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All questions of The p-Block Elements for Class 11 Exam
Which of the following statements is true?a)The atomic radius of Ga is less than B.
b)The atomic radius of Ga is more than Al.c)The atomic radius of Ga is less than Al.d)The atomic radius of Ga is equal to AlCorrect answer is option 'C'. Can you explain this answer?
b)The atomic radius of Ga is more than Al.
c)The atomic radius of Ga is less than Al.
d)The atomic radius of Ga is equal to Al
Correct answer is option 'C'. Can you explain this answer?
|
Neha Joshi answered |
The atomic radius of the Ga is less than Al because of poor screening effect. The atomic radius of Ga is slightly lesser than of Al because in going from Al to Ga, the electrons have already occupied 3d sub shell in Ga
In trivalent state, for example, the trichlorides, being covalent are hydrolysed in water form- a)pentagonal structure
- b)planar structure
- c)trigonal structure
- d)tetrahedral structure
Correct answer is option 'D'. Can you explain this answer?
In trivalent state, for example, the trichlorides, being covalent are hydrolysed in water form
a)
pentagonal structure
b)
planar structure
c)
trigonal structure
d)
tetrahedral structure
|
Riya Banerjee answered |
trihalides hydrolysis to form tetrahedral structure
The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in MF3-6?- a)B
- b)Al
- c)Ga
- d)In
Correct answer is option 'A'. Can you explain this answer?
The exhibition of highest co-ordination number depends on the availability of vacant orbitals in the central atom. Which of the following elements is not likely to act as central atom in MF3-6?
a)
B
b)
Al
c)
Ga
d)
In
|
Anjana Sharma answered |
The element M in the complex ion MF6^3- has a coordination number of six. Since B has only s- and p-orbitals and no d – orbitals, therefore, at the maximum it can show a coordination number of 4. Thus, B cannot form complex of the type MF6^3-, i.e., option (a) is correct.
Which of the following elements exist as liquid in summer among group 13 elements?
- a) Tl
- b) Al
- c) B
- d) Ga
Correct answer is option 'D'. Can you explain this answer?
Which of the following elements exist as liquid in summer among group 13 elements?
a)
Tlb)
Alc)
Bd)
Ga
|
Krishna Iyer answered |
Galium can occur in liquid state if the room is above 29.76C which is its melting point. So,option d is correct
The maximum oxidation state shown by a p-block element is equal to the:- a)Total number of valence electrons (i.e., the sum of the s and p-electrons)
- b)Total number of s electrons
- c)Total number of p electrons
- d)None of these
Correct answer is option 'A'. Can you explain this answer?
The maximum oxidation state shown by a p-block element is equal to the:
a)
Total number of valence electrons (i.e., the sum of the s and p-electrons)
b)
Total number of s electrons
c)
Total number of p electrons
d)
None of these
|
Preeti Khanna answered |
- The oxidation state of an element is related to the number of electrons that an atom loses, gains, or appears to use when joining with another atom in compounds.
- It also determines the ability of an atom to oxidize (to lose electrons) or to reduce (to gain electrons) other atoms or species.
- They should release the total valence electrons to attain stability, so the maximum possible oxidation state is the number of valence electrons.
The order of ionization enthalpy for B, Al and Ga is:- a)B>Al<Ga
- b)B
- c)B>Al>Ga
- d)Ga
Correct answer is option 'A'. Can you explain this answer?
The order of ionization enthalpy for B, Al and Ga is:
a)
B>Al<Ga
b)
B
c)
B>Al>Ga
d)
Ga
|
Ayush Joshi answered |
(A) B>Al<Ga
The trend in ionization enthalpy is because there is decrease in Ionisation enthalpy from B to Al due to increase in size and from Al to Ga. Ga has more ionisation energy than Al due to uneffective screening effect.
Nitrogen dioxide is dissolved in water to produce- a)HNO3 and HNO2
- b)Only HNO3
- c)Only HNO2
- d)HNO2 and N2
Correct answer is option 'A'. Can you explain this answer?
Nitrogen dioxide is dissolved in water to produce
a)
HNO3 and HNO2
b)
Only HNO3
c)
Only HNO2
d)
HNO2 and N2
|
Uday Chakraborty answered |
NO2 + H2O → HNO3 + HNO2
Mixed
anhydride
Mixed
anhydride
One of the following p-block elements has unusually low melting point- a)Indium
- b)boron
- c)gallium
- d)aluminium
Correct answer is option 'C'. Can you explain this answer?
One of the following p-block elements has unusually low melting point
a)
Indium
b)
boron
c)
gallium
d)
aluminium
|
Preeti Iyer answered |
Argon
Argon is most abundant in composition of air percent by volume. It is in 0.934% in composition of air and is one of the major gas in the Earth's atmosphere.
Which of the following group 13 elements oxide is acidic in nature?- a)Al2O3
- b)B2O3
- c)Tl2O3
- d)Ga2O3
Correct answer is option 'B'. Can you explain this answer?
Which of the following group 13 elements oxide is acidic in nature?
a)
Al2O3
b)
B2O3
c)
Tl2O3
d)
Ga2O3
|
Naina Bansal answered |
The acidic character of oxides of group 13 decreases down the group, because non-metallic character of elements decreases down the group and metallic character increases.
And we know that oxides of metals are basic in nature and oxides of non-metals are acidic in nature. So acidic character of oxides of group 13 decreases down the group.
For example boron (1st element of group 13) is non-metal, so its oxide is acidic.
Aluminum (2nd element of group 13) shows characteristics of both metal and non-metal, so its oxide shows amphoteric nature.
As we go down the group, indium and thalium (4th and 5th element of group 13) show metallic properties, so their oxides are basic.
XeF2 is isostructural with- a)SbCl3
- b)BaCl2
- c)TeF2
- d)ICl2–
Correct answer is option 'D'. Can you explain this answer?
XeF2 is isostructural with
a)
SbCl3
b)
BaCl2
c)
TeF2
d)
ICl2–
|
Arya Dasgupta answered |
C) TeF2
XeF2 and TeF2 have the same structure, which is linear with a bond angle of 180 degrees. SbCl3 has a trigonal pyramidal structure, BaCl2 has a linear structure, and ICl2 has a bent structure.
