Make the correct pairs for the following given X and Y. X contains substance and Y has method of manufacture: X Y Extraction of Sulphur p. Contact process Production of Nitric acid q. Frasch method Production of Sulphuric acid r. Haber's process Production of Ammonia gas s. Ostwald's process

$$(1- s), (2- r), (3- q), (4- p)$$

$$(1- r), (2- q), (3- s), (4-p)$$

MCQ Questions for Class 12 Engineering Chemistry The P-Block Elements Quiz 9

The diagram below shows the set up for the laboratory preparation of a pungent alkaline gas.

The balanced equation for the above preparation is :

0%
$2CaO+{ 2NH }_{ 4 }Cl\rightarrow 2{ CaCl }_{ 2 }+{ H }_{ 2 }O+{ 2NH }_{ 3 }$
0%
$CaO+{ NH }_{ 4 }Cl\rightarrow { CaCl }_{ 2 }+{ H }_{ 2 }O+{ NH }_{ 3 }$
0%
$CaO+{ 2NH }_{ 4 }Cl\rightarrow { CaCl }_{ 2 }+{ H }_{ 2 }O+{ 2NH }_{ 3 }$
0%
$2CaO+{ NH }_{ 4 }Cl\rightarrow 2{ CaCl }_{ 2 }+{ H }_{ 2 }O+{ 2NH }_{ 3 }$

Explanation

Ammonia gas

$(NH_3)$ can be prepared in the laboratory by heating calcium oxide and ammonium chloride. The ammonia gas formed is dried over

$CaO$ .

The balanced reaction for above preparation is:

$CaO+{ 2NH }_{ 4 }Cl\rightarrow { CaCl }_{ 2 }+{ H }_{ 2 }O+{ 2NH }_{ 3 }$

Which reaction of ammonia forms the first step of Ostwald's process?

0%
The catalytic oxidation of ammonia by platinum catalyst
0%
The catalytic oxidation of ammonia by cobalt catalyst
0%
The catalytic reduction of ammonia by platinum catalyst
0%
The oxidation of ammonia

Explanation

The first step of Ostwald's process is the catalytic oxidation of ammonia by platinum catalyst for the formation of nitric acid.

$NH_3+O_2 \xrightarrow {Pt} NO+ H_2O$

The set up shown in the diagram is for the laboratory preparation of a pungent alkaline gas. What is the name of drying agent used in the process?

0%
Quick lime
0%
Magnesium oxide
0%
Calcium carbonate
0%
None of these

Explanation

$\begin{array}{l}\text{ The Drying Agent is CaO (Quick lime) .}\text{ It is used to dry ammonia gas }\end{array}$

The set up shown in the diagram is for the laboratory preparation of a pungent alkaline gas. The gas collected in the jar is _________ .

0%
ammonia
0%
chlorine
0%
sulfur dioxide
0%
carbon monoxide

Explanation

$\begin{array}{l}\text{ The mixture in round bottomed flask }\text{ is }\mathrm{NH}_{4}\mathrm{Cl}+\mathrm{Ca}(\mathrm{OH})_{2}\\\text { Gas collected in jar }\mathrm{NH}_{3}\text { (g). }\end{array}$
1992073_202348_ans_efd033ebe4e9494792eda1b35073edd6.png

1992073_202348_ans_efd033ebe4e9494792eda1b35073edd6.png

Which of the following pairs is/are correctly matched?

0%
A halogen which is liquid at room temperature - Bromine
0%
The most electronegative element - Fluorine
0%
The most reactive halogen - Fluorine
0%
The strongest oxidizing agent - Iodine

$NH_4CI, NH_4NO_3$ and

$(NH_4)_2CO_3$ gives

$NH_3$ gas on heating.

