where do the electrons go when group 1 metals react?
Answers
Answer:
Group 1 metals all have one electron in their outer shell. When they react they form positive metal ions by losing this electron. Since there is only one electron to lose, group 1 metals are all extrememely reactive.
Answer:
They form cations by losing their outermost electron.
Explanation:
Group 1 metals have only one electron in their outermost shell.They lose this outermost electron and form cations i.e. positively charged ions .
Group 1 elements are also known as alkali metals.
Their reactivity increases as we go down the group.
All the alkali metals have similar chemical properties because they all have only one electron in their outermost shell.
They are located in the first column of periodic table.
Alkali metals are highly reactive because they have larger atomic radii and low ionization energy.
Group 1 elements include lithium,sodium, potassium, rubidium, cesium and francium.
Ionization energy:-
This is the minimum amount of energy required to remove the outermost valence electron from an atom.
It decreases across the period and increases down the group in a periodic table.
Valence electron:-
The outermost electrons in a shell or energy level of an atom.
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