XeF2 and TeF2 have the same structure, which is linear with a bond angle of 180 degrees. SbCl3 has a trigonal pyramidal structure, BaCl2 has a linear structure, and ICl2 has a bent structure.
When Cl2 gas reacts with hot and concentrated sodium hydroxide solution, the oxidation number of chlorine changes from- a)Zero to – 1 and zero to +3
- b)Zero to + 1 and zero to –3
- c)Zero to + 1 and zero to –5
- d)Zero to – 1 and zero to +5
Correct answer is option 'D'. Can you explain this answer?
When Cl2 gas reacts with hot and concentrated sodium hydroxide solution, the oxidation number of chlorine changes from
a)
Zero to – 1 and zero to +3
b)
Zero to + 1 and zero to –3
c)
Zero to + 1 and zero to –5
d)
Zero to – 1 and zero to +5
|
|
Raghav Bansal answered |
The correct answer is option D
The reaction of chlorine gas with hot and concentrated sodium hydroxide solution is
3Cl2 + 6NaOH⟶NaClO3+ 5NaCl+3H2O
Oxidation number of Cl is 0 in Cl2, −1 in NaCl and +5 in NaClO3
So the oxidation number of chlorine changes from Zero to -1 and Zero to +5.
The reaction of chlorine gas with hot and concentrated sodium hydroxide solution is
3Cl2 + 6NaOH⟶NaClO3+ 5NaCl+3H2O
Oxidation number of Cl is 0 in Cl2, −1 in NaCl and +5 in NaClO3
So the oxidation number of chlorine changes from Zero to -1 and Zero to +5.
As we move from B to Al in the p-block elements the sum of the first three ionisation enthalpies- a)slightly decreases
- b)remains the same
- c)considerably decreases
- d)increases
Correct answer is option 'C'. Can you explain this answer?
As we move from B to Al in the p-block elements the sum of the first three ionisation enthalpies
a)
slightly decreases
b)
remains the same
c)
considerably decreases
d)
increases
|
Om Desai answered |
On moving from B to Al size increases so sum of ionization energies also decreases.
Dry ice is- a)Solid N2
- b)Solid CO2
- c)Solid SO2
- d)Solid NH3
Correct answer is option 'B'. Can you explain this answer?
Dry ice is
a)
Solid N2
b)
Solid CO2
c)
Solid SO2
d)
Solid NH3
|
Krish Ghoshal answered |
Dry ice is solid CO2
The elements of group 14 are slightly more electronegative than group 13 elements because of- a)small size
- b)their being liquids
- c)high melting point
- d)high boiling point
Correct answer is option 'A'. Can you explain this answer?
The elements of group 14 are slightly more electronegative than group 13 elements because of
a)
small size
b)
their being liquids
c)
high melting point
d)
high boiling point
|
Pankaj Sengupta answered |
As we move along the period electronegativity increases due to increase in nuclear charge.
Inert pair effect of p-block elements is due to the- a)the most unstable valence number of p-block elements
- b)the most stable valence number of p-block elements
- c)the group oxidation state of p-block elements
- d)the oxidation state two unit less than the group oxidation state
Correct answer is option 'D'. Can you explain this answer?
Inert pair effect of p-block elements is due to the
a)
the most unstable valence number of p-block elements
b)
the most stable valence number of p-block elements
c)
the group oxidation state of p-block elements
d)
the oxidation state two unit less than the group oxidation state
|
Infinity Academy answered |
Due to the presence of inner lying d and f electrons oxidation state which is 2 unit less than the group oxidation state become popular.
When oxalic acid reacts with conc. H2SO4, two gases produced are of neutral and acidic in nature respectively. Potassium hydroxide absorbs one of the two gases. The product formed during this absorption and the gas which gets absorbed are respectively- a)K2CO3 and CO2
- b)KHCO3 and CO2
- c)K2CO3 and CO
- d)KHCO3 and CO
Correct answer is option 'A'. Can you explain this answer?
When oxalic acid reacts with conc. H2SO4, two gases produced are of neutral and acidic in nature respectively. Potassium hydroxide absorbs one of the two gases. The product formed during this absorption and the gas which gets absorbed are respectively
a)
K2CO3 and CO2
b)
KHCO3 and CO2
c)
K2CO3 and CO
d)
KHCO3 and CO
|
|
Pooja Shah answered |
The non-metal oxides are:- a)acidic or neutral
- b)basic or neutral
- c)basic or acidic
- d)basic
Correct answer is option 'A'. Can you explain this answer?
The non-metal oxides are:
a)
acidic or neutral
b)
basic or neutral
c)
basic or acidic
d)
basic
|
|
Raghav Bansal answered |
nonmetallic oxides are either neutral or acidic. Example CO is neutral while CO2 is acidic.
The element having the noble gas plus 14 f- electrons plus 10 d-electron cores- a)Aluminium
- b)Boron
- c)thallium
- d)Gallium
Correct answer is option 'C'. Can you explain this answer?
The element having the noble gas plus 14 f- electrons plus 10 d-electron cores
a)
Aluminium
b)
Boron
c)
thallium
d)
Gallium
|
Dipika Choudhury answered |
Explanation:
The element that has the noble gas configuration plus 14 f-electrons plus 10 d-electrons in its core is thallium (Tl).
Here is the detailed explanation:
1. Noble Gas Configuration:
The noble gas configuration refers to the electron configuration of a noble gas, which is a group of elements with a stable electron configuration. Noble gases have a completely filled outermost electron shell, making them chemically stable. The noble gas that comes before thallium in the periodic table is xenon (Xe). The electron configuration of xenon is [Kr] 5s2 4d10 5p6.
2. F-electrons:
The f-electrons refer to the electrons in the f sublevel of the atom. The f sublevel can hold a maximum of 14 electrons. In the case of thallium, it has 14 f-electrons in addition to the noble gas configuration.
3. D-electrons:
The d-electrons refer to the electrons in the d sublevel of the atom. The d sublevel can hold a maximum of 10 electrons. In the case of thallium, it has 10 d-electrons in addition to the noble gas configuration and the f-electrons.
