Hydration Energy (Group 1)
Trending Questions
- Rb+>K+>Na+>Li+
- K+>Rb+>Na+>Li+
- Li+>Na+>K+>Rb+
- Na+>K+>Rb+>Li+
- Li+>Na+>K+>Cs+>Rb+
- Na+>Li+>K+>Rb+>Cs+
- Li+>Na+>K+>Rb+>Cs+
- Na+>Li+>K+>Cs+>Rb+
- Schottky defect
- Frenkel defect
- Impurity defect
- Formation of F-centers
- Mg2+
- Sr2+
- Ca2+
- Be2+
All compounds of alkali metals are easily soluble in water but lithium compounds are more soluble in organic solvents. Explain
The ease of adsorption of the hydrated alkali metal ions on an ion-exchange resin follows the order:
Li+<K+<Na+<Rb+
Rb+<K+<Na+<Li+
K+<Na+<Rb+<Li+
Na+<Li+<K+<Rb+
Why Li compounds are soluble in organic solvents?
ionic species having largest size:
A. Li+(g)
B.Na+ (aq)
C. Rb+(aq)
D. Li+(aq)
- Li⊕>Na⊕>K⊕>Rb⊕
- Rb⊕>Na⊕≡K⊕>Li⊕
- Li⊕<Na⊕<K⊕<Rb⊕
- Na⊕≡K⊕>Rb⊕>Li⊕
- Rb+
- Na+
- K+
- Li+
- BeF2 forms a complex with NaF in which, beryllium acts as the cation
- Be dissolves in alkali forming [Be(OH)4]2−
- LiCI is soluble in pyridine
- Alkali metal ions have high hydration enthalpies owing to their small size
- Schottky defect
- Frenkel defect
- Impurity defect
- Formation of F-centers
Identify the correct order of the size of the following:
Ca2+<Ar<K+<Cl−<S2−
Ca2+<K+<Ar<S2−<Cl−
Ca2+<K+<Ar<Cl−<S2−
Ar<Ca2+<K+<Cl−<S2−
- Li+
- Na+
- K+
- Rb+
Ionic mobility of which of the following alkali metal ions is lowest when aqueous solution of their salts are put under an electric field?
- K
- Rb
- Li
- Na
- Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
- Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- Assertion is correct but Reason is incorrect
- Both Assertion and Reason are incorrect
- The hydration energy of Na2SO4 is more than its lattice energy
- The lattice energy of BaSO4 is more than its hydration energy
- The lattice energy has no role to play in solubility
- The lattice energy of Na2SO4 is more than its hydration energy
Sodium sulphate is soluble in water but barium sulphate is sparingly soluble because
The hydration enthalpy of Na2SO4 is more than its lattice enthalpy
The lattice enthalpy of BaSO4 is more than its hydration enthalpy
The lattice enthalpy has no role to play in solubility
The lattice enthalpy of Na2SO4 is more than its hydration enthalpy
- the hydration energy of sodium sulphate is more than its lattice energy.
- the lattice energy of barium sulphate is more than its hydration energy.
- the lattice energy has no role to play in solubility.
- the hydration energy of sodium sulphate is less than its lattice energy.
- K+>Rb+>Na+>Li+
- Rb+>K+>Na+>Li+
- Li+>Na+>K+>Rb+
- Na+>K+>Rb+>Li+
Which has more lattice energy? NaF or NaCl.
NaCl
NaF
Same
Data Insufficient
Answer whether the above statement is true or false.
If true enter 1, else 0
Which of the following is a correct Irving-Williams order (tendency of complex formation)?
- Ni2+<Co2+<Fe2+<Mn2+
- Mn2+<Fe2+<Co2+<Ni2+
- Co2+<Mn2+<Fe2+<Ni2+
- Fe2+<Mn2+<Ni2+<Co2+
When mercuric iodide is added to an aquous solution of KI, the
- freezing pointis raised
- freezing point is lowered
- boiling point does not change
- freezing point does not change
- Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
- Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- Assertion is correct but Reason is incorrect
- Assertion is incorrect but Reason is correct