Li+ has maximum degree of hydration and for this reason lithium salts are mostly hydrated
The chemical reactivity of alkali metals increase when the atomic number increase.
The s-block elements consist of the alkali metals and alkaline earth metals, including hydrogen and helium. Most reactions of s-block elements involve the loss of an electron to form a singly positively charged ion.
Alkali metals get softer down Group 1 due to an increase in atomic size and weaker metallic bonding. As you move down the group, the atomic radius increases, leading to a decrease in the strength of metallic bonding and making the metals softer.
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.
Among alkali metals, lithium ions have the lowest ionic mobility in water due to its smaller size and stronger attraction to water molecules. This results in greater hydration energy, which makes it harder for lithium ions to move in water compared to larger alkali metal ions like potassium or cesium.
When an acid is added to a solution of an alkali, the pH of the solution will decrease. This is because the acid will increase the concentration of hydrogen ions, leading to a more acidic solution.
It is because alkali metals are larger in size than alkaline earth metals.Also, the effective nuclear charge is more in case of alkaline earth metals. This makes their ionization enthalpies larger than alkali metals.
As a strong acid is added slowly to a strong alkali, the pH will gradually decrease due to the neutralization reaction. Initially, the pH will increase as the alkali is added, then start to decrease as the acid is added until it reaches a neutral pH of 7 when the acid and alkali are fully neutralized.
The chemical reactivity of alkali metals increase when the atomic number increase.
What lead the increase in strength of alkali was to improve strength and reliability. Strengths and drying shrinkage is the reasons for the studies to improve alkali.
The s-block elements consist of the alkali metals and alkaline earth metals, including hydrogen and helium. Most reactions of s-block elements involve the loss of an electron to form a singly positively charged ion.
The solution become more and more alkaline and the pH increase.
Sodium, Potassium, and other alkali metals are very reactive due to the low ionization enthalpy. Flourine, Chlorine and other halogens are very reactive due to the high negative electron gain enthalpy.
Sodium, Potassium, and other alkali metals are very reactive due to the low ionization enthalpy. Flourine, Chlorine and other halogens are very reactive due to the high negative electron gain enthalpy.
Alkali metals get softer down Group 1 due to an increase in atomic size and weaker metallic bonding. As you move down the group, the atomic radius increases, leading to a decrease in the strength of metallic bonding and making the metals softer.
Lithium has a small ionic radius and high charge density, which allows it to have a strong attraction to the partial charges on the water molecule. This leads to a stronger ion-dipole interaction with water compared to other larger alkali metal ions.
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.