Ammonia Chemistry

Ammonia acts as a Lewis base due to the presence of lone pair of  on the nitrogen atom.so,it can form coordinate bond transition metal cations to from complex compounds.Ammonia reacts with a solution of $Cu^{2+}$  to from a deep blue coloured complex.The reaction for the above complex  compound can be written as follows:

$Cu^{2+}(aq) + 4 NH _3(aq)\rightarrow [Cu(NH _3) _4]^{2+}(aq)$

                                                                              Deep Blue

Hence option A is correct.

A compound shows acidic nature if the opposite atom or compound of the bond shows basic character. Sodium is a metal and it is basic in nature. $-NH _2$ shows acidic character when it reacts with sodium.

Liquor ammonia has a mild explosive property, so, the bottle are opened only after cooling

Solution:- (A) $Fe{Cl} _{3}$

The acidic nature of the amino group (or more accurately, the hydrogen atoms attached to the nitrogen) can be demonstrated by reactions with strong bases or active metals like sodium, where the hydrogen is replaced.

The formation reaction of ammonia is N2(g) + 3H2(g) -> 2NH3(g) with an enthalpy change of -46.0 kJ per mole of ammonia formed. The reverse reaction given is 2NH3(g) -> N2(g) + 3H2(g), which reverses the sign and doubles the value since 2 moles are involved, yielding +92.0 kJ/mol.

Acetamide, acetanilide, and acetonitrile all contain nitrogen in forms that can be hydrolyzed to release ammonia or ammonium ions. Phenyl isocyanide (phenyl carbylamine) does not undergo hydrolysis to liberate ammonia.

Magnesium, calcium, and lithium react with atmospheric nitrogen when burned to form nitrides (Mg3N2, Ca3N2, Li3N), which release ammonia upon hydrolysis with moisture. Potassium is highly reactive but does not form a stable nitride under these conditions, so it does not produce ammonia.

Ammonium sulfate is made by treating ammonia, often as a by-product from coke oven, with sulfuric acid: 

Finely divided iron is used as catalyst in the manufacture of ammonia by Haber's process

Ammonia $NH _3$ is a compound which can be decomposed chemically in its elements nitrogen and hydrogen but iron, calcium and sulphur are elements that can not be decomposed further.

$NH _3$+$H _2O$ $\rightarrow$$NH _4^+$ +$OH^-$
Water acts as a proton donor in this reaction. Since, a proton donor is an acid, water acts a Bronsted-Lowry acid.

Chlorine reacts with excess of ammonia to form ammonium chloride and nitrogen. 
$8NH _3+3Cl _2\rightarrow 6NH _4Cl+N _2$

Nitrogen gas is obtained by thermal decomposition of ammonium nitrite, ammonia and ammonium dichromate.

$Cu(OH) _2$ is soluble in $NH _3$. It forms a complex.

Nitrating is a process of heating high carbon steels, aluminium, molybdenum etc in atmosphere of $NH _3$. Because of nitrating a case hardened surface of $N _2$ is formed on metal surface which comes from Ammonia.

Organic compound+ $H _2SO _4\longrightarrow$

Hydrogen chloride gas gives dense white fumes (of ammonium chloride) with ammonium hydroxide.
 $\displaystyle HCl + NH _4OH \rightarrow NH _4Cl + H _2O$
Ammonium ion is detected by the addition of an alkali.
Ammonium salts when heated with alkali, give ammonia.
 $\displaystyle NH _4Cl+NaOH \rightarrow NaCl + NH _3 \uparrow +H _2O$
Evolution of ammonia gas can be detected by paper dipped in $\displaystyle CuSO _4$ solution. Ammonia changes the colour of this paper to deep blue due to formation of tetrammine copper complex.
$\displaystyle CuSO _4+4NH _3 \rightarrow [Cu(NH _3) _4]SO _4$

In dilute solutions  of $Na$ in ammonia, the solvated electrons have a deep blue colour.

In more concentrated solutions, the solution takes on a bronze/copper colour.

The solution of sodium in liquid ammonia is quite stable on its own.

You need to add a small amount of a catalyst such as ${ FeCl } _{ 3 }$ for the sodium to react with the ammonia to form sodium amide and hydrogen gas.

$2N{ a } _{ (s) }+2N{ H } _{ 3(l) }\underrightarrow { \quad FeC{ l } _{ 3 } } 2NaN{ H } _{ 2 }(N{ H } _{ 3 })+{ H } _{ 2(g) }$
conclusion : hence the option (A) and(D) is correct.