4. Electron Configuration of Thallium:
To determine the electron configuration of thallium, we start with the noble gas configuration of xenon and add the additional f-electrons and d-electrons.
The electron configuration of thallium is:
[Xe] 6s2 4f14 5d10
This configuration represents the noble gas xenon, followed by 6s2, which accounts for the two electrons in the 6s sublevel, 4f14, which accounts for the 14 f-electrons, and 5d10, which accounts for the 10 d-electrons.
Therefore, the correct answer is option 'C' - Thallium (Tl).
The element that has the noble gas configuration plus 14 f-electrons plus 10 d-electrons in its core is thallium (Tl).
Here is the detailed explanation:
1. Noble Gas Configuration:
The noble gas configuration refers to the electron configuration of a noble gas, which is a group of elements with a stable electron configuration. Noble gases have a completely filled outermost electron shell, making them chemically stable. The noble gas that comes before thallium in the periodic table is xenon (Xe). The electron configuration of xenon is [Kr] 5s2 4d10 5p6.
2. F-electrons:
The f-electrons refer to the electrons in the f sublevel of the atom. The f sublevel can hold a maximum of 14 electrons. In the case of thallium, it has 14 f-electrons in addition to the noble gas configuration.
3. D-electrons:
The d-electrons refer to the electrons in the d sublevel of the atom. The d sublevel can hold a maximum of 10 electrons. In the case of thallium, it has 10 d-electrons in addition to the noble gas configuration and the f-electrons.
4. Electron Configuration of Thallium:
To determine the electron configuration of thallium, we start with the noble gas configuration of xenon and add the additional f-electrons and d-electrons.
The electron configuration of thallium is:
[Xe] 6s2 4f14 5d10
This configuration represents the noble gas xenon, followed by 6s2, which accounts for the two electrons in the 6s sublevel, 4f14, which accounts for the 14 f-electrons, and 5d10, which accounts for the 10 d-electrons.
Therefore, the correct answer is option 'C' - Thallium (Tl).
In which of the following compounds, nitrogen exhibits highest oxidation state?
- a)N3H
- b)NH2OH
- c)N2H4
- d)NH3
Correct answer is option 'A'. Can you explain this answer?
In which of the following compounds, nitrogen exhibits highest oxidation state?
a)
N3H
b)
NH2OH
c)
N2H4
d)
NH3
|
Hansa Sharma answered |
so clearly N3H has the highest oxidation state
Which of the following statements regarding ozone is not correct?
- a)Ozone is used as a germicide and disinfectant for the purification of air.
- b)The ozone molecule is angular in shape
- c)The oxygen-oxygen bond length in ozone is identical with that of molecular oxygen
- d)The ozone is response hybrid of two structures
Correct answer is option 'C'. Can you explain this answer?
Which of the following statements regarding ozone is not correct?
a)
Ozone is used as a germicide and disinfectant for the purification of air.
b)
The ozone molecule is angular in shape
c)
The oxygen-oxygen bond length in ozone is identical with that of molecular oxygen
d)
The ozone is response hybrid of two structures
|
Aryan Sen answered |
bond order of O-O bond in ozone is less than that in oxygen.
Three reactions involving 
are given below
B. 
C. 
In which of the above does act as an acid?
- a)C. only
- b)B. only
- c)A. only
- d)A. and B.
Correct answer is option 'B'. Can you explain this answer?
Three reactions involving are given below
are given below B.
C.
In which of the above does act as an acid?
act as an acid?a)
C. only
b)
B. only
c)
A. only
d)
A. and B.
|
Jaideep Sengupta answered |
in B only is losing its proton therefore act as acid.
is losing its proton therefore act as acid.Among the following which is the strongest oxidizing agent?- a)Cl2
- b)Br2
- c)I2
- d)F2
Correct answer is option 'D'. Can you explain this answer?
Among the following which is the strongest oxidizing agent?
a)
Cl2
b)
Br2
c)
I2
d)
F2
|
Atharva Pillai answered |
F2 is very strong oxidizing agent.
The tendency of BF3, BCl3 and BBr3 to behave as Lewis acid decreases in the sequence:- a)BF3> BCl3> BBr3
- b)BCl3> BF3> BBr3
- c)BBr3> BF3> BCl3
- d)BBR3> BCl3> BF3
Correct answer is option 'D'. Can you explain this answer?
The tendency of BF3, BCl3 and BBr3 to behave as Lewis acid decreases in the sequence:
a)
BF3> BCl3> BBr3
b)
BCl3> BF3> BBr3
c)
BBr3> BF3> BCl3
d)
BBR3> BCl3> BF3
|
|
Geetika Shah answered |
because in BF3 there is backbonding which decreases its acidity. And as we for from BF3 to BBr3 tendency of back bonding decreases so acidity increases,.
Which one of the following does not form hydrogen bonding?- a)NH3
- b)HCl
- c)H2O
- d)HF
Correct answer is option 'B'. Can you explain this answer?
Which one of the following does not form hydrogen bonding?
a)
NH3
b)
HCl
c)
H2O
d)
HF
|
Lead Academy answered |
- Hydrochloric acid (HCl) does not form hydrogen bonding.
- This is because in hydrogen bonding the bonding is formed between hydrogen and elements Nitrogen, Oxygen and Flourine.
- In Hydrochloric acid (HCl) there are no elements like Nitrogen, Oxygen and Flourine so it cannot form hydrogen bonding.
When conc. H2SO4 was treated with K4[Fe(CN)6], CO gas was evolved. By mistake, somebody used dilute H2SO4 instead of conc. H2SO4 then the gas evolved was- a)CO
- b)HCN
- c)N2
- d)CO2
Correct answer is option 'B'. Can you explain this answer?
