4% solution of ethylnitrite in alcohol is known as sweet spirit of nitre and in used as diuretic.

The N₂CI group can be replaced by alkoxy group by warming with alcohol or by acyloxy group by boiling with carboxylic acids.

Esters containing at least one ∝- hydrogen atom undergo self condensation in the presence of a strong base such as sodium ethoxide to form β-keto ester.

(i) for the dehydration of hides.
(ii) as a coagulating agent for rubber latex
(iii) in medicine for treatment of gout
(iv) as an antiseptic in the preservation of fruit juice.

Carboxylic acid reacts with alcohols in the presence of mineral acid as catalyst and forms esters. This reaction is called esterlfleatlon.
\(\underset { Acetic\ acid }{ { CH }_{ 3 }COOH } +\underset { Ethyl\ alcohol }{ { C }_{ 2 }{ H }_{ 5 }OH } \overset { Conc.{ H }_{ 2 }{ SO }_{ 4 } }{ \longrightarrow } \underset { Ethyl\ acetate }{ { CH }_{ 3 }{ COOC }_{ 2 }{ H }_{ 5 } } +{ H }_{ 2 }O\)

(i) Organic compounds containing the carboxyl group -COOH are called carboxylic acids.
(ii) The acid may be monocarboxylic acid if it contains one -COO H group; a dicarboxylic acid if it contains two - COOH groups; a tricarboxylic acid if it contains three - COOH groups.
Eg: CH₃COOH - Acetic acid; (COOH)₂- Oxalic acid

Aromatic aldehydes react with primary amines (aliphatic or aromatic) in the presence of an acid to form Schiff's base.
Example:

Addition reaction with NaHSO₃.
In the addition of sodium bisulphite to give bisulphite compound - OSO₂Na anion is the nucleophile.

(i) \(H-\underset { \overset { || }{ O } }{ C } -H\) - Formaldehyde
(ii) \({ CH }_{ 3 }-\underset { \overset { || }{ O } }{ C } -H\) - Acetaldehyde
(iii) \({ CH }_{ 3 }-\underset { \overset { || }{ O } }{ C } -{ { CH }_{ 3 } }\) - Acetone
(iv) \(\\ { C }_{ 6 }{ H }_{ 5 }-\underset { \overset { || }{ O } }{ C } -{ CH }_{ 5 }\) - Aceopenone

In simple amines the lone pair of electrons is on nitrogen and hence available for protonation. In amides, on the other hand, the electron pair on nitrogen is delocalized to the carbonyl oxygen through resonance.

CCl₃ - NO₂ (trichloronitro. methane) is Chloropicrin.

Equanil.

Antimicrobials inhibits bacterial cell wall biosynthesis
Uses: To treat skin infections, dental infections, ear infections, respiratory tract infections, pneumonia, urinary tract infections, and gonorrhoea.
E.g: Penicillin

Neutralize the acid in the stomach that causes acidity.
Uses: To relieve symptoms such as burning sensation in the chest/ throat area (heart burns) caused by acid reflux.
Eg : Milk of Magnesia, Sodium bicarbonate, calcium bicarbonate, aluminium hydroxide.

The synthesis of mRNA from DNA strand is called transcription.

Proteins.

DNA has double helix whereas RNA has single helix.
The common bases are Adenine, Guanine and Cytosine.

Humans cannot use cellulose as food because our digestive systems do not contain the necessary enzymes (glycosidases or cellulases) that can hydrolyse the cellulose.

Anomers are cyclic monosaccharide differing from each other in the configuration of C₁ if they are aldoses or in the configuration of C₂ if they are ketoses.
E.g. α and βD - glucose.

(i) River water is colloidal solution of clay. Sea water contains a number of electrolytes.
(ii) When river water meets the sea water, the electrolytes present in sea water coagulate the colloidal solution of clay which get deposited with the formation of delta.

Emulsion can be separated into two separate layers. The process is called Deemulsification.

(i) In adsorption, if the concentration of a substance in the interface is high, then it is called positive adsorption.
(ii) In adsorption, if the concentration of a substance in the interface is less, then it is called negative adsorption.

The electrochemical equivalent is defined as the amount of substance deposited or liberated at the electrode by a charge of 1 coulomb.
m = z  (If I = 1 ampere and t = second).

(i) Leclanche cell
(ii) Mercury button cell

It is an Galvanic cell.

Kohlrausch deduced the following empirical relationship between the molar conductance (\({ \Lambda }_{ m }\)) and the concentration of the electrolyte (C).
\(​​{ \Lambda }_{ m }={ \Lambda }_{ m }^{ o }-k\sqrt { C } \)

The resistance of such an electrolytic solution is also directly proportional to the length (l) and inversely proportional to the cross sectional area (A)
R α \(\frac{l}{A}\)
R = ρ \(\frac{l}{A}\)

Test to differentiate alcohol and phenols:
(i) Phenol react with benzene diazonium chloride to form a red orange dye, but ethanol has no reaction with it.
(ii) Phenol gives purple colouration with neutral ferric chloride solution, alcohols do not give such coloration with FeCI₃.
(iii) Phenol reacts with NaOH to give sodium phenoxide. Ethyl alcohol does not react with NaOH.

When C₂H₅OH (Ethanol) is treated with cone H₂SO₄ at 410 K, intermolecular dehydration take place and the product formed will be diethyl ether C₂H₅-O-C₂H₅.

