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All questions of The p - Block Elements for NEET Exam

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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 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

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?

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 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?

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.

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?

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.
 

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?

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.

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?

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.

XeF2 is isostructural with
  • a)
    SbCl3
  • b)
    BaCl2
  • c)
    TeF2
  • d)
    ICl2–
Correct answer is option 'D'. Can you explain this answer?

Preeti Iyer answered
The correct answer is option D
XeF2 is isostructural with ICl2−.
Both contain the same number of lone pairs and bond pairs on the central atom.
There are 3 lone pairs and 2 bond pairs.
This results in linear geometry.

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?

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+3H2​O
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 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?

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 of the following structure is similar to graphite? [NEET 2013]
  • a)
    B
  • b)
    B4C
  • c)
    B2H6
  • d)
    BN
Correct answer is option 'D'. Can you explain this answer?

Arnab Iyer answered
Boron nitride (BN) is known as inorganic graphite. The most stable form is hexagonal one. It has layered structure similar to graphite.

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?

Sahana Ahuja answered
Explanation:

When highly reactive non-metals react with highly reactive metals, the compounds formed are generally ionic in nature. This means that they are made up of positively charged metal ions and negatively charged non-metal ions.

1. Formation of Ionic Compounds:
When a highly reactive non-metal reacts with a highly reactive metal, the non-metal tends to gain electrons and become negatively charged, while the metal tends to lose electrons and become positively charged. This transfer of electrons results in the formation of ions, and these oppositely charged ions are held together by strong electrostatic forces, forming an ionic compound.

2. High Reactivity of Non-Metals and Metals:
Highly reactive non-metals have a strong tendency to gain electrons because their outermost energy level is almost empty, and they can achieve a stable electron configuration by gaining electrons. On the other hand, highly reactive metals have a strong tendency to lose electrons because their outermost energy level is almost full, and they can achieve a stable electron configuration by losing electrons.

3. Ionic Bonding:
The high reactivity of non-metals and metals makes it easier for them to undergo electron transfer, resulting in the formation of ions. The attraction between these oppositely charged ions forms an ionic bond. The ionization energy of metals is generally lower than that of non-metals, which facilitates the loss of electrons by metals. The electronegativity of non-metals is generally higher than that of metals, which promotes the gain of electrons by non-metals. These factors contribute to the formation of ionic compounds.

4. Covalent Bonding:
Covalent bonding occurs when non-metals react with non-metals, where they share electrons to achieve a stable electron configuration. In the case of highly reactive non-metals and highly reactive metals, the difference in reactivity and electron configuration leads to the formation of ionic compounds rather than covalent compounds. The high electronegativity difference and the strong tendency for electron transfer make the formation of covalent bonds less favorable in these combinations.

Therefore, the compounds formed by highly reactive non-metals with highly reactive metals are generally ionic in nature.

Aluminium is extracted from alumina (Al2O3) by electrolysis of a molten mixture of : [2012]
  • a)
    Al2O3 + HF + NaAlF4
  • b)
    Al2O3 + CaF2 + NaAlF4
  • c)
    Al2O3 + Na3AlF6 + CaF2
  • d)
    Al2O3 + KF + Na3AlF6
Correct answer is option 'C'. Can you explain this answer?

Sinjini Datta answered
Extraction of Aluminium from Alumina (Al2O3)

Aluminium is an important metal that is widely used in various industries due to its low density, high strength, and excellent corrosion resistance. It is extracted from its ore, alumina (Al2O3), through a process called electrolysis. The correct combination of molten mixture for the extraction of aluminium by electrolysis is given in option 'C', which consists of Al2O3, Na3AlF6, and CaF2.

Electrolysis of Alumina (Al2O3)

The extraction of aluminium from alumina involves the process of electrolysis. In this process, a molten mixture of alumina, Na3AlF6, and CaF2 is used as an electrolyte. The following steps explain the extraction process in detail:

1. Formation of Cryolite (Na3AlF6):
- Cryolite is a mineral that is added to the mixture to lower the melting point of alumina and improve its conductivity.
- Na3AlF6 is formed by the reaction between alumina and sodium fluoride (NaF).
- 2 Al2O3 + 6 NaF → 2 Na3AlF6 + 3 O2

2. Electrolysis of Alumina (Al2O3):
- The mixture of alumina, Na3AlF6, and CaF2 is heated to a high temperature to form a molten electrolyte.
- The mixture is then placed in an electrolytic cell, which consists of a carbon anode and a carbon cathode.
- The carbon anode is connected to the positive terminal of a power supply, while the carbon cathode is connected to the negative terminal.
- The molten mixture acts as the electrolyte, and alumina is dissolved in it.
- When an electric current is passed through the electrolyte, the following reactions occur:
- At the anode (oxidation): 2 O2- → O2 + 4 e-
- At the cathode (reduction): 4 Al3+ + 12 e- → 4 Al
- The oxygen ions (O2-) are attracted to the anode and combine to form oxygen gas (O2), which is released.
- The aluminium ions (Al3+) are attracted to the cathode and gain electrons to form aluminium metal (Al), which is deposited on the cathode.

Advantages of the Molten Mixture

The molten mixture of alumina, Na3AlF6, and CaF2 has several advantages for the extraction of aluminium:
- Lower Melting Point: The addition of cryolite (Na3AlF6) lowers the melting point of alumina, reducing the amount of energy required for the process.
- Improved Conductivity: The presence of the molten mixture enhances the conductivity of the electrolyte, allowing for efficient electrolysis.
- Electrolyte Stability: The molten mixture remains stable at high temperatures, ensuring the continuous flow of current and the extraction of aluminium.

Conclusion
The correct combination of the molten mixture for the extraction of aluminium from alumina (Al2O3) is option 'C', which consists of Al2O3, Na3AlF6, and CaF

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?