When conc. H2SO4 was treated with K4[Fe(CN)6], CO gas was evolved. By mistake, somebody used dilute H2SO4 instead of conc. H2SO4 then the gas evolved was
a)
CO
b)
HCN
c)
N2
d)
CO2
|
Maheshwar Chawla answered |
K4[Fe(CN)6] + H2SO4 + H2O → K2SO4 + FeSO4 + (NH4)2SO4 + CO
K4[Fe(CN)6] +dil.H2SO4 → K2SO4 + FeSO4 + HCN
K4[Fe(CN)6] +dil.H2SO4 → K2SO4 + FeSO4 + HCN
A sulphate of a metal (A) on heating evolves two gases (B) and (C) and an oxide (D). Gas (B) turns K2Cr2O7 paper green while gas (C) forms a trimer in which there is non S-S bond. Compounds (D) with HCl, forms a Lewis base (E) which exists as a dimer. Compounds (A), (B) (C) , (D) and (E) are respectively- a)FeSO4, SO2, SO3, Fe2O3, FeCl3
- b)Al2(SO4)3, SO2, SO3, Al2O3, FeCl3
- c)FeS, SO2, SO3, FeSO4, FeCl3
- d)FeS, SO2, SO3, Fe2(PO4)3, FeCl2
Correct answer is option 'A'. Can you explain this answer?
A sulphate of a metal (A) on heating evolves two gases (B) and (C) and an oxide (D). Gas (B) turns K2Cr2O7 paper green while gas (C) forms a trimer in which there is non S-S bond. Compounds (D) with HCl, forms a Lewis base (E) which exists as a dimer. Compounds (A), (B) (C) , (D) and (E) are respectively
a)
FeSO4, SO2, SO3, Fe2O3, FeCl3
b)
Al2(SO4)3, SO2, SO3, Al2O3, FeCl3
c)
FeS, SO2, SO3, FeSO4, FeCl3
d)
FeS, SO2, SO3, Fe2(PO4)3, FeCl2
|
Devansh Joshi answered |
3SO3 → S3O9 (trimer)
X 
Y 
B2O3
A tetra atomic molecule (A) on reaction with nitrogen (I) oxide, produces two substances (B) and (C) ,(B) is a dehyderating agent in its monometric form while substance (C) is a diatomic gas which shows almost intert behavior. The substances (A) and (B) and (C) respectively will be- a)P4, P4O10, N2
- b)P4, N2O5, N2
- c)P4, P2O3, Ar
- d)P4, P2O3, H2
Correct answer is option 'A'. Can you explain this answer?
A tetra atomic molecule (A) on reaction with nitrogen (I) oxide, produces two substances (B) and (C) ,(B) is a dehyderating agent in its monometric form while substance (C) is a diatomic gas which shows almost intert behavior. The substances (A) and (B) and (C) respectively will be
a)
P4, P4O10, N2
b)
P4, N2O5, N2
c)
P4, P2O3, Ar
d)
P4, P2O3, H2
|
Siddharth Chaudhary answered |
The function of Fe (OH)3 in the contact process is- a)to remove arsenic impurity
- b)to remove dust particles
- c)to detect colloidal impurity
- d)to remove moisture
Correct answer is option 'A'. Can you explain this answer?
The function of Fe (OH)3 in the contact process is
a)
to remove arsenic impurity
b)
to remove dust particles
c)
to detect colloidal impurity
d)
to remove moisture
|
Siddharth Mehra answered |
The function of Fe(OH)3 in the contact process is to remove arsenic impurity.
The contact process is a method used to produce sulfuric acid on an industrial scale. It involves several steps, including the oxidation of sulfur dioxide to sulfur trioxide, which is then used to produce sulfuric acid. However, the presence of impurities can affect the efficiency of the process and the quality of the final product. One such impurity is arsenic.
1. The Role of Fe(OH)3
Fe(OH)3, also known as ferric hydroxide, is added to the contact process as a catalyst to remove arsenic impurity. It acts as a scavenger or adsorbent for arsenic, effectively removing it from the reaction mixture.
2. Arsenic Impurity
Arsenic is a toxic element that can be present in the raw materials used in the production of sulfuric acid. It can enter the process through impurities in the sulfur or in the air used for the oxidation of sulfur dioxide. Arsenic can poison the catalyst used in the process, reducing its effectiveness and leading to a decrease in the production of sulfuric acid.
3. Adsorption Mechanism
Fe(OH)3 acts as an adsorbent for arsenic impurity. Adsorption is a process by which substances are attracted and adhere to the surface of a solid. In this case, Fe(OH)3 has a high affinity for arsenic ions, and the impurity gets adsorbed onto the surface of the catalyst.
4. Formation of a Complex
The adsorption of arsenic by Fe(OH)3 involves the formation of a complex. Arsenic ions are attracted to the surface of Fe(OH)3 and form chemical bonds with the iron atoms. This complex formation immobilizes the arsenic impurity and prevents it from interfering with the reaction.
5. Removal of Arsenic
Once the arsenic impurity is adsorbed onto the Fe(OH)3 catalyst, it is effectively removed from the reaction mixture. This helps to maintain the purity of the sulfur trioxide produced and ensures the efficiency of the contact process.
6. Regeneration of the Catalyst
After adsorbing the arsenic impurity, the Fe(OH)3 catalyst needs to be regenerated for further use. This can be achieved by washing the catalyst with a suitable solvent or by subjecting it to high temperatures to remove the adsorbed impurities.
In conclusion, Fe(OH)3 is added to the contact process as a catalyst to remove arsenic impurity. It acts as an adsorbent, attracting and immobilizing the arsenic ions. This helps to maintain the purity of the sulfur trioxide produced and ensures the efficiency of the contact process.
The contact process is a method used to produce sulfuric acid on an industrial scale. It involves several steps, including the oxidation of sulfur dioxide to sulfur trioxide, which is then used to produce sulfuric acid. However, the presence of impurities can affect the efficiency of the process and the quality of the final product. One such impurity is arsenic.
1. The Role of Fe(OH)3
Fe(OH)3, also known as ferric hydroxide, is added to the contact process as a catalyst to remove arsenic impurity. It acts as a scavenger or adsorbent for arsenic, effectively removing it from the reaction mixture.
2. Arsenic Impurity
Arsenic is a toxic element that can be present in the raw materials used in the production of sulfuric acid. It can enter the process through impurities in the sulfur or in the air used for the oxidation of sulfur dioxide. Arsenic can poison the catalyst used in the process, reducing its effectiveness and leading to a decrease in the production of sulfuric acid.
