Chemical properties of alkali metals
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Alkali metals take up the leftmost side of the periodic table. The group 1 elements consist of elements:
Lithium (Li)Sodium (Na)Potassium (K)Rubidium (Rb)Caesium (Cs)Francium (Fr)
They belong to the s-block elements of the periodic table as their outermost electron enters the s orbital giving them the electronic configuration of ns1.
As the alkali metals have only 1 electron in their valence shell, they readily lose it, making them count among the most reactive elements on earth. Thus, they are highly electropositive metals. They are called alkali metals because they form strongly alkaline hydroxides with water.
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Lithium (Li)Sodium (Na)Potassium (K)Rubidium (Rb)Caesium (Cs)Francium (Fr)
They belong to the s-block elements of the periodic table as their outermost electron enters the s orbital giving them the electronic configuration of ns1.
As the alkali metals have only 1 electron in their valence shell, they readily lose it, making them count among the most reactive elements on earth. Thus, they are highly electropositive metals. They are called alkali metals because they form strongly alkaline hydroxides with water.
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The chemical property of alkali metals:
Alkali metals are highly reactive metals because of their large size and low ionization enthalpy. Their reactivity increases on moving down the group.
Reactivity towards air: When these metals are kept in dry air, they get tarnished due to the formation of oxides, which become hydroxides on reacting with moisture. The reaction of alkali metals with oxygen is an exothermic reaction. The oxidation state +1.
Example: 4 Li + O2 → 2Li2O (oxide)Reactivity towards dihydrogen:Hydroxide and dihydrogen are formed when an alkali metal reacts with water.
Example: 2M + 2H2O → 2M+ + 2OH– + H2 (M = alkali metal)Reactivity towards dihydrogen: At 673 K, alkali metals reacts with dihydrogen to form hydrides.
Example: 2M + H2 → 2M + H–Reactivity towards halogen: Alkali metals react vigorously with halogens to form ionic halides M+X–.Reducing nature: Alkali metals are a strong reducing agent. Among them, lithium is the strongest, sodium being the least reducing agent.Solutions in liquid ammonia: Alkali metals are soluble in liquid ammonia and form a blue solution which is conducting in nature.
Alkali metals are highly reactive metals because of their large size and low ionization enthalpy. Their reactivity increases on moving down the group.
Reactivity towards air: When these metals are kept in dry air, they get tarnished due to the formation of oxides, which become hydroxides on reacting with moisture. The reaction of alkali metals with oxygen is an exothermic reaction. The oxidation state +1.
Example: 4 Li + O2 → 2Li2O (oxide)Reactivity towards dihydrogen:Hydroxide and dihydrogen are formed when an alkali metal reacts with water.
Example: 2M + 2H2O → 2M+ + 2OH– + H2 (M = alkali metal)Reactivity towards dihydrogen: At 673 K, alkali metals reacts with dihydrogen to form hydrides.
Example: 2M + H2 → 2M + H–Reactivity towards halogen: Alkali metals react vigorously with halogens to form ionic halides M+X–.Reducing nature: Alkali metals are a strong reducing agent. Among them, lithium is the strongest, sodium being the least reducing agent.Solutions in liquid ammonia: Alkali metals are soluble in liquid ammonia and form a blue solution which is conducting in nature.
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