Ammonia is amongst the oldest of all there frigerants and still used widely in the refrigeration applications. It is also the only refrigerant outside the halo-carbons group, still being used to a great extent.Ammonia refrigerant is commonly known as R717 and its chemical formula is $NH _3$.

When $NH _3$ reacts with excess of $Cl$ an explosive substance $NCl _3$ is formed.
$NH _3 + 3Cl _2 \rightarrow NCl _3 + 3HCl$
X is $NH _3$ and Y is $NCl _3$. 

Ammonia cannot be dried by passing over conc. sulphuric acid because ammonia gas reacts chemically with conc. sulphuric acid to form ammonium sulphate.
2NH3 + H2SO4 (conc.) $\rightarrow$(NH4)2SO4.

$CaCO _3\rightarrow \underset{(g)}{CO _2}+\underset{(solid)}{CaO}$
$CaO+H _2O\rightarrow (Ca(OH) _2)\overset{(CO _2)}{\rightarrow}(CaCO _3)\overset{(CO _2)excess}{\rightarrow}(Ca(HCO _3) _2)$
$(CO _2)+NH _3\overset{\Delta}{\rightarrow}(NH _2CONH _2)$
Hence option C is correct.

Reaction:
$4NH _3+ 7O _2 \longrightarrow 4NO _2 + 6H _2O$ 

Reaction:
$NH _3 + I^- \longrightarrow  I _2$ (violet vapours)

Reaction:
$4 NH _3 + 5 O _2 \xrightarrow  {Pt}  4 NO + 6 H _2O$

Reaction:
$NH _3 + H _2O \rightarrow HNO _2 + HNO _3 $

In liquid $NH _3$,
$NH _4Cl\rightarrow NH _4^++Cl^-$ (acid)
$NaNH _2\rightarrow Na^++NH _2^-$ (base)
$CH _3COOH+NH _3\rightarrow NH _4^++CH _3COO^-$ (acid)

${NH} _{3}(g)$$\rightleftharpoons {NH} _{3}(l)+{H} _{2}O\rightleftharpoons  {NH} _{4}OH\rightleftharpoons  {NH} _{4}^{+}+{OH}^{-}$

The combustion of ammonia proceeds to yield nitogen gas and water. With the use of catalyst and under correct conditions of temperature, ammonia reacts with oxygen to produce nitric oxide which is oxidized to nitrogen dioxide and is used in the synthesis of nitric acid.

Ammonia is highly soluble In water. Two other gases showing similar solubility are hydrochloric gas and sulphur dioxide gas.

Anhydrous ammonia is the source of nitrogen for other commercial fertilizers, e.g., urea, ammonium sulfate, urea ammonium nitrate etc.

$NH _3+HOCl \rightarrow NH _4Cl + H _2O$

It should be cooled to lower the pressure of ${NH} _{3}$ inside the bottle, otherwise ${NH} _{3}$ will bump out of the bottle.

$NH _3$ can form complex due to the presence of lone pair of electron on $N$, which is donated to a metal to form coordinate bond.

Ammonia solution turns blue when alkali and alkaline earth metals are dissolved in it. The blue color of the solution is considered to be due to ammoniated electrons which absorb energy corresponding to red region of the visible light for the their excitation to higher energy levels. The transmitted light is blue which imparts blue color to the solutions.

$NH _{3} + HCl \rightarrow NH _{4}Cl$
Ammonia donate its lone pair of electron $HCl$ which will produce $NH _4^+$ and $Cl^-$ ions. Chlorine atom gains one electron and forms chloride ion which has a stable 8 electron configuration in its outermost shell.

$Zn+H _2SO _4 \rightarrow ZnSO _4+H _2$

Ammonia is a colourless gas and is highly soluble in water. 

Alkyl group (an electron releasing $\left(+I\right)$ group) increases electron density at N-atom, hence, basic nature is increased.
In ammonia, no alkyl group is present, so it is least basic.

When ammonia and $HCl$ come in contact, they form ammonium chloride.
$\displaystyle  NH _3+HCl \rightarrow NH _4Cl$

Tellurium $Te$ is an element which can not be further decomposed. Elements are chemically the simplest substances and hence, cannot be broken down using chemical methods. But Ammonia, methane and water are compounds that can be decomposed further into their elements. Lunch is mixture of compounds that can also be decomposed chemically.  

A blue precipitate of cupric hydroxide initially appears which on the addition of excess ammonia dissolves to form a deep blue solution having the tetraamminecopper(II) ion ${ \left[ Cu{ (N{ H } _{ 3 }) } _{ 4 } \right]  }^{ 2+ }$.