3. Adsorption Mechanism
Fe(OH)3 acts as an adsorbent for arsenic impurity. Adsorption is a process by which substances are attracted and adhere to the surface of a solid. In this case, Fe(OH)3 has a high affinity for arsenic ions, and the impurity gets adsorbed onto the surface of the catalyst.
4. Formation of a Complex
The adsorption of arsenic by Fe(OH)3 involves the formation of a complex. Arsenic ions are attracted to the surface of Fe(OH)3 and form chemical bonds with the iron atoms. This complex formation immobilizes the arsenic impurity and prevents it from interfering with the reaction.
5. Removal of Arsenic
Once the arsenic impurity is adsorbed onto the Fe(OH)3 catalyst, it is effectively removed from the reaction mixture. This helps to maintain the purity of the sulfur trioxide produced and ensures the efficiency of the contact process.
6. Regeneration of the Catalyst
After adsorbing the arsenic impurity, the Fe(OH)3 catalyst needs to be regenerated for further use. This can be achieved by washing the catalyst with a suitable solvent or by subjecting it to high temperatures to remove the adsorbed impurities.
In conclusion, Fe(OH)3 is added to the contact process as a catalyst to remove arsenic impurity. It acts as an adsorbent, attracting and immobilizing the arsenic ions. This helps to maintain the purity of the sulfur trioxide produced and ensures the efficiency of the contact process.
Of the following compounds the most acidic is- a)Bi2O3
- b)P2O5
- c)Sb2O3
- d)As2O3
Correct answer is option 'B'. Can you explain this answer?
Of the following compounds the most acidic is
a)
Bi2O3
b)
P2O5
c)
Sb2O3
d)
As2O3
|
Rohit Yadav answered |
More is the oxidation number greater is the acidity of oxide
An explosive compound (A) reacts with water to produce NH4OH and HOCl. Then, the compound (A), is- a)TNG
- b)NCl3
- c)PCl3
- d)HNO3
Correct answer is option 'B'. Can you explain this answer?
An explosive compound (A) reacts with water to produce NH4OH and HOCl. Then, the compound (A), is
a)
TNG
b)
NCl3
c)
PCl3
d)
HNO3
|
Ashish Roy answered |
Explanation:
The given information states that compound (A) reacts with water to produce NH4OH and HOCl. We need to determine the identity of compound (A) from the given options.
Let's analyze each option to see if it fits the given information.
a) TNG:
TNG stands for Trinitroglycerin, which is an explosive compound commonly known as Nitroglycerin. Nitroglycerin does not react with water to produce NH4OH and HOCl, so option a) is not the correct answer.
b) NCl3:
NCl3 stands for Nitrogen Trichloride. Nitrogen Trichloride is an explosive compound that reacts with water to produce NH4OH and HOCl. The reaction can be represented as follows:
NCl3 + 3H2O → NH4OH + HOCl
This reaction fits the given information, so option b) is the correct answer.
c) PCl3:
PCl3 stands for Phosphorus Trichloride. Phosphorus Trichloride does not react with water to produce NH4OH and HOCl, so option c) is not the correct answer.
d) HNO3:
HNO3 stands for Nitric Acid. Nitric Acid does not react with water to produce NH4OH and HOCl, so option d) is not the correct answer.
Conclusion:
From the given options, option b) NCl3 is the only compound that reacts with water to produce NH4OH and HOCl. Therefore, the correct answer is option b) NCl3.
The given information states that compound (A) reacts with water to produce NH4OH and HOCl. We need to determine the identity of compound (A) from the given options.
Let's analyze each option to see if it fits the given information.
a) TNG:
TNG stands for Trinitroglycerin, which is an explosive compound commonly known as Nitroglycerin. Nitroglycerin does not react with water to produce NH4OH and HOCl, so option a) is not the correct answer.
b) NCl3:
NCl3 stands for Nitrogen Trichloride. Nitrogen Trichloride is an explosive compound that reacts with water to produce NH4OH and HOCl. The reaction can be represented as follows:
NCl3 + 3H2O → NH4OH + HOCl
This reaction fits the given information, so option b) is the correct answer.
c) PCl3:
PCl3 stands for Phosphorus Trichloride. Phosphorus Trichloride does not react with water to produce NH4OH and HOCl, so option c) is not the correct answer.
d) HNO3:
HNO3 stands for Nitric Acid. Nitric Acid does not react with water to produce NH4OH and HOCl, so option d) is not the correct answer.
Conclusion:
From the given options, option b) NCl3 is the only compound that reacts with water to produce NH4OH and HOCl. Therefore, the correct answer is option b) NCl3.
In general, nonmetals as compared to metals have- a)higher ionisation enthalpies
- b)non-metals readily form cations
- c)lower covalent charecter of the compounds formed between them
- d)lower ionisation enthalpies
Correct answer is option 'A'. Can you explain this answer?
In general, nonmetals as compared to metals have
a)
higher ionisation enthalpies
b)
non-metals readily form cations
c)
lower covalent charecter of the compounds formed between them
d)
lower ionisation enthalpies
|
Pranav Pillai answered |
Non metals have high value of ionization energy while metals have comparatively low value of ionization energy.
In the manufacture of sulphuric acid by contact process Tyndall box is used to- a) convert SO2 and SO3
- b)test the presence of dust particles
- c)filter dust particles
- d) remove impurities
Correct answer is option 'B'. Can you explain this answer?
In the manufacture of sulphuric acid by contact process Tyndall box is used to
a)
convert SO2 and SO3
b)
test the presence of dust particles
c)
filter dust particles
d)
remove impurities
|
Tanuja Kapoor answered |
In the manufacture of sulphuric acid by contact process, Tyndall box is used to. remove impurities. Solution : Tyndall box is for testing the presence of dust particles.
Fluorine differs from rest of the halogens in some of its properties. This is due to
- a)its smaller size and high electronegativity
- b)lack of d-orbitals
- c)low bond dissociation energy
- d)Both A and B
Correct answer is option 'D'. Can you explain this answer?