0%
True
0%
False

Explanation

Reaction:

$NH_4NO_3\rightarrow N_2O+2H_2O$

$NH_4Cl\rightarrow NH_3+HCl$

$(NH_4)_2CO_3\rightarrow 2 NH_3 + H_2O + CO_2$

One mole of magnesium nitride on reaction with an excess of water gives:

0%
one mole of ammonia
0%
one mole of nitric acid
0%
two moles of ammonia
0%
two moles of nitric acid

Explanation

Hint: Magnesium nitride undergoes decomposition in water to give a pungent odor.

Explanation:

$Mg$ reacts with $N_{2}$ to form $Mg_{3}N_{2}$ .

$Mg_{3}N_{2}$ decomposes in water to form ammonia (having pungent odor) and magnesium hydroxide.

The equation of the reaction is:

Hence, the correct answer is option $C.$

Which one of the following order is not in accordance with the property stated against it?

0%
$F_2 > Cl_2 > Br > I_2$ : Electronegativity
0%
$F_2 > Cl_2 > Br_2 > I_2$ : Bond dissociation energy
0%
$F_2 > Cl_2 > Br_2 > I_2$ : Oxidizing power
0%
$HI > HBr > HCl > HF$ : acidic property in water

Explanation

Explanation

Option (A): We know the electronegativity of atoms decreases down the group. So, the given order is correct for group

$17$ elements.

Option (B): The correct order of bond dissociation energy is

$Cl_2>Br_2>F_2>I_2$ It is because, in the case of

$F_2$ ,

$F$ has a smaller size so the repulsion is more So, bond dissociation energy is less. so the given order is incorrect.
The table below represents the bond dissociation energy of the halogens.
Which of the following pairs of molecules have the almost identical bond dissociation energy:a)F2 and H2b)N2 and COc)F2 and I2d)HF and O2Correct answer is option 'C'. Can you explain this answer? |

Which of the following pairs of molecules have the almost identical bond dissociation energy:a)F2 and H2b)N2 and COc)F2 and I2d)HF and O2Correct answer is option 'C'. Can you explain this answer? |

Option (C): Just like electronegativity, oxidizing power of group

$17$ elements decreases down the group. So, the given order is correct here also.

Option (D):

$HI$ is the most acidic as it readily dissociates into

$H^+$ and

$I^-$ ions when dissolved in water, whereas

$HF$ is the least acidic. This order is also correct.

Correct Option: $B$ .

Superhalogen is:

0%
$F_2$
0%
$Cl_2$
0%
$Br_2$
0%
$I_2$

Explanation

Superhalogen is a halogen which has high electronegativity and high reactivity.

Since

$F_2$ is highly reactive, it is a superhalogen. Also

$F_2$ has the highest electronegativity.

Nitrogen gas can be obtained by heating :

0%
ammonium nitrate
0%
ammonium nitrite
0%
magnesium nitride
0%
ammonium chloride

Explanation

$\begin{array}{l}\text { A.) Ammonium nitrate ( } \mathrm{NH}_{4} \mathrm{NO}_{3} \text { ) } \\\mathrm{NH}_{4} \mathrm{NO}_{3}\longrightarrow\mathrm{\triangle} \underset{\text { Nitrous oxide }}{\mathrm{N}_{2} \mathrm{O}}+2 \mathrm{H}_{2}\mathrm{O}\end{array}$

$\begin{array}{l}\text { B.) Ammonium nitrite }\left(\mathrm{NH}_{4} \mathrm{NO}_{2}\right) \\\mathrm{NH}_{4} \mathrm{NO}_{2}\longrightarrow \mathrm{N}_{2} \uparrow+2 \mathrm{H}_{2}\mathrm{O}\end{array}$

$\begin{array}{l}\text { C) Megnesium nitride }\left(\mathrm{Mg}_{3} \mathrm{~N}_{2}\right) \\\mathrm{Mg}_{3} \mathrm{~N}_{2} \underset{700-150^{\circ} \mathrm{C}}{\longrightarrow} 3\mathrm{Mg}+\mathrm{N}_{2}[\text { Rare Conditim }]\end{array}$

$\begin{array}{l}\text { D ) Ammonium Chloride ( } \mathrm{NH}_{4} \mathrm{Cl} \text { ) } \\\mathrm{NH}_{4} \mathrm{Cl} \quad\underset{\Delta}{\longrightarrow}\mathrm{NH}_{3}+\mathrm{HCl} \\\text { Correct Answer - (B) }\end{array}$

What is found in sulphide ores?

