hydrogen as the negatively charged (H–) ion.
•Covalent Hydrides: SiH4 (silane)
•Metallic Hydrides: TiH aluminium, cadmium, magnesium, etc.
Uses of Hydride
•They are used as reducing agents in many chemical industries.
•Hydrides are highly significant in battery storage technologies such as nickel hydride batteries.
•They are used as drying agents.
•They are used as strong bases in organic synthesis.
•Metal hydrides are also used for their heat storage, hydrogen storage and compressors
capabilities.

5. Ammonia
Ammonia is a colorless gas with a chemical
formula NH3.
It consists of hydrogen and nitrogen.
 In its aqueous form, it is called ammonium
hydroxide.
This inorganic compound has a pungent
smell.
In its concentrated form, it is dangerous and
caustic.
Ammonia is lighter than air with a density of
0.769 kg/m3 at STP.

6. Properties of Ammonia
Properties of Ammonia Value
Molecular Weight/ Molar Mass 17.031 g/mol
Density 0.73 kg/m3
Boiling Point 33.34 °C
Melting Point 77.33 °C

7. STRUCTURE OF NH3
i)3D Structure ii)Lewis Structure

8. • Ammonia is a covalent atom.
• It is seen as a dot structure.
• The particle is shaped because of the overlap of orbitals
of three hydrogen atoms and three sp3 hybrid orbitals of
nitrogen in the structure as the central atom.
• The fourth sp³ hybrid orbital is involved by a lone pair.
• This provides a trigonal pyramidal shape to the
compound. The H-N-H bond edge is 107.3°, which is
somewhat not exactly the tetrahedral edge of 109°28.
• This is on the grounds that the bond pair-lone pair
repulsions push the N-H bonds somewhat inwards. In
solid and liquid states, ammonia is related through
hydrogen bonds.
EXPLANATION OF STRUCTURE OF NH3

9. PREPARATION
1)From Ammonium Chloride
We can generate ammonia gas in the research centre by slowly heating ammonium
chloride (NH4Cl) and slaked lime [Ca(OH)2].
REACTION:
2)By the Hydrolysis of Metal Nitrides
Hydrolyzing metal nitrides like magnesium and aluminium nitrides, with
water or alkalis, can likewise deliver ammonia gas.
REACTION:

11. CHEMICAL PROPERTIES
1) Thermal Stability
Ammonia is exceptionally inert. In any case, we can disintegrate it into
hydrogen and nitrogen by advancing over metallic impetuses that
have been heated.
2) Combustibility
It is flammable in air.
3) Basic Character
The compound has a natural propensity to give its lone pair
electrons of nitrogen to different atoms. Consequently, it acts likes a
strong Lewis base.

12. USES OF AMMONIA(NH3)
• NH3 Uses (Ammonia)
• It is used as fertilizers as it increases the yield of crops
• It is used in the household as a cleaner – NH3 is mixed with water to
clean stainless steel and glass
• It is used in food products as an antimicrobial agent
• It is used in the fermentation industry
• It is used as a refrigerant
• It is used as a pH adjuster in the fermentation process
• It is used to neutralize pollutant like nitrogen oxides emitted from
diesel engines
• It is used as a fuel for rocket engines
• It is used in textile industries
• It is used in the manufacture of synthetic fiber like rayon and nylon

14. HYDRAZINE (N2H4)
• Hydrazine, (N2H4), is a powerful reducing agent.
• It is used in the synthesis of various pesticides, as a base for
blowing agents that make the holes in foam rubber, and as a
corrosion inhibitor in boilers
• Hydrazine is also called as Diamine or Diazane or Nitrogen
hydride and is a strong base
• It is an azane and dangerously unstable. Each subunit of H2N-N
is pyramidal and the N−N bond distance is about 1.45 Å
• Diamine in its anhydrous form, is a colorless, fuming oily liquid
which smells like ammonia. It has a flash point value of 99°F. In
case if traces of air is present during the process of distillation, it
explodes. It is toxic and corrosive to tissues. When it
undergoes combustion, it generates toxic oxides of nitrogen.

15. of Hydrazine
1.3D Structure 2. Lewis Dot
Structure

16. EXPLANATION OF STRUCTURE
• The chemical formula of hydrazine is NH2NH2.
• Its molecular formula is N2H4, and its molar mass is
32.04 g/mol.
• The chemical structure is shown below consisting of
two NH2 groups covalently attached.
• Each of the N-NH2 groups adopts a pyramidal shape.

17. PROPERTIES VALUE
Molecular weight/molar mass 32.0452 g/mol
Density of Hydrazine 1.021 g/cm3
Boiling Point of Hydrazine 114 °C
Melting Point of Hydrazine 2 °C
Properties of Hydrazine – N2H4

18. Preparation
The commercial production of hydrazine is by the Raschig process, in
which sodium hypochlorite solution is treated with excess ammonia
to form a chloramine intermediate, which then gives the final
hydrazine product along with hydrochloric acid.
NaOCl + NH3 → H2N-NH2 + HCl
• It can also be prepared in a related process by using urea (H2N-CO-
NH2) instead of ammonia:
H2N-CO-NH2 + NaOCl + 2 NaOH → N2H4 + H2O + NaCl
+ Na2CO3

19. REACTION OF HYDRAZINE
Hydrazines are part of many organic syntheses.

20. HYDRAZINE DERIATIVE

21. Production of Hydrazine
• Diamine can be obtained from hydrogen peroxide
and ammonia in the ketazine process or Pechiney-
Ugine - Kuhlmann process. The reaction is as follows:
2NH3 + H2O2 → H2NNH2 + 2H2O
• Chloramines reacts with ammonia to generate
nitrogen–nitrogen single bond and hydrogen chloride
as byproducts. The reaction is as follows:
NH2Cl + NH3 → H2NNH2 +HCl

22. • Hydrazine is used as a propellant in space vehicles.
• It is used as a precursor in several pharmaceutical
products.
• It is used as a reducing agent for selenium, arsenic,
and tellurium
• It is used as a corrosion inhibitor in cooling water
reactor.
• It is used in the process of electrolytic plating of
metals on plastic and glass.
• Used in the manufacturing of agricultural chemicals.
• Used as a solvent for inorganic compounds.
USES OF HYDRAZINEUSES OF
HYDRAZINEUSES OF HYDRAZINE
USES OF HYDRAZINE
Hydrazine is used as a propellant in space vehicles.
It is used as a precursor in several pharmaceutical
products.
It is used as a reducing agent for selenium, arsenic, and
tellurium
It is used as a corrosion inhibitor in cooling water reactor.
It is used in the process of electrolytic plating of metals
on plastic and glass.
Used in the manufacturing of agricultural chemicals.
Used as a solvent for inorganic compounds.