Table of Contents
- 1 Which alkali metal has highest hydration enthalpy value?
- 2 Which alkali metal ion has high hydration enthalpy Why?
- 3 Which has highest hydration enthalpy?
- 4 Which ion has greater degree of hydration?
- 5 Why hydration enthalpy of alkaline earth metal ions are larger than those of alkali metal ions?
- 6 Which alkali metal has lowest hydration enthalpy?
- 7 Which has higher hydration enthalpy among first and second group?
- 8 Which one has the highest hydration energy NA+ Li+ Cs+ K+?
- 9 What is the relationship between charge density and hydration enthalpy?
- 10 What is the enthalpy of hydration between M+G and M+AQ?
Which alkali metal has highest hydration enthalpy value?
Of all alkali metals, Li+ is thin, has a high density of charge and is thus the highest hydration energy of all alkali metals. Hydration enthalpy is considered the energy produced as a result of the forming of new bonds between ions and water molecules.
Which alkali metal ion has high hydration enthalpy Why?
Because Li+ is much smaller than the other alkali metal cations, it’s hydration energy is the highest.
Which is the correct order of hydration enthalpy of alkali metal?
Hence the correct order is: Li+>Na+>K+>Rb+>Cs+
Which has highest hydration enthalpy?
In the periodic table, the small lithium-ion has the highest hydration enthalpy in Group1 and the small fluoride ion has the highest hydration enthalpy in Group 7.
Which ion has greater degree of hydration?
Li+ ion has maximum degree of hydration.
What factors affect hydration enthalpy?
The size of the hydration enthalpy is governed by the amount of attraction between the ions and the water molecules.
- The attractions are stronger the smaller the ion. For example, hydration enthalpies fall as you go down a group in the Periodic Table.
- The attractions are stronger the more highly charged the ion.
Why hydration enthalpy of alkaline earth metal ions are larger than those of alkali metal ions?
The hydration enthalpies of alkaline earth metals is larger than that of alkali metals due to their small size. Hence, due to greater nuclear charge on divalent cations, cations of alkaline earth metals are smaller in size than the cations of alkali metals.
Which alkali metal has lowest hydration enthalpy?
Lithium ion
“Lithium ion has the smallest hydration enthalpy of all the alkali metals.” Answer.
What is the order of hydration enthalpy among the following ions?
Na+>Li+>K+>Cs+>Rb+
Which has higher hydration enthalpy among first and second group?
The hydration enthalpies of alkaline earth metal ions are larger than those of alkali metal ions. Thus, compounds of alkaline earth metals are more extensively hydrated than those of alkali metals.
Which one has the highest hydration energy NA+ Li+ Cs+ K+?
Correct option 1 Li+ > Na+ > K+ > Rb+ > Cs+ Explanation:Li⊕ having minimum radius so maximum hydration and maximum hydration radii.
What is the correct order of hydration enthalpies of alkali metal ions?
JEE Main 2019: The correct order of hydration enthalpies of alkali metal ions is – (A) Li+ > Na+ > K+ > Rb+ > Cs+ (B) Li+ > Na+ > K+ > Cs+ > Rb+ ( Tardigrade
What is the relationship between charge density and hydration enthalpy?
The magnitude of hydration enthalpy depends on the charge density of the ions. The charge density is more for smaller ions and hence the smaller ions have higher values of hydration enthalpy. The higher the charge density the higher will be the force of attraction between the ion and the water polar end.
What is the enthalpy of hydration between M+G and M+AQ?
This energy is expressed as the hydration enthalpy or enthalpy of hydration between M +(g) and M +(aq) is that in M +(aq) the ion is surrounded by water molecules forming a weak bond. Hydration enthalpy values of various elements are tabulated in the table given below.
What is the enthalpy of solvation of water?
It can be considered as enthalpy of solvation with the solvent being water. Hydration enthalpy is also called hydration energy and its values are always negative. For a chemical reaction, M + (g) + aq → M + (aq) Enthalpy change = ∆H Hyd. Water is considered to be a polar solvent because it has a positive (H atom) and negative (O atom) poles.