Fluorine differs from rest of the halogens in some of its properties. This is due to
a)
its smaller size and high electronegativity
b)
lack of d-orbitals
c)
low bond dissociation energy
d)
Both A and B
|
Stepway Academy answered |
Fluorine differs from rest of the elements of its family due to (i) its small size (ii) highest electronegativity, (iii) low bond dissociation energy and (iv) absence of d-orbitals in the valence shell.
Carbon give has X% of CO2 and is used as an antidote for poisoning of Y. Then, X and Y are- a)X = 95% and Y = lead poisoning
- b)X = 5% and Y = CO poisoning
- c)X = 30% and Y = CO2 poisoning
- d)X = 45% and Y = CO poisoning
Correct answer is option 'B'. Can you explain this answer?
Carbon give has X% of CO2 and is used as an antidote for poisoning of Y. Then, X and Y are
a)
X = 95% and Y = lead poisoning
b)
X = 5% and Y = CO poisoning
c)
X = 30% and Y = CO2 poisoning
d)
X = 45% and Y = CO poisoning
|
Rounak Desai answered |
C + 2O2 → 2CO + CO2
1 mole
1 mole
A compound X, of boron reacts with NH3 on heating to give another compound. Y which is called inorganic benzene. The compound X can be prepared by treating BF3 with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.- a)B3N3H6, B2H6
- b)B2O3, B3N3H6
- c)B2H6, B3N3H6
- d)BF3, B3N3H6
Correct answer is option 'C'. Can you explain this answer?
A compound X, of boron reacts with NH3 on heating to give another compound. Y which is called inorganic benzene. The compound X can be prepared by treating BF3 with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.
a)
B3N3H6, B2H6
b)
B2O3, B3N3H6
c)
B2H6, B3N3H6
d)
BF3, B3N3H6
|
Tejas Chawla answered |
BF3 reacts with LiAlH4 to form B2H6 which reacts with NH3NH3 in 1:2 ratio forming B3N3H6( Borazine , inorganic benzene
Which is incorrectly matched ?- a)CsBr3
Cs+ + Br3_ - b)I4O9
I3+ + (IO3_)3 - c)AgBrO3
Ag+ + BrO3_ - d)I2O4
IO2_ + IO2+
Correct answer is option 'D'. Can you explain this answer?
Which is incorrectly matched ?
a)
CsBr3 Cs+ + Br3_
Cs+ + Br3_b)
I4O9 I3+ + (IO3_)3
I3+ + (IO3_)3c)
AgBrO3 Ag+ + BrO3_
Ag+ + BrO3_ d)
I2O4 IO2_ + IO2+
IO2_ + IO2+|
|
Neha Joshi answered |
It is strictly covalent does not shows cationic & anionic form.
Aqueous solution of Na2S2O3 on reaction with Cl2Cl2 gives- a)NaHSO4
- b)NaCl
- c)Na2S4O6
- d)NaOH
Correct answer is option 'A'. Can you explain this answer?
Aqueous solution of Na2S2O3 on reaction with Cl2Cl2 gives
a)
NaHSO4
b)
NaCl
c)
Na2S4O6
d)
NaOH
|
Nilesh Saini answered |
Reaction between Na2S2O3 and Cl2:
The reaction between Na2S2O3 (sodium thiosulfate) and Cl2 (chlorine gas) is a redox reaction. It can be represented by the following balanced chemical equation:
Na2S2O3 + Cl2 → NaHSO4 + NaCl + S
Explanation of the reaction:
- Sodium thiosulfate (Na2S2O3) is a salt that consists of sodium cations (Na+) and thiosulfate anions (S2O3^2-).
- Chlorine gas (Cl2) is a diatomic molecule consisting of two chlorine atoms.
- In this reaction, chlorine gas oxidizes thiosulfate ions to form sulfate ions (SO4^2-) and sulfur (S).
- Sodium cations remain unchanged and are present in the final products.
- The balanced equation shows the stoichiometry of the reaction, indicating that for every 1 mole of sodium thiosulfate, 1 mole of sodium bisulfate (NaHSO4), 1 mole of sodium chloride (NaCl), and 1 mole of sulfur are produced.
Explanation of the correct answer:
The correct answer is option 'A' - NaHSO4 (sodium bisulfate). This is because the reaction between Na2S2O3 and Cl2 produces NaHSO4 as one of the products. NaHSO4 is formed when thiosulfate ions are oxidized by chlorine gas. The other products of the reaction are NaCl (sodium chloride) and S (sulfur).
Other options explained:
- Option 'B' - NaCl (sodium chloride) is also formed as a product of the reaction. However, it is not the correct answer because there is an additional product, NaHSO4.
- Option 'C' - Na2S4O6 (sodium tetrathionate) is not formed in this reaction. The reaction between Na2S2O3 and Cl2 does not involve the formation of tetrathionate ions.
- Option 'D' - NaOH (sodium hydroxide) is not a product of this reaction. The reaction does not involve the formation of hydroxide ions.
In conclusion, the reaction between Na2S2O3 and Cl2 produces NaHSO4, NaCl, and S as the products. Sodium bisulfate (NaHSO4) is the correct answer as it is one of the products formed in this redox reaction.
The reaction between Na2S2O3 (sodium thiosulfate) and Cl2 (chlorine gas) is a redox reaction. It can be represented by the following balanced chemical equation:
Na2S2O3 + Cl2 → NaHSO4 + NaCl + S
Explanation of the reaction:
- Sodium thiosulfate (Na2S2O3) is a salt that consists of sodium cations (Na+) and thiosulfate anions (S2O3^2-).
- Chlorine gas (Cl2) is a diatomic molecule consisting of two chlorine atoms.
- In this reaction, chlorine gas oxidizes thiosulfate ions to form sulfate ions (SO4^2-) and sulfur (S).
- Sodium cations remain unchanged and are present in the final products.
- The balanced equation shows the stoichiometry of the reaction, indicating that for every 1 mole of sodium thiosulfate, 1 mole of sodium bisulfate (NaHSO4), 1 mole of sodium chloride (NaCl), and 1 mole of sulfur are produced.
