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Statement-1 . LiCl is covalent whereas ...

Statement-1 . `LiCl` is covalent whereas NaCl is ionic.
Statement-2. Greater the size of the cation, greater is its polarising power.

A

Statement-1 is Ture , Statement-2 is Ture , Statement-2 is a correct explanation for Statement-1.

B

Statement-1 is Ture , Statement-2 is Ture , Statement-2 is not a correct explanation for Statement-1.

C

Statement-1 is True , Statement-2 is False .

D

Statement-1 is False, Statement-2 is True.

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the statements provided regarding the nature of `LiCl` and `NaCl`, we can break down the reasoning as follows: ### Step 1: Understanding Ionic and Covalent Bonds - **Ionic Bonds**: Formed when there is a complete transfer of electrons from one atom to another, typically between metals and non-metals. The resulting ions are held together by electrostatic forces. - **Covalent Bonds**: Formed when two atoms share electrons. This usually occurs between non-metals. ### Step 2: Analyzing LiCl - Lithium (Li) is a small cation with a high charge density. Chlorine (Cl) is a larger anion. - According to Fajans' rules, a small cation with a high charge can polarize the electron cloud of a larger anion, leading to covalent character in the bond. - Therefore, `LiCl` exhibits more covalent character due to the small size and high polarizing power of the Li⁺ ion. ### Step 3: Analyzing NaCl - Sodium (Na) is a larger cation compared to lithium. While Na⁺ can still polarize Cl⁻, it does so to a lesser extent than Li⁺ due to its larger size. - As a result, `NaCl` is more ionic in nature because the bond is primarily formed through the electrostatic attraction between Na⁺ and Cl⁻ without significant polarization. ### Step 4: Evaluating the Statements - **Statement-1**: `LiCl` is covalent whereas `NaCl` is ionic. This statement is true based on the analysis above. - **Statement-2**: Greater the size of the cation, greater is its polarizing power. This statement is false. In fact, the opposite is true: smaller cations have greater polarizing power. ### Conclusion - **Final Evaluation**: Statement-1 is true, and Statement-2 is false.
To analyze the statements provided regarding the nature of `LiCl` and `NaCl`, we can break down the reasoning as follows: ### Step 1: Understanding Ionic and Covalent Bonds - **Ionic Bonds**: Formed when there is a complete transfer of electrons from one atom to another, typically between metals and non-metals. The resulting ions are held together by electrostatic forces. - **Covalent Bonds**: Formed when two atoms share electrons. This usually occurs between non-metals. ### Step 2: Analyzing LiCl - Lithium (Li) is a small cation with a high charge density. Chlorine (Cl) is a larger anion. ...
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Knowledge Check

  • Statement- 1 . CuCl is more covalent than NaCl. Statement- 2 . Na^(+) ion is more polarising than Cu^(+) ion .

    A
    Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for statement-1.
    B
    Statement-1 is True, Statement-2 is True, Statement-2 is not a correct explanation for statement-1.
    C
    Statement-1 is True, Statement-2 is False.
    D
    Statement-1 is False, Statement-2 is True.

  • Which of the following options regarding true/false statement for a van der Waal's gas is correct? Statement-1 : At critical condition, the gas will follow the equation 8 PV=3nRT Statement-2: At Boyle's temperature, Z=1 at all pressures. Statement-3: Greater the size of molecuels, greater will be the vander Waal's constnat 'b'. Statement-4: For H_(2) gas, if P=200 atm and T=300K,Z gt1 .

    A
    Al the statements are correct
    B
    Only statement-2 is incorrect.
    C
    Statement-1 and Statement-2 a re incorrect statements.
    D
    State,emts-1 and Statement-4 are incorrect statements.

  • Statement-1 : IE_(1) ofN is greater than 0 . Statement-2: N-atom is bigger than O in size.

    A
    Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
    B
    Staterment-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1.
    C
    Statement-1 is true, statement-2 is false.
    D
    Statement-1 is false, statement-2 is true.

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    Assertion : Among alkaline earth metals, Be predominantly forms covalent bond. Reason : Be is smaller in size and hence has greater polarising power.

    in an ionic bond the cation tends to polarise the electron cloud of the anion by pulling electron density towards itself This causes development of covalent character in the ionic bond because the electron density gets localised in between the nuclei The tendency of the cation to bring about the polarisation of the anion is expressed as its polasising power The ability of ion to undergo polarisation is called its polarisability The polarising power of a cation or an anion is decided on the basis of F ajans' rules as follows . (i) The smaller the cation, the higher is its polarising power (ii) Cations with pseudo-noble gas configuration (ns^(2)np^(6)nd^(10)) have relatively high polarising power than those with noble gas configuration (ns^(2) np^(6)) (iii) The larger the size of the anion, the higher is its polarisability The ionic conductance of which of the following is the highest ? .

    in an ionic bond the cation tends to polarise the electron cloud of the anion by pulling electron density towards itself This causes development of covalent character in the ionic bond because the electron density gets localised in between the nuclei The tendency of the cation to bring about the polarisation of the anion is expressed as its polasising power The ability of ion to undergo polarisation is called its polarisability The polarising power of a cation or an anion is decided on the basis of F ajans' rules as follows . (i) The smaller the cation, the higher is its polarising power (ii) Cations with pseudo-noble gas configuration (ns^(2)np^(6)nd^(10)) have relatively high polarising power than those with noble gas configuration (ns^(2) np^(6)) (iii) The larger the size of the anion, the higher is its polarisability Arranfe of the following species in dereasing order of polarising powers Ag^(o+),TI^(o+),Na^(o+) .

    in an ionic bond the cation tends to polarise the electron cloud of the anion by pulling electron density towards itself This causes development of covalent character in the ionic bond because the electron density gets localised in between the nuclei The tendency of the cation to bring about the polarisation of the anion is expressed as its polasising power The ability of ion to undergo polarisation is called its polarisability The polarising power of a cation or an anion is decided on the basis of F ajans' rules as follows . (i) The smaller the cation, the higher is its polarising power (ii) Cations with pseudo-noble gas configuration (ns^(2)np^(6)nd^(10)) have relatively high polarising power than those with noble gas configuration (ns^(2) np^(6)) (iii) The larger the size of the anion, the higher is its polarisability Choose the correct order of polarisability for the following I^(Θ),Br^(Θ),CI^(Θ)F^(Θ) .

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