When an acid reacts with a base, a salt and water are formed and the reaction is called neutralization.

Action of heat : When heated, potassium permanganate decomposes to form potassium manganate and manganese dioxide.

\({ k }=2.303\log { \frac { \left[ { A }_{ 0 } \right] }{ \left[ A \right] } } \)
\(t=\frac { 2.303 }{ { 10 }^{ -3 } } \log { \frac { 10 }{ 2.5 } } \)
t = 2303 x 0.301 x 2 = 1386 s.

Rate of a reaction at any time depends on the concentration of the reactants which keeps on decreasing with time.

(i) Sulphur has great catenation property and forms large molecule having high weight, which results higher melting point.
(ii) While oxygen exists as diatomic molecule of less molecular weight, hence has very low melting point.

Ammonia is prepared in the laboratory by heating an ammonium salt with a base.
\({ 2NH }_{ 4 }^{ + }+{ OH }^{ - }\longrightarrow { 2NH }_{ 3 }+{ H }_{ 2 }O\)
\({ 2NH }_{ 4 }Cl+CaO\longrightarrow { CaCl }_{ 2 }+{ 2NH }_{ 3 }+{ H }_{ 2 }O\)

In FeS, Fe²⁺ ions are replaced by Fe³⁺ ions. To maintain electrical neutrality, 3 Fe²⁺ ions are replaced by 2Fe³⁺ ions

The length of the side of the unit cell of the metal is 353.55 pm.
For fee unit cell, a =(2√2) x r
= 2 x 1.414 x 125
= 353.55pm.

(i) In ionic compounds, electricity is conducted by ions.
(ii) In solid state, ions are held together by A strong electrostatic forces and are not free to move about within the solid.
(iii) Hence, ionic solids do not conduct electricity in solid state
(iv) However, in molten state or in solution form, the ions are free to move and can conduct electricity.

(i) Anhydrous AlCl₃ is an electro-deficient compound while hydrated AICl₃ is not.
(ii) Therefore, anhydrous AICl₃ is more soluble in diethyl either because the oxygen atom of ether donates a pair of electrons to the vacant p-orbital on the Al atom in AlCl₃ forming a co-ordinate bond.
(iii) In case of hydrated AlCl₃, Al is not electron deficient, since, H₂O has already donated a pair of e^- to it.

Chlorosilazanes is Cl₃Si - NH - SiCl_3.Silicon tetrachloride undergoes ammonolysis to form chlorosilazanes.
\(2Si{ Cl }_{ 4 }+{ NH }_{ 3 }\overset { 330K }{ \underset { Ether }{ \longrightarrow } } { Cl }_{ 3 }Si-NH-Si{ Cl }_{ 3 }\).

Diboranes reacts with water and alkali to give boric acid and metaborates respectively.
B₂H₆+ 6H₂O ⟶ 2H₃BO₃ + 6H₂
B₂H₆+ 2NaOH + H₂O ⟶ 2NaBO₂ + 6H₂

Transition elements have strong tendency to form:
complexes because of two reasons. They are
(i) Small size and high positive charge density.
(ii) Presence of cant (n-1) d orbitals which are of appropriate energy to accept lone pair and unshared pair of electrons from the ligands for bonding with them.

Cr₂O₇^2- + 14H⁺ + 6Fe²⁺ ⟶ 2Cr³⁺ + 6Fe³⁺ + 7H₂O

(i) Iron is used in the manufacture of wrought iron and steel.
(ii) Cast iron is used for casting stoves, railway sleepers, toys, etc.
(iii) Stainless steel is used for cycles, automobiles, utensils, pens, etc.
(iv) Chrome steel is used for cutting tools and crushing machines

The best known examples of this type of isomerism occur for chromium chloride CrCI₃.6H₂O which may contain 4, 5, (or) 6 coordinated water molecules.
[Cr(H₂O)₄CI₂]Cl.2H₂O -Bright green
Tetraaquadichlorochromium(III)chloride dihydrate
[Cr(H₂O)₅CI]Cl₂.H₂O - grey-green
Pentaaquachlorochromium(III) chloride monohydrate
[Cr(H₂O)₆]CI₃ Violet
Hexaaquachromium (III) chloride 

Isomers that arises in the coordination compounds having both the cation and anion as complex ions. The interchange of one or more ligands between the cationic and the anionic coordination entities result in different isomers.
(i) [Cr(NH₃)₅CN] [Co(NH₃) (CN)₅] and [Co(NH₃)₅CN] [Cr(NH₃)( CN)₅]
(ii) [Pt(NH₃)₄] [Pd(CI)₄] and [Pd(NH₃)₄] [Pt(Cl)₄]

(i) The complex ion of the coordination compound containing the central metal atom/ion and the ligands attached to it is collectively called coordination sphere and are usually enclosed in square brackets with the net charge.
(ii) The other ionisable ions, are written outside the bracket are called counter ions. For example, the coordination compound K₄[Fe(CN)₆] contains the complex ion [Fe(CN)₆]^4- and is referred as the coordination sphere.
(iii) The other associated ion K⁺ is called the counter ion.

(i) Conversion of ores into oxides.
(ii) Reduction of metal oxides.

K₃[Fe(C₂O₄)₃]