Pure chlorine gas may react vigorously with ammonia gas. An excessive mix of the two gases in air can produce hazardous compounds such as nitrogen trichloride.

The following reaction takes place:

$N{ H } _{ 3 }+3{ Cl } _{ 2 }\longrightarrow N{ Cl } _{ 3 }+3HCl$

Ammonia reacts with excess of chlorine to form $ N{ Cl } _{ 3 } $ and $ HCl $.

$ { NH } _{ 3 }+{ HNO } _{ 3 }\longrightarrow { NH } _{ 4 }NO\ { NH } _{ 3 }+HCl\longrightarrow { NH } _{ 4 }Cl\ { NH } _{ 3 }+{ H } _{ 4 }{ PO } _{ 4 }\longrightarrow ({ { NH } _{ 4 }) } _{ 3 }{ PO } _{ 4 }\ { NH } _{ 3 }+{ H } _{ 2 }{ SO } _{ 4 }\longrightarrow { { (NH } _{ 4 }) } _{ 2 }{ PO } _{ 4 }\  $

Because ammonia and water will form some amount of ammonium hydroxide, $N{ H } _{ 4 }OH$. The hydroxide will react with the acid ${ H }^{ + }$ ions from the acid and forms water. Addition of an acid to even a mild base like $N{ H } _{ 4 }OH$ is counter-productive to drying.

Possible reactions of $N{ H } _{ 3 }$ and ${ Cl } _{ 2 }$ are :

As the size of the nitrogen in ammonia is less than the other elements
in the hydrides of that group ammonia has the more affinity towards the
proton than the any other hydride of that group like phosphine, stobine
and arsine.
Hence option D is correct.

Its vaporization property, ammonia is an used as a refrigerant. It was used earlier to the use of chlorofluorocarbons (Freons). Anhydrous ammonia is widely used in industrial refrigeration.

$NH _3$ forms linear polymer due to Hydrogen bonding. Intermolecular Hydrogen bonding occurs between Nitrogen of one molecule and Hydrogen of other molecule. This continues and makes it a linear polymer.

The molecular weights of $\displaystyle NH _3$ and $\displaystyle O _2$ are 17 g/mol and 32 g/mol respectively.
3.4 g $\displaystyle NH _3 = \dfrac {3.4 \ g}{ 17 \ g/mol}=0.2 \ mol$
6.4 g $\displaystyle O _2= \dfrac {6.4 \ g}{32 \ g/mol}=0.2 \ mol$
0.2 moles of $\displaystyle O _2$ will react with $\displaystyle 0.2 \times \dfrac {4}{5}=0.16$ moles of $\displaystyle NH _3$. But 0.2 moles of
$\displaystyle NH _3$ are present. Hence, $\displaystyle O _2$ is the limiting reagent and $\displaystyle NH _3$ is excess reagent.

Ammonia has a strong smell which can be easily detected even from meters of distances. Hence, a slight smell of ammonia bottle can be detected.

Ammonia reacts with copper(II)ions to precipitate light blue copper hydroxide. Ammonia causes the copper ion to go back into the solution as a deep blue ammonia complex. The precipitate dissolves as we add an excess of ammonia.

Ammonium Nitrate caused an explosion at the Port of Texas City. A ship loaded with $NH _4NO _3$ docked at the Port erupted in flames.

${ 4NH } _{ 3 }+{ 3O } _{ 2 }\rightarrow { 2N } _{ 2 }+{ 6H } _{ 2 }O$

$NH _3$ is a base and it forms salt with acids.
Ammonia reacts with Nitric acid to form ammonium nitrate and on further addition with Calcium carbonate it forms Calcium ammonium nitrate.

Conc. $H _{2}SO _{4}$ & $P _{2}O _{5}$ can't be used to dry Ammonia gas.

If $NH _3$ is in excess then $8NH _3 + 3Cl _2 \rightarrow 6NH _4Cl + N _2$
If $Cl _2$ is in excess then $NH _3 + 3Cl _2 \rightarrow NCl _3 + 3HCl$

In Ammonia-Boron trifluoride complex ($H _3N \rightarrow BF _3$), the donor molecule is ammonia and the acceptor molecule is boron trifluoride. N atom of ammonia donates a lone pair of electrons to B atom of boron trifluoride and forms co-ordinate covalent bond.