0%
Phosphorous
0%
Bismuth
0%
Antimony
0%
Arsenic

Explanation

Generally, Bismuth is found in Sulphide ore. The ore is called Bismotninite

$(Bi_2S_3)$

Antimony also occurs with sulphide in nature. eg. Stibnite

$(Cb_2S_3)$ . But it is a mineral, not an ore.

Similarly, Arsenic also occurs with sulphide in nature eg. Arsenic Sulfide

$(AS_2S_3)$ But it is a mineral.

Phosphorous generally occurs as oxide.In iron ores

eg- Phosphate

$\left( { PO }_{ 4 }^{ 3- } \right)$

An element with atomic number

$82$ belongs to the group:

0%
16
0%
12
0%
14
0%
2

Which metal is in ores such as orpiment, realgar etc?

0%
phosphorous
0%
arsenic
0%
nitrogen
0%
bismuth

Explanation

Realgar is represented by

$As_4S_4$ (red colour)

Orpiment is represented by

$As_2S_3$ (yellow-orange colour)

These both are the Sulfide minerals of Arsenic.

Hence arsenic is correct.

Hydride of nitrogen is:

0%
acidic
0%
basic
0%
neutral
0%
none of the above

The atomic number of some elements are as given. Which of the following elements belong to the nitrogen family?

0%
element of atomic number 33
0%
element of atomic number 51
0%
element of atomic number 83
0%
all of the above

Explanation

Atomic number 33 belongs to arsenic

$As$ . Atomic number 51 belongs to Antimony

$Sb$ . Atomic number 83 belongs to Bismuth

$Bi$ . All of them belongs to nitrogen family.

The Xenon compound which has more number of lone pairs in its central atom is :

0%
$XeF_6$
0%
$XeOF_4$
0%
$XeF_4$
0%
$XeO_3$

Explanation

The Xenon compound which has more number of lone pairs in its central atom is

$\displaystyle XeF_4$ .

$Xe$ atom in

$\displaystyle XeF_4$ has 2 lone pairs of electrons and 4 bond pairs of electrons.

Note:

$Xe$ atom in

$\displaystyle XeF_6$ ,

$\displaystyle XeOF_4$ and

$\displaystyle XeO_3$ has 1 lone pair of electrons each.

Hence, option (C) is the correct answer.

Which of the following halide of nitrogen is not explosive in nature?

0%
$NCl_3$
0%
$NI_3$
0%
$NBr_3$
0%
$NF_3$

Explanation

The only stable halide of nitrogen

$NF_3$ is not explosive. The other halides are explosive due to their unstable nature because of much larger sizes.

Hence, the correct option is

$D$

Which of the following halide of nitrogen is unstable in nature?

0%
$NCl_3$
0%
$NBr_3$
0%
$NI_3$
0%
$NF_3$

Explanation

Nitrogen has very small size as compared to the halogens, which have much larger sizes. Due to this, they can not remain bonded to the nitrogen atom and hence are highly unstable.

$NF_3$ is stable because fluorine and nitrogen have comparable sizes and electronegativity.

Xenon reacts with fluorine at 873 K and 7 bar to form

$XeF_4$ . In this reaction the ratio of Xenon and fluorine required is :

0%
1:5
0%
10:1
0%
1:3
0%
5:1

Explanation

Xenon reacts with fluorine at 873 K and

$7$ bar to form

$XeF_4$ . In this reaction, the ratio of Xenon and fluorine required is

$1:5$

$\displaystyle Xe + 2F_2 \xrightarrow [7\ bar ]{873\ K} XeF_4$

Hence, the option (A) is the correct answer.