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.

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?

Muskaan Kumar answered
Introduction:
In this question, we are asked to identify the most acidic compound among the given options. Acidity is a property of compounds that can donate a proton (H+ ion). The stronger the acid, the more easily it donates a proton. To determine the acidity of a compound, we need to consider the strength of the corresponding acid it forms when dissolved in water.

Explanation:
Among the given options, the most acidic compound is P2O5 (option B). Let's understand why.

1. Oxidation state:
The acidity of an oxide compound mainly depends on the oxidation state of the central atom. In this case, the central atom is phosphorus (P).

- In P2O5, the oxidation state of phosphorus is +5.
- In Bi2O3, the oxidation state of bismuth is +3.
- In Sb2O3, the oxidation state of antimony is +3.
- In As2O3, the oxidation state of arsenic is +3.

2. Acidic behavior of oxides:
In general, oxides with higher oxidation states tend to be more acidic. This is because higher oxidation states lead to greater electronegativity, resulting in stronger acidic behavior.

3. Acid formation:
When oxides dissolve in water, they form corresponding acids. The acidity of an oxide is determined by the strength of the acid it forms.

- P2O5 forms phosphoric acid (H3PO4), which is a strong acid.
- Bi2O3 forms bismuthic acid (HBiO3), which is a weak acid.
- Sb2O3 forms antimonious acid (HSbO2), which is a weak acid.
- As2O3 forms arsenious acid (H3AsO3), which is also a weak acid.

4. Conclusion:
Based on the above analysis, we can conclude that P2O5 (option B) is the most acidic compound among the given options. It has the highest oxidation state of +5 and forms phosphoric acid, which is a strong acid.

Which of the following elements is extracted commercially by the electrolysis of an aqueous solution of its compound ? [1993]
  • a)
    Cl
  • b)
    Br
  • c)
    Al
  • d)
    Na
Correct answer is option 'C'. Can you explain this answer?

Arindam Unni answered
Electrolysis is a process that involves the decomposition of a compound through the use of an electric current. It is commonly used to extract metals from their compounds. In this case, we are looking for an element that is commercially extracted by the electrolysis of an aqueous solution of its compound.

The correct answer is option C, chlorine (Cl).

Explanation:

Electrolysis of an Aqueous Solution:
When an aqueous solution is electrolyzed, the compound in the solution is broken down into its constituent elements. The positive ions (cations) migrate towards the negative electrode (cathode), where reduction occurs, while the negative ions (anions) migrate towards the positive electrode (anode), where oxidation occurs.

Chlorine Extraction:
Chlorine is commercially extracted by the electrolysis of an aqueous solution of its compound, typically sodium chloride (NaCl), which is commonly known as table salt. During the electrolysis of sodium chloride solution, chlorine gas is released at the anode, while hydrogen gas is released at the cathode.

At the anode:
At the anode, chloride ions (Cl-) are oxidized to chlorine gas (Cl2). The half-reaction at the anode is:

2Cl- -> Cl2 + 2e-

At the cathode:
At the cathode, water molecules are reduced to hydrogen gas (H2) and hydroxide ions (OH-). The half-reaction at the cathode is:

2H2O + 2e- -> H2 + 2OH-

Overall Reaction:
The overall reaction during the electrolysis of sodium chloride solution can be represented as:

2NaCl(aq) + 2H2O(l) -> Cl2(g) + H2(g) + 2NaOH(aq)

Importance of Chlorine:
Chlorine is an important element in various industries. It is used for the production of PVC (polyvinyl chloride), which is widely used in the manufacturing of pipes, cables, and other plastic products. Chlorine is also used in the production of bleach, disinfectants, and various organic compounds.

Conclusion:
In conclusion, chlorine is commercially extracted by the electrolysis of an aqueous solution of its compound, such as sodium chloride. The process involves the oxidation of chloride ions at the anode, resulting in the release of chlorine gas, while hydrogen gas is released at the cathode. Chlorine is an important element used in different industries for various purposes.

Which of the following types of forces bind together the carbon atoms in diamond ? [1992]
  • a)
    Ionic
  • b)
    Covalent
  • c)
    Dipolar
  • d)
    vander Waals.
Correct answer is option 'B'. Can you explain this answer?

Bhargavi Choudhury answered
In diamond each carbon atom is sp 3 hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.

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?

Puja Pillai answered
Tetra atomic molecule (A) reacts with nitrogen (I) oxide to produce two substances (B) and (C). Substance (B) is a dehydrating agent in its monomeric form, while substance (C) is a diatomic gas that exhibits almost inert behavior. The substances (A), (B), and (C) can be determined as follows:

1. Substance A:
Since substance A is a tetra atomic molecule, it consists of four atoms. The molecular formula of substance A is P4 (phosphorus tetramer). Phosphorus exists as a tetra atomic molecule in its elemental form.

2. Substance B:
Substance B is a dehydrating agent in its monomeric form. This means that it removes water molecules. The dehydrating agent formed by the reaction of substance A with nitrogen (I) oxide is P4O10 (phosphorus pentoxide). Phosphorus pentoxide is a white, crystalline solid that readily absorbs moisture from the air and reacts with water to form phosphoric acid.

3. Substance C:
Substance C is a diatomic gas that exhibits almost inert behavior. Nitrogen (I) oxide is a diatomic gas with the formula N2O. It is commonly known as nitrous oxide or laughing gas. Nitrous oxide is a colorless, sweet-smelling gas that is used in anesthesia and as a propellant in aerosol cans.

Therefore, the substances (A), (B), and (C) produced in the reaction are:
- Substance A: P4 (phosphorus tetramer)
- Substance B: P4O10 (phosphorus pentoxide)
- Substance C: N2O (nitrous oxide)

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