Polarisability and Fajan's Rule
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Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R.
Assertion A : The size of the ion is less than the ion.
Reason R : The above is a consequence of the lanthanoid contraction.
In the light of the above statements , choose the correct Ans: from the options given below:
A is false but R is true
Both A and R are true but R is not the correct explanation of A
A is true but R is false
Both A and R are true and R is the correct explanation of A
Which alkali metal has maximum degree of hydration?
Which is more covalent ?
Which is more Ionic ?
- MF>MCl>MBr>MI
- MF>MCl>MI>MBr
- MI>MBr>MCl>MF
- MCl>MI>MBr>MF
Na2CO3 does not decompose on heating where as CaCO3 decomposes. Why?
Higher cation charge
Presence of Oxygen
Lower anion charge
Insufficient data
Correct order of increasing covalent character is:
LiCl > BeCl2 > BCl3 > CCl4
LiCl < BeCl2 < BCl3 < CCl4
LiCl> BeCl2 > CCl4 > BCl3
LiCl < BCl3 < BeCl2 < CCl4
KCl has higher melting point than AgCl. Why?
[rAg+ ≈ rK+]
Cation size
Anion size
Pseudo noble gas cation
Cation charge
Na2CO3 does not decompose on heating where as CaCO3 decomposes. Why?
Higher cation charge
Presence of Oxygen
Lower anion charge
Insufficient data
- Li+(aq)
- Na+(aq)
- K+(aq)
- Cs+(aq)
- I−>Br−>Cl−>F−
- I−>Br−=Cl−>F−
- I−=Br−=Cl−>F−
- I−=Br−=F−<Cl−
- The heat of hydration of the dipositive alkaline earth metals ions increases with increase in their ionic size.
- Hydration of alkali metal ions is less than that of alkaline earth metals.
- Alkaline earth metal ions, because of their much larger charge to size ratio, exert a much stronger electrostatic attraction on the oxygen of water molecule surrounding them.
- The melting point of sodium halides follow the order NaF>NaCl>NaBr>NaI.
(I) Polarizability of S2− is lower than Se2−
(II) Polarizability of S2− is higher than Cl−
(III) Polarizability of S2− is lower than P3−
(IV) Polarizability of O2− is higher than S2−
- I, II and III
- I and II
- II and IV
- All of these
LiCl is hydrated while NaCl is not. Why?
Presence of 2 s shell
Presence of anion
Smaller cation
LiCl is hydrophobic
Which of the following halide possess the highest covalent character?
- LiF
- LiCl
- LiBr
- Lil
- LiCl>BeCl2>BCl3>CCl4
- LiCl<BeCl2<BCl3<CCl4
- LiCl>BeCl2>CCl4>BCl3
- BeCl2>LiCl>BCl3>CCl4
KCl has higher melting point than AgCl. Why?
[rAg+ ≈ rK+]
Cation size
Anion size
Pseudo noble gas cation
Cation charge
(i) Polarizability of S2− is lesser than Se2−
(ii) Polarizability of S2− is higher than Cl−
(iii) polarizability of S2− is lesser than P3−
(iv) Polarizability of O2− is higher than S2−
- I, II, and III
- I and II
- II and IV
- None of these
Correct order of increasing covalent character is:
LiCl > BeCl2 > BCl3 > CCl4
LiCl < BeCl2 < BCl3 < CCl4
LiCl> BeCl2 > CCl4 > BCl3
LiCl < BCl3 < BeCl2 < CCl4
I) BeCO3
II) MgCO3
III) CaCO3
- I < II < III
- I > II > III
- I < III < II
- II < I < III
- LiCl>BeCl2>BCl3>CCl4
- LiCl<BeCl2<BCl3<CCl4
- LiCl>BeCl2>CCl4>BCl3
- BeCl2>LiCl>BCl3>CCl4
- BeCO3>MgCO3>CaCO3>SrCO3>BaCO3
- BaCO3>SrCO3>CaCO3>MgCO3>BeCO3
- BaCO3>MgCO3>CaCO3>SrCO3>BeCO3
- BeCO3>CaCO3>MgCO3>SrCO3>BaCO3
S1 : AgI is less soluble in water than AgF due to more polarization of I− in comparison to F− ion.
S2 : The melting point of BaCl2 is higher than the melting point of BeCl2 due to greater ionic nature of BaCl2.
S3 : The order of hydrated radii is : Al3+(aq)>Mg2+(aq)>Na+(aq)
- T T T
- T T F
- T F T
- F T T
The correct order of decreasing polarisability of ion is :
- Cl−>Br−>I−>F−
- F−>I−>Br−>Cl−
- I−>Br−>Cl−>F−
- F−>Cl−>Br−>I−
The correct increasing covalent nature is:
- NaCl<LiCl<BeCl2
- BeCl2<NaCl<LiCl
- BeCl2<LiCl<NaCl
- LiCl>NaCl>BeCl2
- MF>MCl>MBr>MI
- MF>MCl>MI>MBr
- MI>MBr>MCl>MF
- MCl>MI>MBr>MF
S1 : AgI is less soluble in water than AgF due to more polarization of I− in comparison to F− ion.
S2 : The melting point of BaCl2 is higher than the melting point of BeCl2 due to greater ionic nature of BaCl2.
S3 : The order of hydrated radii is : Al3+(aq)>Mg2+(aq)>Na+(aq)
- T T T
- T T F
- T F T
- F T T