Why are alkaline earth metal hydroxides less basic than alkali metal hydroxides?

ions as their ionization enthalpies are lower than alkaline earth metals. Hence, the oxides of alkali metals are more basic than the corresponding alkaline earth metal oxides. Hence, the solubility of hydroxides of alkaline earth metals is lower than corresponding hydroxides of alkali metals.

Why alkaline earth metal oxides are less basic than those of alkali metals?

This happens due to the highly electropositive nature of alkali metals, which makes these oxides highly ionic. Hence, they readily dissociate in water to give hydroxide ions. This is because alkaline earth metals are less electropositive than alkali metals.

Are alkaline earth metals less basic than alkali metals?

Compare the alkali metals and alkaline earth metals with respect to (i) ionisation enthalpy (ii) basicity of oxides and (iii) solubility of hydroxides.

How do the hydroxides of the alkali metals differ from those of the alkaline earth metals?

Nature of the Metal Hydroxide Alkali Metals: Hydroxides of alkali metals are strongly basic. Alkaline Earth Metals: Hydroxides of alkaline earth metals are relatively less basic.

Why are alkaline earth metals Basic?

As with the alkali metals of Group 1 (Ia), the atoms of the alkaline-earth metals easily lose electrons to become positive ions (cations). The oxides of the alkaline-earth metals are basic (i.e., alkaline, in contrast to acidic).

Why are hydroxides of Group II metals less basic than those of group I two points?

Because the first ionization energy of the alkali metals decreases down the group, it is easier for the outermost electron to be removed from the atom and participate in chemical reaction, thus increasing reactivity down the group.

Why are the hydroxides of Group 2 weaker bases than the hydroxides of Group 1?

The Mg2+ ions in Mg(OH)2 will exert a greater pull on the electrons from the OH- ions than the Na+ ions will. This means that it is easier to break the sodium to hydroxide bonds than the magnesium to hydroxide bonds making group one bases more soluble and so stronger.

Why hydroxides of alkali metals are basic in nature?

The hydroxides are basic in nature and basic strength increases down the group. This is due to the low ionization energies of these metals where the M-O bond in MOH is weak and it can cleave to give OH- ions in solution. As the ionization energy decreases down the group, the basic strength of the hydroxides increases.

Why hydroxides of alkali metals are strong bases?

The alkali metal hydroxides are the strongest of all bases because the dissolve freely in water with evolution of much heat on account of intense hydration.

Why hydroxides of alkali metal are basic in nature?

What would be the basic predominance of hydroxides of the following alkaline earth metals?

Alkali metal

Why are hydroxides less basic than alkali earth metals?

However, these hydroxides are less basic than the corresponding alkali metal hydroxides because of higher ionization energies, smaller ionic sizes and greater lattice energies. Alkaline earth metals hydroxides are less soluble in water as compared to alkali metals.

What is the solubility of alkaline earth metals in water?

(ii) Solubility in Water. Alkaline earth metals hydroxides are less soluble in water as compared to alkali metals. The solubility of the alkaline earth metal hydroxides in water increases with increase in atomic number down the group.

Why do alkaline earth metals have a high lattice entalpy?

This is because hydroxides of alkaline earth metals have high lattice entalpy due to small size and more charge as compared to alkali metals, so they don’t disssociate easily in water . The strength of both bases and acids depends upon how completely they dissociate in water.

What are the properties of halides of alkaline earth metals?

Properties of Halides of Alkali Earth Metals All beryllium halides are essentially covalent and are soluble in organic solvents. The halides of all other alkaline earth metals are ionic. Except BeCl 2 all other chlorides of group 2 form hydrates but their tendency to form hydrates decreases for eg –