Alkali metals belong to the s-block elements occupying the leftmost side of the periodic table. Alkali metals readily lose electrons, making them count among the most reactive elements on earth. In this article, we will explain the electronic configurations, ionization enthalpy, hydration enthalpy Contact online >>
Alkali metals belong to the s-block elements occupying the leftmost side of the periodic table. Alkali metals readily lose electrons, making them count among the most reactive elements on earth. In this article, we will explain the electronic configurations, ionization enthalpy, hydration enthalpy and atomic, ionic radii and other physical and chemical properties of the group one alkali metals.
In general, ‘alkali’ refers to the basic or alkaline nature of their metal hydroxides. The compounds are called alkali metals because when they react with water, they usually form alkalies which are nothing but strong bases that can easily neutralise acids.
Alkali metals have a corresponding [Noble gas] ns1 electronic configuration. They occupy the first column of the periodic table. Alkali elements are Lithium(Li), Sodium(Na), Potassium (K), Rubidium (Ru), Cesium (Cs) and Francium (Fr), occupying successive periods from first to seven. Francium is a radioactive element with a very low half-life.
However, the main reason why hydrogen (H) is not considered an alkali metal is that it is mostly found as a gas when the temperature and pressure are normal. Hydrogen can show properties or transform into an alkali metal when it is exposed to extremely high pressure.
Down the column, the nuclear charge increases, and a new orbital gets added to each alkali atom. Here, we will discuss some important trends in the physical properties of alkali metals as we go down the column.
Having the largest radius and volume, alkali elements have the lowest density. So, they are very soft and can be cut with a knife. Lithium, sodium and potassium are lighter than water. Potassium has the lowest density among alkali metals.
Alkali metals will donate a single valence electron to get a noble gas configuration. Thus, they are all univalent electropositive metals. The ionization energy needed for the removal of the valence electron will be highest for the small lithium atom.
With increasing atomic size, the valence electron gets shielded by the inner electrons and becomes easily removable with less energy requirement. Hence, the ionization energy decreases with an increasing atomic number.
Lithium-ion is the most soluble, and the solubility decreases with increasing size, so the Cesium ion is the least water-soluble alkali metal ion. Solubility in water is related to the ionic nature and size. Smaller ions have higher charge density and can be solvated by more water molecules. This releases a higher enthalpy of hydration and makes the hydrated ions more stable.
As ionization energy decreases down the column, reducing property is expected to increase from lithium to caesium. While reducing ability increases from sodium to caesium, lithium has the highest reduction potential (-3.04V) and is the strongest reducing agent of all elements.
Alkali metals react with water to form basic hydroxides and liberate hydrogen. The reaction of the metal is exothermic, and the enthalpy increases from lithium to caesium. Alkali metal floats on the water during the reaction.
The density of Sodium and potassium is lower than water. In heavier alkali metals, reaction enthalpy is high such that the metal gets melted and raises to the surface. Hence, the reaction with water becomes faster, highly exothermic and explosive, leading to fire from lithium to caesium.
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