$NH^+ _4$ is iso structural with $CH _4$. Both have tetrahedral geometry.$N$ atom in $NH^+ _4$ and $C$ atom in $CH _4$ have 4 bond pairs and zero lone pairs of electrons.

$AgCl+NH _3\rightarrow [Ag(NH _3) _2]^++Cl^-$
$(NH _4)Cr _2O _7\xrightarrow {\Delta}N _2+Cr _2O _3+4H _2O$
$CaNCN+3H _2O\rightarrow \underset {(white\ ppt.)}{CaCO _3}+2NH _3$
So, all the three statements are correct.

The reaction between two gases does not always produce a solid. For example, the reaction between hydrogen and chlorine gases produces hydrogen chloride gas.

(i) Hybridisation $= \frac{1}{2}$ [no.of $e^-$ in valence shell of central atom + no. of monovalent atoms + charge on anion - charge on cation]
(ii) Shape or geometry of molecule depends on lone pair and bond pair of electrons present in it.
Hybridisation  of N in $NH _3$
$=\frac{1}{2}(5+3+0)$
$=4$
$\therefore sp^3$ hybridisation.
$\because$, its has 3 bond pair and 1 lone pair of electrons, so it has distorted tetrahedron shape. 

carbonyl chloride is $COCl _2$.the reaction between $COCl _2$&$NH _3$ is given as 

Ammonia acts as a reducing agent in many reactions, such as reducing metal oxides to metals. The statement that it does not act as a reducing agent is therefore false.

Ammonical liquor is a solution of ammonia in water and is also called as ammonium hydroxide.

Due to higher tendency of nitrogen to donate its lone pair of electron to form coordinate bond which is not common in other hydrides of VA group elements, it has maximum complex forming ability.

Uses of ammonia: as a refrigerant, In manufacture of  nitrogeneous fertilizer, Explosives, dry cells, nitrogen gas

Ammonia is a strong reducing agent. It dissolves alkali metals and other electropositive metals such as Mg,Ca,Sr,Ba etc. At low concentration deep blue solutions are formed these contain metal cations and solvated electrons.
${ Li }^{ + }+{ e }^{ - }\rightleftharpoons Li\ { Na }^{ + }+{ e }^{ - }\rightleftharpoons Na$

Ammonical solution of common salt.

Pure chlorine gas may react vigorously with ammonia gas. An excessive mix of the two gases in the air can produce hazardous compounds such as the explosive nitrogen trichloride. In facilities that use chloramination, the pure chlorine and ammonia need to be stored in separate, sealed rooms or buildings.

When ammonia is excess,

$3 Cl _2 + 8 NH _3 \rightarrow 6 NH _4Cl + N _2 (g)$

The ammonium ion (NH4+) has a central nitrogen atom bonded to four hydrogen atoms. Using the formal charge formula (valence electrons minus non-bonding electrons minus half of bonding electrons), we get 5 - 0 - (8/2) = +1.

Solution:- (D) The reaction of nitrogen with hydrogen has high activation energy.

Reaction:

Ammonia readily dissolves in water with the liberation of heat. These aqueous solutions of ammonia are basic and are called ammonium hydroxide.
$ { NH } _{ 3 }+{ H } _{ 2 }O\rightleftharpoons { { NH } _{ 4 } }^{ + }+OH^{ - }$

On combustion, ammonia gas burns with pale yellowish green flame.

${ 2NH } _{ 3 }+3CuO\rightarrow { N } _{ 2 }+{ 3H } _{ 2 }O+3Cu$

Ammonia is basic in nature which turns red litmus paper to blue and confirms that ammonia is alkaline gas.

${ 2NH } _{ 3 }+{ H } _{ 2 }{ SO } _{ 4 }\rightarrow { \left( { NH } _{ 4 } \right)  } _{ 2 }{ SO } _{ 4 }$

Ammonia readily dissolves in water with the liberation of heat. The ions which are formed are ammonium ion and hydroxyl ion. The aqueous solution of ammonia is ammonium hydroxide.
$ { NH } _{ 3 }+{ H } _{ 2 }O\rightleftharpoons { NH } _{ 4 }^{ + }+{ OH }^{ - }$

Ammonia is oxidised by chlorine gas.
$8{ NH } _{ 3 }+{ 3Cl } _{ 2 }\rightarrow 6{ NH } _{ 4 }Cl+{ N } _{ 2 }$

Ammonium sulphate is the compound formed which on heating with sodium hydroxide produces a gas which forms dense white fumes with hydrogen chloride.

