The only one that does move is the outer electron. That is why they have a valency of 1 and it is also why their reactivity increases down the group as the attraction of the nucleus becomes less as the outter electron becomes further away from it.
Group 1- the Alkali metals and also Hydrogen.
Group 1 elements (alkali metals such as sodium, potassium) lose 1 electron to form ions with a +1 charge.
Alkali metals belong to Group 1 of the periodic table and include elements like lithium, sodium, and potassium. Group 2 metals are known as alkaline earth metals and include elements like magnesium and calcium. The main difference is that alkali metals are more reactive than Group 2 metals because they have one valence electron, while Group 2 metals have two valence electrons.
The group 1 metals, namely lithium, sodium, potassium, rubidium, cesium, and francium (although francium is exceedingly rare and unstable) all easily lose a single electron to form +1 ions. Many other metals (especially the group 2 metals) also readily give up electrons to form ions, although the group 1 elements are by far the most reactive in this regard.
That element would be in the Alkali Metals (group one)
Alkali metals, Ist group.
Alkali metals
Group 1- the Alkali metals and also Hydrogen.
The alkali metals in group 1 react by losing one electron.
This group is known as the alkali metals, and they consist of elements in Group 1 of the periodic table such as sodium and potassium. Having one electron in their outer level makes them highly reactive and eager to lose that electron to achieve a stable electron configuration.
Alkali metals
These metals lose easily an electron.
Group 1 elements (alkali metals such as sodium, potassium) lose 1 electron to form ions with a +1 charge.
Group I elements (that is alkali metals)
Alkali metals belong to Group 1 of the periodic table and include elements like lithium, sodium, and potassium. Group 2 metals are known as alkaline earth metals and include elements like magnesium and calcium. The main difference is that alkali metals are more reactive than Group 2 metals because they have one valence electron, while Group 2 metals have two valence electrons.
Group one metals are the Alkali Metals, but Hydrogen is placed in group one because of its electron arrangement. All group one metals have one electron in their valence shell (outer most shell) and hydrogen is no exception. It has one electron in its last shell, and is therefore placed in group one even though it is not an alkali metal.
The group 1 metals, namely lithium, sodium, potassium, rubidium, cesium, and francium (although francium is exceedingly rare and unstable) all easily lose a single electron to form +1 ions. Many other metals (especially the group 2 metals) also readily give up electrons to form ions, although the group 1 elements are by far the most reactive in this regard.