Explanation of the correct answer:
The correct answer is option 'A' - NaHSO4 (sodium bisulfate). This is because the reaction between Na2S2O3 and Cl2 produces NaHSO4 as one of the products. NaHSO4 is formed when thiosulfate ions are oxidized by chlorine gas. The other products of the reaction are NaCl (sodium chloride) and S (sulfur).
Other options explained:
- Option 'B' - NaCl (sodium chloride) is also formed as a product of the reaction. However, it is not the correct answer because there is an additional product, NaHSO4.
- Option 'C' - Na2S4O6 (sodium tetrathionate) is not formed in this reaction. The reaction between Na2S2O3 and Cl2 does not involve the formation of tetrathionate ions.
- Option 'D' - NaOH (sodium hydroxide) is not a product of this reaction. The reaction does not involve the formation of hydroxide ions.
In conclusion, the reaction between Na2S2O3 and Cl2 produces NaHSO4, NaCl, and S as the products. Sodium bisulfate (NaHSO4) is the correct answer as it is one of the products formed in this redox reaction.
The correct order of acid strength of oxyacids of chlorine is- a)HClO < HClO2 < HClO3 < HClO4
- b)HClO4 < HClO3 < HClO2 < HClO
- c)HClO > HClO4 > HClO3 > HClO2
- d)HClO4 < HClO2 > HClO3 > HClO
Correct answer is option 'A'. Can you explain this answer?
The correct order of acid strength of oxyacids of chlorine is
a)
HClO < HClO2 < HClO3 < HClO4
b)
HClO4 < HClO3 < HClO2 < HClO
c)
HClO > HClO4 > HClO3 > HClO2
d)
HClO4 < HClO2 > HClO3 > HClO
|
Saumya Datta answered |
Understanding Acid Strength of Oxyacids of Chlorine
The strength of oxyacids is influenced by the number of oxygen atoms bonded to the central atom (chlorine in this case). The general trend indicates that as the number of oxygen atoms increases, the acid strength also increases.
Acid Strength Hierarchy
- HClO: This is hypochlorous acid, with one oxygen atom. It is the weakest among the series due to fewer oxygen atoms that stabilize the negative charge on the conjugate base (ClO⁻).
- HClO2: Known as chlorous acid, it has two oxygen atoms. The additional oxygen allows for better stabilization of the conjugate base compared to HClO, making it stronger.
- HClO3: This is chloric acid, with three oxygen atoms. The increased number of oxygen atoms further enhances the ability to hold the negative charge, significantly increasing acid strength.
- HClO4: Perchloric acid has four oxygen atoms. It is the strongest acid in this series because the high number of oxygen atoms maximizes stabilization of the conjugate base, making it highly effective in donating protons.
Conclusion
Thus, the correct order of acid strength for the oxyacids of chlorine is:
- HClO < hclo2="" />< hclo3="" />< />
This aligns with option A. The increasing number of oxygen atoms leads to stronger acids, confirming that HClO4 is the strongest and HClO is the weakest.
The strength of oxyacids is influenced by the number of oxygen atoms bonded to the central atom (chlorine in this case). The general trend indicates that as the number of oxygen atoms increases, the acid strength also increases.
Acid Strength Hierarchy
- HClO: This is hypochlorous acid, with one oxygen atom. It is the weakest among the series due to fewer oxygen atoms that stabilize the negative charge on the conjugate base (ClO⁻).
- HClO2: Known as chlorous acid, it has two oxygen atoms. The additional oxygen allows for better stabilization of the conjugate base compared to HClO, making it stronger.
- HClO3: This is chloric acid, with three oxygen atoms. The increased number of oxygen atoms further enhances the ability to hold the negative charge, significantly increasing acid strength.
- HClO4: Perchloric acid has four oxygen atoms. It is the strongest acid in this series because the high number of oxygen atoms maximizes stabilization of the conjugate base, making it highly effective in donating protons.
Conclusion
Thus, the correct order of acid strength for the oxyacids of chlorine is:
- HClO < hclo2="" />< hclo3="" />< />
This aligns with option A. The increasing number of oxygen atoms leads to stronger acids, confirming that HClO4 is the strongest and HClO is the weakest.
Which of the following species is not a pseudohalide ?- a)CNO-
- b)RCOO-
- c)OCN-
- d) N3-
Correct answer is option 'B'. Can you explain this answer?
Which of the following species is not a pseudohalide ?
a)
CNO-
b)
RCOO-
c)
OCN-
d)
N3-
|
Anand Khanna answered |
Pseudo halides are
CN-, NC-, OCN-, SCN-, SeCN-
NCS-, N3-, NCO-
CN-, NC-, OCN-, SCN-, SeCN-
NCS-, N3-, NCO-
In a molecule of phosphorus (V) oxide, there are- a)4P-P, 10 P-O and 4P = O bonds
- b)12P-O, and 4P=O bonds
- c)2P-O and 4P = P bonds
- d)6P-P, 12P-O and 4P = P bonds
Correct answer is option 'B'. Can you explain this answer?
In a molecule of phosphorus (V) oxide, there are
a)
4P-P, 10 P-O and 4P = O bonds
b)
12P-O, and 4P=O bonds
c)
2P-O and 4P = P bonds
d)
6P-P, 12P-O and 4P = P bonds
|
Soumya Mukherjee answered |
Preamble:
Phosphorus (V) oxide is a chemical compound with the formula P4O10. It is a highly reactive compound that is formed by the combination of four phosphorus atoms and ten oxygen atoms. In this molecule, the phosphorus atoms can form different types of bonds with each other and with the oxygen atoms.
Explanation:
The correct answer is option B, which states that there are 12 P-O bonds and 4 P=O bonds in a molecule of phosphorus (V) oxide. Let's break down the molecule and analyze the bonding.
Structure of Phosphorus (V) Oxide:
- Phosphorus (V) oxide consists of four phosphorus atoms (P) and ten oxygen atoms (O).
- The phosphorus atoms are arranged in a tetrahedral shape, with each phosphorus atom bonded to three other phosphorus atoms.
- The oxygen atoms are bonded to the phosphorus atoms, forming P-O bonds.
