Ionization energy of halogens compare to alkali metals
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Alkali metals
Alkali metals have less density compared to other metals.
They have loosely bound valence electron
They contain large radii in the period
They have low ionization energy and electronegativity.
They are highly reactive in nature
Halogens
These are high reactive elements in the group and have high electron affinity.
They have low dissociation energy which means they can dissociate very easily to combine with other substances.
They are highly volatile and are readily reacted with alkali metals and alkaline earth metals.
Halogens readily react with hydrogen to form hydrogen halides as binary compounds.
Reactivity
In the outermost shell of the alkali metals, they have 1 electron, by loosing that electron, the alkali metals get the stable electronic configuration. In case of halogens, they are electron short in the outermost shell, adding an electron it creates a stable electronic configuration. As we move from lithium to francium, the electrons are further more away from the nucleus, hence it is easy to remove an electron from the outermost shell.
In case of halogens, when we go up in the series, the electrons are much closer to the nucleus hence more will be the electronegativity of the element. Hence in the alkali metals and halogens, the most reactivity combination would be ceasium – fluoride.
The common thing in both alkali metals and halogens is the chemistry of loosing and gaining the electrons. Since the alkali metals and halogens comes under 1st group and 17th group, they have one electron and seven electrons in the outermost shell. Alkali metals lose an electron to gain valency +1 and halogens gain an electron to attain -1 valence. In this way, both posses same valence number but one looses and one gains. Hence this is also the major reason for the attraction of these elements.
Alkali metals have less density compared to other metals.
They have loosely bound valence electron
They contain large radii in the period
They have low ionization energy and electronegativity.
They are highly reactive in nature
Halogens
These are high reactive elements in the group and have high electron affinity.
They have low dissociation energy which means they can dissociate very easily to combine with other substances.
They are highly volatile and are readily reacted with alkali metals and alkaline earth metals.
Halogens readily react with hydrogen to form hydrogen halides as binary compounds.
Reactivity
In the outermost shell of the alkali metals, they have 1 electron, by loosing that electron, the alkali metals get the stable electronic configuration. In case of halogens, they are electron short in the outermost shell, adding an electron it creates a stable electronic configuration. As we move from lithium to francium, the electrons are further more away from the nucleus, hence it is easy to remove an electron from the outermost shell.
In case of halogens, when we go up in the series, the electrons are much closer to the nucleus hence more will be the electronegativity of the element. Hence in the alkali metals and halogens, the most reactivity combination would be ceasium – fluoride.
The common thing in both alkali metals and halogens is the chemistry of loosing and gaining the electrons. Since the alkali metals and halogens comes under 1st group and 17th group, they have one electron and seven electrons in the outermost shell. Alkali metals lose an electron to gain valency +1 and halogens gain an electron to attain -1 valence. In this way, both posses same valence number but one looses and one gains. Hence this is also the major reason for the attraction of these elements.
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