Which of the following elements does not forms stable diatomic molecules :

0%
$I$
0%
$P$
0%
$N$
0%
$O$

Which of the following element has metallic lustre?

0%
$F$
0%
$Cl$
0%
$Br$
0%
$I$

$NaOCl$ is used as a bleaching agent and sterilising agent. It can be prepared by the action of:

0%
$NaCl$ with $H_2O$
0%
$NH_4Cl$ with $NaOH$
0%
$Cl_2$ with cold and dil. $NaOH$
0%
$Cl_2$ with hot and conc. $NaOH$

Explanation

Chlorine with cold and dilute sodium hydroxide give mixture of chloride salt, hypochlorite and water.

$Cl_2 (l) + 2NaOH (aq) \rightarrow NaCl+ NaClO (aq) + H_2O(l)$

Chlorine with hot and dilute sodium hydroxide give mixture of chloride salt, hypochlorite and water.

$3 Cl_2 (l) + 6 NaOH (aq) \rightarrow 5 NaCl + NaClO_3 (aq) + 3 H_2O (l)$

Hence, the correct option is

$C$

Which compounds is related to Haber's process:

0%
$CO_2$
0%
$H_2$
0%
$NO_2$
0%
$NH_3$

Explanation

Haber's process is used to synthesize ammonia (

$NH_3$ ) from nitrogen and hydrogen gases using in 1:3 ratio and

$Fe,Mo$ is used as catalyst and promoter respectively.

$N_2+3H_2\xrightarrow[Fe]{Mo}2NH_3$
Hence option D is correct

Which of the following

$P$ most stable?

0%
Red
0%
White
0%
Black
0%
All of these

Explanation

Black phosphorus is the most stable allotrope of phosphorus. It has a layered structure. It is a very highly polymerised form of the element.

We can find black phosphorus in two main forms. They are alpha black phosphorus and beta black phosphorus.

While beta black phosphorus forms when white phosphorus is heated at 473K, alpha black phosphorus forms when we heat red phosphorus at 803K.

Beta black phosphorus conducts electricity while alpha black phosphorus doesn’t conduct electricity.

Hence, the correct option is

$C$

When plant and animal decay, the organic

$N$ is converted into inorganic

$N$ . The inorganic

$N$ is in the form of:

0%
$NH_3$
0%
element of $N$
0%
nitrates
0%
nitrides

Explanation

During plant and animal decay the organic nitrogen converts into

$NH_3$ which is inorganic.

In an organic compound

$P$ is estimated as:

0%
$Mg_{2}P_2O_7$
0%
$Mg_3(PO_4)_2$
0%
$H_3PO_4$
0%
$P_2O_5$

Explanation

In the qualitative analysis Phosphorous is estimated by the formation of

$Mg_{2}{ P }_{ 2 }{ O }_{ 7 }$ .

The three important oxidation state of

$P$ are:

0%
$-3,+3,+5$
0%
$-3,+3,-5$
0%
$-3,+4,-4$
0%
$-3,+3,+4$

Explanation

Three important oxidation states of phosporous are :
+3 is due to the participation of only

$3P^{3}$ (due to inert pair effect). Only three electrons involve in bond formation.
+5 is due to the participation of

$3s^{2}3P^{3}$ (due to absence of inert pair effect). All the five electrons involves in bond formation.
-3 is due to gain of three electrons as it has five electrons in valence shell so as to attain octet configaration.
Hence option D is correct.

Formula of Freon is:

0%
$CCl_2F_2$
0%
$COCl_2$
0%
$SO_2Cl_2$
0%
none of these

Explanation

$CCl_2F_2$ is called as freons or chloro floro carbons.

Hence option A is correct.