${ 2NH } _{ 3 }+3CuO\rightarrow { N } _{ 2 }+{ 3H } _{ 2 }O+3Cu$

$AgCl+2NH _{4}OH\rightarrow \left [ Ag(NH _{3}) _{2} \right ]Cl+2H _{2}O$
$AgCl+2Na _{2}S _{2}O _{3}\rightarrow NaCl+Na _{3}\left [ Ag(S _{2}O _{3}) _{2} \right ]$
$AgCl+NH _{3}\rightarrow \left [ Ag(NH _{3}) _{2} \right ]Cl$
So, only $NaNO _{3}$ does not react with AgCl.

$2NH _{3} + OCl^{-} \rightarrow N _{2}H _{4} + Cl^{-} + H _{2}O$

Liquid ammonia has hydrogen bonding which results in high vapour pressure at room temperature.

${ NH } _{ 3 }$ is highly soluble in water.

${ K } _{ 2 }[Hg{ I } _{ 4 }]$ ( potassium mercuric iodide) is known as nesseler's reagent.

Sodium (Na) dissolves in liquid ammonia ($NH _3$) solution to form a blue colored solution characteristic of a solvated electron in liquid ammonia which is conducting in nature due to presence of solvated electrons.

Ammonia and the ammonium ion can be differentiated by a proton $\displaystyle (H^+)$.
Ammonia is $\displaystyle NH _3$ and ammonium ion is $\displaystyle NH _4^+$.
$\displaystyle NH _3 + H^+ \rightarrow NH _4^+$

${ AlCl } _{ 3 }+3{ NH } _{ 3 }+3{ H } _{ 2 }O\rightarrow Al\left( OH \right) _{ 3 }+3{ NH } _{ 4 }Cl$

When  ammonia is heated and passed over solid copper(II)oxide at high temperatures, nitrogen gas is formed.

$2NH _3(g)+3CuO(s)\rightarrow N _2(g)+3Cu(s)+3H _2O(g)$

Hence option A is correct.

When excess chlorine reacts with ammonia (3Cl2 + 4NH3), the products are nitrogen trichloride (NCl3) and HCl. In NCl3, nitrogen is bonded to three more electronegative chlorine atoms, giving nitrogen an oxidation state of +3.

An alkaline earth metal $(M)$ dissolves in liquid ammonia forming a deep blue-black solution. The reaction involved is $M + (x + 2y) NH _{3}\rightarrow [M(NH _{3}) _{x}]^{2+} + 2[e(NH _{3}) _{y}]^{-}$ (e represents electron).
An alkaline earth metal $(M)$ will lose two electrons to form $M^{2+}$ ions.
$M \rightarrow M^{2+}+2e^-$
Both $M^{2+}$ ions and electrons are solvated (surrounded by ammonia molecules to form $[M(NH _{3}) _{x}]^{2+} + 2[e(NH _{3}) _{y}]^{-}$).

Urea was first discovered in urine in 1727 by the Dutch scientist Herman Boerhaave, This was the first time an organic compound was artificially synthesized from inorganic starting materials, without the involvement of living organisms.

A. $AgF$ and $CaCl _2$ are polar compounds. Hence, they are soluble in water which is a polar solvent. Thus, the option A is correct.

Ammonia is a weak base so it has pK value of 4. So the order of basicity is ammonia<primary<tertiary amines <secondary amines. This order depends on steric hindrance. The size of alkyl group is more than that of hydrogen atom. So alkyl group hinders the attack of hydrogen atom and decreases the basicity of molecule. So more the number of alkyl groups lesser will be its basicity.

Hydrogen bonding occurs when hydrogen is covalently bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine. Ammonia (NH3) satisfies this condition.

Nitrogen, oxygen and hydrogen can be collected by water displacement because they are only slightly soluble in water. But hydrogen chloride or ammonia can not be separated since both are very highly soluble in water and will react to form hydrochloric acid or ammonium hydroxide respectively so statement 1 is not true.

$8 NH _3 + 3 Cl _2 \rightarrow  6 NH _4Cl+N _2$

 Compound A is $NH _4Cl$ 

$1(x)+4(1)+1(-1)=0$

$x+4-1=0$

$x=-3$

The oxidation state of compound A is $-3$

Hence option A is correct.

$8 NH _3 + 3 Cl _2 \rightarrow  6 NH _4Cl+N _2$

$3Cl _2+4NH _3 \rightarrow  3NH _4Cl+NCl _3$

 Compound  B is $N _2$ Here as the nitrogen is in elemental state so its oxidation state is $0$

 Hence option A is correct.