Types of Bonds:
1. P-O bonds:
- Each phosphorus atom forms three P-O bonds with three oxygen atoms.
- As there are four phosphorus atoms, the total number of P-O bonds is 4 x 3 = 12.
2. P=O bonds:
- The remaining oxygen atoms are involved in the formation of P=O bonds.
- Each P=O bond consists of a double bond between a phosphorus atom and an oxygen atom.
- As there are four oxygen atoms available for the formation of P=O bonds, the total number of P=O bonds is 4.
Therefore, the molecule of phosphorus (V) oxide contains 12 P-O bonds and 4 P=O bonds, which is consistent with option B.
Conclusion:
In conclusion, a molecule of phosphorus (V) oxide contains 12 P-O bonds and 4 P=O bonds. The P-O bonds are formed between the phosphorus and oxygen atoms, while the P=O bonds involve double bonds between a phosphorus atom and an oxygen atom.
Phosphorus (V) oxide is a chemical compound with the formula P4O10. It is a highly reactive compound that is formed by the combination of four phosphorus atoms and ten oxygen atoms. In this molecule, the phosphorus atoms can form different types of bonds with each other and with the oxygen atoms.
Explanation:
The correct answer is option B, which states that there are 12 P-O bonds and 4 P=O bonds in a molecule of phosphorus (V) oxide. Let's break down the molecule and analyze the bonding.
Structure of Phosphorus (V) Oxide:
- Phosphorus (V) oxide consists of four phosphorus atoms (P) and ten oxygen atoms (O).
- The phosphorus atoms are arranged in a tetrahedral shape, with each phosphorus atom bonded to three other phosphorus atoms.
- The oxygen atoms are bonded to the phosphorus atoms, forming P-O bonds.
Types of Bonds:
1. P-O bonds:
- Each phosphorus atom forms three P-O bonds with three oxygen atoms.
- As there are four phosphorus atoms, the total number of P-O bonds is 4 x 3 = 12.
2. P=O bonds:
- The remaining oxygen atoms are involved in the formation of P=O bonds.
- Each P=O bond consists of a double bond between a phosphorus atom and an oxygen atom.
- As there are four oxygen atoms available for the formation of P=O bonds, the total number of P=O bonds is 4.
Therefore, the molecule of phosphorus (V) oxide contains 12 P-O bonds and 4 P=O bonds, which is consistent with option B.
Conclusion:
In conclusion, a molecule of phosphorus (V) oxide contains 12 P-O bonds and 4 P=O bonds. The P-O bonds are formed between the phosphorus and oxygen atoms, while the P=O bonds involve double bonds between a phosphorus atom and an oxygen atom.
Which one of the following compounds on strong heating evolves ammonia gas ?- a)(NH4)2SO4
- b)HNO3
- c)(NH4)2Cr2O7
- d)NH3NO3
Correct answer is option 'A'. Can you explain this answer?
Which one of the following compounds on strong heating evolves ammonia gas ?
a)
(NH4)2SO4
b)
HNO3
c)
(NH4)2Cr2O7
d)
NH3NO3
|
Ameya Mukherjee answered |
Answer:
When certain compounds are heated strongly, they undergo decomposition reactions, leading to the release of various gases. In this case, we need to determine which of the given compounds evolves ammonia gas upon strong heating.
(NH4)2SO4 is ammonium sulfate, which does not evolve ammonia gas upon strong heating. Instead, it decomposes to give off sulfur dioxide gas, water vapor, and nitrogen dioxide gas.
HNO3 is nitric acid, which does not evolve ammonia gas upon strong heating. It undergoes decomposition to release nitrogen dioxide gas, oxygen gas, and water vapor.
(NH4)2Cr2O7 is ammonium dichromate. It is a highly unstable compound and decomposes explosively upon heating. The decomposition reaction produces chromium(III) oxide, nitrogen gas, and water vapor. The evolution of nitrogen gas may give an impression of ammonia gas, but it is not the same.
NH3NO3 is ammonium nitrate, which does not evolve ammonia gas upon strong heating. Rather, it decomposes to produce nitrogen gas, oxygen gas, and water vapor.
Among the given compounds, only (NH4)2SO4 (ammonium sulfate) does not evolve ammonia gas upon strong heating. Therefore, the correct answer is option 'A'.
Introduction:
When certain compounds are heated strongly, they undergo decomposition reactions, leading to the release of various gases. In this case, we need to determine which of the given compounds evolves ammonia gas upon strong heating.
Explanation:
1. (NH4)2SO4:
(NH4)2SO4 is ammonium sulfate, which does not evolve ammonia gas upon strong heating. Instead, it decomposes to give off sulfur dioxide gas, water vapor, and nitrogen dioxide gas.
2. HNO3:
HNO3 is nitric acid, which does not evolve ammonia gas upon strong heating. It undergoes decomposition to release nitrogen dioxide gas, oxygen gas, and water vapor.
3. (NH4)2Cr2O7:
(NH4)2Cr2O7 is ammonium dichromate. It is a highly unstable compound and decomposes explosively upon heating. The decomposition reaction produces chromium(III) oxide, nitrogen gas, and water vapor. The evolution of nitrogen gas may give an impression of ammonia gas, but it is not the same.
4. NH3NO3:
NH3NO3 is ammonium nitrate, which does not evolve ammonia gas upon strong heating. Rather, it decomposes to produce nitrogen gas, oxygen gas, and water vapor.
Conclusion:
Among the given compounds, only (NH4)2SO4 (ammonium sulfate) does not evolve ammonia gas upon strong heating. Therefore, the correct answer is option 'A'.
The compounds formed by highly reactive non-metals with highly reactive metals are generally- a)slightly different in their ionisation enthalpies
- b)ionic
- c)slightly different in their electronegativities
- d)covalent
Correct answer is option 'B'. Can you explain this answer?
The compounds formed by highly reactive non-metals with highly reactive metals are generally
a)
slightly different in their ionisation enthalpies
b)
ionic
c)
slightly different in their electronegativities
d)
covalent
|
Mihir Patel answered |
Compunds formed by highly reactive non metals and metals is ionic bond.
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