Cyanamide process is used in formation of-

0%
$N_2$
0%
$HNO_3$
0%
$NH_3$
0%
$PH_3$

Explanation

Cyanamide process is a nitrogen fixation process in which Calcium Carbide and nitrogen react with each other at a high temperature to form Calcium Cyanamide.
The following reaction takes place:

$CaC_2$

$+$

$N_2$

$\longrightarrow$

$CaCN_2$

$+$

$C$

At high temperature Calcium Cyanamide react with steam as follows:

$CaCN_2$

$+$

$3H_2O$

$\longrightarrow$

$CaCO_3$

$+$

$2NH_3$

Hence,

$NH_3$ is formed.

Among the following halogens, the one which does not form an oxyacid is:

0%
Fluorine
0%
Chlorine
0%
Bromine
0%
Iodine

Which of the following does not contain nitrogen?

0%
Proteins in plants and animals
0%
Members of apatite family
0%
Indian saltpetre
0%
Chile saltpetre

Explanation

Apatite is a group of phosphate minerals, usually referring to hydroxylapatite, fluorapatite and chlorapatite, with high concentrations of

$OH^{-},F{-},Cl{-}$ respectively, in the crystal. Proteins in plants and animals have nitrogen. Chile saltpetre and Indian saltpetre are

$NaNO_3$ and

$KNO_3$ respectively.

Which of the following gives purest form of nitrogen?

0%
Thermal decomposition of ammonium nitrate
0%
Treating aqueous solution of ammonium chloride with sodium nitrite
0%
Thermal decomposition of sodium or barium azide
0%
Liquefaction and fractional distillation of air

Explanation

$2NaN_3 \rightarrow 2Na +3N_2$

Pure nitrogen can be obtained from thermal decomposition of sodium or barium azide.

Chlorine water oxidises thiosulphates to:

0%
sulphate
0%
persulphate
0%
sulphide
0%
none of these

Explanation

Chlorine is a oxidizing agent, when chlorine water react with Sodium thiosulphate, it oxidises sodium thiosulphate to sulphur which is formed as precipitate.

$Na_2S_2O_3$

$+$

$Cl_2$

$+$

$H_2O$

$\longrightarrow$

$2HCl$

$+$

$Na_2SO_4$

$+$

$S$

Green Colur of chlorine water get change to Colourless Oxidate.

The impurities formed during laboratory preparation of dinitrogen from ammonium chloride and sodium nitride is/are:

0%
$HCl$
0%
$HNO_3 and NO$
0%
$NO_2$
0%
$HNO_2$

Explanation

$NH_4Cl+NaNO_2 \rightarrow N_2+NaCl+2H_2O$

The impurities formed are small amount of

$NO$ and

$HNO_3$ , which can be removed by passing gas through aqueous sulphuric acid containing potassium dichromate.

The single

$X-X$ bond made by

$N$ is weaker than that of

$P$ because:

0%
of repulsion between nitrogen nucleus due to smaller size of nitrogen atom
0%
of repulsion between non-bonded electrons due to smaller size of nitrogen atom
0%
of higher bond enthalpy of nitrogen
0%
all of the above

Explanation

The single

$N-N$ bonds formed is weaker than single

$P-P$ bonds because of lone pair repulsion on small nitrogen molecule.

The multiple bonds that nitrogen forms with itself are:

0%
$d\pi-d\pi$ bonds
0%
$d\pi-p\pi$ bonds
0%
$p\pi-p\pi$ bonds
0%
none of the above

Explanation

When bonding occurs between elements having their valence electron and vacant place in

$p$ orbital then its called

$p\pi-p\pi$ bonding. The nitrogen atom has valence electron in

$p$ orbital so with itself form

$p\pi-p\pi$ bonds.

What results in the weak catenation property of nitrogen?

0%
Smaller size
0%
Repulsion between non-bonded electrons
0%
Repulsion between protons
0%
High electronegativity

Which of the following does exist?

0%
$HFO_2$
0%
$HClO_2$
0%
$HBrO_2$
0%
$HIO_2$

Explanation

$HClO_2$ is a chlorous acid which is oxyacid of halogen.

Remaining oxyacids of halogens do not exist.

Bromous acid $HBrO_2$ and Iodous acid $HIO_2$ and fluorous acid are not likely to exist in nature as they would decompose into oxides and water vapour when trying to isolate them from their respective acid solutions.

Hence, option $B$ is correct.

Which of the following can produce ammonia from ammonium salts?

0%
Quick lime
0%
Caustic soda
0%
slaked lime
0%
All

Explanation

Quick lime is

$CaO$ ,caustic soda is

$NaOH$ , slaked lime is

$Ca(OH)_2$ .

$NH_4Cl+NaOH \rightarrow NH_3+H_2O+NaCl$

$NH_4Cl+Ca(OH)_2 \rightarrow NH_3+H_2O+CaCl_2$

The complex formed in Brown Ring Test is ___________.

0%
$[Fe(H_2O)_4(NO)_2]^{2+}$
0%
$[Fe(H_2O)_5(NO)]^{2+}$
0%
$[Fe(H_2O)_3(NO)_3]^{2+}$
0%
$[Fe(H_2O)_6(NO)]^{2+}$

Explanation

$[Fe(H_2O)_5(NO)]SO_4$ is the complex formed in brown ring test done to identify the presence of nirates.

Urea on reacting with water gives:

0%
$NH_3$
0%
$N_2O_3$
0%
$HNO_2$
0%
$HNO_3$

Explanation

$NH_2CONH_2+H_2O \rightarrow 2NH_3+CO_2$

Urea on reaction with water gives carbondioxide and ammonia.

Nitrogen can combine with:

0%
only metals
0%
only non-metals
0%
both metals and non-metals
0%
neither metals nor non-metals

Explanation

Nitrogen can combine with both metals and non metals.

$N_2+3H_2 \rightarrow NH_3$

$N_2+Li \rightarrow 2Li_3N$

Make the correct pairs for the following given X and Y. X contains substance and Y has method of manufacture:

X	Y
Extraction of Sulphur	p. Contact process
Production of Nitric acid	q. Frasch method
Production of Sulphuric acid	r. Haber's process
Production of Ammonia gas	s. Ostwald's process

0%
$(1- s), (2- r), (3- q), (4- p)$
0%
$(1- r), (2- q), (3- s), (4-p)$
0%
$(1-q), (2-s), (3-p), (4-r)$
0%
$(1-s), (2-q), (3-r), (4-p)$

Explanation

Sulphur is extracted by the Frasch method.
It is extracted from deposits in Louisiana by this process.

Nitric acid is produced by Ostwald's process.
Ammonia is oxidized to

$\displaystyle NO$ .

$\displaystyle NO$ is further oxidised to

$\displaystyle NO_2$

$\displaystyle NO_2$ is dissolved in water.

Sulphuric acid is produced by Contact process.
S is oxidized to

$\displaystyle SO_2$ which is further oxidized to

$\displaystyle SO_3$ .

$\displaystyle SO_3$ is then dissolved in oleum and diluted.

Ammonia is produced by Haber's process.
It involves direct combination of

$\displaystyle N_2$ gas with

$\displaystyle H_2$ gas.

Hence, option

$C$ is correct.

Which of the following is true regarding derivation of the name of chlorine?

0%
The name of chlorine was derived from its color.
0%
The name of chlorine was derived from the name of the place where it was found for the first time.
0%
The name of chlorine was derived from the name of the scientist who discovered it.
0%
The name of chlorine was derived from mythological character name.

$N_2(g)+3H_2(g)\overset{773K}{\underset{200-300\ bar}{\longrightarrow}}2NH_3(g)+$ heat

Which of the following works as a catalyst?

0%
$Al_2O_3$
0%
$K_2O$
0%
$Fe$
0%
$V_2O_5$

Explanation

The Haber process for the manufacture of ammonia is carried out by mixing dihydrogen and dinitrogen gases in the ratio of

$3:1$ by volume. This mixture is passed over iron catalyst at

$200-300$ bar pressure and temperature of

$773\ K$ .

When

$262\ g$ of xenon (atomic mass

$= 131$ ) reacted completely with

$152\ g$ of fluorine (atomic mass

$= 19)$ , a mixture of

$XeF_{2}$ and

$XeF_{6}$ was produced. The molar ratio

$XeF_{2} : XeF_{6}$ is :

0%
$1 : 2$
0%
$1 : 4$
0%
$1 : 1$
0%
$1 : 3$

Explanation

$\underset {\dfrac {262}{131}}{Xe} + \underset {\dfrac {152}{38}}{F_2} \rightarrow \underset {a\ mole}{XeF_{2}} + \underset {b\ mole}{XeF_{6}}$

Let

$a$ mole

$XeF_{2}$ form and

$b$ mole

$XeF_{6}$ from.

Apply

$POAC$ ,

$a\times 1 + b\times 1 = 2$ -------

$(1)$

$2a + 6b = 8$ ---------

$(2)$

After solving eq.

$(1)$ and

$(2)$

$a = 1\ mole$ and

$b = 1\ mole$ .

Which element among the following does form

$P \pi- P \pi$ multiple bonds ?

0%
Arsenic
0%
Nitrogen
0%
Phosphorus
0%
Antimony

Explanation

Nitrogen forms

$\displaystyle P \pi- P \pi$ multiple bonds.
In diatomic

$\displaystyle : N \equiv N:$ , 1 bond is sigma and the remaining 2 bonds are

$\displaystyle P \pi- P \pi$ bonds.

Other elements of group 15 do not form

$\displaystyle P \pi- P \pi$ multiple bonds due to repulsion between non bonded electrons of the inner core and size.

There is no such repulsion in case of smaller nitrogen atoms as they have only

$1s^2$ electrons in their inner core and hence, their p orbitals easily overlap to form

$\displaystyle P \pi- P \pi$ multiple bonds.

Which property is most important in making fluorine, the strongest oxidising halogen?

0%
Hydration enthalpy
0%
Bond dissociation energy
0%
Ionisation enthalpy
0%
Electron gain enthalpy

Explanation

$\displaystyle\frac{1}{2}F_2+e^-+aq. \rightarrow F^-(aq),$

$\Delta H=\underset{(+ve)}{H_{Gibbs}}+\underset{Hydrogen \ enthalpy}{\underset{(-ve)}{H_{Elec. gain}}+\underset{(-ve)}{H_{hyd}}}=-ve$

Since the heat of hydration for fluorine is very high and

$-$ ve. (due to small size)

The overall reaction is highly exothermic and therefore fluorine shows strongest oxidizing nature.

Hence, option

$A$ is correct.

Which of the following is not a peroxy acid?

0%
Perphosphoric acid
0%
Pernitric acid
0%
Perdisulphuric acid
0%
Perchloric acid

Helium is used in balloons in place of hydrogen because it is:

0%
Incombustible
0%
Lighter than hydrogen
0%
Radioactive
0%
More abundant than hydrogen

Explanation

Helium is used in balloons in place of hydrogen because it is incombustible. $He$ do not catch fire like hydrogen. $He$ is a inert element. Hence, option A is correct.

CBSE Questions for Class 12 Engineering Chemistry The P-Block Elements Quiz 9 - MCQExams.com

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Practice Class 12 Engineering Chemistry Quiz Questions and Answers

CBSE Questions for Class 12 Engineering Chemistry The P-Block Elements Quiz 9 - MCQExams.com

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Practice Class 12 Engineering Chemistry Quiz Questions and Answers

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